Chemistry The Molecular Science 5th Edition by John W. Moore - Test Bank
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Chemistry The Molecular Science 5th Edition by John W. Moore - Test Bank

Chemistry The Molecular Science 5th Edition by John W. Moore - Test Bank   Instant Download - Complete Test Bank With Answers     Sample Questions Are Posted Below   1. A photon of light has a frequency of 3.26 × 1015 hertz. What is its wavelength? The speed of light is 3.00 × 108 m/s. …

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Chemistry The Molecular Science 5th Edition by John W. Moore – Test Bank

 

Instant Download – Complete Test Bank With Answers

 

 

Sample Questions Are Posted Below

 

1. A photon of light has a frequency of 3.26 × 1015 hertz. What is its wavelength? The speed of light is 3.00 × 108 m/s.

  a. 109 nm
  b. 9.78 × 1014 nm
  c. 978 nm
  d. 1.09 × 107 nm
  e. 92.0 nm

 

ANSWER:   e
RATIONALE:   Related to Problem-Solving Example 5.1
POINTS:   1
TOPICS:   5.1 Electromagnetic Radiation and Matter
OTHER:   Application
NOTES:   Solve problems with required skills or knowledge

 

2. Light has a frequency of 7.21 × 1013 hertz. What is its wavelength? The speed of light is 3.00 × 108 m/s.

  a. 4.16 × 103 nm
  b. 2.40 × 105 nm
  c. 2.40 × 10−4 nm
  d. 4.16 × 10−6 nm
  e. 2.16 × 109 nm

 

ANSWER:   a
RATIONALE:   Related to Problem-Solving Example 5.1
POINTS:   1
TOPICS:   5.1 Electromagnetic Radiation and Matter
OTHER:   Application
NOTES:   Solve problems using required skills and knowledge

 

3. Light has a wavelength of 444 nm. What is its frequency? The speed of light is 3.00 × 108 m/s.

  a. 6.76 × 10−4 Hz
  b. 1.48 × 102 Hz
  c. 1.48 × 10−6 Hz
  d. 1.48 × 10−15 Hz
  e. 6.76 × 1014 Hz

 

ANSWER:   e
RATIONALE:   Related to Problem-Solving Example 5.1
POINTS:   1
TOPICS:   5.1 Electromagnetic Radiation and Matter
OTHER:   Application
NOTES:   Solve problems using required skills and knowledge

 

4. Light has a wavelength of 582 nm. What is its frequency? The speed of light is 3.00 × 108 m/s.

  a. 1.94 × 103 Hz
  b. 5.15 × 1014 Hz
  c. 1.75 × 102 Hz
  d. 1.75 × 1020 Hz
  e. 1.94 × 1013 Hz

 

ANSWER:   b
RATIONALE:   Related to Problem-Solving Example 5.1
POINTS:   1
TOPICS:   5.1 Electromagnetic Radiation and Matter
OTHER:   Application
NOTES:   Solve problems using required skills and knowledge

 

5. Which wavelength of light is the fastest?

  a. 626.1 nm
  b. 563.8 nm
  c. 418.6 nm
  d. 554.9 nm
  e. All have the same speed.

 

ANSWER:   e
POINTS:   1
TOPICS:   5.1 Electromagnetic Radiation and Matter
OTHER:   Comprehension
NOTES:   Grasp meaning

 

6. Which of the following statements is/are correct?

I. The frequency of light is the number of waves that pass a given point in a second.
II. The shorter the wavelength of light, the greater its energy.
III. The wavelength of light increases as the frequency increases.

 

  a. I only
  b. II only
  c. III only
  d. I and II
  e. II and III

 

ANSWER:   d
POINTS:   1
TOPICS:   5.1 Electromagnetic Radiation and Matter
OTHER:   Analysis
NOTES:   Organizing parts

 

7. Arrange the following four electromagnetic spectral regions in order of decreasing energy.
visible X-ray microwave radio

  a. X-ray, radio, visible, microwave
  b. X-ray, visible, microwave, radio
  c. microwave, radio, X-ray, visible
  d. radio, visible, X-ray, microwave
  e. microwave, visible, X-ray, radio

 

ANSWER:   b
RATIONALE:   Connects information presented in Figure 5.2 with Planck’s relationship.
POINTS:   1
TOPICS:   5.2 Planck’s Quantum Theory
OTHER:   Analysis
NOTES:   Organization of parts

 

8. What is the phenomenon that occurs when certain metals emit electrons when illuminated by particular wavelengths of light?

  a. electromagnetic spectrum
  b. Planck’s constant
  c. emission spectrum
  d. quantum theory
  e. photoelectric effect

 

ANSWER:   e
POINTS:   1
TOPICS:   5.2 Planck’s Quantum Theory
KEYWORDS:   Knowledge
OTHER:   Knowledge of major ideas

 

9. What is the phenomenon that occurs when excited gaseous elements emit only a few colored lines?

  a. Planck’s constant
  b. photoelectric effect
  c. electromagnetic spectrum
  d. quantum theory
  e. line spectrum

 

ANSWER:   e
POINTS:   1
TOPICS:   5.3 The Bohr Model of the Hydrogen Atom
OTHER:   Knowledge
NOTES:   Knowledge of major ideas

 

10. Which statement about light is true?

  a. It exhibits both wave and particle-like behavior at the same time.
  b. It behaves as a particle only.
  c. It has neither wave nor particle-like behavior.
  d. It oscillates back and forth between wave and particle-like behavior.
  e. It behaves as a wave only.

 

ANSWER:   a
POINTS:   1
TOPICS:   5.2 Planck’s Quantum Theory
OTHER:   Comprehension
NOTES:   Grasp meaning

 

11. Determine the energy of a photon that has a frequency of 5.23 × 1014 Hz. Given: h = 6.63 × 10−34 J s.

  a. 1.27 × 10−48 J
  b. 3.47 × 10−19 J
  c. 1.16 × 10−27 J
  d. 1.04 × 10−10 J
  e. 7.87 × 1047 J

 

ANSWER:   b
POINTS:   1
TOPICS:   5.2 Planck’s Quantum Theory
OTHER:   Application
NOTES:   Solve problems using required skills or knowledge

 

12. Determine the energy of a photon that has a wavelength of 488 nm. The speed of light is 3.00 × 108 m/s and h = 6.63 × 10−34 J s.

  a. 9.71 × 10−23 J
  b. 4.52 × 10−36 J
  c. 4.08 × 10−19 J
  d. 1.63 × 10−15 J
  e. 4.08 × 10−28 J

 

ANSWER:   c
POINTS:   1
TOPICS:   5.2 Planck’s Quantum Theory
OTHER:   Application
NOTES:   Solve problems using required skills or knowledge

 

13. What is a photon?

  a. a massless “particle” or bundle of energy that moves at the speed of light
  b. very high frequency light
  c. a high speed electron that gives off light when it strikes an object
  d. light that comes from a cathode ray tube
  e. very long wavelength light

 

ANSWER:   a
POINTS:   1
TOPICS:   5.2 Planck’s Quantum Theory
OTHER:   Knowledge
NOTES:   Recall of information

 

14. Which of the following is not a characteristic of the Bohr model of the atom?

  a. An electron is restricted to specific energy levels around the nucleus.
  b. Each orbit has a discrete energy associated with it.
  c. Orbits have a defined circumference.
  d. An electron is located in an orbit around the nucleus.
  e. Orbits have any radii.

 

ANSWER:   e
POINTS:   1
TOPICS:   5.3 The Bohr Model of the Hydrogen Atom
OTHER:   Comprehension
NOTES:   Grasp meaning

 

15. According to the Bohr model for the hydrogen atom, the energy necessary to excite an electron from n = 2 to n = 3 is ________ the energy necessary to excite an electron from n = 3 to n = 4.

  a. either more than or equal to
  b. equal to
  c. less than
  d. more than
  e. either less than or equal to

 

ANSWER:   d
RATIONALE:   See Problem-Solving Example 5.3
POINTS:   1
TOPICS:   5.3 The Bohr Model of the Hydrogen Atom
OTHER:   Comprehension
NOTES:   Predict consequences

 

16. What is a major shortcoming of the Bohr model?

  a. It implies that a one electron system can have four colors of light in its line spectrum.
  b. It accounts for the existence of line spectra.
  c. It explains the spectral characteristics of hydrogen.
  d. It requires that the energy in the atom be quantized.
  e. It does not deal with multielectron atoms.

 

ANSWER:   e
RATIONALE:   Though the Bohr Model is introduced in 5.3, the limits of this model are introduced in the first paragraph of 5.4.
POINTS:   1
TOPICS:   5.4 Beyond the Bohr Model: The Quantum Mechanical Model of the Atom
OTHER:   Comprehension
NOTES:   Interpret facts

 

17. Which idea was proposed by Louis de Broglie?

  a. Excited state orbits have higher energy than ground state orbits.
  b. Electrons are located in orbits.
  c. Small particles, such as electrons, move in waves.
  d. Electrons have clockwise or counter-clockwise spins.
  e. Energy in the atom is quantized.

 

ANSWER:   c
POINTS:   1
TOPICS:   5.4 Beyond the Bohr Model: The Quantum Mechanical Model of the Atom
OTHER:   Knowledge
NOTES:   Recall of information

 

18. Which idea was proposed by Werner Heisenberg?

  a. Photons used to determine the location of electrons have no measurable effect on electrons.
  b. Certain metals emit electrons when illuminated by light with low enough wavelength.
  c. Simultaneously determining the exact momentum and exact position of an electron is impossible.
  d. Light waves passing through a diffraction parting produce a diffraction pattern.
  e. Light waves have particle properties, and particles of matter have wave-like properties.

 

ANSWER:   c
POINTS:   1
TOPICS:   5.4 Beyond the Bohr Model: The Quantum Mechanical Model of the Atom
KEYWORDS:   Knowledge
OTHER:   Recall of information

 

19. Which statement regarding an orbital is false?

  a. Only one electron is allowed per orbital.
  b. An orbital is three dimensional.
  c. An electron shell consists of a collection of orbitals with the same principal quantum number.
  d. An orbital may be designated with the letters s, p, d, f.
  e. An orbital boundary surface would need to be infinitely large to guarantee that an electron would always be found inside the orbital.

 

ANSWER:   a
RATIONALE:   Orbitals are first defined in 5.4, but some of the choices are from 5.5.
POINTS:   1
TOPICS:   5.5 Quantum Numbers, Energy Levels and Atomic Orbitals
OTHER:   Comprehension
NOTES:   Grasp meaning

 

20. Match the names of the four quantum numbers with their symbols.
azimuthal magnetic principal spin

  a. ml, ms, l, n
  b. n, l, ml, ms
  c. ml, l, n, ms
  d. l, ml, n, ms
  e. l, ms, n, ml

 

ANSWER:   d
POINTS:   1
TOPICS:   5.5 Quantum Numbers, Energy Levels and Atomic Orbitals
OTHER:   Knowledge
NOTES:   Observation and recall of information

 

21. Which word or phrase least applies to the quantum number represented by the symbol n?

  a. shape
  b. distance from nucleus
  c. shell
  d. size
  e. principal

 

ANSWER:   a
POINTS:   1
TOPICS:   5.5 Quantum Numbers, Energy Levels and Atomic Orbitals
OTHER:   Comprehension
NOTES:   Interpret facts, compare

 

22. Which word or phrase least applies to the quantum number represented by the symbol l?

  a. shape
  b. orientation
  c. subshell
  d. s, p, d, f
  e. azimuthal

 

ANSWER:   b
POINTS:   1
TOPICS:   5.5 Quantum Numbers, Energy Levels and Atomic Orbitals
OTHER:   Comprehension
NOTES:   Interpret facts, compare

 

23. Which azimuthal quantum numbers can exist for n = 3?

  a. l = 0, 1
  b. l = 0, 1, 2, 3
  c. l = 0, 1, 2
  d. l = 0
  e. l = 0, 1, 2, 3, 4

 

ANSWER:   c
POINTS:   1
TOPICS:   5.5 Quantum Numbers, Energy Levels and Atomic Orbitals
OTHER:   Application
NOTES:   Use information

 

24. If l = 2, what value can ml have?

  a. ml = +1
  b. ml = 0, +1, +2
  c. ml = +2
  d. ml = −1, 0, +1
  e. ml = −2, −1, 0, +1, +2

 

ANSWER:   e
POINTS:   1
TOPICS:   5.5 Quantum Numbers, Energy Levels and Atomic Orbitals
OTHER:   Application
NOTES:   Use information

 

25. How many electrons can the third principal quantum level hold?

  a. 18
  b. 8
  c. 2
  d. 16
  e. 32

 

ANSWER:   a
POINTS:   1
TOPICS:   5.5 Quantum Numbers, Energy Levels and Atomic Orbitals
OTHER:   Analysis
NOTES:   Recognition of hidden meanings

 

26. How many orbitals are contained in the 4d subshell?

  a. 14
  b. 5
  c. 2
  d. 10
  e. 6

 

ANSWER:   b
POINTS:   1
TOPICS:   5.5 Quantum Numbers, Energy Levels and Atomic Orbitals
OTHER:   Application
NOTES:   Use concepts in new situations

 

27. How many electrons can be contained in the 2p subshell?

  a. 2
  b. 1
  c. 4
  d. 3
  e. 6

 

ANSWER:   e
POINTS:   1
TOPICS:   5.5 Quantum Numbers, Energy Levels and Atomic Orbitals
OTHER:   Application
NOTES:   Use concepts in new situations

 

28. Which statement is true?

  a. The 3d orbitals have lower energy than the 2p orbitals.
  b. The 2p orbitals hold up to 6 electrons.
  c. The 4p orbitals hold more electrons than the 3d orbitals.
  d. The p orbitals occur in groups of 5.
  e. Two electrons in the 1s orbital will have the same spin.

 

ANSWER:   b
POINTS:   1
TOPICS:   5.5 Quantum Numbers, Energy Levels and Atomic Orbitals
OTHER:   Application
NOTES:   Use information

 

29. The d orbitals occur in groups of __________ and hold up to __________ electrons.

  a. 7, 14
  b. 3, 6
  c. 5, 10
  d. 6, 12
  e. 4, 8

 

ANSWER:   c
POINTS:   1
TOPICS:   5.5 Quantum Numbers, Energy Levels and Atomic Orbitals
OTHER:   Knowledge
NOTES:   Observation and recall of information

 

30. Which set of quantum numbers is not allowed?

  a. n = 2, l = 1, ml = 1, ms = +1/2
  b. n = 0, l = 0, ml = 0, ms = +1/2
  c. n = 4, l = 3, ml = 0, ms = −1/2
  d. n = 3, l = 1, ml = 0, ms = +1/2
  e. n = 1, l = 0, ml = 0, ms = +1/2

 

ANSWER:   b
POINTS:   1
TOPICS:   5.5 Quantum Numbers, Energy Levels and Atomic Orbitals
OTHER:   Comprehension
NOTES:   Interpret facts/predict consequences

 

31. Which type of atomic orbital has two lobes of electron density?

  a. d
  b. p and d
  c. s
  d. p
  e. s and p

 

ANSWER:   d
RATIONALE:   3p orbitals are represented with four lobes in Figure 5.18.
POINTS:   1
TOPICS:   5.6 Shapes of Atomic Orbitals
OTHER:   Comprehension
NOTES:   Understanding information

 

32. What is the correct electron configuration for beryllium (Be)?

  a. 1s22s22p6
  b. 1s22s2
  c. 1s22s22p1
  d. 1s22s22p2
  e. 1s22s22p4

 

ANSWER:   b
POINTS:   1
TOPICS:   5.7 Atom Electron Configurations
OTHER:   Application
NOTES:   Use methods, concepts, theories in new situations

 

33. What is the correct electron configuration for aluminum?

  a. 1s22s22p63s23p1
  b. 1s22s22p43s23p3
  c. 1s22s22p23s23p23d24s1
  d. 1s22s22p23s23p24s25s1
  e. 1s22s1

 

ANSWER:   a
POINTS:   1
TOPICS:   5.7 Atom Electron Configurations
OTHER:   Application
NOTES:   Use methods, concepts, theories in new situations

 

34. What is the correct electron configuration for gallium?

  a. 1s22s22p63s23p64s24d104p1
  b. 1s22s22p63s23p63d104p3
  c. 1s22s22p63s23p1
  d. 1s22s22p63s23p63d104s24p1
  e. 1s22s22p63s23p64s24p1

 

ANSWER:   d
POINTS:   1
TOPICS:   5.7 Atom Electron Configurations
OTHER:   Application
NOTES:   Use methods, concepts, theories in new situations

 

35. Give the element that has the electron configuration:
1s22s22p63s23p63d104s24p65s2

  a. In
  b. Sr
  c. Ni
  d. Fe
  e. Pd

 

ANSWER:   b
POINTS:   1
TOPICS:   5.7 Atom Electron Configurations
OTHER:   Application
NOTES:   Use methods, concepts, theories in new situations

 

36. Nearly all the first row transition metal elements will form a +2 cation, what is the best explanation of this observation?

  a. Electrons are always removed in pairs.
  b. Electrons are placed in the s-orbital before filling the d-orbtials, and the s-orbitals can hold 2 electrons.
  c. All of the +2 cations will become isoelectronic with a noble gas element, thus they are most stable.
  d. Electrons are removed from the s-orbital first because s-orbital is of higher energy than the d-orbital when there are both s– and d– electrons present.
  e. The s– and d-orbitals are very close in energy, and all of the transition elements will rearrange their electronic configuration to get filled or half-filled shells

 

ANSWER:   d
POINTS:   1
TOPICS:   5.7 Atom Electron Configurations
OTHER:   Synthesis
NOTES:   Generalize from given facts

 

37. Which of the following corresponds to the electron configuration of a noble gas?

  a. 1s22s22p63s23p6
  b. 1s22s22p63s23p63d104s24p2
  c. 1s22s2
  d. 1s22s22p63s23p63d104s24p3
  e. 1s22s22p4

 

ANSWER:   a
POINTS:   1
TOPICS:   5.7 Atom Electron Configurations
OTHER:   Application
NOTES:   Use methods, concepts, theories in new situations

 

38. What is the correct shorthand notation for the electron configuration given?
1s22s22p63s23p64s23d104p65s2

  a. [Ar]3s23p63d104p65s2
  b. [Ar]5s2
  c. [Rb]5s1
  d. [Kr]5s2
  e. [Ca]3d104p65s2

 

ANSWER:   d
POINTS:   1
TOPICS:   5.7 Atom Electron Configurations
OTHER:   Application
NOTES:   Use methods, concepts, theories in new situations

 

39. What is the electron configuration of arsenide ion, As3−?

  a. 1s22s22p63s23p63d104s24p6
  b. 1s22s22p63s23p64s24d10
  c. 1s22s22p63s23p63d104s2
  d. 1s22s22p63s23p63d10
  e. 1s22s22p63s23p64s24d104p6

 

ANSWER:   a
POINTS:   1
TOPICS:   5.8 Ion Electron Configurations
OTHER:   Application
NOTES:   Use methods, concepts, theories in new situations

 

40. What is the electron configuration of O2−?

  a. 1s22s22p3
  b. 1s22s22p5
  c. 1s22s22p4
  d. 1s22s22p6
  e. 1s22s22p2

 

ANSWER:   d
POINTS:   1
TOPICS:   5.8 Ion Electron Configurations
OTHER:   Application
NOTES:   Use methods, concepts, theories in new situations

 

41. What is the electron configuration of Li+?

  a. 1s1
  b. 1s22s22p1
  c. 1s22s2
  d. 1s2
  e. 1s22s1

 

ANSWER:   d
POINTS:   1
TOPICS:   5.8 Ion Electron Configurations
OTHER:   Application
NOTES:   Use methods, concepts, theories in new situations

 

42. What is the electron configuration of Al3+?

  a. 1s22s22p5
  b. 1s22s22p6
  c. 1s22s22p4
  d. 1s22s22p2
  e. 1s22s22p63s23p1

 

ANSWER:   b
POINTS:   1
TOPICS:   5.8 Ion Electron Configurations
OTHER:   Application
NOTES:   Use methods, concepts, theories in new situations

 

43. Which one of the following does not have the electron configuration [Ne]3s23p6?

  a. Ca2+
  b. Ar
  c. K+
  d. Br−
  e. Cl−

 

ANSWER:   d
POINTS:   1
TOPICS:   5.8 Ion Electron Configurations
OTHER:   Analysis
NOTES:   Seeing patterns

 

44. Substances that have the same electron configuration are:

  a. lanthanides.
  b. paramagnetic.
  c. isoelectronic.
  d. diamagnetic.
  e. ferromagnetic.

 

ANSWER:   c
POINTS:   1
TOPICS:   5.8 Ion Electron Configurations
OTHER:   Analysis
NOTES:   Seeing patterns

 

45. Atoms or ions without unpaired electrons are:

  a. ferromagnetic.
  b. diamagnetic.
  c. lanthanides.
  d. paramagnetic.
  e. isoelectronic.

 

ANSWER:   b
POINTS:   1
TOPICS:   5.8 Ion Electron Configurations
OTHER:   Knowledge
NOTES:   Knowledge of major ideas

 

46. Permanent magnets are:

  a. lanthanides.
  b. isoelectronic.
  c. diamagnetic.
  d. ferromagnetic.
  e. paramagnetic.

 

ANSWER:   d
POINTS:   1
TOPICS:   5.8 Ion Electron Configurations
OTHER:   Knowledge
NOTES:   Knowledge of major ideas

 

47. Xenon, the iodide ion and the cesium ion are:

I. diamagnetic.
II. isoelectronic.
III. ferromagnetic.

 

  a. I only
  b. II only
  c. III only
  d. I and II
  e. II and III

 

ANSWER:   d
POINTS:   1
TOPICS:   5.8 Ion Electron Configurations
OTHER:   Analysis
NOTES:   Recognition of hidden meanings

 

48. Which element has the largest atomic radius?

  a. O
  b. Na
  c. He
  d. H
  e. F

 

ANSWER:   b
POINTS:   1
TOPICS:   5.9 Periodic Trends: Atomic Radii
OTHER:   Analysis
NOTES:   Seeing patterns

 

49. Which element has the largest atomic radius?

  a. Br
  b. P
  c. As
  d. F
  e. Se

 

ANSWER:   c
POINTS:   1
TOPICS:   5.9 Periodic Trends: Atomic Radii
OTHER:   Analysis
NOTES:   Seeing patterns

 

50. Arrange the elements given in order from largest to smallest atomic radii.
K Ne Ar Na P

  a. Ne > Ar > P > Na > K
  b. Ar > P > Na > Ne > K
  c. K > Ar > P > Na > Ne
  d. Ar > K > Na > Ne >P
  e. K > Na > P > Ar > Ne

 

ANSWER:   e
POINTS:   1
TOPICS:   5.9 Periodic Trends: Atomic Radii
OTHER:   Analysis
NOTES:   Organization of parts

 

51. Which of the following has the largest ionic radius?

  a. F−
  b. Cl−
  c. K+
  d. Na+
  e. P3−

 

ANSWER:   e
POINTS:   1
TOPICS:   5.10 Periodic Trends: Ionic Radii
OTHER:   Analysis
NOTES:   Seeing patterns

 

52. Which statement is false?

  a. Mg2+ is smaller than Ca2+.
  b. Cl− is smaller than S2−.
  c. N3− is larger than Ne.
  d. Br− is larger than Kr.
  e. K+ is smaller than Ar.

 

ANSWER:   e
POINTS:   1
TOPICS:   5.10 Periodic Trends: Ionic Radii
OTHER:   Analysis
NOTES:   Seeing patterns/organization of parts

 

53. Which element has the largest first ionization energy?

  a. Ca
  b. Be
  c. Mg
  d. Ba
  e. Sr

 

ANSWER:   b
POINTS:   1
TOPICS:   5.11 Periodic Trends: Ionization Energies
OTHER:   Analysis
NOTES:   Seeing patterns

 

54. Arrange the following in order of increasing ionization energy.
Ar Cl Li Na P

  a. Na < Li < P < Cl < Ar
  b. P < Cl < Ar < Li < Na
  c. P < Cl < Ar < Na < Li
  d. Ar < Cl < Na < Li < P
  e. Cl < Ar < Na < Li < P

 

ANSWER:   a
POINTS:   1
TOPICS:   5.11 Periodic Trends: Ionization Energies
OTHER:   Analysis
NOTES:   Organization of parts

 

55. Which element has an electron affinity greater than zero?

  a. Te
  b. As
  c. Br
  d. Kr
  e. I

 

ANSWER:   d
POINTS:   1
TOPICS:   5.12 Periodic Trends: Electron Affinities
OTHER:   Analysis
NOTES:   Seeing patterns

 

56. Which statement about the formation of solid sodium chloride from sodium metal atoms and chlorine atoms is false?

  a. Sodium chloride contains alternating atoms in a crystal lattice.
  b. The sodium cation has an octet of outer electrons.
  c. Sodium atoms transfer electrons to chlorine atoms.
  d. The formation of sodium chloride releases energy to the surroundings.
  e. The chloride anion has an octet of outer electrons.

 

ANSWER:   a
POINTS:   1
TOPICS:   5.13 Ion Formation and Ionic Compounds
OTHER:   Comprehension
NOTES:   Interpret facts

 

57. Which statement about the Born-Haber cycle is false?

  a. The cycle involves an ionization energy.
  b. The cycle involves an electron affinity.
  c. The cycle is an application of Hess’s Law.
  d. The cycle is involves a lattice energy.
  e. The cycle involves an enthalpy of fusion.

 

ANSWER:   e
POINTS:   1
TOPICS:   5.13 Energy Considerations in Ionic Compound Formation
OTHER:   Comprehension
NOTES:   Interpret facts

 

58. What is the time span between wave peaks called?

ANSWER:   period
POINTS:   1

 

59. _____________ is how often two successive peaks or troughs in electromagnetic radiation pass per second.

ANSWER:   frequency
POINTS:   1

 

60. In a vacuum, all light travels with the same _____________.

ANSWER:   speed
POINTS:   1

 

61. Electrons in the lowest _____________ level are in the ground state.

ANSWER:   energy
POINTS:   1

 

62. The _____________ cycle is a multistep application of Hess’ law that allows for the calculation of the lattice energy of a crystal.

ANSWER:   Born-Haber
POINTS:   1

 

63. A rainbow is an example of a continuous _____________.

ANSWER:   spectrum
POINTS:   1

 

64. The first ionization energy is the amount of energy required to remove one _____________ from a neutral atom.

ANSWER:   electron
POINTS:   1

 

65. Which halogen has the largest ionization energy?

ANSWER:   fluorine
POINTS:   1

 

66. On a given atom, each electron must have a unique set of four _____________.

ANSWER:   quantum numbers
POINTS:   1

 

67. Which halogen has the smallest atomic radius?

ANSWER:   fluorine
POINTS:   1

 

68. The atomic radius _____________ going from left to right across a row of the periodic table.

ANSWER:   decreases
POINTS:   1

 

69. Sketch the 4s, 4px, and 4dxy orbitals on the three axes provided.

ANSWER:   See drawings in the text.
POINTS:   1

 

70. Describe the similarities and the differences between the 1s and 2s atomic orbitals.

ANSWER:   Both orbitals have a similar electron density distribution (are both spherical).

The 2s orbital has a larger radius than the 1s orbital.

The energy of the 2s orbital is greater than the energy of he 1s orbital.
POINTS:   1

 

Match the following:

a. 1s22s22p63s2
b. 4s
c. 3.00 × 108 m/s
d. Co
e. photon
f. 1s22s22p6
g. n = 2
h. 6.626 × 10−34 J·s
i. orbital
j. Cr
k. n = 3
l. K+
m. 6.02 × 1023

 

71. speed of light

ANSWER:   c
POINTS:   1

 

72. isoelectronic with Ca2+

ANSWER:   l
POINTS:   1

 

73. noble gas electron configuration

ANSWER:   f
POINTS:   1

 

74. paramagnetic element

ANSWER:   j
POINTS:   1

 

75. Planck’s constant

ANSWER:   h
POINTS:   1

 

76. quantum level containing 4 orbitals

ANSWER:   g
POINTS:   1

 

77. value of n for which l can only = 0, 1, 2

ANSWER:   k
POINTS:   1

 

78. a spherical orbital

ANSWER:   b
POINTS:   1

 

79. ferromagnetic element

ANSWER:   d
POINTS:   1

 

80. particle of light

ANSWER:   e
POINTS:   1

 

 

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