1. Ch. 7 Clicker Review

2. Cations are formed when neutral☺
A. atoms lose electrons
B. atoms gain electrons
C. atoms gain protons
D. atoms lose neutrons

3. The formula for magnesium oxide is☺
A. MgO
B. Mg2O
C. MgO2
D. Mg2O2

4. Valence electrons are found in the _____ energy level of an atom.
A. innermost
B. weakest
C. outermost
D. lowest ☺

5. Which element has one less valence electron than Carbon?
A. Be
B. N
C. Si
D. B ☺

6. Which atom or ion has the electron configuration of a noble gas?
A. Mg1+
B. Cu
C. S
D. Ca2+ ☺

7. The formula for Lithium Oxide would be
A. LiO
B. LiO2
C. Li2O2
D. Li2O ☺

8. Which element has three valence electrons?☺
A. Al
B. Si
C. Ge
D. S

9. Which element would be used to write the noble gas configuration of Aluminum?
A. He
B. Ne
C. Kr
D. Ar ☺

10. The correct formula for Calcium Nitride would be☺
A. Ca3N2
B. Ca2N3
C. CaN
D. Ca2N2

11. Electrons are __, neutrons are __ and protons are __
A. positive, negative, neutral
B. negative, positive, neutral
C. positive, neutral, negative
D. negative, neutral, positive ☺

12. Which is the correct electron dot structure for Nitrogen?A. B. C. D. ☺

13. What is the correct electron dot structure for the oxygen ionB. C. D. ☺

14. What is modeled as a sea of electrons?
A. valence electrons in non metals
B. valence electrons in gases
C. valence electrons in solids
D. valence electrons is metals ☺

15. What is the electron configuration of Cl-?☺
A. 1s22s22p63s23p6
B. 1s22s22p63s23d6
C. 1s22s22p63s24p6
D. 1s22s22p63s23p5

16. An oxygen ion has the same number of electrons as a neutral atom of
A. He
B. Ne
C. Ar
D. Kr ☺

17. A(n) ______ has superior properties to the metals they are composed of.
A. alkali metal
B. alloy
C. alkaline earth metal
D. noble gas ☺

18. The ______of an ion is equal to the sum of the positive charge of each proton and the negative charge of each electron.
A. mass
B. energy
C. charge
D. electronegativity ☺

19. _______ are formed when neutral atoms gain electrons.☺
A. anions
B. cations
C. atoms
D. metals

20. Ionic compounds when dissolved in water ___
A. melt
B. conduct electricity
C. heat up
D. cool down ☺

21. How many electrons does the copper ion have when it forms the ionic compound CuCl2?
B. 28
C. 27
D. 26 ☺

22. What kind of bond involves the transfer of electrons?
A. covalent
B. ionic
C. complex
D. metallic ☺

23. An atom with an electron configuration of 1s22s22p63s23p2 is most likely to form an ion that has a charge of
A. 2+
B. 4+
C. 3-
D. 2- ☺

24. The Ca2+ ion contains __ electrons.
B. 19
C. 18
D. 17 ☺

25. An ion that has 9 protons and 10 electrons is
A. Ne+
B. F+
C. Ne-
D. F- ☺

26. Cations are __ and Anions are ___
A. negative, positive
B. positive, negative
C. neutral, negative
D. positive,neutral ☺

27. Representative elements lose or gain electrons to gain the ___ of a noble gas.
A. electronegativity
B. ionization energy
C. atomic radius
D. electron configuration ☺

28. __ play a necessary function in chemical reactions called bonding.
A. protons
B. electrons
C. neutrons
D. alpha particles ☺

29. Ch. 8 Clicker Review

30. Transferring of electrons between atoms would describe a(n)
A. splitting bond
B. ionic bond
C. covalent bond
D. molecular bond ☺

31. Intermolecular forces are ___ than ionic or covalent bonds
A. stronger
B. weaker
C. narrower
D. shorter ☺

32. When a metal and a nonmetal form a bond you would expect what type of bond?☺
A. ionic
B. covalent
C. metallic
D. molecular

33. Dipole interactions are weak attractions between
A. non polar molecules
B. ions
C. neutrons
D. polar molecules ☺

34. When two nonmetals form a bond, you would expect
A. transfer of electrons for a covalent bond
B. sharing of electrons for an ionic bond
C. sharing of electrons for a covalent bond
D. transfer of electrons for an ionic bond ☺

35. Electrons can be lost, shared or ____ during bonding processes.☺
A. gained
B. demoted
C. emitted
D. spun off

36. Which of the following would contain an ionic bond?
A. HCl
B. MgCl2
C. N2
D. SiH4 ☺

37. What is the shape of NH3? ☺ A. bent B. trigonal planar C. tetrahedral
D. pyramidal ☺

38. What is the shape of H2O? ☺ A. Bent B. Linear C. trigonal planar
D. pyramidal

39. What is the shape of CH4? ☺ A. pyramidal B. tetrahedral
C. trigonal planar
D. bent ☺

40. What is the shape of SiO2? ☺ A. Linear B. Bent C. trigonal planar
D. pyramidal

41. Which element will form a covalent bond with oxygen?
A. neon
B. phosphorus
C. potassium
D. magnesium ☺

42. Ionic compounds generally have __ melting points than covalent compounds?
A. lower
B. higher
C. less predictable
D. less consistant ☺

43. Van der Waals forces include
A. dipole interactions only
B. dipole interactions and dispersion forces only
C. dipole interactions and hydrogen bonding only
D. hydrogen bonding and dispersion forces only ☺

44. When nitrogen triple bonds with another nitrogen atom, there are/is
A. no lone pairs of electrons on either nitrogen atom
B. two lone pairs of electrons on each nitrogen atom
C. one lone pair of electrons on each nitrogen atom
D. one lone pair of electrons on only one of the nitrogen atoms ☺

45. What types of bonds can be found in a solid sample of H2S?
A. covalent bonding only
B. both ionic and covalent bonding
C. hydrogen bonding only
D. both covalent and hydrogen bonding ☺

46. Which structure is nonpolar?B. C. D. ☺

47. Which element does not naturally occur as a diatomic molecule?
A. H
B. Br
C. N
D. C ☺

48. The reason a water skimmer/strider can walk on water is because of
A. dispersion forces
B. hydrogen bonds
C. electric fields
D. van der Waals forces ☺

49. What is the shape of SiO32-?☺
A. trigonal planar
B. bent
C. pyramidal
D. tetrahedral

50. Hydrogen bonding always involves
A. non polar molecules
B. hydrogen
C. neutrons
D. dispersion forces ☺

51. Which of the following would be nonpolar?
A NF3
B. H2Se
C. SiH4
D. H2S ☺

52. What type of bonds are in ethanol?
A. ionic
B. nuclear
C. metallic
D. covalent ☺

53. Which of the following would be polar?
A. He
B. N2
C. SiO2
D. SeO2 ☺

54. The lewis dot structure for a molecule of SiO32- would have
A. 3 single bonds
B. 2 single bonds and two double bonds
C. 1 single bonds and two double bonds
D. 2 single bonds and 1 double bond ☺

55. What type of bond forms in N2, Br2 and O2
A. an ionic bond formed by the gain of electrons
B. a covalent bond formed by the sharing of electrons
C. a metallic bond formed by the transfer of electrons
D. a nuclear bond formed by the sharing of electrons ☺

56. If all of the electrons are distributed ____ in a molecule, the molecule is non-polar.☺
A. equally
B. within p orbitals
C. unequally
D. randomly

57. Hydrogen bonding is the ___ intermolecular force
A. evasive
B. strongest
C. least polar
D. weakest ☺

58. Which compound would have a covalent bond?
A. CaBr2
B. KCl
C. PO
D. NaBr ☺

59. This shows the formation of a _____ bond.☺
A. non polar covalent
B. polar covalent
C. metallic
D. non polar ionic

60. How many bonds are shown in the structural formula below?
A. 1 covalent, 8 ionic
B. one double covalent, 8 ionic
C. 8 double covalent, 1 single covalent
D. 1 double covalent, 8 single covalent ☺

61. When a molecule is polar, it behaves as if one end of the molecule is ___ and the other end of the molecule is ___. ☺
A. negative, positive
B. magnetic, nonmagnetic
C. ionic, nonionic
D. neutral, positive

62. Ch. 9 Clicker review

63. What is the correct name for CrSO4?
A. Chromium (I) sulfate
B. Chromium (II) sulfate
C. Chromium (III) sulfate
D. Chromium (IV) sulfate ☺

64. What is the correct formula for copper(II)bromide?☺
A. CuBr2
B. Cu2Br2
C. Cu2Br
D. CuBr

65. What is the correct name for (NH4)3PO4?
A. Ammonium (I) phosphate
B. Ammonium phosphate
C. Ammonium (II) phosphate
D. Ammonium (IV) phosphate ☺

66. What is the correct formula for diphosphorus pentoxide?
A. P2O2
B. P5O2
C. P2O5
D. PO5 ☺

67. What is the name of NH3? Other than “ammonia”…
A. mononitrogen hydride
B. mononitrogen trihydride
C. nitrogen(III) hydride
D. Nitrogen trihydride ☺

68. What is the name of SiO2? ☺ A. silicon dioxide B. monosilicon oxide
C. silicon(IV) oxide
D. silicon monoxide

69. What is the name of H2O? Other than “water”…☺
A. dihydrogen monoxide
B. hydrogen monoxide
C. hydroxic acid
D. dihyrdogen oxide

70. What is the name of CH4? Other than methane…
A. pyramidal
B. carbon tetrahydride
C. trigonal planar
D. bent ☺

71. What is the name of BF3? ☺ A. boron trifluoride
B. monoboron trifluoride
C. boron(III) fluoride
D. boron fluoride

72. What does the roman numeral mean in copper(II)bromide?
A. number of molecules
B. number of atoms
C. number of valence electrons
D. charge on the ion ☺ ☺

73. What is the correct name for Ca(NO3)2
A. Calcium dinitrate
B. Calcium(II) nitrate
C. Calcium nitrate
D. Calcium(II) dinitrate ☺

74. What is the correct name for MgCO3☺
A. Magnesium carbonate
B. Magnesium(II) carbonate
C. Magnesium carbonate
D. Magnesium (II) carbonate

75. What is the correct name for MnBr3?
A. Manganese(I) bromide(III)
B. Manganese(III) bromide(III)
C. Manganese bromide (III)
D. Manganese(III) bromide ☺

76. What is the? correct name for Fe3P2?
A. Iron (III) phosphide
B. Iron (II) phosphide
C. Iron phosphide
D. Iron (II) phosphide(III) ☺

77. What is the correct formula containing magnesium and carbonate?☺
A. MgCO3
B. Mg2CO3
C. Mg(II)CO3
D. Mg3CO3

78. What is the name for Fe(OH)3?
A. Iron hydroxide
B. Iron trihyroxide
C. Iron (II) hydroxide
D. Iron (III) hydroxide ☺

79. What is the formula for silver nitrate?
A. Ag3NO3
B. Ag2NO3
C. Ag(I)NO3
D. AgNO3 ☺

80. What is the name of Cd(CO3)2?
A. Cadmium(I) carbonate
B. Cadmium(II) carbonate
C. Cadmium(III) carbonate
D. Cadmium carbonate ☺

81. What is the name of Zn(OH)2?
A. Zinc (I) hydroxide
B. Zinc(II) hydroxide
C. Zinc(III) hydroxide
D. Zinc hydroxide ☺

82. What is the name of NH4NO3? ☺ A. Ammonium nitrate
B. Nitrogen hydrogen nitrate
C. Nitrogen hydroxide
D. Ammonium nitride

83. The 3 in NH4NO3is a(n) ☺ A. coefficient B. subscript
C. oxidation number
D. exponent ☺

84. What element has the same electron dot structure as boron?
Carbon
Nitrogen
Oxygen
Aluminum ☺

85. Which of the following most likely has an ionic bond?
A. H2
B. MgCl2
C. SO2
D. CH4 ☺

86. Which of the following most likely has an covalent bond?
A. AlN
B. KCl
C. CaO
D. CO ☺

87. When ionic compounds are named, the name of the anion (if it’s not polyatomic!) will be
A. –ite
B. –ide
C. –ic
D. -ate ☺

88. Which particles are lost, shared or gained when bonding?
A. protons
B. electrons
C. neutrons
D. alpha particles ☺

89. In most cases, how many valence electrons are needed for stability?☺

90. Which noble gas has an electron configuration that is stable with only two electrons?
A. H
B. He
C. Ar
D. Kr ☺

91. When hydrogen bonds covalently with fluorine, hydrogen shares ___ pair(s) of electrons.☺
A. 1
B. 2
C. 3
D. 4

92. Ionic bonds occur between cations and ___
A. hydrogen ions
B. anions
C. polar molecules
D. coordinate covalent bonds ☺

93. 9.4 and 9.5 Review

94. Name HF ☺ A. hydrogen fluoride B. hydrogen trifluoride C. hydric acid
D. hydrofluoric acid ☺

95. Name H2S ☺ A. hydrosulfuric acid B. dihydrogen sulfide
C. hydro(II) sulfuric acid
D. sulfurous acid

96. Name H2SO4 ☺ A. Sulfous acid B. hydrosulfuric acid C. Sulfuric acid
D. hydrosulfic acid ☺

97. Name HNO2 ☺ A. hydronitrite B. Nitrous acid C. hydronitrite acid
D. hydronitrate ☺

98. What is the formula for Nitric acid?
A. HNO2
B. H2NO3
C. H2NO
D. HNO3 ☺

99. What is the formula for sulfurous acid?☺
A. H2SO3
B. H2SO4
C. HSO3
D. H2S

100. What is the formula for Carbonic acid?
A. H2SO3
B. H2CO3
C. H2CO2
D. HCO3 ☺

101. What is the formula for phosphoric acid?☺
A. H3PO4
B. HPO3
C. H3PO2
D. HPO2

102. What is the formula for hydrochloric acid?
A. H2Cl2
B. HCl2
C. H2Cl
D. HCl ☺

103. What is the formula for sodium hydroxide?
A. Na2(OH)2
B. Na(OH)2
C. NaOH
D. Na2OH ☺

104. What is the formula for Iron(II) hydroxide?☺
A. Fe(OH)2
B. Fe2(OH)2
C. FeOH
D. Fe(OH)3

105. What is the name of Mg(OH)2?
A. Magnesium(II) hydroxide
B. Magnesium (I) hydroxide
C. Magnesic acid
D. Magnesium hydroxide ☺

106. What is the name of Zn(OH)2?☺
A. Zinc hydroxide
B. Zinc(II) hydroxide
C. Zinc (I) hydroxide
D. Zincic acid

107. What is the name of Mn(OH)3?
A. Manganese hydroxide
B. Manganese (I) hydroxide
C. Manganese(III) hydroxide
D. Manganic acid ☺

108. Which law states that in samples of any chemical compound, the masses of the elements are always in the same proportions.
A. Law of multiple proportions
B. Law of definite proportions
C. Law of conservation of energy
D. Law of entropy ☺

109. Which law states whenever the same two elements form more than one compound, the different masses of one element that combine with the same mass of the other element are in the ratio of small whole numbers. ☺
A. The Law of Multiple Proportions
B. The Law of Definite Proportions
C. The Law of Conservation of Matter
D. Dalton’s Atomic Law