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