Modified True/False s1

Unit 2 Review

Modified True/False Indicate whether the sentence or statement is true or false. If false, change the identified word or phrase to make the sentence or statement true.

____ 1. Bohr's atomic theory states that electrons may only possess specific amounts of energy. ______2. The quantum mechanical model of the atom is capable of determining the exact location of an electron in an atom. ______3. All alkali earth metals have valence electrons in s orbitals when they are in their ground state. ______4. The hydrogen atom will produce a complete spectrum when it is energized. ______5. Schrodinger's equation describes the electron as a wave. ______6. Transition metals are monovalent because they attempt to get more stable electron configurations like half- filled and empty orbitals. ______7. The 2p orbitals in oxygen have three unpaired electrons. ______

____ 8. The shape of SO2 is trigonal planar. ______9. Absorption spectra are the result of energy that has been absorbed by electrons. ______10. Electrons are most likely found near the nucleus, regardless of the type of orbital they 'occupy'. ______11. The Pauli exclusion principle requires that two electrons in the same orbital have the same spin. ______12. Quantum mechanics involves using probabilities to determine the shape of an atom. ______13. The electron configuration for sulfur, S is shown below. ______  3p 3s   2p 2s  1s ____ 14. The valence p orbitals in phosphorus, P, are half-filled. ______15. All of the valence electrons in Fe2+ must have the same spin. ______16. Hund's rule states that you must fill electrons into the lowest energy levels first. ______17. A laser produces monochromatic light. ______18. Spectrophotometers cannot be used for qualitative observations. ______19. X-rays are made up of extremely high energy photons. ______20. MRI stands for magnetic reflection imaging. ______21. A photon of light is equal to one quantum of energy. ______22. Superconductors are substances that conduct electricity with extremely low voltage. ______23. The energy of electrons is quantized as photons. ______24. Ionic compounds have higher melting points than molecular compounds because of strong attractive forces between particles. ______

____ 25. The shape of boron trifluoride, BF3, is tetrahedral. ______26. VSEPR theory predicts molecular shapes based on keeping protons as far apart as possible. ______

____ 27. Carbon tetrafluoride, CF4, contains four polar bonds and is a polar molecule. ______28. The surface tension of water is due to the hydrogen bonding between water molecules. ______29. A molecule whose central atom is surrounded by two lone pairs and four atoms will have a square planar shape. ______

____ 30. CH3Cl is a polar molecule. ______31. An ionic compound would be expected to have a low melting point. ______32. Diamond does not conduct electricity because it contains delocalized electrons. ______33. Molten or dissolved ionic compounds conduct electricity because they contain delocalized electrons. ______

o ____ 34. Sulfur dioxide, SO2, is a bent molecule with a bond angle that is slightly less than 109 . ______

____ 35. Xenon tetrafluoride, XeF4, is a tetrahedral molecule. ______

____ 36. Methane, CH4, contains polar bonds. ______

____ 37. Carbon dioxide, CO2, is a polar molecule. ______38. Water is adhesive because it is bi-polar. ______39. Hydrogen bonding may explain why ice is less dense than liquid water. ______40. Dr. Richard Bader uses computers to create electron density maps for large complex molecules. ______41. Dr. Robert LeRoy developed a technique for determining bond lengths. ______42. Dr. Robert LeRoy is interested in intermolecular forces. ______43. A dipole occurs when two atoms with similar electronegativities bond to each other. ______

Completion Complete each sentence or statement. 44. A region in which there is a high probability of finding an electron is called an ______. 45. Bohr's model works perfectly for ______. 46. ______determined that it is impossible to predict the exact location of an electron. 47. ______orbitals are non-directional. 48. There are ______different orientations in space for p-orbitals. 49. When an electron is in its lowest energy level, it is in the ______. 50. In his model of the atom, Bohr identified each energy level using an integer, n, and called it the ______. 51. Cl1-, Ar and Ca2+ are ______. 52. ______are high energy electromagnetic radiation. 53. ______produce parallel, monochromatic light. 54. Spin changes in hydrogen nuclei of water molecules can be detected using ______. 55. At extremely low temperatures, helium is a ______. 56. S-block elements are all ______. 57. A photon is a ______of light. 58. The electron configuration for ______is 1s22s22p63s23p6. 59. The oxide, O2-, is ______with neon, Ne. 60. The "1" in helium's (He) electron configuration represents the ______. 61. The concept of the duality of matter means that an electron is both a particle and a ______. 62. The surface tension of water is due to the ______between its particles. 63. ______of electrons take up more room than bonded pairs. 64. The shape of sulfur dioxide would most likely be ______.

65. The shape of MnI5 would most likely be ______. 66. The metal ions in a metallic solid are surrounded by delocalized electrons because metals have low ______.

67. The shape of sulphur hexachloride, SCl6, is ______.

68. The shape of methane, CH4, is ______.

69. The shape of ammonia, NH3, is ______.

70. The shape of xenon tetrafluoride, XeF4, is ______.

71. The shape of beryllium fluoride, BeF2, is ______.

72. The shape of boron trihydride, BH3, is ______.

73. The shape of hydrogen sulfide, H2S, is ______. 74. The shape of phosphorus pentahydride, PH5, is ______. 75. VSEPR theory predicts the ______of molecules. 76. The molecules in any glue must have the ability to ______with molecules of other substances. 77. ______tend to be brittle. 78. Due to its structure, diamond is classified as a ______. 79. The electrostatic forces between ions in ionic compounds cause ______boiling points. 80. Insects can walk on water because of ______. 81. Dispersion forces are ______than covalent bonds. 82. Adhesive properties of glues can be explained by examining ______forces. 83. The large difference in electronegativities between hydrogen and chlorine produces a ______in the hydrogen chloride molecule.

84. Ernest Rutherford is known as the father of nuclear chemistry. Describe his Gold Foil experiment and then explain how he used this experimental evidence to hypothesize about the existence of a nucleus. 85. Compare and contrast the Bohr-Rutherford model of the atom with the quantum mechanical model. 86. Explain, in your own words, how Bohr developed his model of the atom. 87. Explain water's properties using what you know about its inter- and intramolecular forces. 88. Explain VSEPR theory in your own words. Use examples. 89. We are able to "see" the shapes of molecules with X-ray crystallography. However, even without this

technology, there is a great deal of evidence that water, H2O, is a bent, polar molecule. Discuss this evidence and explain how it relates to our model of the water molecule. 90. Explain, in your own words, how to determine the polarity of a substance. Use examples if you wish. 91. Describe, in your own words, two allotropes of carbon. Include a comparison of physical and chemical properties. 92. Describe some contributions that Canadians have made to the scientific community's understanding of the structures and properties of chemicals. Unit 2 Review Answer Section

MODIFIED TRUE/FALSE

1. ANS: T REF: K/U OBJ: 3.4 LOC: SP1.01 2. ANS: F, probable REF: K/U OBJ: 3.7 LOC: SP1.02 3. ANS: T REF: K/U OBJ: 3.6 LOC: SP1.03 4. ANS: F, line REF: K/U OBJ: 3.4 LOC: SP1.01 5. ANS: T REF: K/U OBJ: 3.7 LOC: SP1.02 6. ANS: F, multi-valent REF: K/U OBJ: 3.6 LOC: SP1.03 7. ANS: F, two REF: I OBJ: 3.5 LOC: SP1.02 8. ANS: F bent angular

REF: I OBJ: 4.3 LOC: SP2.03 9. ANS: T REF: K/U OBJ: 3.4 LOC: SP1.01 10. ANS: T REF: K/U OBJ: 3.5 LOC: SP1.02 11. ANS: F, different spins REF: K/U OBJ: 3.6 LOC: SP2.01 12. ANS: F an orbital orbitals

REF: K/U OBJ: 3.7 LOC: SP2.01 13. ANS: F, chlorine, Cl REF: I OBJ: 3.6 LOC: SP2.02 14. ANS: T REF: I OBJ: 3.6 LOC: SP2.02 15. ANS: F can might

REF: I OBJ: 3.6 LOC: SP2.02 16. ANS: F, Auf bau principle REF: K/U OBJ: 3.6 LOC: SP2.02 17. ANS: T REF: MC OBJ: 3.8 LOC: SP3.01 18. ANS: F, can REF: MC OBJ: 3.8 LOC: SP3.01 19. ANS: T REF: MC OBJ: 3.8 LOC: SP3.01 20. ANS: F, magnetic resonance imaging REF: MC OBJ: 3.8 LOC: SP3.01 21. ANS: T REF: K/U OBJ: 3.3 LOC: SP1.01 22. ANS: F, resistance REF: MC OBJ: 3.7 LOC: SP3.02 23. ANS: T REF: K/U OBJ: 3.3 LOC: SP1.01 24. ANS: T REF: K/U OBJ: 4.6 LOC: SP2.05 25. ANS: F, trigonal planar REF: I OBJ: 4.3 LOC: SP2.03 26. ANS: F, electron pairs REF: K/U OBJ: 4.3 LOC: SP1.05 27. ANS: F, non polar REF: I OBJ: 4.4 LOC: SP2.04 28. ANS: T REF: K/U OBJ: 4.5 LOC: SP1.04 29. ANS: T REF: K/U OBJ: 4.3 LOC: SP1.03 30. ANS: T REF: I OBJ: 4.4 LOC: SP2.04 31. ANS: F, high REF: I OBJ: 4.6 LOC: SP2.05 32. ANS: F, no delocalized electrons REF: K/U OBJ: 4.6 LOC: SP1.04 33. ANS: F, [mobile] ions REF: K/U OBJ: 4.6 LOC: SP1.04 34. ANS: F, 120o REF: I OBJ: 4.3 LOC: SP2.03 35. ANS: F, square planar REF: I OBJ: 4.3 LOC: SP2.03 36. ANS: T REF: I OBJ: 4.4 LOC: SP2.04 37. ANS: F, non polar REF: I OBJ: 4.4 LOC: SP2.04 38. ANS: F, polar REF: K/U OBJ: 4.5 LOC: SP1.04 39. ANS: T REF: K/U OBJ: 4.5 LOC: SP1.04 40. ANS: F, small simple molecules REF: MC OBJ: 4.3 LOC: SP3.03 41. ANS: F, small molecule radii REF: MC OBJ: 4.5 LOC: SP3.03 42. ANS: T REF: MC OBJ: 4.5 LOC: SP3.03 43. ANS: F, very different REF: I OBJ: 4.4 LOC: SP2.01

COMPLETION

44. ANS: orbital REF: C OBJ: 3.5 LOC: SP2.01 45. ANS: hydrogen REF: K/U OBJ: 3.4 LOC: SP1.01 46. ANS: Heisenberg REF: K/U OBJ: 3.7 LOC: SP1.02 47. ANS: S REF: K/U OBJ: 3.6 LOC: SP1.03 48. ANS: three REF: K/U OBJ: 3.6 LOC: SP1.03 49. ANS: ground state REF: K/U OBJ: 3.4 LOC: SP1.01 50. ANS: principal quantum number REF: K/U OBJ: 3.4 LOC: SP1.01 51. ANS: iso-electronic REF: K/U OBJ: 3.6 LOC: SP1.03 52. ANS: X-rays REF: MC OBJ: 3.8 LOC: SP3.01 53. ANS: Lasers REF: MC OBJ: 3.8 LOC: SP3.01 54. ANS: MRI magnetic resonance imaging

REF: MC OBJ: 3.8 LOC: SP3.01 55. ANS: superconductor REF: MC OBJ: 3.7 LOC: SP3.02 56. ANS: metals REF: K/U OBJ: 3.6 LOC: SP1.03 57. ANS: packet particle

REF: C OBJ: 3.3 LOC: SP2.01 58. ANS: argon REF: C OBJ: 3.6 LOC: SP2.02 59. ANS: iso-electronic REF: C OBJ: 3.6 LOC: SP2.02 60. ANS: energy level REF: C OBJ: 3.6 LOC: SP2.02 61. ANS: wave REF: K/U OBJ: 3.7 LOC: SP1.02 62. ANS: hydrogen bonding REF: K/U OBJ: 4.5 LOC: SP1.04 63. ANS: Unbonded pairs Lone pairs

REF: K/U OBJ: 4.3 LOC: SP1.05 64. ANS: bent REF: I OBJ: 4.3 LOC: SP2.03 65. ANS: square pyramidal REF: I OBJ: 4.3 LOC: SP2.03 66. ANS: electron affinity REF: K/U OBJ: 4.6 LOC: SP1.04 67. ANS: octahedral REF: I OBJ: 4.3 LOC: SP2.03 68. ANS: tetrahedral tetrahedron

REF: I OBJ: 4.3 LOC: SP2.03 69. ANS: trigonal pyramidal trigonal pyramid

REF: I OBJ: 4.3 LOC: SP2.03 70. ANS: square planar REF: I OBJ: 4.3 LOC: SP2.03 71. ANS: linear REF: I OBJ: 4.3 LOC: SP2.03 72. ANS: trigonal planar REF: I OBJ: 4.3 LOC: SP2.03 73. ANS: bent REF: I OBJ: 4.3 LOC: SP2.03 74. ANS: trigonal bipyramidal REF: I OBJ: 4.3 LOC: SP2.03 75. ANS: shape REF: K/U OBJ: 4.3 LOC: SP1.05 76. ANS: bond REF: MC OBJ: 4.5 LOC: SP1.04 77. ANS: Ionic compounds Salts

REF: I OBJ: 4.6 LOC: SP2.05 78. ANS: network solid REF: I OBJ: 4.6 LOC: SP2.05 79. ANS: high REF: I OBJ: 4.6 LOC: SP2.05 80. ANS: hydrogen bonding REF: K/U OBJ: 4.5 LOC: SP1.04 81. ANS: weaker REF: K/U OBJ: 4.6 LOC: SP1.04 82. ANS: intermolecular REF: MC OBJ: 4.5 LOC: SP3.02 83. ANS: dipole REF: C OBJ: 4.4 LOC: SP2.04