1. Year-Long Review
Chemistry

2. copper (II) bromide + aluminum chloride 
Identify the type of reaction
Determine the products
Balance the reaction
copper (II) bromide + aluminum chloride 

3. Moles in 1590 L sulfur hexafluoride at STP
71.0 mol SF6

4. Mass of carbon in 56.3 g of propane, C3H8
15.4 g C

5. Fe(NO3)3

6. iron(II) bromide

7. CCl4

8. lithium hydroxide

9. Given the compound ammonia, NH3, illustrate the presence of the polar bonds. NEN – 3.0 HEN – 2.1 Identify if the molecule is polar

10. Given the compound carbon dioxide, CO2, illustrate the presence of the polar bonds. CEN – 2.5 OEN – 3.5 Identify if the molecule is polar

11. Provide a Lewis Dot Diagram for calcium In addition, identify the class of the element

12. Illustrate the following for: - orbital hybridizations
chloroform (CHCl3)
- structural formula
- perspective drawing
- VSEPR shape
- type(s) of bonds
- orbital hybridizations

13. Given the compound hydrogen sulfide, H2S, illustrate the presence of the polar bonds. HEN – 2.1 SEN – 2.5 Identify if the molecule is polar

14. Provide a Lewis Dot Diagram for oxygen In addition, identify the class of the element

15. Illustrate the structural formula of the following molecule: chlorine

16. Illustrate the movement of electrons to form an ionic bond between the reactants and products of the following ionic compound: aluminum nitride

17. Describe how covalent bonds are formed

18. Larger atomic size?
Aluminum
Chlorine

19. Electron configuration for:
Arsenic

20. Electron configuration for:
Francium

21. Circle the p block on a sketch of the periodic table

22. Identify how the modern periodic table is organized

23. Identify the at least 5 elements that make up the representative elements

24. What happens to atomic attraction from left to right across a period?

25. What happens to electronegativity from left to right across a period?

26. Electron configuration for:
Silicon

27. Larger ionic size?
Magnesium
Silicon

28. What happens to shielding down a group?

29. Circle the f block on a sketch of the periodic table

30. Identify the elements that make up the noble gases

31. What happens to atomic size from left to right across a period?

32. What happens to ionization energy down a group?

33. Briefly explain why light is emitted from an excited gas

34. Determine the number of subatomic particles in an isotope of iron-58

35. The two isotopes that make up chlorine’s atomic mass are 35Cl & 37Cl
Chlorine’s atomic mass is 35.45
What does this indicate about the abundance of the chlorine isotopes?

36. Identify what Rutherford’s Gold-Foil Experiment concluded

37. Describe what defines an element’s atomic number

38. Write the electron configuration of a strontium atom

39. Fill the Aufbau diagram to correctly place the electrons for a nitrogen atom

40. Identify what Thomson’s Cathode Ray Tube Experiment concluded

41. Define a quantum

42. Iron (II) sulfide + hydrochloric acid 
Identify the type of reaction
Determine the products
Balance the reaction
Iron (II) sulfide + hydrochloric acid 

43. potassium hydroxide (aq) + iron (III) nitrate (aq) 
Determine the products
Balance the reaction
Determine the NET ionic equation
potassium hydroxide (aq) + iron (III) nitrate (aq) 

44. calcium acetate + sodium carbonate 
Identify the type of reaction
Determine the products
Balance the reaction
calcium acetate + sodium carbonate 

45. Moles in 77.3 g of beryllium oxide
3.09 mol BeO

46. Volume of 8.65 mol argon at STP

47. Moles in 159 g of ammonium
8.83 mol NH4+

48. sodium chloride + iodine 
Identify the type of reaction
Determine the products
Balance the reaction
sodium chloride + iodine 

49. Volume of 4.81 mol carbon dioxide at STP
107 L CO2

50. Density of oxygen gas at STP
0.714 g/L

51. Moles in 113 L chlorine gas at STP
5.04 mol Cl2

52. Co(ClO3)3

53. Al2(SO4)3

54. FeCl2

55. aluminum cyanide

56. Molecular formula with a percent composition of 32. 0% carbon, 4
Molecular formula with a percent composition of 32.0% carbon, 4.0% hydrogen, and 64.0% oxygen, with a molar mass of g
C4H6O6

57. Mo(HPO4)3

58. sulfur trioxide

59. potassium chlorate  potassium chloride + oxygen
Identify the type of reaction
Determine the products
Balance the reaction
potassium chlorate  potassium chloride + oxygen

60. silver nitrate (aq) + nickel (s) 
Determine the products
Balance the reaction
Determine the NET ionic equation
silver nitrate (aq) + nickel (s) 

61. Atoms in 2.79 mol of sodium hydroxide
5.04 x 1024 atoms Na, O, H

62. Illustrate the structural formula of the following molecule: nitrogen

63. Pb(SO4)2

64. zinc hydroxide  zinc oxide + water
Identify the type of reaction
Determine the products
Balance the reaction
zinc hydroxide  zinc oxide water

65. pentacarbon dioxide

66. silver hydroxide

67. Illustrate the following for: hydrogen cyanide (HCN)
- structural formula
- perspective drawing
- VSEPR shape
- type(s) of bonds
- orbital hybridizations

68. Ca(OH)2

69. titanium(IV) fluoride

70. Mass of 6.22 mol potassium iodide
1.03 x 103 g KI

71. Molecular formula with a percent composition of 92. 3% carbon and 7
Molecular formula with a percent composition of 92.3% carbon and 7.7% hydrogen, with a molar mass of 78.0 g
C6H6

72. Provide a Lewis Dot Diagram for neon In addition, identify the class of the element

73. Illustrate the movement of electrons to form an ionic bond between the reactants and products of the following ionic compound: sodium bromide

74. Illustrate the movement of electrons to form an ionic bond between the reactants and products of the following ionic compound: aluminum phosphide

75. Identify what determines whether a bond is nonpolar, polar, or ionic

76. iron(III) acetate

77. Provide a Lewis Dot Diagram for sulfur In addition, identify the class of the element

78. Ca(ClO)2

79. Molar mass of an unknown gas with a density of 0.902 g/L at STP
20.2 g – Ne

80. Identify the elements that make up the halogens

81. SnSe2

82. Provide a Lewis Dot Diagram for phosphorus In addition, identify the class of the element

83. Illustrate the movement of electrons to form an ionic bond between the reactants and products of the following ionic compound: sodium sulfide

84. Identify the unique component of metals that lead to their properties

85. Illustrate the structural formula of the following molecule: oxygen

86. Formula units in 6.48 mol of acetic acid, C2H4O2
3.90 x 1024 form. units C2H4O2

87. Provide a Lewis Dot Diagram for sodium In addition, identify the class of the element

88. Larger ionization energy?
Sodium
Chlorine

89. Larger atomic size?
Nitrogen
Tin

90. Electron configuration for:
Xenon

91. silver nitrate + nickel 
Identify the type of reaction
Determine the products
Balance the reaction
silver nitrate + nickel 

92. What happens to atomic attraction down a group?

93. Identify the at least 5 elements that make up the nonmetals

94. Illustrate the following for: - orbital hybridizations
formaldehyde (H2CO)
- structural formula
- perspective drawing
- VSEPR shape
- type(s) of bonds
- orbital hybridizations

95. Identify the elements that make up the metalloids

96. What happens to atomic size down a group?

97. Larger electronegativity?
Lithium
Francium

98. Illustrate the movement of electrons to form an ionic bond between the reactants and products of the following ionic compound: calcium fluoride

99. NH4HSO3

100. Electron configuration for:
Cadmium

101. Circle the d block on a sketch of the periodic table

102. Larger electronegativity?
Cesium
Fluorine

103. Illustrate the following for: - orbital hybridizations
carbon dioxide (CO2)
- structural formula
- perspective drawing
- VSEPR shape
- type(s) of bonds
- orbital hybridizations

104. Larger ionic size?
Iodine
Fluorine

105. Provide a Lewis Dot Diagram for potassium In addition, identify the class of the element

106. Write the electron configuration of a phosphorus atom

107. What happens to shielding from left to right across a period?

108. Illustrate the structural formula of the following molecule: iodine

109. Write the electron configuration of a calcium atom

110. Larger electronegativity?
Oxygen
Sulfur

111. What happens to ionization energy from left to right across a period?

112. As2O5

113. Larger electronegativity?
Beryllium
Nitrogen

114. aluminum + oxygen  Identify the type of reaction
Determine the products
Balance the reaction
aluminum + oxygen 

115. Identify the number of total electrons that could fit into the 2nd energy level

116. Moles in 8.47 x 1026 molecules C6H12O6
1.41 x 103 mol C6H12O6

117. Mass of mol silver
3.57 g Ag

118. Illustrate the following for:
ammonia (NH3)
- structural formula
- perspective drawing
- VSEPR shape

119. HClO4

120. Describe how ionic bonds are formed

121. Circle the s block on a sketch of the periodic table

122. Provide a Lewis Dot Diagram for nitrogen In addition, identify the class of the element

123. Determine the number of subatomic particles in an isotope of cesium-133

124. Molar mass of iron(III) phosphate
150.8 g/mol FePO4

125. Identify the four main sublevels in order from least energetic to most energetic

126. Provide a Lewis Dot Diagram for chlorine In addition, identify the class of the element

127. Higher atomic number = _________ attraction

128. silver + sulfur  Identify the type of reaction Determine the products
Balance the reaction
silver + sulfur 

129. Describe an atom

130. What happens to ionic size from left to right across a period?

131. Illustrate the following for: - orbital hybridizations
phosphane (PH3)
- structural formula
- perspective drawing
- VSEPR shape
- type(s) of bonds
- orbital hybridizations

132. Moles in 3.54 x 1023 atoms sulfur
5.88 mol S

133. Larger ionization energy?
Oxygen
Selenium

134. butane (C4H10) + oxygen  Identify the type of reaction
Determine the products
Balance the reaction
butane (C4H10) + oxygen 

135. Provide a Lewis Dot Diagram for carbon In addition, identify the class of the element

136. What is the goal of any atom part of a molecular compound?

137. Describe what defines an isotope’s mass number

138. aluminum bromide + chlorine 
Identify the type of reaction
Determine the products
Balance the reaction
aluminum bromide + chlorine 

139. Identify the elements that make up the alkali metals

140. Illustrate the movement of electrons to form an ionic bond between the reactants and products of the following ionic compound: magnesium nitride

141. sulfuric acid

142. Identify the elements that make up the alkaline earth metals

143. Percent composition of silver nitrate
63.51% Ag
8.24% N
28.3% O

144. Illustrate the structural formula of the following molecule: bromine

145. What happens to ionic size down a group?

146. What is the goal of any atom part of an ionic compound?

147. Larger atomic size?
Calcium
Bromine

148. If electrons are filling the 3rd energy level, identify the possible sublevels that electrons would have access to.

149. Larger ionization energy?
Hydrogen
Helium

150. Provide a Lewis Dot Diagram for aluminum In addition, identify the class of the element

151. A frequency of 1.58 x 1018 Hz will produce what wavelength, in meters?
Where would this fall on the electromagnetic spectrum?

152. Provide a Lewis Dot Diagram for fluorine In addition, identify the class of the element

153. Determine the average atomic mass of neon
Answer
Determine the average atomic mass of neon
20Ne %
21Ne %
22Ne 9.25%

154. Determine the average atomic mass of chromium
Answer
Determine the average atomic mass of chromium
50Cr %
52Cr %
53Cr %
54Cr %

155. NaOH

156. Contrast the three subatomic particles

157. hydrogen + chlorine  Identify the type of reaction
Determine the products
Balance the reaction
hydrogen + chlorine 

158. Zn3P2

159. perchloric acid

160. What happens to electronegativity down a group?

161. benzene (C6H6) + oxygen  Identify the type of reaction
Determine the products
Balance the reaction
benzene (C6H6) + oxygen 

162. Illustrate the structural formula of the following molecule: fluorine

163. copper (II) chloride (aq) + sodium hydroxide (aq) 
Determine the products
Balance the reaction
Determine the NET ionic equation
copper (II) chloride (aq) + sodium hydroxide (aq) 

164. Percent composition of a compound containing 5. 82 g aluminum and 5
Percent composition of a compound containing 5.82 g aluminum and 5.18 g oxygen
52.9% Al
47.1% O

165. Define an alloy

166. Identify the overall charge on a molecular compound

167. Illustrate the following for: - orbital hybridizations
methane (CH4)
- structural formula
- perspective drawing
- VSEPR shape
- type(s) of bonds
- orbital hybridizations

168. hydrosulfuric acid

169. copper(II) oxide

170. Identify the at least 5 elements that make up the transition metals

171. Cu(NO2)2

172. Electron configuration for:
Copernicium

173. Illustrate the following for: - orbital hybridizations
water (H2O)
- structural formula
- perspective drawing
- VSEPR shape
- type(s) of bonds
- orbital hybridizations

174. Identify the five scientists that progressed atomic structure
Illustrate each scientist’s model of the atom

175. H2CO3

176. Larger ionic size?
Cesium
Potassium

177. HC2H3O2

178. Illustrate the following for: carbon tetrachloride (CCl4)
- structural formula
- perspective drawing
- VSEPR shape

179. Provide a Lewis Dot Diagram for beryllium In addition, identify the class of the element