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27. Elements that have properties of both the metals and the 36. The Bohr model of the atom described the energy state of
nonmetals are electrons with one quantum number. The quantum mechanics
a. semimetals. model uses how many quantum numbers to describe the energy
b. transition elements. state of an electron?
c. semiconductors. a. One
d. noble gases. b. Two
28. Transition elements c. Four
a. are metals. d. Ten
b. belong to the B group. 37. An electron in the second main energy level and the second
c. have variable charges. sublevel is described by the symbols
d. All of the above are correct. a. 1s.
29. The energy of a photon b. 2s.
a. varies inversely with the frequency. c. 1p.
b. is directly proportional to the frequency. d. 2p.
c. varies directly with the velocity. 38. The space in which it is probable that an electron will be found is
d. is inversely proportional to the velocity. described by a (an)
30. A photon of which of the following has the most energy? a. circular orbit.
a. Red light b. elliptical orbit.
b. Orange light c. orbital.
c. Green light d. geocentric orbit.
d. Blue light 39. Two different isotopes of the same element have
31. The lines of color in a line spectrum from a given element a. the same number of protons, neutrons, and electrons.
a. change colors with changes in the temperature. b. the same number of protons and neutrons but different
b. are always the same, with a regular spacing pattern. numbers of electrons.
c. are randomly spaced, having no particular pattern. c. the same number of protons and electrons but different
d. have the same colors, with a spacing pattern that varies with numbers of neutrons.
the temperature. d. the same number of neutrons and electrons but different
numbers of protons.
32. Hydrogen, with its one electron, produces a line spectrum in the
visible light range with 40. The isotopes of a given element always have
a. one color line. a. the same mass and the same chemical behavior.
b. two color lines. b. the same mass and a different chemical behavior.
c. three color lines. c. different masses and different chemical behaviors.
d. four color lines. d. different masses and the same chemical behavior.
33. According to the Bohr model, an electron gains or loses energy 41. If you want to know the number of protons in an atom of a given
only by element, you look up the
a. moving faster or slower in an allowed orbit. a. mass number.
b. jumping from one allowed orbit to another. b. atomic number.
c. being completely removed from an atom. c. atomic weight.
d. jumping from one atom to another atom. d. abundance of isotopes compared to the mass number.
34. According to the Bohr model, when an electron in a hydrogen 42. If you want to know the number of neutrons in an atom of a
atom jumps from an orbit farther from the nucleus to an orbit given element, you
closer to the nucleus, it a. round the atomic weight to the nearest whole number.
a. emits a single photon with energy equal to the energy b. add the mass number and the atomic number.
difference of the two orbits. c. subtract the atomic number from the mass number.
b. emits four photons, one for each of the color lines observed d. add the mass number and the atomic number, then divide
in the line spectrum of hydrogen. by 2.
c. emits a number of photons dependent on the number of orbit 43. Which of the following is always a whole number?
levels jumped over. a. Atomic mass of an isotope
d. None of the above is correct. b. Mass number of an isotope
35. The Bohr model of the atom c. Atomic weight of an element
a. explained the color lines in the hydrogen spectrum. d. None of the above is correct.
b. could not explain the line spectrum of atoms larger than 44. The quantum mechanics and Bohr models of the atom both
hydrogen. agree on
c. had some made-up rules without explanations. a. the significance of the de Broglie wavelength and the
d. All of the above are correct. circumference of an orbit.
b. the importance of momentum in determining the size of an
orbit.
c. how electrons are able to emit light.
d. None of the above is correct.

224 CHAPTER 8 Atoms and Periodic Properties 8-22