chem 1411 test 3 review

chem 1411 test 3 review 1. Which form of electromagnetic radiation has the longest wavelengths? A) gamma rays B) microwaves C) radio waves D) infrared radiation E) x-rays 2. Which of the following frequencies corresponds to light with the longest wavelength? A) 3.00 10 13 s 1 B) 4.12 10 5 s 1 C) 8.50 10 20 s 1 D) 9.12 10 12 s 1 E) 3.20 10 9 s 1 3. Which of the following are incorrectly paired? A) wavelength B) frequency C) speed of light c D) hertz s 1 E) x-rays shortest wavelength 4. Which one of the following types of radiation has the shortest wavelength, the greatest energy, and the highest frequency? A) Ultraviolet radiation. B) Infrared radiation. C) Visible red light. D) Visible blue light. E) None, because short wavelength is associated with low energy and low frequency, not high energy and high frequency. 5. Which of the following is incorrect? A) The emission spectrum of hydrogen contains a continuum of colors. B) Diffraction produces both constructive and destructive interference. C) All matter displays both particle and wavelike characteristics. D) Niels Bohr developed a quantum model for the hydrogen atom. E) The lowest possible energy state of a molecule or atom is called its ground state. 6. Which of the following best describes an orbital? A) space where electrons are unlikely to be found in an atom B) space which may contain electrons, protons, and/or neutrons C) the space in an atom where an electron is most likely to be found D) small, walled spheres that contain electrons E) a single space within an atom that contains all electrons of that atom 7. Consider the following representation of a 2p-orbital:

Which of the following statements best describes the movement of electrons in a p-orbital? A) The electrons move along the outer surface of the p-orbital, similar to a figure 8 type of movement. B) The electrons move within the two lobes of the p-orbital, but never beyond the outside surface of the orbital. C) The electrons are concentrated at the center (node) of the two lobes. D) The electrons are only moving in one lobe at any given time. E) The electron movement cannot be exactly determined. 8. Which of the following combinations of quantum numbers is not allowed? A) n = 1, l = 1, ml = 0, ms = B) n = 3, l = 0, ml = 0, ms = - C) n = 2, l = 1, ml = -1, ms = D) n = 4, l = 3, ml = -2, ms = - E) n = 4, l = 2, ml = 0, ms = 9. Which of the following was not an elemental property usually predicted by Mendeleev for as-yet-unknown elements? A) electron configuration B) atomic mass C) density D) boiling point E) oxide formula 10. Which of the following atoms or ions has three unpaired electrons? A) N B) O C) Al D) S 2 E) Ti 2+ 11. The electron configuration for the barium atom is: A) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 B) [Xe]6s 2 C) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 D) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 12. The complete electron configuration of tin is A) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5d 10 5p 2 B) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4d 10 4p 2 C) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 4p 6 5s 2 4d 10 5d 10 5p 2 D) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 2

13. Which of the following statements about quantum theory is incorrect? A) The energy and position of an electron cannot be determined simultaneously. B) Lower energy orbitals are filled with electrons before higher energy orbitals. C) When filling orbitals of equal energy, two electrons will occupy the same orbital before filling a new orbital. D) No two electrons can have the same four quantum numbers. E) All of these are correct. 14. An element with the electron configuration [Xe] 6s 2 4f 14 5d 7 would belong to which class on the periodic table? A) transition elements B) alkaline earth elements C) halogens D) rare earth elements E) none of the above 15. All alkaline earths have the following number of valence electrons: A) 1 B) 3 C) 6 D) 2 16. In which group do all the elements have the same number of valence electrons? A) P, S, Cl B) Ag, Cd, Ar C) Na, Ca, Ba D) P, As, Se 17. Of the following elements, which has occupied d orbitals in its ground-state neutral atoms? A) Ba B) Ca C) Si D) P E) Cl 18. Of the following elements, which needs three electrons to complete its valence shell? A) Ba B) Ca C) Si D) P E) Cl 19. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 2 is the correct electron configuration for which of the following atoms? A) Ca B) Ti C) Ge

D) Zr 20. Which of the following electron configurations is different from that expected? A) Ca B) Sc C) Ti D) V E) Cr 21. Which of the following have 10 electrons in the d orbitals? A) Mn B) Fe C) Cu D) Zn E) two of the above 22. Which of the following exhibits the correct orders for both atomic radius and ionization energy, respectively? (smallest to largest) A) S, O, F, and F, O, S B) F, S, O, and O, S, F C) S, F, O, and S, F, O D) F, O, S, and S, O, F 23. Which of the following concerning second ionization energies is true? A) That of Al is higher than that of Mg because Mg wants to lose the second electron, so it is easier to take the second electron away. B) That of Al is higher than that of Mg because the electrons are taken from the same energy level, but the Al atom has one more proton. C) That of Al is lower than that of Mg because Mg wants to lose the second electron, thus the energy change is greater. D) That of Al is lower than that of Mg because the second electron taken from Al is in a p orbital, thus it is easier to take. E) The second ionization energies are equal for Al and Mg. 24. Consider the ionization energy (IE) of the magnesium atom. Which of the following is not true? A) The IE of Mg is lower than that of sodium. B) The IE of Mg is lower than that of neon. C) The IE of Mg is lower than that of beryllium. D) The IE of Mg is higher than that of calcium. E) The IE of Mg is lower than that of Mg +. 25. Of the following elements, which has the lowest first ionization energy? A) Ba B) Ca C) Si D) P

E) Cl 26. Which of the following atoms has the largest ionization energy? A) O B) Li C) Ne D) Be E) K 27. Which of the following statements is true? A) The first ionization potential of H is greater than that of He. B) The ionic radius of Fe + is larger than that of Fe 3+. C) The ionization energy of S 2 is greater than that of Cl. D) The atomic radius of Li is larger than that of Cs. E) All are false. 28. Which of the following statements is false? A) A sodium atom has a smaller radius than a potassium atom. B) A neon atom has a smaller radius than an oxygen atom. C) A fluorine atom has a smaller first ionization energy than an oxygen atom. D) A cesium atom has a smaller first ionization energy than a lithium atom. E) All are true. 29. Which of the following statements is true about the ionization energy of Mg +? A) It will be equal to the ionization energy of Li. B) It will be equal to and opposite in sign to the electron affinity of Mg. C) It will be equal to and opposite in sign to the electron affinity of Mg +. D) It will be equal to and opposite in sign to the electron affinity of Mg 2+. E) None of the above. 30. In the quantum theory, the angular orbital momentum quantum number is most directly associated with which property of orbitals? A) energy C) orientation B) size D) shape 31. The ground state electron configuration for Te is: A) [Kr]5s 2 4d 10 5p 4 B) [Kr]5s 2 5p 6 4d 8 C) [Kr]5s 2 5d 10 5p 4 D) [Kr]5s 2 4f 14 E) Kr]5s 2 5d 10 5p 6 32. Select the correct electron configuration for Cu. A) [Ar]4s 2 3d 9 B) [Ar]4s 1 3d 10 C) [Ar]4s 2 4p 6 3d 3 D) [Ar]4s 2 4d 9 E) [Ar]3d 10

33. The force between two bodies having identical electric charges A) is a force of repulsion B) is a force of repulsion if the charges are negative, and one of attraction if they are positive C) increases as the bodies are moved further apart D) is independent of the distance between them E) is directly proportional to the distance between them 34. Which of the following groups contains no ionic compounds? A) HCN, NO2, Ca(NO3)2 B) PCl5, LiBr, Zn(OH)2 C) KOH, CCl4, SF4 D) NaH, CaF2, NaNH2 E) CH2O, H2S, NH3 35. In which pair do both compounds exhibit predominantly ionic bonding? A) SCl6 and HF B) Na2SO3 and NH3 C) KI and O3 D) LiF and H2O E) LiBr and MgO 36. In which case is the bond polarity incorrect? A) + H F B) + K O C) + Mg H D) + Cl I E) + Si S 37. The electron pair in a C-F bond could be considered A) closer to C because carbon has a larger radius and thus exerts greater control over the shared electron pair B) closer to F because fluorine has a higher electronegativity than carbon C) closer to C because carbon has a lower electronegativity than fluorine D) an inadequate model since the bond is ionic E) centrally located directly between the C and F 38. Based on electronegativity differences, which of the following is most likely to be ionic? A) CaF2 B) Br2 C) BH3 D) NO E) CF4 39. In which of the following compounds does the bond between the central atom and bromine have the greatest ionic character? A) LiBr B) KBr

C) SeBr2 D) AsBr3 E) CaBr2 40. Which of the following statements is incorrect? A) Ionic bonding results from the transfer of electrons from one atom to another. B) Dipole moments result from the unequal distribution of electrons in a molecule. C) The electrons in a polar bond are found nearer to the more electronegative element. D) A molecule with very polar bonds can be nonpolar. E) Linear molecules cannot have a net dipole moment. 41. Which of these is an isoelectronic series? A) Na +, K +, Rb +, Cs + B) K +, Ca 2+, Ar, S 2 C) Na +, Mg 2+, S 2, Cl D) Li, Be, B, C (A-D) 42. Which of the following has the smallest radius? A) F B) Ne C) O 2 D) Mg 2+ E) Na + 43. Which of the following species would be expected to have the lowest ionization energy? A) F B) Ne C) O 2 D) Mg 2+ E) Na + 44. Which of the following ionic compounds has the smallest lattice energy (i.e., the lattice energy least favorable to a stable lattice)? A) LiF B) CsI C) NaCl D) BaO E) MgO 45. Which of the following statements are true concerning ionic bonding? A) Ionic bonding occurs between a metal, which has a high affinity for electrons, and a nonmetal, which loses electrons relatively easy. B) CaCl2 forms because Ca 2+ is always a more stable species than the calcium atom alone. C) Compounds with ionic bonds tend to have low melting points. D) The electronegativity difference between the bonding atoms of ionic compounds is small since the electrons are not shared but rather held together by electrostatic

forces. E) All of the above statements are false. 46. Which of the following statements concerning lattice energy is false? A) It is often defined as the energy released when an ionic solid forms from its ions. B) MgO has a larger lattice energy than NaF. C) The lattice energy for a solid with 2+ and 2 ions should be two times that for a solid with 1+ and 1 ions. D) MgO has a larger lattice energy than LiF. E) All of these are true. 47. Which of the following statements is false? A) Models are human interpretations, not the same as reality. B) Models are often wrong. C) Models usually start out simple and become more complex over time. D) We often learn more when a model is wrong than when it is right. E) A model should be discarded when any exception to it is found. 48. Which of the following molecules exhibits the greatest bond energy? A) F2 B) Cl2 C) Br2 D) I2 E) all the same 49. As the number of bonds between two carbon atoms increases, which one of the following decreases? A) number of electrons between the carbon atoms B) bond energy C) bond length D) all of these 50. Which of the following molecules contains a double bond? A) CO2 B) NH3 C) H2O D) all E) none 51. Which of the following compounds contains only one unshared pair of valence electrons? A) NH3 B) H2O C) CH4 D) NaCl E) BF3 52. Which of the following atoms cannot exceed the octet rule in a molecule? A) N

B) S C) P D) I E) All of the atoms (A-D) can exceed the octet rule. 53. Choose the electron dot formula that most accurately describes the bonding in CS2. (Hint: Consider formal charges.) A) B) C) D) E) 54. Which of the following molecules (or ions) has a dipole moment? A) CO2 B) CO3 2 C) NH4 + D) PF3 E) two of them 55. Choose the statement that best describes the PbCl4 molecule in the gas phase. A) The bond angles are all about 109. B) The molecule is polar. C) The molecule has a dipole moment. D) The bonds are nonpolar. E) More than one of the above. 56. Which of the following has a zero dipole moment? A) NH3 B) NO2 C) PF5 D) SO2 E) HCN 57. Of the following, which molecule has the largest bond angle? A) O3 B) OF2 C) HCN D) H2O E) More than one of the above have equally large bond angles. 58. Which of the following molecules is non-polar overall? A) SF4 B) SF2 C) CCl4 D) H2S

E) OCl2 59. Which of the following molecules has a nonlinear structure? A) XeF2 B) BeCl2 C) O3 D) CO2 E) N2O (central atom is N) 60. Which of the following species has a trigonal bipyramid structure? A) NH3 B) IF5 C) I3 D) PCl5 Select the correct molecular structure for the given species from the choices below: 61. PCl4 + A) pyramidal B) tetrahedral C) square planar D) octahedral 62. XeF6 A) pyramidal B) tetrahedral C) square planar D) octahedral 63. NI3 A) pyramidal B) tetrahedral C) square planar D) octahedral 64. IF4 A) pyramidal B) tetrahedral C) square planar D) octahedral Select the correct molecular structure for the given species from the choices below:

65. NO3 A) linear B) trigonal planar C) tetrahedral D) bent 66. According to VSEPR theory, which of the following species has a square planar molecular structure? A) TeBr4 B) BrF3 C) IF5 D) XeF4 E) SCl2 67. The hybridization of the central atom in XeF5 + is: A) sp B) sp 2 C) sp 3 D) dsp 3 E) d 2 sp 3 68. The hybridization of the central atom in ClF2 + is: A) sp B) sp 2 C) sp 3 D) dsp 3 E) d 2 sp 3 69. Which of the following molecules contains a central atom with sp 2 hybridization? A) B) C) D) E)

70. The hybridization of the central atom, Al, in AlBr3 is A) sp B) sp 2 C) sp 3 D) dsp 3 E) d 2 sp 3 71. The hybridization of the central atom in NO3 is A) p 3 B) sp 2 C) sp 3 D) sp E) dsp 2 72. Consider the molecule C2H4. The hybridization of each C atom is A) sp B) sp 2 C) sp 3 D) dsp 3 E) d 2 sp 3 73. A (pi) bond is the result of the A) overlap of two s orbitals B) overlap of an s orbital and a p orbital C) overlap of two p orbitals along their axes D) sidewise overlap of two parallel p orbitals E) sidewise overlap of two s orbitals 74. When a carbon atom has sp 3 hybridization, it has A) four bonds B) three bonds and one bond C) two bonds and two bonds D) one bond and three bonds E) four bonds 75. For which of the following diatomic molecules would the bond order become greater if an electron is removed (i.e., if the molecule is converted to the positive ion in its ground state)? A) B2 B) C2 C) P2 D) F2 E) Na2 76. The fact that O2 is paramagnetic can be explained by A) the Lewis structure of O2 B) resonance C) a violation of the octet rule

D) the molecular orbital diagram for O2 E) hybridization of atomic orbitals in O2 77. Which of the following has the shortest bond length? A) O2 2 B) O2 C) O2 D) O2 + E) Two of these have the shortest bond length. 78. Which of the following has a bond order of 1.5? A) O2 + B) N2 C) O2 D) C2 79. Which of the nitrogen-containing molecules below is paramagnetic in its lowest energy state? A) N2 B) NO C) NH3 D) N2H4 80. Which of the following electron distributions among the molecular orbitals best describes the NO molecule? 2s 2s * 2py= 2px 2pz 2py * = 2px * 2pz * A) 2 2 4 2 4 2 B) 2 2 4 2 4 1 C) 2 2 4 1 3 0 D) 2 2 4 2 2 0 E) 2 2 4 2 1 0 81. Which of these statements about benzene is true? A) All carbon atoms in benzene are sp 3 hybridized. B) Benzene contains only bonds between C atoms. C) The bond order of each C C bond in benzene is 1.5. D) Benzene is an example of a molecule that displays ionic bonding. E) All of these statements are false. 82. Which of the following would you expect to have the highest boiling point? A) F2 B) Cl2 C) Br2 D) I2 E) All of the above have the same boiling point. 83. Which substance involves no bonding forces except London dispersion forces?

A) NaCl(l) B) HF(l) C) N2(s) D) H2O(l) E) K(s) 84. When a water molecule forms a hydrogen bond with another water molecule, which atoms are involved in the interaction? A) a hydrogen from one molecule and a hydrogen from the other molecule B) a hydrogen from one molecule and an oxygen from the other molecule C) an oxygen from one molecule and an oxygen from the other molecule D) an oxygen and a hydrogen from the same molecule E) two hydrogens from one molecule and one hydrogen from the other molecule 85. Which of the following compounds has the lowest viscosity? A) CCl4(l) B) N2(g) C) H2O(l) D) CH3-(CH2)25-CH3(l) E) HCl(g) 86. Which of the following statements about liquids is true? A) Droplet formation occurs because of the higher stability associated with increased surface area. B) Substances that can form hydrogen bonds will display lower melting points than predicted from periodic trends. C) London dispersion forces arise from a distortion of the electron clouds within a molecule or atom. D) Liquid rise within a capillary tube because of the small size lowers the effective atmospheric pressure over the surface of the liquid. E) The boiling point of a solution is dependent solely on the atmospheric pressure over the solution. 87. Which of the following is paired incorrectly? A) crystalline solids highly regular arrangement of their components B) amorphous solids considerable disorder in their structures C) unit cell the smallest repeating unit of the lattice D) gold metal simple cubic unit cell E) glass amorphous solid 88. Which of the following statements about steel is false? A) It contains carbon atoms in the holes of its iron crystals. B) The presence of carbon-iron bonds in the alloy make steel harder and stronger than pure iron. C) Pure iron is relatively soft and ductile because it lacks directional bonding. D) The amount of carbon directly affects the properties of steel. E) All of these are true.

89. Which of the following statements is true about p-type silicon? A) It is produced by doping Si with P or As. B) Protons are the mobile charge carriers. C) It does not conduct electricity as well as pure Si. D) All are true. E) None is true. 90. Which of the compounds below is an example of a network solid? A) S8(s) B) SiO2(s) C) MgO(s) D) NaCl(s) E) C25H52(s) 91. Which of these statements is incorrect? A) Molecular solids have high melting points. B) The binding forces in a molecular solid include London dispersion forces. C) Ionic solids have high melting points. D) Ionic solids are insulators. E) All of the statements (A-D) are correct. 92. Which of the following has the highest melting temperature? A) H2O B) CO2 C) S8 D) MgF2 E) P4 93. Which of the following is most likely to be a solid at room temperature? A) Na2S B) HF C) NH3 D) N2 E) H2O 94. On the basis of your knowledge of bonding in liquids and solids, which of the following has the lowest melting temperature? A) NaCl B) Na C) Cl2 D) SiO2 E) More information is needed. 95. The process of condensation happens when which of the following occurs? A) A solid becomes a liquid. B) A liquid becomes a solid. C) A gas becomes a liquid. D) A liquid becomes a gas.

E) A gas becomes a solid. 96. Which of the following processes must exist in equilibrium with the evaporation process when a measurement of vapor pressure is made? A) fusion B) vaporization C) sublimation D) boiling E) condensation 97. Which statement regarding water is true? A) Energy must be given off in order to break down the crystal lattice of ice to a liquid. B) Hydrogen bonds are stronger than covalent bonds. C) Liquid water is less dense than solid water. D) Only covalent bonds are broken when ice melts. E) All of the statements (A D) are false. 98. Choose the correct statement about the diagram below. A) The diagram is qualitatively correct for water. B) The diagram shows that the melting point of the solid increases with increasing pressure. C) The diagram shows the triple point above 1 atm pressure. D) The diagram could represent the phase diagram of CO2. E) None of the above statements is correct. 99. Which of the following compounds is expected to have the HIGHEST melting point? A) CH3OCH3 B) CH3CH2OH C) CH3CH2CH2CH3 D) CH3CH2CH3 E) CH3Cl 100. The measure of resistance to flow of a liquid is A) van der Waals forces B) vapor pressure C) London forces D) surface tension E) viscosity

chem 1411 test 3 review Answer Section 1. ANS: C PTS: 1 DIF: Easy REF: 7.1 KEY: Chemistry general chemistry atomic theory light electromagnetic radiation 2. ANS: B PTS: 1 DIF: Easy REF: 7.1 KEY: Chemistry general chemistry atomic theory light electromagnetic radiation 3. ANS: E PTS: 1 DIF: Easy REF: 7.1 KEY: Chemistry general chemistry atomic theory light electromagnetic radiation 4. ANS: A PTS: 1 DIF: Easy REF: 7.2 KEY: Chemistry general chemistry atomic theory light electromagnetic radiation 5. ANS: A PTS: 1 DIF: Easy REF: 7.4 KEY: Chemistry general chemistry atomic theory 6. ANS: C PTS: 1 DIF: Easy REF: 7.5 KEY: Chemistry general chemistry atomic theory quantum mechanics 7. ANS: E PTS: 1 DIF: Moderate REF: 7.7 KEY: Chemistry general chemistry atomic theory quantum mechanics wave functions Heisenberg's uncertainty principle 8. ANS: A PTS: 1 DIF: Easy REF: 7.8 KEY: Chemistry general chemistry atomic theory quantum mechanics quantum numbers 9. ANS: A PTS: 1 DIF: Moderate REF: 7.1 KEY: Chemistry general chemistry atomic theory periodicity of the elements Mendeleev's predictions 10. ANS: A PTS: 1 DIF: Moderate REF: 7.11 configuration aufbau principle 11. ANS: B PTS: 1 DIF: Easy REF: 7.11 configuration aufbau principle 12. ANS: D PTS: 1 DIF: Easy REF: 7.11 configuration aufbau principle 13. ANS: C PTS: 1 DIF: Easy REF: 7.11 KEY: Chemistry general chemistry atomic theory 14. ANS: A PTS: 1 DIF: Easy REF: 7.11 configuration and the periodic table 15. ANS: D PTS: 1 DIF: Easy REF: 7.11

configuration and the periodic table 16. ANS: E PTS: 1 DIF: Easy REF: 7.11 configuration 17. ANS: A PTS: 1 DIF: Easy REF: 7.11 configuration and the periodic table 18. ANS: D PTS: 1 DIF: Easy REF: 7.11 configuration and the periodic table 19. ANS: B PTS: 1 DIF: Easy REF: 7.11 configuration 20. ANS: E PTS: 1 DIF: Easy REF: 7.11 configuration and the periodic table exceptions to the aufbau principle 21. ANS: E PTS: 1 DIF: Moderate REF: 7.11 configuration and the periodic table 22. ANS: D PTS: 1 DIF: Moderate REF: 7.12 KEY: Chemistry general chemistry atomic theory periodicity of the elements periodic properties 23. ANS: B PTS: 1 DIF: Moderate REF: 7.12 KEY: Chemistry general chemistry atomic theory periodicity of the elements periodic properties ionization energy 24. ANS: A PTS: 1 DIF: Easy REF: 7.12 KEY: Chemistry general chemistry atomic theory periodicity of the elements periodic properties ionization energy 25. ANS: A PTS: 1 DIF: Easy REF: 7.12 KEY: Chemistry general chemistry atomic theory periodicity of the elements periodic properties ionization energy 26. ANS: C PTS: 1 DIF: Easy REF: 7.12 KEY: Chemistry general chemistry atomic theory periodicity of the elements periodic properties ionization energy 27. ANS: B PTS: 1 DIF: Moderate REF: 7.12 KEY: Chemistry general chemistry atomic theory periodicity of the elements periodic properties 28. ANS: C PTS: 1 DIF: Easy REF: 7.12 KEY: Chemistry general chemistry atomic theory periodicity of the elements periodic properties atomic radius 29. ANS: D PTS: 1 DIF: Moderate REF: 7.12 KEY: Chemistry general chemistry atomic theory periodicity of the elements periodic properties 30. ANS: D PTS: 1 DIF: Easy REF: 7.6

KEY: Chemistry general chemistry atomic theory quantum mechanics quantum numbers angular quantum number 31. ANS: A PTS: 1 DIF: Easy REF: 7.11 configuration aufbau principle 32. ANS: B PTS: 1 DIF: Easy REF: 7.11 configuration and the periodic table exceptions to the aufbau principle 33. ANS: A PTS: 1 DIF: Easy REF: 8.1 KEY: Chemistry general chemistry bonding 34. ANS: E PTS: 1 DIF: Easy REF: 8.1 KEY: Chemistry general chemistry bonding ionic bonding 35. ANS: E PTS: 1 DIF: Easy REF: 8.1 KEY: Chemistry general chemistry bonding ionic bonding 36. ANS: D PTS: 1 DIF: Easy REF: 8.2 KEY: Chemistry general chemistry bonding covalent bonding electronegativity 37. ANS: B PTS: 1 DIF: Easy REF: 8.2 KEY: Chemistry general chemistry bonding covalent bonding electronegativity 38. ANS: A PTS: 1 DIF: Easy REF: 8.2 KEY: Chemistry general chemistry bonding covalent bonding electronegativity 39. ANS: B PTS: 1 DIF: Moderate REF: 8.2 KEY: Chemistry general chemistry bonding covalent bonding electronegativity 40. ANS: E PTS: 1 DIF: Easy REF: 8.3 KEY: Chemistry general chemistry bonding molecular geometry dipole moment 41. ANS: B PTS: 1 DIF: Easy REF: 8.4 KEY: Chemistry general chemistry bonding ionic bonding 42. ANS: D PTS: 1 DIF: Easy REF: 8.4 KEY: Chemistry general chemistry bonding ionic bonding ionic radii 43. ANS: C PTS: 1 DIF: Easy REF: 8.5 KEY: Chemistry general chemistry bonding ionic bonding Born-Haber cycle 44. ANS: B PTS: 1 DIF: Moderate REF: 8.5 KEY: Chemistry general chemistry bonding ionic bonding Born-Haber cycle 45. ANS: E PTS: 1 DIF: Moderate REF: 8.5 KEY: Chemistry general chemistry bonding ionic bonding 46. ANS: C PTS: 1 DIF: Easy REF: 8.5 KEY: Chemistry general chemistry bonding ionic bonding Born-Haber cycle

47. ANS: E PTS: 1 DIF: Easy REF: 8.7 KEY: Chemistry general chemistry bonding 48. ANS: B PTS: 1 DIF: Easy REF: 8.8 KEY: Chemistry general chemistry bonding covalent bonding bond energy 49. ANS: C PTS: 1 DIF: Easy REF: 8.8 KEY: Chemistry general chemistry bonding covalent bonding 50. ANS: A PTS: 1 DIF: Easy REF: 8.1 KEY: Chemistry general chemistry bonding covalent bonding multiple bonds 51. ANS: A PTS: 1 DIF: Easy REF: 8.1 KEY: Chemistry general chemistry bonding covalent bonding Lewis dot formula 52. ANS: A PTS: 1 DIF: Easy REF: 8.11 KEY: Chemistry general chemistry bonding covalent bonding exceptions to the octet rule 53. ANS: A PTS: 1 DIF: Easy REF: 8.12 KEY: Chemistry general chemistry bonding covalent bonding formal charge 54. ANS: D PTS: 1 DIF: Moderate REF: 8.13 KEY: Chemistry general chemistry bonding molecular geometry dipole moment 55. ANS: A PTS: 1 DIF: Moderate REF: 8.13 KEY: Chemistry general chemistry bonding molecular geometry 56. ANS: C PTS: 1 DIF: Moderate REF: 8.13 KEY: Chemistry general chemistry bonding molecular geometry dipole moment 57. ANS: C PTS: 1 DIF: Moderate REF: 8.13 KEY: Chemistry general chemistry bonding molecular geometry bond angle 58. ANS: C PTS: 1 DIF: Moderate REF: 8.13 KEY: Chemistry general chemistry bonding molecular geometry dipole moment 59. ANS: C PTS: 1 DIF: Moderate REF: 8.13 KEY: Chemistry general chemistry bonding molecular geometry the valence-shell electron-pair repulsion model 60. ANS: D PTS: 1 DIF: Moderate REF: 8.13 KEY: Chemistry general chemistry bonding molecular geometry the valence-shell electron-pair repulsion model trigonal bipyramidal arrangement 61. ANS: B PTS: 1 DIF: Moderate REF: 8.13 KEY: Chemistry general chemistry bonding molecular geometry the valence-shell electron-pair repulsion model

62. ANS: E PTS: 1 DIF: Moderate REF: 8.13 KEY: Chemistry general chemistry bonding molecular geometry the valence-shell electron-pair repulsion model 63. ANS: A PTS: 1 DIF: Moderate REF: 8.13 KEY: Chemistry general chemistry bonding molecular geometry the valence-shell electron-pair repulsion model 64. ANS: C PTS: 1 DIF: Moderate REF: 8.13 KEY: Chemistry general chemistry bonding molecular geometry the valence-shell electron-pair repulsion model 65. ANS: B PTS: 1 DIF: Moderate REF: 8.13 KEY: Chemistry general chemistry bonding molecular geometry the valence-shell electron-pair repulsion model 66. ANS: D PTS: 1 DIF: Moderate REF: 8.13 KEY: Chemistry general chemistry bonding molecular geometry the valence-shell electron-pair repulsion model 67. ANS: E PTS: 1 DIF: Moderate REF: 9.1 KEY: Chemistry general chemistry bonding bonding theories hybridization 68. ANS: C PTS: 1 DIF: Moderate REF: 9.1 KEY: Chemistry general chemistry bonding bonding theories hybridization 69. ANS: B PTS: 1 DIF: Easy REF: 9.1 KEY: Chemistry general chemistry bonding bonding theories hybridization 70. ANS: B PTS: 1 DIF: Easy REF: 9.1 KEY: Chemistry general chemistry bonding bonding theories hybridization 71. ANS: B PTS: 1 DIF: Moderate REF: 9.1 KEY: Chemistry general chemistry bonding bonding theories hybridization 72. ANS: B PTS: 1 DIF: Moderate REF: 9.1 KEY: Chemistry general chemistry bonding bonding theories hybridization 73. ANS: D PTS: 1 DIF: Easy REF: 9.1 KEY: Chemistry general chemistry bonding bonding theories multiple bonding 74. ANS: E PTS: 1 DIF: Easy REF: 9.1 KEY: Chemistry general chemistry bonding bonding theories hybridization 75. ANS: D PTS: 1 DIF: Moderate REF: 9.3 KEY: Chemistry general chemistry bonding bonding theories diatomic molecule 76. ANS: D PTS: 1 DIF: Easy REF: 9.3 KEY: Chemistry general chemistry bonding bonding theories diatomic molecule

77. ANS: D PTS: 1 DIF: Moderate REF: 9.3 KEY: Chemistry general chemistry bonding bonding theories diatomic molecule 78. ANS: C PTS: 1 DIF: Moderate REF: 9.3 KEY: Chemistry general chemistry bonding bonding theories molecular orbital theory bond order 79. ANS: B PTS: 1 DIF: Moderate REF: 9.4 KEY: Chemistry general chemistry bonding bonding theories diatomic molecule 80. ANS: E PTS: 1 DIF: Moderate REF: 9.4 KEY: Chemistry general chemistry bonding bonding theories molecular orbital theory 81. ANS: C PTS: 1 DIF: Moderate REF: 9.5 KEY: Chemistry general chemistry bonding bonding theories 82. ANS: D PTS: 1 DIF: Easy REF: 10.1 KEY: Chemistry general chemistry phases liquid intermolecular forces 83. ANS: C PTS: 1 DIF: Easy REF: 10.1 KEY: Chemistry general chemistry phases intermolecular forces London forces 84. ANS: B PTS: 1 DIF: Easy REF: 10.1 KEY: Chemistry general chemistry phases intermolecular forces hydrogen bonding 85. ANS: B PTS: 1 DIF: Easy REF: 10.2 KEY: Chemistry general chemistry phases liquid properties of liquids viscosity 86. ANS: C PTS: 1 DIF: Easy REF: 10.2 KEY: Chemistry general chemistry phases liquid properties of liquids 87. ANS: D PTS: 1 DIF: Easy REF: 10.3 KEY: Chemistry general chemistry phases solid classification of solids 88. ANS: E PTS: 1 DIF: Easy REF: 10.4 KEY: Chemistry general chemistry materials chemistry metal 89. ANS: E PTS: 1 DIF: Easy REF: 10.5 KEY: Chemistry general chemistry materials chemistry metal semiconductor 90. ANS: B PTS: 1 DIF: Easy REF: 10.5 KEY: Chemistry general chemistry phases solid structures of crystalline solids covalent network solid 91. ANS: A PTS: 1 DIF: Easy REF: 10.7 KEY: Chemistry general chemistry phases solid classification of solids

92. ANS: D PTS: 1 DIF: Easy REF: 10.7 KEY: Chemistry general chemistry phases solid properties of solids melting point 93. ANS: A PTS: 1 DIF: Easy REF: 10.7 KEY: Chemistry general chemistry phases solid classification of solids 94. ANS: C PTS: 1 DIF: Moderate REF: 10.7 KEY: Chemistry general chemistry phases solid classification of solids 95. ANS: C PTS: 1 DIF: Easy REF: 10.8 KEY: Chemistry general chemistry phases phase transitions 96. ANS: E PTS: 1 DIF: Easy REF: 10.8 KEY: Chemistry general chemistry phases phase transitions vapor pressure 97. ANS: E PTS: 1 DIF: Easy REF: 10.9 KEY: Chemistry general chemistry phases phase transitions 98. ANS: B PTS: 1 DIF: Easy REF: 10.9 KEY: Chemistry general chemistry phases phase transitions phase diagram 99. ANS: B PTS: 1 DIF: Moderate REF: 10.1 KEY: Chemistry general chemistry phases intermolecular forces hydrogen bonds 100. ANS: E PTS: 1 DIF: Easy REF: 10.2 KEY: Chemistry general chemistry phases liquid properties of liquids