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
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34.
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35. Why would you expect lithium (Li) and sulfur (S) to have different chemical and
physical properties? Three reasons
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36. Compare the first ionization energy lithium to that of beryllium.
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37. Compare the elements in group 1 with the elements in group 7, in terms of electronegativity, ionization, and atomic radii?
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38. Explain why the sulfide ion (S2) is larger than the chloride ion (Cl).
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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
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40. The Mg2+ and Na+ ions each have ten electrons. Which ion would you expect to have the smaller radius? Explain your choice
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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
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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.
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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?
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44. Describe the trends in first ionization energy within groups and across periods in the periodic table. Provide examples.
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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.

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

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