EP 6 Make up Exam--you must write answers in your notebook

Match each item with the correct statement below.
a. substitution reaction J hydrogenation reaction
b. addition reaction k. dehydrogenation reaction
c. hydration reaction l. asymmetric carbon
d. substituent m. trans configuration
e. structural isomers n. cis configuration
f. geometric isomers o. lignite
g. stereoisomers p. bituminous coal
h. aromatic compound q aliphatic hydrocarbon
i anthracite coal


____ 1. a reaction in which an atom or group of atoms replaces another atom or group of atoms

____ 2. a reaction in which a substance is added at the double or triple bond of an alkene or alkyne

____ 3. a reaction involving the addition of hydrogen to a carbon—carbon double bond to produce an alkane

____ 4. a reaction involving the addition of water to an alkene

____ 5. a reaction involving the loss of hydrogen
____ 6. atom or group of atoms that can take the place of a hydrogen in a parent hydrocarbon molecule

____ 7. compounds that have the same molecular formula, but the atoms are joined in a different order

____ 8. arrangement in which substituted groups are on the same side of a double bond

____ 9. molecules in which atoms are joined in the same order but differ in the arrangements of their atoms in space

____ 10. arrangement in which substituted groups are on opposite sides of a double bond

____ 11. compounds that differ in the orientation of groups around a double bond

____ 12. carbon atom to which four different atoms or groups are attached
__ 13. any straight-chain or branched-chain alkane, alkene, or alkyne

____ 14. any hydrocarbon compound in which a ring has bonding similar to benzene

____ 15. hard coal, having a carbon content of over 80%

____ 16. brown coal, having a carbon content of approximately 50%

____ 17. soft coal, having a carbon content of 70–80%

Multiple Choice ( 5 points each, 25 points total)
Identify the letter of the choice that best completes the statement or answers the question.

____ 18. Aldehydes have the general structure ____________.
a.
c.

b.
d.



____ 19. A ketone has the general structure ____________.
a.
ROR c.

b.
d.





____ 20. Which carbon skeleton contains a carboxyl group?
a.
CCCO c.

b.

d.



____ 21. Which of the following carbon skeletons represents a carboxylic acid?
a.
CCCCCO c.

b.

d.



____ 22. Which carbon skeleton represents an ester?
a.
CCCCCOCC c.

b.
d.



Short Answer ( 20 points each, 80 points total)

23. Write an equation using structural formulas for the reaction of benzene and chlorine.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

24. Write complete, balanced equations for the reaction of 2-pentene and water. Use structural formulas.
____________________________________________________________________________________________________________________________________________________________________________
______________________________________________________________________________________
______________________________________________________________________________________
______________________________________________________________________________________





25. What is the expected product when the following compound is oxidized?
CH CH CH CH OH
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

26. Complete the condensation polymerization reaction between two amino acids to form a peptide bond:

______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

Problem ( 20 points each 340 points total)

27.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

28.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

29. Write an equation for the synthesis of
a. 2-chlorobutane from 1-butene and hydrogen chloride
b. bromobenzene from benzene and bromine
______________________________________________________________________________________


______________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________


30.
______________________________________________________________________________________


______________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________


31.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

32.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

33. Write the structural formula for each of the following compounds.
a. 3-ethyl-2,3-dimethylpentane
b. 3,4-diethylhexane
c. 2,3,4,5-tetramethylnonane
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________


34.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

35.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

36.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

37.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

38. Match the description with the appropriate description.


39. Identify the hydrogen ion donor(s) and hydrogen ion acceptor(s) for ionization
of H2SO4 in water. Label the conjugate acidbase pairs.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

40. Classify the following acids as monoprotic, diprotic, or triprotic.
a. HCOOH b. HBr c. H2SO3 d. H3ClO4
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

41. Rank 1M of these compounds in order of increasing hydrogen ion
concentration: weak acid, strong acid, strong base, weak base.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

42. Write the expression for the acid dissociation constant of the strong acid
hydrofluoric acid, HF. ______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________


43. Describe a polymerization condensation reaction. Give an example.
______________________________________________________________________________________

EP 5 Make up Exam--Write answers in your notebook

you must write the vocab out.

Match each item with the correct statement below.
a. Boyle's law i. Graham's law
b. Charles's law f. Gay-Lussac's law
c. Dalton's law g. ideal gas law

d. effusion h. diffusion
e. compressibility i. partial pressure

f. Henry's law j. supersaturated solution
g. immiscible k concentration
h. saturated solution

____ 1. For a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure.

____ 2. The volume of a fixed mass of gas is directly proportional to its Kelvin temperature, if the pressure is kept constant.

____ 3. The pressure of a gas is directly proportional to its Kelvin temperature if the volume is kept constant.

____ 4. P  V = n  R  T

____ 5. At constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases.

____ 6. The rate at which a gas will effuse is inversely proportional to the square root of the gas’s molar mass.

____ 7. a measure of how much the volume of matter decreases under pressure

____ 8. the pressure exerted by a gas in a mixture

____ 9. the escape of gas through a small hole in a container

____ 10. tendency of molecules to move to regions of lower concentration


____ 11. describes liquids that are insoluble in one another

____ 12. solution containing maximum amount of solute

____ 13. solution containing more solute than can theoretically dissolve at a given temperature

____ 14. At a given temperature, the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid.

____ 15. measure of the amount of solute dissolved in a specified quantity of solvent

Multiple Choice ( 5 points each, 35 points total)
Identify the letter of the choice that best completes the statement or answers the question.

____ 16. To increase the solubility of a gas at constant temperature from 1.20 g/L, at 1.4 atm, to 2.3 g/L, the pressure would have to be increased to ____.
a. 0.37 atm c. 1.37 atm
b. 0.7 atm d. 2.7 atm


____ 17. What is the molarity of a solution containing 7.0 moles of solute in 569 mL of solution?
a. 81M c. 12M
b. 0.081M d. 4.0M


____ 18. What is the molarity of a solution containing 56 grams of solute in 959 mL of solution? (molar mass of solute = 26 g/mol)
a. 1.5M c. 2.1M
b. 2.2M d. 0.0022M


____ 19. The volume of alcohol present in 620 mL of a 40.0% (v/v) solution of alcohol is ____.
a. 372 mL c. 248 mL
b. 40.0 mL d. 580 mL


____ 20. What is the molality of a solution containing 8.0 grams of solute in 0.50 kg of solvent? (molar mass of solute = 24 g)
a. 0.67m c. 1.67m
b. 4m d. 0.17m


____ 21. The freezing point of a solution that contains 0.550 moles of NaI in 615 g of water is ____. (K = 1.86 C/m; molar mass of water = 18 g)
a. 1.66 C c. 3.33 C
b. –1.66 C d. –3.33 C


____ 22. What is the boiling point of a solution that contains 3 moles of KBr in 2000 g of water? (K = 0.512 C/m; molar mass of water = 18 g)
a. 97 C c. 101.4 C
b. 99.7 C d. 103 C


Short Answer (10 points each, 40 points total)

23. The gaseous product of a reaction is collected in a 25.0-L container at 27 C. The pressure in the container is 300.0 kPa and the gas has a mass of 96.0 g. How many moles of the gas are in the container?
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
24. What is the pressure exerted by 32 g of O in a 22.0-L container at 30.0 C?
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
25. A mixture of gases at a total pressure of 95 kPa contains N , CO , and O . The partial pressure of the CO is 24 kPa and the partial pressure of the N is 48 kPa. What is the partial pressure of the O ?
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
26. Use Graham’s law to calculate how much faster fluorine gas, F , will effuse than chlorine gas, Cl , will. The molar mass of F = 38.0; the molar mass of Cl = 70.9.
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
Problem (15 pts each, 235 points total)

27. Use kinetic theory to explain why on a cold autumn morning a camper’s air
mattress may appear to be somewhat flatter than when it was blown up the
afternoon before. Assume no leaks.
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
28. A sample of O2 with an initial temperature of 50.0C and a volume of 105 L
is cooled to 25C. The new pressure is 105.4 kPa and the new volume is
55.0 L. What was the initial pressure of the sample?
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
29. Is it possible for a balloon with an initial pressure of 200.0 kPa to naturally
expand to four times its initial volume when the temperature remains
constant and atmospheric pressure is 101.3 kPa?
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
30. A 35.0-L tank contains 7.00 mol of compressed air. If the pressure inside the
tank is 500.0 kPa, what is the temperature of the compressed gas?
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
31. What is the volume occupied by 0.355 mole of nitrogen gas at STP?
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
32. A gaseous mixture consisting of nitrogen, argon, and oxygen is in a 3.5-L vessel
at 25C. Determine the number of moles of oxygen if the total pressure is 98.5
kPa and the partial pressures of nitrogen and argon are 22.0 kPa and 50.0 kPa,
respectively.
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
33. Compare the effusion rates of O2 (molar mass, 32.0 g/mol) and N2 (molar mass,
28.0 g/mol).
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
34. The volume of a gas at 155.0 kPa changes from 22.0 L to 10.0 L. What is the
new pressure if the temperature remains constant
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
35. 1. In your own words, explain hydrogen bonds.
a. Draw a diagram of the hydrogen bonding between three water molecules.
b. Explain why the density of ice at 0°C is less than the density of liquid water at 0°C.
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
36. Which of the following compounds are soluble in water? Which are insoluble?
a. CaCl2
b. N2
c. HBr
d. NH2C2H3O2
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

37. 1. Distinguish colloids and suspensions from solutions by discussing their
properties. Classify each of the following mixtures as a colloid, suspension, or solution.
a. fog
b. milk
c. sodium chloride dissolved in water
d. cornstarch in water
e. potting soil shaken with water
f. soap suds
g. a mixture of sucrose and water
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
38. The solubility of CO2 in water at 1.22 atm is 0.54 g/L. What is the solubility of
carbon dioxide at 1.86 atm? Assume that temperature is constant.
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
39. Calculate the molarity of each of the following solutions.
a. 0.40 mol of NaCl dissolved in 1.6 L of solution
b. 20.2 g of potassium nitrate, KNO3, in enough water to make 250.0 mL of
solution
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
40. Calculate the number of grams of solute needed to prepare each of the
following solutions.
a. 2500.0 mL of a 3.0M solution of potassium hydroxide, KOH
b. 2.0 liters of 2.0M nitric acid, HNO3, solution
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
41. What is the concentration in percent by volume, %(v/v), of the following
solutions?
a. 60.0 mL of methanol in a total volume of 500.0 mL
b. 25.0 mL of rubbing alcohol (C3H7OH) diluted to a volume of 200.0 mL
with water
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
42. What is the boiling point of a solution that contains 2 mol of magnesium
chloride in 100.0 g of water?
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
43. Calculate the mole fraction of solute in each of the following solutions.
a. 3.0 moles of lithium bromide, LiBr, dissolved in 6.0 moles of water
b. 125.0 g of potassium nitrate, KNO3, dissolved in 800.0 g of water
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

Essay (20 pts each, 60 pts total)

44. What are some of the differences between a real gas and an ideal gas? ________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

45. Explain on a particle basis how the addition of a solute affects the boiling point, the freezing point, and the vapor pressure of the solvent. ________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________


46. Compare and contrast molarity and molality.
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

EP 4 Make up Exam--must be hand written in notebook

Matching ( five points each, 120 points in all)
Match each item with the correct statement below.
a. absolute zero m. mass
b. Kelvin temperature scale n. significant figure
c. Celsius temperature scale o. precision
d. weight p. accuracy

e. proton q. electron
f. nucleus r. neutron
g. atom s. periodic law
h. electronegativity t. cation
i. ionization energy u. period
j. atomic radius v. group
k. metal w. electrons
l. transition metal x. Mr. Gary

____ 1. closeness to true value

____ 2. narrowness of range of measurements

____ 3. known or estimated in a measurement

____ 4. the quantity of matter an object contains

____ 5. the lowest point on the Kelvin scale

____ 6. the SI scale for temperature

____ 7. the force of gravity on an object

____ 8. the non-SI scale for temperature

____ 9. the smallest particle of an element that retains the properties of that element

____ 10. a positively charged subatomic particle

____ 11. a negatively charged subatomic particle

____ 12. a subatomic particle with no charge

____ 13. the central part of an atom, containing protons and neutrons


____ 14. horizontal row in the periodic table

____ 15. vertical column in the periodic table

____ 16. A repetition of properties occurs when elements are arranged in order of increasing atomic number.

____ 17. type of element that is a good conductor of heat and electric current

____ 18. type of element characterized by the presence of electrons in the d orbital

____ 19. one-half the distance between the nuclei of two atoms when the atoms are joined

____ 20. type of ion formed by Group 2A elements

____ 21. subatomic particles that are transferred to form positive and negative ions

____ 22. ability of an atom to attract electrons when the atom is in a compound

____ 23. energy required to remove an electron from an atom

Multiple Choice (5 points each. 40 pts in all)
Identify the letter of the choice that best completes the statement or answers the question.

____ 24. The expression of 5008 km in scientific notation is ____.
a. 5.008 10 km c. 5.008 10 km
b. 50.08 10 km d. 5.008 10 km


____ 25. Which of the following measurements contains two significant figures?
a. 0.004 00 L c. 0.000 44 L
b. 0.004 04 L d. 0.004 40 L


____ 26. Which group of measurements is the most precise? (Each group of measurements is for a different object.)
a. 2 g, 3 g, 4 g c. 2 g, 2.5 g, 3 g
b. 2.0 g, 3.0 g, 4.0 g d. 1 g, 3 g, 5 g




____ 27. How many significant figures are in the measurement 0.003 4 kg?
a. two c. five
b. four d. This cannot be determined.


____ 28. How many significant figures are in the measurement 40,500 mg?
a. two c. four
b. three d. five


____ 29. Why did J. J. Thomson reason that electrons must be a part of the atoms of all elements?
a. Cathode rays are negatively-charged particles.
b. Cathode rays can be deflected by magnets.
c. An electron is 2000 times lighter than a hydrogen atom.
d. Charge-to-mass ratio of electrons was the same, regardless of the gas used.


____ 30. Who conducted experiments to determine the quantity of charge carried by an electron?
a. Rutherford c. Dalton
b. Millikan d. Thomson


____ 31. How do the isotopes hydrogen-1 and hydrogen-2 differ?
a. Hydrogen-2 has one more electron than hydrogen-1.
b. Hydrogen-2 has one neutron; hydrogen-1 has none.
c. Hydrogen-2 has two protons; hydrogen-1 has one.
d. Hydrogen-2 has one proton; hydrogen-1 has none.


Problem (20 pts each. 180 pts in all)

32.

33. Write a complete electron configuration of each atom.
a. hydrogen
b. vanadium
c. magnesium
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________



34.
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________


35. Why would you expect lithium (Li) and sulfur (S) to have different chemical and
physical properties? Three reasons
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________


36. Compare the first ionization energy lithium to that of beryllium.
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________



37. Compare the elements in group 1 with the elements in group 7, in terms of electronegativity, ionization, and atomic radii?
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________



38. Explain why the sulfide ion (S2) is larger than the chloride ion (Cl).
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________



39. Identify each property--DEFINE THEM and then, which is more characteristic of a metal or a nonmetal.

1. a gas at room temperature
2. brittle
3. malleable
4. poor conductor of electric current
5. shiny
6. ductile
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________




40. The Mg2+ and Na+ ions each have ten electrons. Which ion would you expect to have the smaller radius? Explain your choice
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________



41. Identify each process as a chemical or physical change.
1 melting of iron
2 lighting a match
3 grinding corn
4 souring of milk
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________




Essay (20 pts each. 100 pts in all)

42. Explain how Dalton improved upon atomic theory more than 2000 years after Democritus’s hypotheses about atoms.
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________



43. What observations by Rutherford led to the hypothesis that atoms are mostly empty space, and that almost all of the mass of the atom is contained in an atomic nucleus?
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________



























































































44. Describe the trends in first ionization energy within groups and across periods in the periodic table. Provide examples.
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________




45. Positive ions are smaller than the atoms from which they are formed, but negative ions are larger than the atoms from which they are formed. Explain why this is so.

________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________



46. Describe the trends in electronegativity within groups and across periods in the periodic table. Provide examples.

________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

Assignments for July 27 week

EP 4 HW: Read ch 7.1 and 7.2 Do Vocabulary definitions due from end of chapter 7, and answer questions page 193 1-11 (#11 bonus due to difficulty) due next week during NOTEBOOK CHECK

Topics: Ionic bonds--defined, nature of, and properties. Introduction to naming rules and molecular geometry--VSEPR.

Powerpoint presentation: Ch 7 Introduction to Ionic Bonds--clarification of electronegativity and origin of electrons within the bond, and geometry and Ch 7.1 Naming of ionic bonds and charge

Prep for lab 7.1: Molecular models using Valence Shell Electron Pair Repulsion Theory VSEPR

helpful link: http://www.chem.purdue.edu/gchelp/vsepr/rules2.html

EP 5: HW: Read Ch 17.1 and 17.2 Thermochemistry. Do Vocabulary definitions from end of ch 17. Do problems 1-8 17.1

Topics: Thermochemistry introduction--enthalpy, specific heat, and heat of reaction. Introduction to phase diagramming and state of matter transformation and corresponding heat of formation, heat of vaporization, etc.

Powerpoint presentation: Ch 18 Introduction to Thermochemistry and key terms. Ch 18.1 Phase Diagrams and Kinetic Theory of phases.

prep for lab for next week: Bomb Calorimetry.

EP 6: HW: Read Ch 19.4 and 19.5 Buffers in Acidic/Basic environments. Do problems in section 19.5.

Topics: Buffers--properties, reactions, and creation. Use of Ka and Kb in acid/base concentration calculations along with the autoionization of water equation and Kw constant. Introduction to Titration

Powerpoint: Ch 19.5 Buffers--studying the bicarbonate buffer and subsequent pertinent equations and reactions.

Prep for demonstration lab: Titration and pH reading using indicators.

Bonus: What are occupations that are specifically using Organic Chemistry

Debate League 3 at Patumwan Demonstration School Results

AC 1 of Vitchitpol, Thanakorn, and Suthipat ran into some solid teams from PDS1 and TU1, unfortunately, it wasn't our day as the adjudicators felt we fell a bit short in our arguments while the team of AC 2 faced PDS 2 and PDS 1, pulling off the upset of PDS 1--they of EUTU Finals fame--winning in a clear decision.

Congratulations to AC 2--Jakkrapat, Apinut, and Sathuwut of EP 6/1.

The debaters had a great time as the league continues to introduce debate to many new high schoolers. PDS had about 25 people while SES brought in another 15. It was a very successful tourney.

Round 4 is at AC on August 29th.

THB: PSP's should be legal in Schools the Opposition Whip speech

Opposition Whip

THB: PSP's should be legal in Schools the Government Whip speech

Government Whip speech

Chemistry Events/Reading

EP 6 Read Ch 19.4 and 19.5
EP 5 Read Ch 16.4
EP 6 Read Ch 7.1 and 7.2

Did I mention...have a great weekend?

Re-test will be posted this weekend

I don't want people to do it unless you need to. we can make it a bonus if you want to

Make up Exam will be posted tomorrow

Mr. G got food poisoned today...

Why you should Debate

It is something that will help your writing and speaking--the debate format really helps your writing ability as we construct things logically and orderly

EP 4 Sample Exam Questions Midterm 1 ch 6

ep 4 review

Matching

Match each item with the correct statement below.
a. electronegativity f. periodic law
b. ionization energy g. cation
c. atomic radius h. period
d. metal i. group
e. transition metal j. electrons


____ 1. horizontal row in the periodic table

____ 2. vertical column in the periodic table

____ 3. A repetition of properties occurs when elements are arranged in order of increasing atomic number.

____ 4. type of element that is a good conductor of heat and electric current

____ 5. type of element characterized by the presence of electrons in the d orbital

____ 6. one-half the distance between the nuclei of two atoms when the atoms are joined

____ 7. type of ion formed by Group 2A elements

____ 8. subatomic particles that are transferred to form positive and negative ions

____ 9. ability of an atom to attract electrons when the atom is in a compound

____ 10. energy required to remove an electron from an atom

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.

____ 11. In which of the following sets are the charges given correctly for all the ions?
a. Na , Mg , Al c. Rb , Ba , P
b. K , Sr , O d. N , O , F


____ 12. In which of the following groups of ions are the charges all shown correctly?
a. Li , O , S c. K , F , Mg
b. Ca , Al , Br d. Na , I , Rb


____ 13. What is the element with the lowest electronegativity value?
a. cesium c. calcium
b. helium d. fluorine


____ 14. Which of the following elements has the smallest first ionization energy?
a. sodium c. potassium
b. calcium d. magnesium


____ 15. Which of the following elements has the lowest electronegativity?
a. lithium c. bromine
b. carbon d. fluorine


____ 16. Which statement is true about electronegativity?
a. Electronegativity is the ability of an anion to attract another anion.
b. Electronegativity generally increases as you move from top to bottom within a group.
c. Electronegativity generally is higher for metals than for nonmetals.
d. Electronegativity generally increases from left to right across a period.


____ 17. Compared with the electronegativities of the elements on the left side of a period, the electronegativities of the elements on the right side of the same period tend to be ____.
a. lower c. the same
b. higher d. unpredictable


____ 18. Which of the following factors contributes to the increase in ionization energy from left to right across a period?
a. an increase in the shielding effect
b. an increase in the size of the nucleus
c. an increase in the number of protons
d. fewer electrons in the highest occupied energy level


____ 19. As you move from left to right across the second period of the periodic table ____.
a. ionization energy increases c. electronegativity decreases
b. atomic radii increase d. atomic mass decreases


____ 20. Of the following elements, which one has the smallest first ionization energy?
a. boron c. aluminum
b. carbon d. silicon


Short Answer

21. Which group of elements in the periodic table is known as the alkali metals?

22. Which group in the periodic table is known as the noble gases?

23. An element has an atomic number of 80. How many protons and electrons are in an atom of the element?

24. About what percent of elements is classified as metals?

25. What is the electron configuration of oxygen?

26. What is the electron configuration of sulfur?

27. The s and p sublevels of an atom of an element in period 3 are filled with electrons. Which orbitals are filled in this atom?

28. From which orbital in a lithium atom is an electron transferred to form Li ?

29. What orbital is filled when iodine gains an electron to become a negative ion?

30. In which group in the periodic table do the elements have the highest electronegativity values?

ep 4 review
Answer Section

MATCHING

1. ANS: H DIF: L1 REF: p. 157 OBJ: 6.1.1

2. ANS: I DIF: L1 REF: p. 157 OBJ: 6.1.1

3. ANS: F DIF: L1 REF: p. 157 OBJ: 6.1.1

4. ANS: D DIF: L1 REF: p. 158 OBJ: 6.1.3

5. ANS: E DIF: L1 REF: p. 166 OBJ: 6.2.2

6. ANS: C DIF: L1 REF: p. 170 OBJ: 6.3.1

7. ANS: G DIF: L1 REF: p. 172 OBJ: 6.3.2

8. ANS: J DIF: L1 REF: p. 172 OBJ: 6.3.2

9. ANS: A DIF: L1 REF: p. 177 OBJ: 6.3.3

10. ANS: B DIF: L1 REF: p. 173 OBJ: 6.3.3

MULTIPLE CHOICE

11. ANS: B DIF: L3 REF: p. 162, p. 163, p. 172
OBJ: 6.3.2

12. ANS: B DIF: L3 REF: p. 162, p. 163, p. 172
OBJ: 6.3.2

13. ANS: A DIF: L1 REF: p. 177 OBJ: 6.3.3

14. ANS: C DIF: L2 REF: p. 173 OBJ: 6.3.3

15. ANS: A DIF: L2 REF: p. 177 OBJ: 6.3.3

16. ANS: D DIF: L2 REF: p. 177 OBJ: 6.3.3

17. ANS: B DIF: L2 REF: p. 177, p. 178
OBJ: 6.3.3

18. ANS: C DIF: L3 REF: p. 174 OBJ: 6.3.3

19. ANS: A DIF: L3 REF: p. 178 OBJ: 6.2.1, 6.3.3

20. ANS: C DIF: L3 REF: p. 173 OBJ: 6.3.3

SHORT ANSWER

21. ANS:
1A

DIF: L1 REF: p. 161 OBJ: 6.1.1

22. ANS:
8A

DIF: L1 REF: p. 164 OBJ: 6.1.1

23. ANS:
80 protons, 80 electrons

DIF: L1 REF: p. 157 OBJ: 6.2.1

24. ANS:
80%

DIF: L2 REF: p. 158 OBJ: 6.1.3, 6.2.1

25. ANS:
1s 2s 2p

DIF: L2 REF: p. 162, p. 166 OBJ: 6.2.2

26. ANS:
1s 2s 2p 3s 3p

DIF: L2 REF: p. 166 OBJ: 6.2.2

27. ANS:
1s, 2s, 2p

DIF: L3 REF: p. 166 OBJ: 6.2.2

28. ANS:
2s

DIF: L2 REF: p. 164, p. 172 OBJ: 6.3.2

29. ANS:
5p

DIF: L3 REF: p. 166 OBJ: 6.2.2, 6.3.2

30. ANS:
7A

DIF: L2 REF: p. 177 OBJ: 6.3.3

EP 5 Sample Ch 15 questions

ep 5 review 2 midterm 1

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.

____ 1. How does the surface tension of water compare with the surface tensions of most other liquids?
a. It is lower.
b. It is about the same.
c. It is higher.
d. It is higher when a surfactant is added.


____ 2. What causes water's low vapor pressure?
a. dispersion forces c. hydrogen bonding
b. covalent bonding d. ionic attractions


____ 3. What is the shape of the water molecule?
a. linear c. trigonal planar
b. tetrahedral d. bent


____ 4. Which of the following is primarily responsible for holding water molecules together in the liquid state?
a. dispersion forces c. ionic bonds
b. hydrogen bonds d. polar covalent bonds


____ 5. Which atom in a water molecule has the greatest electronegativity?
a. one of the hydrogen atoms
b. both hydrogen atoms
c. the oxygen atom
d. There is no difference in the electronegativities of the atoms in a water molecule.


____ 6. The bonds between adjacent water molecules are called ____.
a. hydrogen bonds c. nonpolar covalent bonds
b. ionic bonds d. polar covalent bonds


____ 7. What is primarily responsible for the surface tension of water?
a. dispersion forces c. ionic attractions
b. hydrogen bonding d. covalent bonding


____ 8. Which of the following is NOT a result of surface tension in water?
a. Surface area is maximized.
b. Water has an unusually low vapor pressure.
c. Surface appears to have a "skin."
d. Drops tend to become spherical.


____ 9. Surface tension ____.
a. is the inward force which tends to minimize the surface area of a liquid
b. may be increased by detergents
c. is decreased by hydrogen bonding
d. causes beads of water to spread out


____ 10. The bonds between the hydrogen and oxygen atoms in a water molecule are ____.
a. hydrogen bonds c. nonpolar covalent bonds
b. ionic bonds d. polar covalent bonds


____ 11. How much heat is absorbed when 6.30 g of water melts?
a. 21 kJ c. 2.10 kJ
b. 0.210 kJ d. 21.0 J


____ 12. The fact that ice is less dense than water is related to the fact that ____.
a. the molecular structure of ice is much less orderly than that of water
b. the molecules of ice are held to each other by covalent bonding
c. ice has a molecular structure in which water molecules are arranged randomly
d. ice has a molecular structure that is an open framework held together by hydrogen bonds


____ 13. Which is responsible for the high thermal energy required to melt ice?
a. covalent bonding c. hydrogen bonding
b. dispersion forces d. ionic attractions


____ 14. What is the term for the dissolving medium in a solution?
a. solvent c. solvator
b. solute d. emulsifier


____ 15. A solution has which of the following properties?
a. Gravity separates its parts.
b. The top layer is different in composition than the bottom layer.
c. The average diameter of its solute particles usually is less than 1 nm.
d. A filter can remove the solute.


____ 16. Which of the following substances is the most soluble in water?
a. sodium chloride c. bromine
b. methane d. carbon


____ 17. What occurs in solvation?
a. Solute ions separate from solvent molecules.
b. Solvent molecules surround solute ions.
c. Solvent molecules bind covalently to solute molecules.
d. Ionic compounds are formed.


____ 18. Which of the following substances dissolves most readily in gasoline?
a. CH c. NH
b. HCl d. NaBr


____ 19. A solution is a mixture ____.
a. from which the solute can be filtered
b. that has the same properties throughout
c. that is heterogeneous
d. in which a solid solute is always dissolved in a liquid solvent


____ 20. Predict which one of the following compounds would be insoluble in water.
a. NaCl c. CF
b. HCl d. CuSO


____ 21. Why are two nonpolar substances able to dissolve in each other?
a. They have similar attractive forces in their molecules.
b. They combine to produce a polar substance.
c. There is no attractive force between them.
d. Nonpolar substances cannot dissolve in each other.


____ 22. Which of these would you expect to be soluble in the nonpolar solvent carbon disulfide, CS ?
a. c. NaCl
b. CI d. SnS


____ 23. Which of the following substances dissolves most readily in water?
a. BaSO c. NH
b. CaCO d. CH


____ 24. What type of compound is always an electrolyte?
a. polar covalent c. ionic
b. nonpolar covalent d. network solid


____ 25. An electric current can be conducted by ____.
a. methane gas c. a salt solution
b. a sugar solution d. rubbing alcohol


____ 26. Which of the following compounds conducts electricity only in the molten state?
a. sodium bromide c. calcium hydroxide
b. magnesium sulfate d. barium sulfate


____ 27. Which of the following compounds is a nonelectrolyte?
a. sodium bromide c. copper chloride
b. magnesium sulfate d. carbon tetrachloride


____ 28. Which of the following compounds is an electrolyte?
a. rubbing alcohol c. carbon tetrachloride
b. sugar d. sodium hydroxide


____ 29. Which of the following compounds is a nonelectrolyte when pure, but an electrolyte when dissolved in water?
a. rubbing alcohol c. carbon tetrachloride
b. sugar d. ammonia


____ 30. Which of the following are weak electrolytes in water?
a. ionic compounds that partially dissociate in water
b. ionic compounds that are soluble
c. polar compounds that ionize
d. nonpolar compounds that do not ionize


MULTIPLE CHOICE

1. ANS: C DIF: L1 REF: p. 447 OBJ: 15.1.1

2. ANS: C DIF: L1 REF: p. 447 OBJ: 15.1.1

3. ANS: D DIF: L2 REF: p. 446 OBJ: 15.1.1

4. ANS: B DIF: L2 REF: p. 446 OBJ: 15.1.1

5. ANS: C DIF: L2 REF: p. 446 OBJ: 15.1.1

6. ANS: A DIF: L2 REF: p. 446 OBJ: 15.1.1

7. ANS: B DIF: L2 REF: p. 446, p. 447
OBJ: 15.1.1

8. ANS: A DIF: L2 REF: p. 447 OBJ: 15.1.1

9. ANS: A DIF: L2 REF: p. 447 OBJ: 15.1.1

10. ANS: D DIF: L3 REF: p. 446 OBJ: 15.1.1

11. ANS: C DIF: L1 REF: p. 449 OBJ: 15.1.2

12. ANS: D DIF: L2 REF: p. 448, p. 449
OBJ: 15.1.2

13. ANS: C DIF: L3 REF: p. 449 OBJ: 15.1.2

14. ANS: A DIF: L1 REF: p. 450 OBJ: 15.2.1

15. ANS: C DIF: L2 REF: p. 450 OBJ: 15.2.1

16. ANS: A DIF: L2 REF: p. 451 OBJ: 15.2.2

17. ANS: B DIF: L2 REF: p. 451 OBJ: 15.2.2

18. ANS: A DIF: L2 REF: p. 451 OBJ: 15.2.2

19. ANS: B DIF: L3 REF: p. 450 OBJ: 15.2.2

20. ANS: C DIF: L3 REF: p. 451 OBJ: 15.2.2

21. ANS: A DIF: L3 REF: p. 451 OBJ: 15.2.2

22. ANS: B DIF: L3 REF: p. 451 OBJ: 15.2.2

23. ANS: C DIF: L3 REF: p. 451, p. 453
OBJ: 15.2.2

24. ANS: C DIF: L1 REF: p. 452 OBJ: 15.2.3

25. ANS: C DIF: L1 REF: p. 452, p. 453
OBJ: 15.2.3

26. ANS: D DIF: L2 REF: p. 452 OBJ: 15.2.3

27. ANS: D DIF: L2 REF: p. 452 OBJ: 15.2.3

28. ANS: D DIF: L2 REF: p. 453 OBJ: 15.2.3

29. ANS: D DIF: L2 REF: p. 453 OBJ: 15.2.3

30. ANS: A DIF: L2 REF: p. 453 OBJ: 15.2.3

DLO Speech: THB: PSP should be legal in school.

The DLO speech

DPM Speech: THB: PSP should be legal in school.

Our DPM speech

LO Speech: THB: PSP should be legal in school.

The LO speech.

PM Speech: THB: PSP should be legal in school.

PM speech

EP 4 Midterm review 2

ep 4 review final

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.

____ 1. What element has the electron configuration 1s 2s 2p 3s 3p ?
a. nitrogen c. silicon
b. selenium d. silver


____ 2. Elements that are characterized by the filling of p orbitals are classified as ____.
a. groups 3A through 8A c. inner transition metals
b. transition metals d. groups 1A and 2A


____ 3. Atomic size generally ____.
a. increases as you move from left to right across a period
b. decreases as you move from top to bottom within a group
c. remains constant within a period
d. decreases as you move from left to right across a period


____ 4. Which of the following elements has the smallest atomic radius?
a. sulfur c. selenium
b. chlorine d. bromine


____ 5. The metals in Groups 1A, 2A, and 3A ____.
a. gain electrons when they form ions c. all have ions with a 1 charge
b. all form ions with a negative charge d. lose electrons when they form ions


____ 6. In which of the following sets are the charges given correctly for all the ions?
a. Na , Mg , Al c. Rb , Ba , P
b. K , Sr , O d. N , O , F


____ 7. Which of the following elements has the smallest ionic radius?
a. Li c. O
b. K d. S


____ 8. For Group 2A metals, which electron is the most difficult to remove?
a. the first
b. the second
c. the third
d. All the electrons are equally difficult to remove.


____ 9. Which statement is true about electronegativity?
a. Electronegativity is the ability of an anion to attract another anion.
b. Electronegativity generally increases as you move from top to bottom within a group.
c. Electronegativity generally is higher for metals than for nonmetals.
d. Electronegativity generally increases from left to right across a period.


____ 10. Compared with the electronegativities of the elements on the left side of a period, the electronegativities of the elements on the right side of the same period tend to be ____.
a. lower c. the same
b. higher d. unpredictable


____ 11. Which of the following statements correctly compares the relative size of an ion to its neutral atom?
a. The radius of an anion is greater than the radius of its neutral atom.
b. The radius of an anion is identical to the radius of its neutral atom.
c. The radius of a cation is greater than the radius of its neutral atom.
d. The radius of a cation is identical to the radius of its neutral atom.


____ 12. Which of the following factors contributes to the increase in ionization energy from left to right across a period?
a. an increase in the shielding effect
b. an increase in the size of the nucleus
c. an increase in the number of protons
d. fewer electrons in the highest occupied energy level


____ 13. Of the following elements, which one has the smallest first ionization energy?
a. boron c. aluminum
b. carbon d. silicon


____ 14. In the Bohr model of the atom, an electron in an orbit has a fixed ____.
a. position c. energy
b. color d. size


____ 15. The principal quantum number indicates what property of an electron?
a. position c. energy level
b. speed d. electron cloud shape


____ 16. What is the shape of the 3p atomic orbital?
a. sphere c. bar
b. dumbbell d. two perpendicular dumbbells


____ 17. What is the maximum number of orbitals in the p sublevel?
a. 2 c. 4
b. 3 d. 5


____ 18. The shape (not the size) of an electron cloud is determined by the electron's ____.
a. energy sublevel c. speed
b. position d. principal quantum number


____ 19. The letter "p" in the symbol 4p indicates the ____.
a. spin of an electron c. principle energy level
b. orbital shape d. speed of an electron


____ 20. What types of atomic orbitals are in the third principal energy level?
a. s and p only c. s, p, and d only
b. p and d only d. s, p, d, and f


____ 21. According to the aufbau principle, ____.
a. an orbital may be occupied by only two electrons
b. electrons in the same orbital must have opposite spins
c. electrons enter orbitals of highest energy first
d. electrons enter orbitals of lowest energy first


____ 22. What is the electron configuration of potassium?
a. 1s 2s 2p 3s 3p 4s c. 1s 2s 3s 3p 3d
b. 1s 2s 2p 3s 3p d. 1s 2s 2p 3s 3p 4s


____ 23. How many unpaired electrons are in a sulfur atom (atomic number 16)?
a. 0 c. 2
b. 1 d. 3


____ 24. How many half-filled orbitals are in a bromine atom?
a. 1 c. 3
b. 2 d. 4


____ 25. Which electron configuration of the 4f energy sublevel is the most stable?
a. 4f c. 4f
b. 4f d. 4f


____ 26. Which of the following electron configurations of outer sublevels is the most stable?
a. 4d 5s c. 4d 5s
b. 4d 5s d. 4d 5s


____ 27. Which color of visible light has the shortest wavelength?
a. yellow c. blue
b. green d. violet


____ 28. Which of the following electromagnetic waves have the highest frequencies?
a. ultraviolet light waves c. microwaves
b. X-rays d. gamma rays


____ 29. Which type of electromagnetic radiation includes the wavelength 10 m?
a. gamma ray c. radio wave
b. microwave d. visible light


____ 30. What is the wavelength of an electromagnetic wave that travels at 3 10 m/s and has a frequency of 60 MHz? (1 MHz = 1,000,000 Hz)
a.
b. 60 MHz 300,000,000 m/s
c.
d. No answer can be determined from the information given.


____ 31. The light given off by an electric discharge through sodium vapor is ____.
a. a continuous spectrum c. of a single wavelength
b. an emission spectrum d. white light


____ 32. Emission of light from an atom occurs when an electron ____.
a. drops from a higher to a lower energy level
b. jumps from a lower to a higher energy level
c. moves within its atomic orbital
d. falls into the nucleus


____ 33. As changes in energy levels of electrons increase, the frequencies of atomic line spectra they emit ____.
a. increase c. remain the same
b. decrease d. cannot be determined


____ 34. The atomic emission spectra of a sodium atom on Earth and of a sodium atom in the sun would be ____.
a. the same
b. different from each other
c. the same as those of several other elements
d. the same as each other only in the ultraviolet range


____ 35. What is the approximate energy of a photon having a frequency of 4 10 Hz? (h = 6.6 10 J s)
a. 3 10 J c. 2 10 J
b. 3 10 J d. 3 10 J


____ 36. What is the approximate frequency of a photon having an energy 5 10 J? (h = 6.6 10 J s)
a. 8 10 Hz c. 3 10 Hz
b. 3 10 Hz d. 1 10 Hz


____ 37. Which of the following quantum leaps would be associated with the greatest energy of emitted light?
a. n = 5 to n = 1 c. n = 2 to n = 5
b. n = 4 to n = 5 d. n = 5 to n = 4


____ 38. Which variable is directly proportional to frequency?
a. wavelength c. position
b. velocity d. energy


ep 4 review final
Answer Section

MULTIPLE CHOICE

1. ANS: C DIF: L2 REF: p. 164 OBJ: 6.2.2

2. ANS: A DIF: L2 REF: p. 166 OBJ: 6.2.2

3. ANS: D DIF: L2 REF: p. 171 OBJ: 6.3.1

4. ANS: B DIF: L3 REF: p. 171, p. 175
OBJ: 6.3.1

5. ANS: D DIF: L2 REF: p. 162, p. 163, p. 172, p. 176
OBJ: 6.3.2

6. ANS: B DIF: L3 REF: p. 162, p. 163, p. 172
OBJ: 6.3.2

7. ANS: A DIF: L2 REF: p. 175 OBJ: 6.3.3

8. ANS: C DIF: L2 REF: p. 173 OBJ: 6.3.3

9. ANS: D DIF: L2 REF: p. 177 OBJ: 6.3.3

10. ANS: B DIF: L2 REF: p. 177, p. 178
OBJ: 6.3.3

11. ANS: A DIF: L2 REF: p. 172, p. 176
OBJ: 6.3.3

12. ANS: C DIF: L3 REF: p. 174 OBJ: 6.3.3

13. ANS: C DIF: L3 REF: p. 173 OBJ: 6.3.3

14. ANS: C DIF: L2 REF: p. 128 OBJ: 5.1.2

15. ANS: C DIF: L2 REF: p. 131 OBJ: 5.1.3

16. ANS: B DIF: L2 REF: p. 131 OBJ: 5.1.3

17. ANS: B DIF: L2 REF: p. 131, p. 132
OBJ: 5.1.3

18. ANS: A DIF: L2 REF: p. 131 OBJ: 5.1.4

19. ANS: B DIF: L2 REF: p. 131 OBJ: 5.1.4

20. ANS: C DIF: L2 REF: p. 131 OBJ: 5.2.1

21. ANS: D DIF: L2 REF: p. 133 OBJ: 5.2.1

22. ANS: D DIF: L2 REF: p. 133, p. 134, p. 135
OBJ: 5.2.1

23. ANS: C DIF: L3 REF: p. 133, p. 134
OBJ: 5.2.1

24. ANS: A DIF: L3 REF: p. 133, p. 134
OBJ: 5.2.1

25. ANS: D DIF: L2 REF: p. 136 OBJ: 5.2.2

26. ANS: A DIF: L3 REF: p. 133, p. 134, p. 135, p. 136
OBJ: 5.2.2

27. ANS: D DIF: L2 REF: p. 139 OBJ: 5.3.1

28. ANS: D DIF: L2 REF: p. 139 OBJ: 5.3.1

29. ANS: D DIF: L2 REF: p. 139 OBJ: 5.3.1

30. ANS: C DIF: L3 REF: p. 140 OBJ: 5.3.1

31. ANS: B DIF: L2 REF: p. 141 OBJ: 5.3.2

32. ANS: A DIF: L2 REF: p. 141 OBJ: 5.3.2

33. ANS: A DIF: L2 REF: p. 142, p. 143
OBJ: 5.3.2

34. ANS: A DIF: L2 REF: p. 141 OBJ: 5.3.2, 5.3.3

35. ANS: A DIF: L2 REF: p. 142 OBJ: 5.3.3

36. ANS: A DIF: L2 REF: p. 142 OBJ: 5.3.3

37. ANS: A DIF: L2 REF: p. 143 OBJ: 5.3.3

38. ANS: D DIF: L3 REF: p. 142 OBJ: 5.3.3

EP 4 Sample Exam Questions Midterm 1

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.

____ 1. Who was the man who lived from 460B.C.–370B.C. and was among the first to suggest the idea of atoms?
a. Atomos c. Democritus
b. Dalton d. Thomson


____ 2. Which of the following was NOT among Democritus’s ideas?
a. Matter consists of tiny particles called atoms.
b. Atoms are indivisible.
c. Atoms retain their identity in a chemical reaction.
d. Atoms are indestructible.


____ 3. The smallest particle of an element that retains the properties of that element is a(n) ____.
a. atom c. proton
b. electron d. neutron


____ 4. Dalton's atomic theory included which idea?
a. All atoms of all elements are the same size.
b. Atoms of different elements always combine in one-to-one ratios.
c. Atoms of the same element are always identical.
d. Individual atoms can be seen with a microscope.


____ 5. Which of the following is NOT a part of Dalton's atomic theory?
a. All elements are composed of atoms.
b. Atoms are always in motion.
c. Atoms of the same element are identical.
d. Atoms that combine do so in simple whole-number ratios.


____ 6. Which of the following was originally a tenet of Dalton's atomic theory, but had to be revised about a century ago?
a. Atoms are tiny indivisible particles.
b. Atoms of the same element are identical.
c. Compounds are made by combining atoms.
d. Atoms of different elements can combine with one another in simple whole number ratios.


____ 7. The comparison of the number of atoms in a copper coin the size of a penny with the number of people on Earth is made to illustrate which of the following?
a. that atoms are indivisible
b. that atoms are very small
c. that atoms are very large
d. that in a copper penny, there is one atom for every person on Earth


____ 8. The range in size of most atomic radii is approximately ____.
a. 2 to 5 cm c. 5 10 m to 2 10 m
b. 2 to 5 nm d. 5 10 m to 2 10 m


____ 9. Dalton hypothesized that atoms are indivisible and that all atoms of an element are identical. It is now known that ____.
a. all of Dalton's hypotheses are correct
b. atoms of an element can have different numbers of protons
c. atoms are divisible
d. all atoms of an element are not identical but they must all have the same mass


____ 10. Why did J. J. Thomson reason that electrons must be a part of the atoms of all elements?
a. Cathode rays are negatively-charged particles.
b. Cathode rays can be deflected by magnets.
c. An electron is 2000 times lighter than a hydrogen atom.
d. Charge-to-mass ratio of electrons was the same, regardless of the gas used.


____ 11. Which of the following is true about subatomic particles?
a. Electrons are negatively charged and are the heaviest subatomic particle.
b. Protons are positively charged and the lightest subatomic particle.
c. Neutrons have no charge and are the lightest subatomic particle.
d. The mass of a neutron nearly equals the mass of a proton.


____ 12. Who conducted experiments to determine the quantity of charge carried by an electron?
a. Rutherford c. Dalton
b. Millikan d. Thomson


____ 13. What is the relative mass of an electron?
a. 1/1840 the mass of a hydrogen atom c. 1/1840 the mass of a C-12 atom
b. 1/1840 the mass of a neutron + proton d. 1/1840 the mass of an alpha particle


____ 14. Which hypothesis led to the discovery of the proton?
a. When a neutral hydrogen atom loses an electron, a positively-charged particle should remain.
b. A proton should be 1840 times heavier than an electron.
c. Cathode rays should be attracted to a positively-charged plate.
d. The nucleus of an atom should contain neutrons.


____ 15. Which of the following is correct concerning subatomic particles?
a. The electron was discovered by Goldstein in 1886.
b. The neutron was discovered by Chadwick in 1932.
c. The proton was discovered by Thomson in 1880.
d. Cathode rays were found to be made of protons.


____ 16. All atoms are ____.
a. positively charged, with the number of protons exceeding the number of electrons
b. negatively charged, with the number of electrons exceeding the number of protons
c. neutral, with the number of protons equaling the number of electrons
d. neutral, with the number of protons equaling the number of electrons, which is equal to the number of neutrons


____ 17. The particles that are found in the nucleus of an atom are ____.
a. neutrons and electrons c. protons and neutrons
b. electrons only d. protons and electrons


____ 18. As a consequence of the discovery of the nucleus by Rutherford, which model of the atom is thought to be true?
a. Protons, electrons, and neutrons are evenly distributed throughout the volume of the atom.
b. The nucleus is made of protons, electrons, and neutrons.
c. Electrons are distributed around the nucleus and occupy almost all the volume of the atom.
d. The nucleus is made of electrons and protons.


____ 19. The nucleus of an atom is ____.
a. the central core and is composed of protons and neutrons
b. positively charged and has more protons than neutrons
c. negatively charged and has a high density
d. negatively charged and has a low density


____ 20. The atomic number of an element is the total number of which particles in the nucleus?
a. neutrons c. electrons
b. protons d. protons and electrons


____ 21. An element has an atomic number of 76. The number of protons and electrons in a neutral atom of the element are ____.
a. 152 protons and 76 electrons c. 38 protons and 38 electrons
b. 76 protons and 0 electrons d. 76 protons and 76 electrons


____ 22. The sum of the protons and neutrons in an atom equals the ____.
a. atomic number c. atomic mass
b. nucleus number d. mass number


____ 23. What does the number 84 in the name krypton-84 represent?
a. the atomic number c. the sum of the protons and electrons
b. the mass number d. twice the number of protons


____ 24. All atoms of the same element have the same ____.
a. number of neutrons c. mass numbers
b. number of protons d. mass


____ 25. Isotopes of the same element have different ____.
a. numbers of neutrons c. numbers of electrons
b. numbers of protons d. atomic numbers


____ 26. Isotopes of the same element have different ____.
a. positions on the periodic table c. atomic numbers
b. chemical behavior d. mass numbers


____ 27. In which of the following sets is the symbol of the element, the number of protons, and the number of electrons given correctly?
a. In, 49 protons, 49 electrons c. Cs, 55 protons, 132.9 electrons
b. Zn, 30 protons, 60 electrons d. F, 19 protons, 19 electrons


____ 28. The mass number of an element is equal to ____.
a. the total number of electrons in the nucleus
b. the total number of protons and neutrons in the nucleus
c. less than twice the atomic number
d. a constant number for the lighter elements


____ 29. Using the periodic table, determine the number of neutrons in O.
a. 4 c. 16
b. 8 d. 24


____ 30. How many protons, electrons, and neutrons does an atom with atomic number 50 and mass number 125 contain?
a. 50 protons, 50 electrons, 75 neutrons c. 120 neutrons, 50 protons, 75 electrons
b. 75 electrons, 50 protons, 50 neutrons d. 70 neutrons, 75 protons, 50 electrons

Answer Section

MULTIPLE CHOICE

1. ANS: C DIF: L2 REF: p. 101 OBJ: 4.1.1

2. ANS: C DIF: L2 REF: p. 101 OBJ: 4.1.1

3. ANS: A DIF: L1 REF: p. 101, p. 102
OBJ: 4.1.1, 4.1.2

4. ANS: C DIF: L2 REF: p. 102 OBJ: 4.1.2

5. ANS: B DIF: L2 REF: p. 102 OBJ: 4.1.2

6. ANS: A DIF: L2 REF: p. 104 OBJ: 4.1.2

7. ANS: B DIF: L2 REF: p. 103 OBJ: 4.1.3

8. ANS: C DIF: L2 REF: p. 103 OBJ: 4.1.3

9. ANS: C DIF: L1 REF: p. 104 OBJ: 4.2.1

10. ANS: D DIF: L2 REF: p. 105 OBJ: 4.2.1

11. ANS: D DIF: L2 REF: p. 104, p. 105, p. 106
OBJ: 4.2.1

12. ANS: B DIF: L2 REF: p. 105 OBJ: 4.2.1

13. ANS: A DIF: L2 REF: p. 105 OBJ: 4.2.1

14. ANS: A DIF: L3 REF: p. 106 OBJ: 4.2.1

15. ANS: B DIF: L3 REF: p. 105, p. 106
OBJ: 4.2.1

16. ANS: C DIF: L3 REF: p. 106 OBJ: 4.2.1

17. ANS: C DIF: L2 REF: p. 106, p. 107
OBJ: 4.2.1, 4.2.2

18. ANS: C DIF: L2 REF: p. 108 OBJ: 4.2.2

19. ANS: A DIF: L2 REF: p. 107, p. 108
OBJ: 4.2.2

20. ANS: B DIF: L1 REF: p. 110 OBJ: 4.3.1

21. ANS: D DIF: L1 REF: p. 110 OBJ: 4.3.1

22. ANS: D DIF: L1 REF: p. 111 OBJ: 4.3.1

23. ANS: B DIF: L1 REF: p. 111 OBJ: 4.3.1

24. ANS: B DIF: L1 REF: p. 110 OBJ: 4.3.1

25. ANS: A DIF: L1 REF: p. 112, p. 113
OBJ: 4.3.1

26. ANS: D DIF: L1 REF: p. 112, p. 113
OBJ: 4.3.1

27. ANS: A DIF: L2 REF: p. 110 OBJ: 4.2.1, 4.3.1

28. ANS: B DIF: L2 REF: p. 111 OBJ: 4.3.1

29. ANS: B DIF: L2 REF: p. 111 OBJ: 4.3.1

30. ANS: A DIF: L2 REF: p. 111 OBJ: 4.3.1

Sample Exam EP 5 Midterm 2009 ch 16 questions

ep 5 sample exam

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.

____ 1. Which of the following usually makes a substance dissolve faster in a solvent?
a. agitating the solution
b. increasing the particle size of the solute
c. lowering the temperature
d. decreasing the number of particles


____ 2. What is the maximum amount of KCl that can dissolve in 200 g of water?
(The solubility of KCl is 34 g/100 g H2O at 20 C.)
a. 17 g c. 68 g
b. 34 g d. 6800 g


____ 3. What is the solubility of silver nitrate if only 11.1 g can dissolve in 5.0 g of water at 20 C?
a. at 20 C c. at 20 C
b. at 20 C d. at 20 C


____ 4. Which of the following expressions is generally used for solubility?
a. grams of solute per 100 grams of solvent
b. grams of solute per 100 milliliters of solvent
c. grams of solute per 100 grams of solution
d. grams of solute per 100 milliliters of solution


____ 5. Which of the following pairs of factors affects the solubility of a particular substance?
a. temperature and the nature of solute and solvent
b. temperature and degree of mixing
c. particle size and degree of mixing
d. particle size and temperature


____ 6. If a crystal added to an aqueous solution causes many particles to come out of the solution, the original solution was ____.
a. unsaturated c. an emulsion
b. saturated d. supersaturated


____ 7. Which of the following substances is less soluble in hot water than in cold water?
a. CO c. NaNO
b. NaCl d. KBr


____ 8. Which of the following occurs as temperature increases?
a. Solubility decreases. c. Solubility remains the same.
b. Solubility increases. d. Molarity doubles.


____ 9. The solubility of a gas in a liquid is ____.
a. proportional to the square root of the pressure of the gas above the liquid
b. directly proportional to the pressure of the gas above the liquid
c. inversely proportional to the pressure of the gas above the liquid
d. unrelated to the pressure of the gas above the liquid


____ 10. If the solubility of a particular solute is at 20 C, which of the following solution concentrations would represent a supersaturated aqueous solution of that solute?
a. at 25 C c. at 20 C
b. at 15 C d. at 20 C


____ 11. What happens to the solubility of a gas, in a liquid, if the partial pressure of the gas above the liquid decreases?
a. The solubility decreases. c. The solubility remains the same.
b. The solubility increases. d. The solubility cannot be determined.


____ 12. To increase the solubility of a gas at constant temperature from 1.20 g/L, at 1.4 atm, to 2.3 g/L, the pressure would have to be increased to ____.
a. 0.37 atm c. 1.37 atm
b. 0.7 atm d. 2.7 atm


____ 13. If the solubility of a gas in water is 4.0 g/L when the pressure of the gas above the water is 3.0 atm, what is the pressure of the gas above the water when the solubility of the gas is 1.0 g/L?
a. 0.75 atm c. 4.0 atm
b. 1.3 atm d. 12 atm


____ 14. In a concentrated solution there is ____.
a. no solvent c. a small amount of solute
b. a large amount of solute d. no solute


____ 15. What is the molarity of a solution that contains 6 moles of solute in 2 liters of solution?
a. 6M c. 7M
b. 12M d. 3M


____ 16. In which of the following is the solution concentration expressed in terms of molarity?
a. c.
b. d.


____ 17. Which of the following operations yields the number of moles of solute?
a. molarity moles of solution c. molarity mass of solution
b. molarity liters of solution d. moles of solution volume of solution


____ 18. What is the molarity of a solution containing 7.0 moles of solute in 569 mL of solution?
a. 81M c. 12M
b. 0.081M d. 4.0M


____ 19. What is the molarity of 200 mL of solution in which 2.0 moles of sodium bromide is dissolved?
a. 2.0M c. 0.40M
b. 10M d. 4.0M


____ 20. What is the number of moles of solute in 250 mL of a 0.4M solution?
a. 0.1 mol c. 0.62 mol
b. 0.16 mol d. 1.6 mol


____ 21. What is the molarity of a solution containing 56 grams of solute in 959 mL of solution? (molar mass of solute = 26 g/mol)
a. 1.5M c. 2.1M
b. 2.2M d. 0.0022M


____ 22. What mass of sucrose, C H O , is needed to make 500.0 mL of a 0.200M solution?
a. 34.2 g c. 17.1 g
b. 100 g d. 68.4 g


____ 23. What mass of Na SO is needed to make 2.5 L of 2.0M solution? (Na = 23 g; S = 32 g; O = 16 g)
a. 178 g c. 356 g
b. 284 g d. 710 g


____ 24. What does NOT change when a solution is diluted by the addition of solvent?
a. volume of solvent c. number of moles of solute
b. mass of solvent d. molarity of solution


____ 25. How many mL of a 2.0M NaBr solution are needed to make 200.0 mL of 0.50M NaBr?
a. 25 mL c. 100 mL
b. 50 mL d. 150 mL


____ 26. The volume of 6.00M HCl needed to make 319 mL of 6.80M HCl is ____.
a. 0.128 mL c. 281 mL
b. 7.8 mL d. 362 mL


____ 27. If 2.0 mL of 6.0M HCl is used to make a 500.0-mL aqueous solution, what is the molarity of the dilute solution?
a. 0.024M c. 0.30M
b. 0.24M d. 0.83M


____ 28. To 225 mL of a 0.80M solution of KI, a student adds enough water to make 1.0 L of a more dilute KI solution. What is the molarity of the new solution?
a. 180M c. 0.35M
b. 2.8M d. 0.18M


____ 29. If the percent by volume is 2.0% and the volume of solution is 250 mL, what is the volume of solute in solution?
a. 0.5 mL c. 5.0 mL
b. 1.25 mL d. 12.5 mL


____ 30. In which of the following is concentration expressed in percent by volume?
a. 10% (v/v) c. 10% (m/m)
b. 10% (m/v) d. 10%


____ 31. If the percent (mass/mass) for a solute is 4% and the mass of the solution is 200 g, what is the mass of solute in solution?
a. 8.0 g c. 80 g
b. 50 g d. 800 g


____ 32. The volume of alcohol present in 620 mL of a 40.0% (v/v) solution of alcohol is ____.
a. 372 mL c. 248 mL
b. 40.0 mL d. 580 mL


____ 33. How many milliliters of alcohol are in 167 mL of an 85.0% (v/v) alcohol solution?
a. 252 mL c. 145 mL
b. 228 mL d. 142 mL


____ 34. In which of the following is concentration expressed in percent by volume?
a. 100% c. 100%
b. 100% d. 100%


____ 35. Which of the following is NOT a colligative property of a solution?
a. boiling point elevation c. vapor pressure lowering
b. supersaturation d. freezing point depression


____ 36. Colligative properties depend upon the ____.
a. nature of the solute c. number of solute particles in a solution
b. nature of the solvent d. freezing point of a solute


____ 37. A solute depresses the freezing point because the solute ____.
a. is colder than the solvent
b. disrupts crystal formation of the solvent
c. tends to sink to the bottom of the solution
d. has bigger molecules than the solvent



answers:
MULTIPLE CHOICE

1. ANS: A DIF: L2 REF: p. 471, p. 472
OBJ: 16.1.1

2. ANS: C DIF: L2 REF: p. 473 OBJ: 16.1.2

3. ANS: D DIF: L2 REF: p. 473 OBJ: 16.1.2

4. ANS: A DIF: L2 REF: p. 473 OBJ: 16.1.2

5. ANS: A DIF: L2 REF: p. 473, p. 474
OBJ: 16.1.3

6. ANS: D DIF: L2 REF: p. 474 OBJ: 16.1.3

7. ANS: A DIF: L2 REF: p. 475 OBJ: 16.1.3

8. ANS: B DIF: L2 REF: p. 474 OBJ: 16.1.3

9. ANS: B DIF: L2 REF: p. 476 OBJ: 16.1.3

10. ANS: D DIF: L3 REF: p. 474 OBJ: 16.1.3

11. ANS: A DIF: L1 REF: p. 476, p. 477
OBJ: 16.1.4

12. ANS: D DIF: L2 REF: p. 476, p. 477
OBJ: 16.1.4

13. ANS: A DIF: L3 REF: p. 476, p. 477
OBJ: 16.1.4

14. ANS: B DIF: L1 REF: p. 480 OBJ: 16.2.1

15. ANS: D DIF: L1 REF: p. 481 OBJ: 16.2.1

16. ANS: D DIF: L1 REF: p. 480, p. 481
OBJ: 16.2.1

17. ANS: B DIF: L2 REF: p. 480 OBJ: 16.2.1

18. ANS: C DIF: L2 REF: p. 480, p. 481
OBJ: 16.2.1

19. ANS: B DIF: L2 REF: p. 481 OBJ: 16.2.1

20. ANS: A DIF: L2 REF: p. 480, p. 482
OBJ: 16.2.1

21. ANS: B DIF: L3 REF: p. 481 OBJ: 16.2.1

22. ANS: A DIF: L3 REF: p. 481, p. 482
OBJ: 16.2.1

23. ANS: D DIF: L3 REF: p. 481, p. 482
OBJ: 16.2.1

24. ANS: C DIF: L1 REF: p. 483 OBJ: 16.2.2

25. ANS: B DIF: L2 REF: p. 483, p. 484
OBJ: 16.2.2

26. ANS: D DIF: L2 REF: p. 483, p. 484
OBJ: 16.2.2

27. ANS: A DIF: L2 REF: p. 483, p. 484
OBJ: 16.2.2

28. ANS: D DIF: L3 REF: p. 483, p. 484
OBJ: 16.2.2

29. ANS: C DIF: L1 REF: p. 485 OBJ: 16.2.3

30. ANS: A DIF: L1 REF: p. 485 OBJ: 16.2.3

31. ANS: A DIF: L1 REF: p. 486 OBJ: 16.2.3

32. ANS: C DIF: L2 REF: p. 485 OBJ: 16.2.3

33. ANS: D DIF: L2 REF: p. 485 OBJ: 16.2.3

34. ANS: B DIF: L2 REF: p. 485 OBJ: 16.2.3

35. ANS: B DIF: L1 REF: p. 487 OBJ: 16.3.1

36. ANS: C DIF: L2 REF: p. 487, p. 488
OBJ: 16.3.1

37. ANS: B DIF: L2 REF: p. 488 OBJ: 16.3.2

EP 6 Midterm Suggestions

I would read through the sample questions/problems in the text--ch 22, 23, and 19. Make sure you can name the alkanes, alkenes, alkynes--know your functional groups and cylcos, study the matching, and be able to do an autoionization of water problem along with ph problems--Ph-h, h-ph, ph-poh, etc.

any questions?

Any questions?

if you have any questions, I will be answering specific questions until July 19th 10 a.m.