Transcript Chapter 1
1. Which of the following list quantities that are directly proportional?
A) The wavelength and frequency of a light wave.
B) The frequency of a light wave and the energy of a photon of the light.
C) The wavelength of a light wave and the energy of a photon of the light.
D) None of the above.
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2. It takes about 650 kJ of energy to boil a cup of water. A photon of the electromagnetic radiation used in microwave ovens has an energy of about 1.62 X 10 -24 J .
About how many microwave photons are needed to boil a cup of water?
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A) 4.0 X 10 29 J B) 9.7 X 10 38 J C) 6.02 X 10 23 J D) Need the wavelength to know.
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3. Which of the following apply to the principal quantum number?
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A) The higher the value, the greater the average distance of the electron from the nucleus.
B) Integer values of 1 or greater are possible.
C) Both A and B.
D) None of the above.
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4. Which of the following does not apply to the angular momentum quantum number?
A) All integer values are allowed.
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B) The value corresponds to the general shape of the orbital.
C) The largest possible value depends on the value of the principle quantum number.
D) Negative values are not allowed.
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5. The possible values of the magnetic quantum number depend on the value of the angular momentum quantum number.
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A) True B) False
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6. The possible values of the electron spin quantum number depend on the value of the magnetic quantum
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number.
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A) True B) False
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7. Which of the following electron configurations does not correspond to a ground state atom?
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A) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 B) 1s 2 2s 2 2p 6 3s 2 3p 6 3d 1 C) 1s 2 2s 2 2p 6 3s 2 3p 6 D) 1s 2 2s 2 2p 6
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8. Which of the following is not a possible electron configuration for a ground state or excited state atom?
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A) 1s 2 2s 2 2p 6 3s 2 3p 6 3d 1 B) 1s 2 2p 6 3s 2 3p 6 4s 1 C) 1s 2 1p 6 2s 2 2p 6 3s 2 3p 6 4s 1 D) 1s 1 2s 1 2p 1 3s 1 3p 1 3d 1
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9. Irregularities from the expected electron configurations based on the Aufbau principle and Hund's rule occur for certain
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A) alkali metals.
B) transition metals.
C) halogens.
D) all of the above.
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10. Calculate the energy of a photon with a wavelength of 4.00x10
-2 nm.
A) 2.65x10
-35 J B) 2.65x10
-44 J C) 4.97x10
-24 J D) 4.97x10
-15 J
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11. Which of the following are all the values for quantum number m l = 4?
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A) 0, 1, 2, 3 when n
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B) 1, 2, 3, 4 C) -3,-2,-1, 0, 1, 2, 3 D) -4,-3,-2,-1, 0, 1, 2, 3, 4 E) -1/2, +1/2
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12. What is the maximum number of orbitals that can be contained in the 5 th shell of an atom? (not including inner shells)
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A) 5 B) 25 C) 2 D) 8 E) 18
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13. Which of the following represents the electron configuration of a silver atom?
A) [Ne] 3s 2 3p 2 B) [Kr] 5s 2 4d 9 C) [Ar] 5s 1 4d 10 D) [Kr] 5s 1 4d 10 E) [Ar] 5s 2 4d 9
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14. Which of the following represents the electron configuration of the ferrous ion?
A) [Ar] 4s 2 3d 6
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B) [Ar] 4s 2 3d 4 C) [Ar] 4s 2 3d 3 D) [Ar] 4s 0 3d 5 E) [Ar] 4s 0 3d 6
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15. How many unpaired electrons does an atom of phosphorus have in the ground 1.
A) 0 state?
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B) 1 C) 2 D) 3 E) 4
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16. Which of the following would have a larger ionic radius?
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A) sulfide ion B) chloride ion C) potassium ion D) calcium ion
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17. Metals tend to have lower first ionization energies than nonmetals.
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A) True B) False
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18. If an element readily forms only one common ion and that ion has a charge of +2 , then the element must have A) first and second ionization energies that are considerably smaller than the third.
B) a high 2nd electron affinity.
C) a very high effective nuclear charge.
D) a noble gas electron configuration.
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19. The electron configurations of stable ions of the representative elements are frequently the same as A) the neutral atom.
B) a noble gas.
C) the atom that is diagonal on the periodic table.
D) the element above it in the same group.
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20. Which of the following statements is true?
A) An ion is always smaller than the neutral atom.
B) An anion is always smaller than the neutral atom.
C) A cation is always smaller than the neutral atom.
D) None of the above.
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21. What is characteristic of a nonmetal?
A) low ionization energy, low electron affinity B) low ionization energy, high electron affinity C) high ionization energy, low electron affinity D) high ionization energy, high electron affinity
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