1. Ch.12-1 & 12-2 Review

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

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

4. How many moles of hydrochloric acid (HCl) are needed to form 3.5 x 10 3 moles of chlorine gas? HCl + O 2  H 2 O + Cl 2 7.0 x 10 3 mol HCl

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

6. Mo(HPO 4 ) 3

7. pentacarbon dioxide

8. Molecular formula with a percent composition of 92.3% carbon and 7.7% hydrogen, with a molar mass of 78.0 g C6H6C6H6

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

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

11. Larger atomic size? Nitrogen Tin

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

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

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

15. Larger electronegativity? Oxygen Sulfur

16. As 2 O 5

17. How many moles of nitrogen dioxide can be formed from the decomposition of 1.25 g of dinitrogen pentoxide? N 2 O 5  NO 2 + O 2 0.0231 mol NO 2

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

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

20. Chlorine was once produced by heating hydrochloric acid with pyrolusite (manganese(IV) oxide). How many molecules of water are produced from the reaction of 5.0 g of HCl? HCl + MnO 2  H 2 O + MnCl 2 + Cl 2 4.1 x 10 22 molecules H 2 O

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

22. Moles in 3.54 x 10 23 atoms sulfur 5.88 mol S

23. Larger ionization energy? Oxygen Selenium

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

25. sulfuric acid

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

27. If 3.23 x 10 23 molecules of methanol were placed in a reaction vessel with an excess of carbon monoxide, how many grams of acetic acid (HC 2 H 3 O 2 ) can be produced? CH 3 OH + CO  HC 2 H 3 O 2 32.2 g HC 2 H 3 O 2

28. What happens to ionic size down a group?

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

30. Larger atomic size? Calcium Bromine

31. Determine the average atomic mass of neon 20 Ne90.48% 21 Ne0.271% 22 Ne9.25% Answer - 20.2

32. Determine the average atomic mass of chromium 50 Cr4.345% 52 Cr83.789% 53 Cr9.501% 54 Cr2.365% Answer - 52.06

33. copper (II) chloride (aq) + sodium hydroxide (aq)  1.Determine the products 2.Balance the reaction 3.Determine the NET ionic equation

34. How many grams of sodium peroxide (Na 2 O 2 ) must react with water to produce 35.0 L of oxygen (and sodium hydroxide) ? 244 g Na 2 O 2

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

36. Define an alloy

37. Illustrate the following for: methane (CH 4 ) - structural formula - perspective drawing - VSEPR shape - type(s) of bonds - orbital hybridizations

38. copper(II) oxide

39. Electron configuration for: Copernicium

40. H 2 CO 3

41. HC 2 H 3 O 2

42. Mass of carbon in 56.3 g of propane, C 3 H 8 15.4 g C

43. Fe(NO 3 ) 3

44. Given the compound carbon dioxide, CO 2, illustrate the presence of the polar bonds. C EN – 2.5 O EN – 3.5 Identify if the molecule is polar

45. copper (II) bromide + aluminum chloride  1.Identify the type of reaction 2.Determine the products 3.Balance the reaction

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

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

48. Given the compound hydrogen sulfide, H 2 S, illustrate the presence of the polar bonds. H EN – 2.1 S EN – 2.5 Identify if the molecule is polar

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

50. Describe what defines an element’s atomic number

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

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

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

54. Electron configuration for: Silicon

55. What volume of oxygen is necessary to completely react with 125 L of methane gas (CH 4 ) ? 250. L O 2

56. Iron (II) sulfide + hydrochloric acid  1.Identify the type of reaction 2.Determine the products 3.Balance the reaction

57. What happens to ionization energy down a group?

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

59. Co(ClO 3 ) 3

60. Atoms in 2.79 mol of sodium hydroxide 5.04 x 10 24 atoms Na, O, H

61. potassium chlorate  potassium chloride + oxygen 1.Identify the type of reaction 2.Determine the products 3.Balance the reaction

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

63. FeCl 2

64. Volume of 4.81 mol carbon dioxide at STP 107 L CO 2

65. Electron configuration for: Francium

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

67. What happens to shielding down a group?

68. Identify the elements that make up the halogens

69. Percent composition of a compound containing 5.55 g hydrogen from a 50.00 g sample containing only hydrogen & oxygen 11.1% H 88.90% O

70. Electron configuration for: Arsenic

71. sulfur trioxide

72. Al 2 (SO 4 ) 3

73. Larger electronegativity? Cesium Fluorine

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

75. aluminum cyanide

76. potassium hydroxide (aq) + iron (III) nitrate (aq)  1.Determine the products 2.Balance the reaction 3.Determine the NET ionic equation

77. calcium acetate + sodium carbonate  1.Identify the type of reaction 2.Determine the products 3.Balance the reaction

78. Electron configuration for: Xenon

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

80. iron(III) acetate

81. Electron configuration for: Cadmium

82. Mass of 6.22 mol potassium iodide 1.03 x 10 3 g KI

83. Larger electronegativity? Lithium Francium

84. sodium chloride + iodine  1.Identify the type of reaction 2.Determine the products 3.Balance the reaction

85. Define a quantum

86. Higher atomic number = _________ attraction

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

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

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

90. Moles in 8.47 x 10 26 molecules C 6 H 12 O 6 1.41 x 10 3 mol C 6 H 12 O 6

91. What happens to atomic size down a group?

92. When 0.50 g of magnesium reacts with silver nitrate, how many grams of silver are prepared? 4.4 g Ag

93. aluminum + oxygen  1.Identify the type of reaction 2.Determine the products 3.Balance the reaction

94. Describe an atom

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

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

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

98. HClO 4

99. Contrast the three subatomic particles

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

101. aluminum bromide + chlorine  1.Identify the type of reaction 2.Determine the products 3.Balance the reaction

102. Describe how ionic bonds are formed

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

104. Illustrate the following for: carbon dioxide (CO 2 ) - structural formula - perspective drawing - VSEPR shape - type(s) of bonds - orbital hybridizations

105. How many sodium atoms are needed to react with 1.25 x 10 24 molecules of water? Na + H 2 O  H 2 + NaOH 1.25 x 10 24 atoms Na

106. Molar mass of iron(III) phosphate 150.8 g/mol FePO 4

107. Mass of 0.0331 mol silver 3.57 g Ag

108. Identify the elements that make up the alkali metals

109. Ca(ClO) 2

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

111. Larger ionic size? Iodine Fluorine

112. benzene (C 6 H 6 ) + oxygen  1.Identify the type of reaction 2.Determine the products 3.Balance the reaction

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

114. SnSe 2

115. hydrosulfuric acid

116. A frequency of 1.58 x 10 18 Hz will produce what wavelength, in meters? Where would this fall on the electromagnetic spectrum?

117. butane (C 4 H 10 ) + oxygen  1.Identify the type of reaction 2.Determine the products 3.Balance the reaction

118. Ca(OH) 2

119. CCl 4

120. Larger ionization energy? Hydrogen Helium

121. Describe how covalent bonds are formed

122. When 60.0 g of aluminum react with hydrochloric acid (HCl), how many grams of hydrochloric acid react? 243 g HCl

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

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

125. Write the electron configuration of a phosphorus atom

126. Pb(SO 4 ) 2

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

128. A radar wavelength of 2.03 x 10 -1 m will produce what frequency?

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

130. Larger ionic size? Cesium Potassium

131. Identify the elements that make up the noble gases

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

133. lithium hydroxide

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

135. Illustrate the following for: ammonia (NH 3 ) - structural formula - perspective drawing - VSEPR shape

136. Larger ionic size? Magnesium Silicon

137. Cu(NO 2 ) 2

138. hydrogen + chlorine  1.Identify the type of reaction 2.Determine the products 3.Balance the reaction

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

140. Fill the Aufbau diagram to correctly place the electrons for a nitrogen atom 1s2s2p

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

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

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

144. NH 4 HSO 3

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

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

147. Illustrate the following for: phosphane (PH 3 ) - structural formula - perspective drawing - VSEPR shape - type(s) of bonds - orbital hybridizations

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

149. What happens to atomic attraction down a group?

150. titanium(IV) fluoride

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

152. How many grams of sodium metal are needed to give 7.81 g of hydrogen by this reaction? Na + H 2 O  H 2 + NaOH (use 1.00 g/mol for molar mass of hydrogen) 180. g Na

153. Illustrate the following for: formaldehyde (H 2 CO) - structural formula - perspective drawing - VSEPR shape - type(s) of bonds - orbital hybridizations

154. Given the compound ammonia, NH 3, illustrate the presence of the polar bonds. N EN – 3.0 H EN – 2.1 Identify if the molecule is polar

155. Zn 3 P 2

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

157. Describe what defines an isotope’s mass number

158. What happens to electronegativity down a group?

159. NaOH

160. Identify the elements that make up the metalloids

161. Illustrate the following for: carbon tetrachloride (CCl 4 ) - structural formula - perspective drawing - VSEPR shape

162. Formula units in 6.48 mol of acetic acid, C 2 H 4 O 2 3.90 x 10 24 form. units C 2 H 4 O 2

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

164. perchloric acid

165. zinc hydroxide  zinc oxide + water 1.Identify the type of reaction 2.Determine the products 3.Balance the reaction

166. Identify the overall charge on a molecular compound

167. Larger atomic size? Aluminum Chlorine

168. silver hydroxide

169. Moles in 113 L chlorine gas at STP 5.04 mol Cl 2

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

171. Illustrate the following for: chloroform (CHCl 3 ) - structural formula - perspective drawing - VSEPR shape - type(s) of bonds - orbital hybridizations

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

173. Identify how the modern periodic table is organized

174. iron(II) bromide

175. Write the electron configuration of a strontium atom

176. silver nitrate + nickel  1.Identify the type of reaction 2.Determine the products 3.Balance the reaction

177. Write the electron configuration of a calcium atom

178. Larger electronegativity? Beryllium Nitrogen

179. silver nitrate (aq) + nickel (s)  1.Determine the products 2.Balance the reaction 3.Determine the NET ionic equation

180. Moles in 159 g of ammonium 8.83 mol NH 4 +

181. silver + sulfur  1.Identify the type of reaction 2.Determine the products 3.Balance the reaction

182. Moles in 1590 L sulfur hexafluoride at STP 71.0 mol SF 6

183. Volume of 8.65 mol argon at STP 194 L Ar

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

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

186. Illustrate the following for: water (H 2 O) - structural formula - perspective drawing - VSEPR shape - type(s) of bonds - orbital hybridizations

187. Molecular formula with a percent composition of 32.0% carbon, 4.0% hydrogen, and 64.0% oxygen, with a molar mass of 150.0 g C4H6O6C4H6O6

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

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

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

191. Larger ionization energy? Sodium Chlorine