ch. 8 Multiple Choice

12. This isotope provides the standard to which the masses of all other isotopes are compared: a. carbon-12 b. oxygen-16 c. hydrogen-1 d. gold-197

a. carbon-12

22. The arrangement of electrons in orbitals is called a. electron configuration. b. periodic table. c. quantum numbers. d. energy levels.

a. electron configuration

14. Energy of the electron is expressed in units of a. electron volts. b. electron watts. c. quantum leaps. d. orbit numbers.

a. electron volts.

19. An electron moving from an excited state to the ground state a. emits a photon. b. gains a photon. c. gains a charge. d. loses a charge.

a. emits a photon

34. According to the Bohr model, when an electron in a hydrogen atom jumps from an orbit farther from the nucleus to an orbit closer to the nucleus, it a. emits a single photon with energy equal to the energy difference of the two orbits. b. emits four photons, one for each of the color lines observed in the line spectrum of hydrogen. c. emits a number of photons dependent on the number of orbit levels jumped over. d. None of the above is correct.

a. emits a single photon with energy equal to the energy difference of the two orbits.

26. The gain or loss of electrons from an atom results in the formation of a (an) a. ion. b. metal. c. semiconductor. d. isotope.

a. ion

46. A photon is emitted from the electronic structure of an atom when an electron a. jumps from a higher to a lower energy level. b. jumps from a lower to a higher energy level. c. reverses its spin by 180°. d. is removed from an atom by a high quantum of energy.

a. jumps from a higher to a lower energy level

6. The atomic number is the number of a. protons. b. protons plus neutrons. c. protons plus electrons. d. protons, neutrons, and electrons in an atom.

a. protons.

1. Thomson was convinced that he had discovered a subatomic particle, the electron, from the evidence that a. the charge-to-mass ratio was the same for all materials. b. cathode rays could move through a vacuum. c. electrons were attracted toward a negatively charged plate. d. the charge was always 1.60 x 10^- 19 coulomb

a. the charge-to-mass ratio was the same for all materials

43. Which of the following is always a whole number? a. Atomic mass of an isotope b. Mass number of an isotope c. Atomic weight of an element d. None of the above is correct.

b. Mass number of an isotope

48. In what are atoms of 126 C and 146 C different? a. Number of protons b. Number of neutrons c. Number of electrons d. None of the above is correct.

b. Number of neutrons

23. Group IIA elements are called a. alkali metals. b. alkaline earth metals. c. alkaline salts. d. beryllium metals.

b. alkaline earth metals

31. The lines of color in a line spectrum from a given element a. change colors with changes in the temperature. b. are always the same, with a regular spacing pattern. c. are randomly spaced, having no particular pattern. d. have the same colors, with a spacing pattern that varies with the temperature.

b. are always the same, with a regular spacing pattern.

41. If you want to know the number of protons in an atom of a given element, you look up the a. mass number. b. atomic number. c. atomic weight. d. abundance of isotopes compared to the mass number.

b. atomic number.

13. In 1910, Max Planck introduced the idea that matter emits and absorbs energy in a. light waves. b. discrete units called quanta. c. pulses with no particular pattern. d. pulses that vary in magnitude over time.

b. discrete units called quanta.

29. The energy of a photon a. varies inversely with the frequency. b. is directly proportional to the frequency. c. varies directly with the velocity. d. is inversely proportional to the velocity.

b. is directly proportional to the frequency

33. According to the Bohr model, an electron gains or loses energy only by a. moving faster or slower in an allowed orbit. b. jumping from one allowed orbit to another. c. being completely removed from an atom. d. jumping from one atom to another atom.

b. jumping from one allowed orbit to another.

16. Light from an incandescent gas is dispersed into narrow lines of colors with no light between the lines. This is called a (an) a. impossible spectrum. b. line spectrum. c. Balmer spectrum. d. Newton spectrum.

b. line spectrum

10. The sum of the numbers of protons and neutrons in the nucleus of an atom is the a. nucleon number. b. mass number. c. atomic weight. d. isotope number.

b. mass number.

21. Any moving particle has a wavelength that is associated with its mass and velocity. This is a statement that proposed the existence of a. photoelectric effect. b. matter waves. c. quanta. d. photons.

b. matter waves

8. The main problem with a solar system model of the atom is that a. electrons move in circular, not elliptical orbits. b. the electrons should lose energy since they are accelerating. c. opposite charges should attract one another. d. the mass ratio of the nucleus to the electrons is wrong.

b. the electrons should lose energy since they are accelerating.

49. An atom has 6 protons, 6 electrons, and 6 neutrons, so the isotope symbol is a. 18 \\ 12 Mg b. 12 \\ 12 Mg c. 12 \\ 6 C d. 18 \\ 6 C

c. 12 \\ 6 C

25. The element chlorine belongs to which group? a. Alkali metals b. Lanthanides c. Halogens d. Noble gases

c. Halogens

20. The existence of matter waves was proposed by a. Planck. b. Bohr. c. de Broglie. d. Einstein.

c. de Broglie

36. The Bohr model of the atom described the energy state of electrons with one quantum number. The quantum mechanics model uses how many quantum numbers to describe the energy state of an electron? a. One b. Two c. Four d. Ten

c. four

17. The lowest energy state or level of an atom is the a. bottom state. b. lowest level. c. ground state. d. basement state.

c. ground state.

44. The quantum mechanics and Bohr models of the atom both agree on a. the significance of the de Broglie wavelength and the 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.

c. how electrons are able to emit light

9. Atoms of an element that have different numbers of neutrons are called a. allotropes. b. isomers. c. isotopes. d. radioactive.

c. isotopes.

5. Rutherford's estimate of the radius of an atomic nucleus was based on a. the drift of oil droplets in an electric field. b. speculation about expected symmetry in gold foil. c. measurements of radioactive particle deflections from gold foil. d. measurements of the breakup of a nitrogen atom by collisions with radioactive particles.

c. measurements of radioactive particle deflections from gold foil.

38. The space in which it is probable that an electron will be found is described by a (an) a. circular orbit. b. elliptical orbit. c. orbital. d. geocentric orbit.

c. orbital

24. The elements in A groups are called a. alkali elements. b. transition elements. c. representative elements. d. metals.

c. representative elements

27. Elements that have properties of both the metals and the nonmetals are a. semimetals. b. transition elements. c. semiconductors. d. noble gases.

c. semiconductors

2. The existence of a tiny, massive, and positively charged nucleus was deduced from the observation that a. fast, massive, and positively charged radioactive particles all move straight through metal foil. b. radioactive particles were deflected by a magnetic field. c. some radioactive particles were deflected by metal foil. d. None of the above is correct.

c. some radioactive particles were deflected by metal foil.

42. If you want to know the number of neutrons in an atom of a given element, you a. round the atomic weight to the nearest whole number. b. add the mass number and the atomic number. c. subtract the atomic number from the mass number. d. add the mass number and the atomic number, then divide by 2.

c. subtract the atomic number from the mass number

15. The major success of the Bohr theory was in explaining a. how electrons move in circular orbits. b. why radiationless orbits existed. c. the colors in the hydrogen line spectrum. d. why the angular momentum of the electron should be by orbit quantum numbers.

c. the colors in the hydrogen line spectrum.

39. Two different isotopes of the same element have a. the same number of protons, neutrons, and electrons. b. the same number of protons and neutrons but different numbers of electrons. c. the same number of protons and electrons but different numbers of neutrons. d. the same number of neutrons and electrons but different numbers of protons.

c. the same number of protons and electrons but different numbers of neutrons

45. Hydrogen, with its one electron, can produce a line spectrum with four visible colors because a. an isotope of hydrogen has four electrons. b. electrons occur naturally with four different colors. c. there are multiple energy levels that an electron can occupy. d. electrons are easily scattered.

c. there are multiple energy levels that an electron can occupy.

37. An electron in the second main energy level and the second sublevel is described by the symbols a. 1s. b. 2s. c. 1p. d. 2p

d. 2p

28. Transition elements a. are metals. b. belong to the B group. c. have variable charges. d. All of the above are correct.

d. All of the above are correct.

35. The Bohr model of the atom a. explained the color lines in the hydrogen spectrum. b. could not explain the line spectrum of atoms larger than hydrogen. c. had some made-up rules without explanations. d. All of the above are correct.

d. All of the above are correct.

47. Which of the following represents a hydrogen isotope? a. 1 \\ 1 H b. 2 \\ 1 H c. 3 \\ 1 H d. All of the above are correct.

d. All of the above are correct.

7. All neutral atoms of an element have the same a. atomic number. b. number of electrons. c. number of protons. d. All of the above are correct.

d. All of the above are correct.

30. A photon of which of the following has the most energy? a. Red light b. Orange light c. Green light d. Blue light

d. Blue light

11. Atomic weight is a. determined by weighing individual atoms. b. an average weight of the isotopes of an element. c. the number of protons and neutrons in a nucleus. d. a weighted average of the masses of isotopes of an element based on abundance.

d. a weighted average of the masses of isotopes of an element based on abundance.

40. The isotopes of a given element always have a. the same mass and the same chemical behavior. b. the same mass and a different chemical behavior. c. different masses and different chemical behaviors. d. different masses and the same chemical behavior.

d. different masses and the same chemical behavior

3. According to Rutherford's calculations, the volume of an atom is mostly a. occupied by protons and neutrons. b. filled with electrons. c. occupied by tightly bound protons, electrons, and neutrons. d. empty space.

d. empty space.

32. Hydrogen, with its one electron, produces a line spectrum in the visible light range with a. one color line. b. two color lines. c. three color lines. d. four color lines.

d. four color lines.

4. Millikan measured the charge on oil droplets and found that all the droplets had a. different charges. b. random charges, without any pattern. c. five groupings of different charges. d. the same or multiples of the same charge.

d. the same or multiples of the same charge.

18. The basis of the quantum mechanics theory of the atom is a. spin and quantum leaps of electron masses. b. elliptical orbits of electrons. c. how electron particles move in orbits. d. the wave nature of electrons.

d. the wave nature of electrons.

quizlet won't let me type subscripts and superscripts, so in the next cards (questions 47 and 49), the superscript will be the number listed first and then the subscript will be the number listed second, separated by \\

quizlet won't let me type subscripts and superscripts, so in the next cards (questions 47 and 49), the superscript will be the number listed first and then the subscript will be the number listed second, separated by \\