Download AP Exam Two Retake Qualifying Assignment

Name_______________________________________Date___________________________ Class_________
AP Exam Two Retake Qualifying Assignment
Matching
Match each item with the correct statement below.
a. atomic orbital
d. ground state
b. aufbau principle
e. Pauli exclusion principle
c. electron configuration
f. Heisenberg uncertainty principle
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1.
2.
3.
4.
5.
6.
region of high probability of finding an electron
states the impossibility of knowing both velocity and position of a moving particle at the same time
lowest energy level
tendency of electrons to enter orbitals of lowest energy first
arrangement of electrons around atomic nucleus
each orbital has at most two electrons
Match each item with the correct statement below.
a. atomic emission spectrum
d. photon
b. frequency
e. quantum
c. wavelength
f. spectrum
____ 7. discrete bundle of electromagnetic energy
____ 8. energy needed to move an electron from one energy level to another
____ 9. number of wave cycles passing a point per unit of time
____ 10. distance between wave crests
____ 11. separation of light into different wavelengths
____ 12. frequencies of light emitted by an element
Match each item with the correct statement below.
a. coordinate covalent bond
d. single covalent bond
b. double covalent bond
e. polar bond
c. structural formula
f. hydrogen bond
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13.
14.
15.
16.
17.
18.
a depiction of the arrangement of atoms in molecules and polyatomic ions
a covalent bond in which only one pair of electrons is shared
a covalent bond in which two pairs of electrons are shared
a covalent bond in which the shared electron pair comes from only one of the atoms
a covalent bond between two atoms of significantly different electronegativities
a type of bond that is very important in determining the properties of water and of important biological
molecules such as proteins and DNA
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
____ 19. The principal quantum number indicates what property of an electron?
a. position
c. energy level
b. speed
d. electron cloud shape
____ 20. How many energy sublevels are in the fourth principal energy level?
a. 1
c. 3
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____ 21.
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____ 28.
____ 29.
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____ 33.
b. 2
d. 4
What is the maximum number of d orbitals in a principal energy level?
a. 1
c. 3
b. 2
d. 5
What is the maximum number of electrons in the fourth principal energy level?
a. 2
c. 18
b. 8
d. 32
When an electron moves from a lower to a higher energy level, the electron ____.
a. always doubles its energy
b. absorbs a continuously variable amount of energy
c. absorbs a quantum of energy
d. moves closer to the nucleus
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
If the spin of one electron in an orbital is clockwise, what is the spin of the other electron in that orbital?
a. zero
c. counterclockwise
b. clockwise
d. both clockwise and counterclockwise
What types of atomic orbitals are in the fourth 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
What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p?
a. 2d
c. 3f
b. 3d
d. 4s
If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the
three orbitals?
a. one electron in each orbital
b. two electrons in one orbital, one in another, none in the third
c. three in one orbital, none in the other two
d. Three electrons cannot fill three empty 2p atomic orbitals.
What is the basis for exceptions to the aufbau diagram?
a. Filled and half-filled energy sublevels are more stable than partially-filled energy sublevels.
b. Electron configurations are only probable.
c. Electron spins are more important than energy levels in determining electron configuration.
d. Some elements have unusual atomic orbitals.
How does the speed of visible light compare with the speed of X rays, when both speeds are measured in a
vacuum?
a. The speed of visible light is greater.
b. The speeds are the same.
c. The speed of gamma rays is greater.
d. No answer can be determined from the information given.
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
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
The atomic emission spectra of a sodium atom on Earth and of a sodium atom in the sun would be ____.
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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
____ 34. What are quanta of light called?
a. charms
c. muons
b. excitons
d. photons
____ 35. What is the formula unit of sodium nitride?
a. NaN
c. Na N
b. Na N
d. NaN
____ 36. Which of the following pairs of elements is most likely to form an ionic compound?
a. magnesium and fluorine
c. oxygen and chlorine
b. nitrogen and sulfur
d. sodium and aluminum
____ 37. Ionic compounds are normally in which physical state at room temperature?
a. solid
c. gas
b. liquid
d. plasma
____ 38. Which of the following is true about the melting temperature of potassium chloride?
a. The melting temperature is relatively high.
b. The melting temperature is variable and unpredictable.
c. The melting temperature is relatively low.
d. Potassium chloride does not melt.
____ 39. Under what conditions can potassium bromide conduct electricity?
a. only when melted
b. only when dissolved
c. only when it is in crystal form
d. only when melted or dissolved in water
____ 40. Which of the following is NOT a characteristic of most ionic compounds?
a. They are solids.
b. They have low melting points.
c. When melted, they conduct an electric current.
d. They are composed of metallic and nonmetallic elements.
Short Answer
41. What is the frequency of ultraviolet light with wavelength 2.94
10
42. What is the energy of a microwave photon that has a frequency of 1.12
m? (c = 3.00
10
10 m/s)
Hz? (h = 6.63
10
J s)
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Name_______________________________________Date___________________________ Class_________
43. An electron moves from the second energy level (n = 2) to the fith energy level (n = 5).
a) Indicated whether the H atom emits energy of whether it absorbs energy during the transition.
Justify your answer.
b) Calculate the minimum wavelenth of light, in nm, of the radiation associated with the electrons
transition.
Numeric Response
44. How many unpaired electrons are in there in a neutral carbon atom?
45. How many electrons are in the highest occupied energy level of a neutral strontium atom?
46. How many electrons are in the highest occupied energy level of copper?
47. How many valence electrons are in phosphorus?
48. How many electrons does a aluminum atom give up when it becomes an ion?
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49. How many electrons does a nitrogen atom need to gain in order to attain a noble-gas electron configuration?
50. How many electrons does carbon need to gain in order to obtain a noble-gas electron configuration?
51. How many electrons are shared in a double covalent bond?
52. How many covalent bonds are in a covalently bonded molecule containing 1 phosphorus atom and 3 chlorine
atoms?
53. What is the bond angle in a molecule of methane (CH )?
54. What is the bond angle in a XeF ?
55. What is the bond angle in a COF ?
56. How many unpaired electrons does a neutral atom of cesium have?
57. How many unpaired electrons does a neutral atom of phosporous have?
58. If oxygen could exist as O how many unpaired electrons would it have?
Essay
59. What has a greater exothermic lattice energy and why, MgF2 or MgI2?
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60. Which compound would be expected to have a higher melting point, Mg3N2 or NaF?
61. Draw a Lewis structure for nitrogen trichloride (NCl3). Is the compound ionic or covalent and how do you
know? Is the compound polar or nonpolar and how do you know?
62. Write a Lewis structure for SO2Cl2. Sulfur is the central atom. What is the formal charge on the Sulfur atom
when the best Lewis structure is draw? What is the geometry and bond angle for each atom? Does the
molecule display a net dipole moment?
63. Write a Lewis structure for Xe2F4. What is the formal charge on the Xe atom when the best Lewis structure is
drawn? What is the geometry and bond angle for each atom? Does the molecule display a net dipole
moment?
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