2. Draw a Lewis electron-dot diagram for a chlorine atom in the ground state.
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1 100 Bonding Questions 1. Based on electronegativity values, which type of elements tends to have the greatest attraction for electrons in a bond? 1. metals 2. metalloids 3. nonmetals 4. noble gases 2. Draw a Lewis electron-dot diagram for a chlorine atom in the ground state. 3. Which element has atoms with the greatest attraction for electrons in a chemical bond? 1. beryllium 2. fluorine 3. lithium 4. oxygen 4. Draw a Lewis electron-dot diagram of a aluminum atom in the ground state. 5. Which of the following atoms has the greatest tendency to attract electrons? 1. barium 2. beryllium 3. boron 4. bromine 6. Which of the following elements has the highest electronegativity? 1. H 2. K 3. Al 4. Ca 7. The strength of an atom's attraction for the electrons in a chemical bond is the atom's 1. electronegativity 2. ionization energy 3. heat of reaction 4. heat of formation 8. What is represented by the dots in a Lewis electron-dot diagram of an atom of an element in Period 2 of the Periodic Table? 1. the number of neutrons in the atom 2. the number of protons in the atom 3. the number of valence electrons in the atom 4. the total number of electrons in the atom 9. As a neutral sulfur atom gains two electrons, what happens to the radius of the atom? 10. As two chlorine atoms combine to form a molecule, energy is 1. absorbed 2. released 3. created 4. destroyed 11. What occurs when an atom of chlorine forms a chloride ion? 1. The chlorine atom gains an electron, and its radius becomes smaller. 2. The chlorine atom gains an electron, and its radius becomes larger. 3. The chlorine atom loses an electron, and its radius becomes smaller. 4. The chlorine atom loses an electron, and its radius becomes larger. 12. What occurs when an atom of chlorine and an atom of hydrogen become a molecule of hydrogen monochloride? 1. A chemical bond is broken and energy is released. 2. A chemical bond is formed and energy is released. 3. A chemical bond is broken and energy is absorbed. 4. A chemical bond is formed and energy is absorbed.
2 14. Which of these elements has the least attraction for electrons in a chemical bond? 1. oxygen 2. fluorine 3. nitrogen 4. chlorine 15. Which change occurs when a barium atom loses two electrons? 1. It becomes a negative ion and its radius decreases. 2. It becomes a positive ion and its radius decreases. 3. It becomes a negative ion and its radius increases. 4. It becomes a positive ion and its radius increases. 16. Which Lewis electron-dot diagram represents a boron atom in the ground state? B B B B 17. Based on Reference Table S, the atoms of which of these elements have the strongest attraction for electrons in a chemical bond? 1. N 2. Na 3. P 4. Pt 18. Draw the electron-dot (Lewis) structure of calcium chloride. 19. Draw the Lewis dot diagram for carbon dioxide. 20. Draw the Lewis dot diagram for water. 21. Draw the Lewis dot diagram for aluminum phosphide. 22. Which compound contains ionic bonds? 1. NO 2. NO 2 3. CaO 4. CO Which formula represents an ionic compound? 1. NaCl 2. N 2 O 3. HCl 4. H 2 O 24. What is the total number of pairs of electrons shared in a molecule of N 2? 1. one 2. two 3. three 4. four 25. What is the total number of electrons shared in a molecule of N 2? 1. one 2. two 3. three 4. six 26. Which type of bond results when one or more valence electrons are transferred from one atom to another? 1. a hydrogen bond 2. an ionic bond 3. a nonpolar covalent bond 4. a polar covalent bond
3 27. What is the total number of electrons shared in the bonds between the two carbon atoms in a molecule of C 2 H 2? A metal, M, forms an oxide compound with the general formula M 2 O. In which group on the Periodic Table could metal M be found? 1. Group 1 2. Group 2 3. Group Group The two diagrams at right should make you remember 1. CO 2 is bent and is a polar molecule 2. CO 2 is straight and is a polar molecule 3. CO 2 is bent and is a nonpolar molecule 4. CO 2 is straight and is a nonpolar molecule. Draw an electron-dot diagram for each of the following substances: 30. calcium oxide, CaO 31. hydrogen monobromide, HBr 32. ethane, C 2 H Which molecule contains a triple covalent bond? 1. H 2 2. N 2 3. O 2 4. Cl Which of these formulas contains the most polar bond? 1. H-Br 2. H-Cl 3. H-F 4. H-I 35. Which element has atoms that can form single, double, and triple covalent bonds with other atoms of the same element? 1. hydrogen 2. oxygen 3. fluorine 4. carbon 36. Which type of chemical bond is formed between two atoms of bromine? 1. metallic 2. hydrogen 3. ionic 4. covalent 37. Which type of bond is formed when electrons are transferred from one atom to another? 1. metallic 2. hydrogen 3. ionic 4. covalent 38. The bond between Br atoms in a Br 2 1. ionic and is formed by the sharing of two valence electrons 2. covalent and is formed by the sharing of two valence electrons 3. ionic and is formed by the transfer of two valence electrons 4. covalent and is formed by the transfer of two valence electrons 39. Covalent bonds are formed when electrons are 1. transferred from one atom to another 2. captured by the nucleus 3. mobile within a metal 4. shared between two atoms 40. The bonds between hydrogen and oxygen in a water molecule are classified as 1. polar covalent 2. nonpolar covalent 3. ionic 4. metallic
4 41. Which compound contains only covalent bonds? 1. NaOH 2. Ba(OH) 2 3. Ca(OH) 2 4. CH 3 OH 42. In the diagram at right, which electrons are represented by all of the dots? 1. only carbon valence electrons 2. only hydrogen valence electrons 3. the carbon + hydrogen valence electrons 4. all of the carbon + hydrogen electrons 43. Which substance is correctly paired with its type of bonding? 1. NaBr - nonpolar covalent 2. HCl - nonpolar covalent 3. NH 3 - polar covalent 4. Br 2 - polar covalent 44. Which compound contains both ionic and covalent bonds? 1. CaCO 3 2. PCl 3. MgF 2 4. CH 2 O 45. Which formula represents a nonpolar molecule containing polar covalent bonds? 1. H 2 O 2. CCl 4 3. NH 3 4. H The degree of polarity of a chemical bond in a molecule of a compound can be predicted by determining the difference in the 1. melting points of the elements in the compound 2. densities of the elements in the compound 3. electronegativities of the bonded atoms in a molecule of the compound 4. atomic masses of the bonded atoms in a molecule of the compound 47. Which formula represents a nonpolar molecule? 1. CH 4 2. HCl 3. H 2 O 4. NH The strongest forces of attraction occur between molecules of 1. HCl 2. HF 3. HBr 4. HI 49. Using the symbols in the key at right, draw at least 12 water molecules with proper orientation to the potassium nitrate ions. KEY water potassium ca on nitrate anion
5 50. Explain why CCl 4 is classified as a nonpolar molecule. 51. Explain why NH 3 has stronger intermolecular forces of a rac on than Cl Draw the electron-dot (Lewis) structure for the ammonia molecule. 53. Explain why the bonding in KCl is different than the compounds in ques ons 50, 51, and Which molecule is nonpolar? 1. H 2 O 2. NH 3 3. CO 4. CO Which of the following compounds has the highest boiling point? 1. H 2 O 2. H 2 S 3. H 2 Se 4. H 2 Te 56. Which type of molecule is CF 4? 1. polar, with a symmetrical distribu on of charge 2. nonpolar, with a symmetrical distribu on of charge 3. polar, with an asymmetrical distribu on of charge 4. nonpolar, with an asymmetrical distribu on of charge 57. Molecules in a sample of NH 3(L) are held closely together by intermolecular forces 1. exis ng between ions 2. exis ng between electrons 3. caused by different numbers of neutrons 4. caused by unequal charge distribu on 58. Based on intermolecular forces, which of these substances would have the highest boiling point? 1. He 2. O 2 3. CH 4 4. NH 3 Base your answers to ques ons on your knowledge of chemical bonding and on the Lewis electron-dot diagrams of CO 2, H 2 S, and F 2 below. 59. Which atom, when bonded as shown, has the same electron configura on as an atom of argon? 60. Explain, in terms of structure and/or distribu on of charge, why CO 2 is a nonpolar molecule. 61. Explain, in terms of electronega vity, why a C O bond in CO 2 is more polar than the F F bond in F 2
6 62. Draw a Lewis electron-dot diagram for a molecule of chlorine, Cl Explain, in terms of electrons, why the bonding in NaCl is ionic. 64. Which element is malleable and can conduct electricity in the solid phase? 1. iodine 2. phosphorus 3. sulfur 4. n 65. Which type of bond is found in sodium bromide? 1. covalent 2. hydrogen 3. ionic 4. metallic 66. Explain, in terms of molecular polarity, why hydrogen monochloride is more soluble than hydrogen in water under the same condi ons of temperature and pressure. Base your answers for ques ons 67, 68, and 69 on the informa on below. Tes ng of an unknown solid shows that it has the proper es listed here: It has a low mel ng point, it s nearly insoluble in water, it s a nonconductor of electricity, and it is a rela vely so solid. 67. State the type of bonding that would be expected in the par cles of this substance. 68. Explain in terms of a rac ons between par cles why the unknown solid has a low mel ng point. 69. Explain why the par cles of this substance are nonconductors of electricity. 70. Metallic bonding occurs between atoms of 1. sulfur 2. copper 3. fluorine 4. carbon 71. The high electrical conduc vity of metals is primarily due to 1. high ioniza on energies 2. filled energy levels 3. mobile electrons 4. high electronega vi es 72. Which substance contains metallic bonds? 1. Hg (L) 2. H 2 O (L) 3. NaCl (S) 4. C 6 H 12 O 6(S) 73. Which is a property of most nonmetallic solids? 1. high thermal conduc vity 2. high electrical conduc vity 3. bri leness 4. malleability 74. Which statement describes a chemical property of iron? 1. Iron can be fla ened into sheets. 2. Iron conducts electricity and heat. 3. Iron combines with oxygen to form rust. 4. Iron can be drawn into a wire. 75. Which characteris c is a property of molecular substances? 1. good heat conduc vity 2. good electrical conduc vity 3. low mel ng point 4. high mel ng point 76. A substance that does not conduct electricity as a solid but does conduct electricity when melted is most likely classified as 1. an ionic compound 2. a molecular compound 3. a metal 4. a nonmetal 77. What sort of symmetry does a nonpolar molecule exhibit?
7 78. What sort of bonding exists in a carbon monoxide molecule? 79. What sort of bonding exists in an ozone molecule? 80. What sort of bonding exists in the compound copper (II) sulfate pentahydrate? 81. Draw six water molecules and clearly show the hydrogen bonding that exists between them. 82. Draw the Lewis dot diagram for sodium chloride 83. Draw the Lewis dot diagram for water. 84. Explain why fluorine and chlorine are gases at STP, but bromine is liquid, and iodine is a solid. 85. Name two compounds with molecular bonds only. 86. Name two compounds with ionic bonds only. 87. Why does Cl 2 have a nonpolar bond while HCl has a polar bond? 88. Rank these bonds from strongest to weakest polarity: HCl HF HI HBr 89. Which element has atoms that can form single, double, or triple covalent bonds with atoms of the same element? 1. H 2. O 3. C 4. F 90. Which substance represents a compound? 1. C (S) 2. Co (S) 3. CO (G) 4. O 2(G) 91. As two chlorine atoms combine to form one molecule of chlorine, energy is 1. absorbed 2. released 3. created 4. destroyed 92. Which bond type is formed when electrons are transferred from one atom to another atom? 1. covalent 2. ionic 3. hydrogen 4. metallic 93. Covalent bonds are formed when electrons are 1. transferred from one atom to another 2. captured by the nucleus 3. mobile within a metal 4. shared between two atoms 94. Which of these substances contains a coordinate covalent bond? 1. CO 2. CO 2 3. NaCl 4. Au 95. Which molecule here does not have radial symmetry and is polar? 1. CBr 4 2. CHCl 3 3. CH 4 4. N Explain why CCl 4 is a nonpolar molecule but contains polar bonds. 97. Explain what the valence electrons are doing in the molecule boron tri-iodide 98. Draw the electron dot diagram for sodium chloride 99. Draw the Lewis dot diagram for phosphorous trichloride 100. Contrast electron dispersion forces with dipole a rac on forces.
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