1. What is the wavelength of radiation that has a frequency of 2.10 ´ 1014 s -1?
a. 6.30 ´ 1022 m
b. 7.00 ´ 102 nm
c. 7.00 ´ 105 m
d. 1.43 ´ 10-6 m
2. What is the energy in joules of one photon of microwave radiation with a wavelength 0.122 m? (c = 2.9979 ´ 108 m/s; h = 6.626 ´ 10-34 J×s)
a. 2.70 ´ 10-43 J
b. 5.43 ´ 10-33 J
c. 1.63 ´ 10-24 J
d. 4.07 ´ 10-10 J
3. What is the binding energy of an electron in a metal whose threshold frequency for photoelectrons is 2.50 ´ 1014 /s?
a. 99.7 kJ/mol
b. 1.66 ´ 10-19 J/mol
c. 2.75 ´ 10-43 J/mol
d. 7.22 ´ 1017 kJ/mol
4. Complete this sentence: Atoms emit visible and ultraviolet light as:
a. electrons jump from lower energy levels to higher levels.
b. the atoms condense from a gas to a liquid.
c. electrons jump from higher energy levels to lower levels.
d. they are heated and the solid melts to form a liquid.
5. Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 6 to the n = 3 principal energy level. Recall that for hydrogen, En = -2.18 ´ 10-18 J(1/n2).
a. 1.64 ´ 1015 /s
b. 9.13 ´ 1013 /s
c. 3.65 ´ 1014 /s
d. 2.74 ´ 1014/s
6. If a hydrogen atom and a helium atom are traveling at the same speed,
a. the wavelength of the hydrogen atom will be about 4 times longer than the wavelength of the helium atom.
b. the wavelength of the hydrogen atom will be about 2 times longer than the wavelength of the helium.
c. the wavelength of the hydrogen atom will be roughly equal to the wavelength of the helium atom.
d. the wavelength of the helium atom will be about 2 times longer than the wavelength of the hydrogen atom.
7. What is the maximum number of electrons in an atom that can have the following set of quantum numbers? n = 4 l = 3 ml = -2 ms = +1/2
a. 0
b. 1
c. 2
d. 6
8. Electrons in an orbital with l = 3 are in a(n):
a. d orbital.
b. f orbital.
c. g orbital.
d. p orbital.
9. The maximum number of electrons that can occupy an energy level described by the principal quantum number, n, is:
a. n.
b. n + 1.
c. 2n.
d. 2n2.
10. How many orbitals are allowed in a subshell if the angular momentum quantum number for electrons in that subshell is 3?
a. 1
b. 3
c. 5
d. 7
11. Which element has the following ground-state electron configuration?: 1s22s22p63s2
a. Na
b. Mg
c. Al
d. Si
12. Which element has the following ground-state electron configuration?: [Kr]5s24d105p3
a. Sn
b. Sb
c. Pb
d. Bi
13. How many electrons in a ground-state tellurium atom are in orbitals labeled by l = 1?
a. 4
b. 10
c. 12
d. 22
14. Which of the following ground-state atoms is diamagnetic?
a. Ca
b. As
c. Cu
d. Fe
15. When the electron in a hydrogen atom falls from the n = 3 excited energy level to the ground state energy level, a photon with wavelength, l, is emitted. An electron having this same wavelength would have a velocity of:
a. 7.10 ´ 103 m/s.
b. 2.93 ´ 106 m/s.
c. 2.93 ´ 103 m/s.
d. 7.10 m/s.
16. In order to fill an orbital, electrons must be:
a. paired.
b. parallel.
c. ejected.
d. promoted.
e. round.
17. Unpaired electrons are found in:
a. Hund's rule.
b. paramagnetic compounds.
c. magnetic compounds.
d. Hund's rule and paramagnetic compounds.
e. Hund's rule and magnetic compounds.
18. The Aufbau Principle states that:
a. in the ground state, electrons are all excited.
b. each successive electron naturally gets placed in the next most stable orbital.
c. electrons which are placed, are stable.
d. an electron's location and speed cannot be known.
e. electrons are bound to atoms.
19. The structure of the periodic table was created by:
a. Mendeleev.
b. Pauli.
c. Aufbau.
d. Einstein.
e. Bohr.
20. If we somehow knock a proton off of a Fluorine atom, we are left with:
a. the nucleus of a carbon atom.
b. the nucleus of an oxygen atom.
c. the nucleus of a fluorine atom.
d. the nucleus of a neon atom.
e. the nucleus of a boron atom.
21. The element with 32 protons can only be:
a. Germanium.
b. Silicon.
c. Bismuth.
d. Gadolinium.
e. Arsenic.
22. A valence electron is:
a. any electron in the shell of an atom.
b. all those of the highest principle quantum number, plus any in partially-filled orbitals.
c. all electrons in the atom.
d. the core electrons.
e. the majority of electrons.
23. A core electron:
a. is extremely difficult to remove from the atom.
b. is close to the center of the atom.
c. is tightly held.
d. can be removed with very high energy beams.
e. all of the choices apply.
24. When an electron is gained or lost, a(n) ________ is formed.
a. cation
b. ion
c. anion
d. all of the choices apply
25. Electrons repel each other,:
a. unless they are paired.
b. unless they are in different orbitals.
c. unless Hund's rule fails.
d. unless they reach equilibrium.
e. unless they are lost.
26. An atom with all electrons paired, not attracted by magnets, is called:
a. paramagnetic.
b. diamagnetic.
c. magnetic.
d. geomagnetic.
e. unmagnetic.
27. An atom with all electrons unpaired, and attracted by magnets, is called:
a. paramagnetic.
b. diamagnetic.
c. magnetic.
d. geomagnetic.
e. unmagnetic.
28. Most of the volume in the atom is occupied by:
a. the valence electrons.
b. the core electrons.
c. the nucleus.
d. the quanta.
e. the neutrons.
29. Electron affinity is defined as:
a. the tendency of an atom to repel an electron.
b. the energy change when an electron is added to an atom.
c. the ionization energy.
d. the work required to add an electron to a system.
e. the first electron to leave an atom.
30. The size of an atomic radius is determined by:
a. how tightly that atom holds its electrons.
b. how the atoms fit together.
c. how the atoms repel each other.
d. how much the electrons try to leave.
e. how the atom boosts its energy through repulsion.