1. What is Chemistry?

2. The study of the properties of matter and the changes that matter undergoes.

3. What is the modern definition of the atom?

4. The smallest representative particle of an element that has all of the properties of that element.

5. What is an element?

6. A substance that cannot be separated into simpler substances by chemical means. All atoms of an element are alike in properties and reactivities.

7. What is a molecule?

8. A molecule is formed when two or more atoms bond covalently.

9. What are the four states of matter in order of increasing energy?

10. solid→ liquid→gas→plasma

11. What is the Law of Constant Composition?

12. The elemental composition of a pure compound is always the same.

13. What is the difference between a chemical and physical change?

14. In a physical change the substance alters its appearance, but not its chemical composition. Water becomes ice, but is still H 2 O

15. In a chemical change, the substance is transformed into a different substance.

16. All changes of state are what type of changes?

17. Physical

18. All combustion reactions are what type of reaction? Chemical Combustion reactions always have O 2 as a reactant.

19. What are the three subatomic particles that chemists are concerned with?

20. Protons, neutrons and electrons

21. What is the electrical charge of a proton or electron?

22. 1.602 x 10 -19 C is the amount of charge per electron or proton. Protons positive Electrons are negative

23. For simplicity, what do we consider to be the charge on an electron or proton?

24. -1 electron +1 proton

25. How do the number of protons and electrons compare in an atom of an element?

26. They are equal.

27. Which subatomic particles are found in the nucleus of an atom?

28. Protons and neutrons

29. What makes up most of the volume of an atom?

30. The electron cloud

31. Atoms have extremely small masses (the heaviest atom is on the order of 4 x 10 -22 g) We use the amu to describe the mass of atoms and molecules. What is the amu?

32. The atomic mass unit. The mass of a proton and neutron are both considered to be 1 amu. An electron is about 2000 times smaller than a proton and is considered to be 0 amu.

33. On what element was the amu based?

34. Carbon -12

35. Atoms are extremely small. Most have diameters on the order of 10 -10 m. What unit is commonly used to express the diameter of atoms?

36. Picometers and the Angstrom (Å) 1 Å = 10 -10 m 1pm = 10 -12 m

37. The diameter of a carbon atom is 1.54 Å, express this diameter in picometers.

38. 1.54Å x (10 -10 m) x (10 12 pm) 1Å 1m =154 pm

39. What are the four basic forces?

40. Gravitational Electromagnetic Strong nuclear force Weak nuclear force

41. Which subatomic particle determines the identity of the element?

42. The number of protons determines the element Each atom of an element has the same number of protons.

43. What are isotopes?

44. Atoms of a given element that have different numbers of neutrons.

45. What is the atomic number? The number of protons

46. What is the mass number?

47. The total number of protons and neutrons in the atom

48. How do we identify isotopes Mass number Symbol Atomic number For example 12 C 6

49. What is a nuclide

50. An atom of a specific isotope

51. How protons, neutrons and electrons are in an atom of 197 Au.

52. All atoms of Au have 79 protons. It is an atom so there are 79 electrons There are 197 – 79 =118 neutrons

53. How many protons, electrons and neutrons are in an atom of 138 Ba?

54. Protons and electrons 56 138 -56 = 82 neutrons

55. Magnesium has three isotopes with mass numbers 24,25,and 26. a.)write the complete chemical symbol for each of these three isotopes b.)How many neutrons are in a nuclide of each isotope?

56. 24 Mg 25 Mg 26 Mg 121212 b.) 12, 13, and 14

57. Give the complete chemical symbol for the nuclide that contains 82 protons, 82 electrons and 126 neutrons.

58. 208 Pb 82

59. How is the atomic mass unit currently defined?

60. 1/12 the mass of a carbon 12 nuclide

61. How is the average atomic mass of an element determined?

62. It is a weighted average. The masses of the various isotopes and their relative abundances are used.

63. Atomic weight is also known as the average atomic mass. Atomic mass is listed on the periodic table.

64. Naturally occurring chlorine is 75.78% 35 Cl, which has a mass of 34.969, and 24.22% 37 Cl which has an atomic mass of 36.966 amu. Calculate the average atomic mass of chlorine.

65. (.7578)(34969amu) + (.2422)(36.966) 26.50 amu + 8.953 amu = 35.45 amu

66. Three isotopes of silicon occur in nature: 28 Si (92.23%) with a mass of 27.97693 amu ; 29 Si (4.68%) with a mass of 28.97649 ; 30 Si (3.09%) with a mass of 29.97377 amu. Calculate the atomic weight of silicon.

67. (.9223)(27.97693 amu) + (.0468)(28.97649 amu) + (.0309)(29.97377 amu) =28.09 amu

68. What is the Periodic Table?

69. It is a very important tool that chemists use to organize and remember chemical facts.

70. What is the Periodic Table? The elements are arranged in order of increasing atomic number. The elements with similar properties are found in the same vertical columns.

71. What do we call the vertical columns on the periodic table?

72. A group or family

73. Why are the elements within a family similar in properties and chemical reactivity?

74. They have the same number of valence electrons

75. What are the common names associated with the following groups? Group 1- Alkali metals Group 2 –Alkaline earth metals Groups 3-12 - Transition metals

76. Group 13- Boron family Group 14- Carbon family Group 15- Nitrogen family Group 16- Oxygen family Group 17- Halogens Group 18- Noble gases

77. Where are the metals on the periodic table?

78. The metals are found to the left of the metalloids. Most elements are metals.

79. Nonmetals? Nonmetals are found to the right of the metalloids.

80. Metalloids? The metalloids separate the metals and nonmetals. All elements except Al and Po that border the zig zag line are metalloids.

81. What are characteristics of metals?

82. High luster Good conductors of heat and electricity Malleable Ductile Tend to lose electrons

83. What are characteristics of nonmetals? Dull Poor conductors Brittle Tend to gain electrons or to bond covalently with other nonmetals

84. What is the only family of elements in which the atoms are found in nature as isolated atoms?

85. The noble gases

86. What is a molecule?

87. Two or more atoms bonded covalently. Most molecular substances contain only nonmetals

88. What is a diatomic molecule?

89. A molecule composed of two atoms of the same type.

90. What are the 7 diatomic molecules?

91. F 2 Cl 2 Br 2 I 2 H 2 O 2 N 2 The halogens HON!

92. What is a molecular formula?

93. A chemical formula that indicates the actual number and types of atoms in a molecule.

94. What is an empirical formula? Chemical formulas that give only the smallest whole number ratio of types of atoms.

95. What is the empirical formula for a.)C 6 H 12 O 6 b.) N 2 O c.) B 2 H 6

96. What is the empirical formula for a.)C 6 H 12 O 6 - CH 2 O b.) N 2 O - N 2 O c.) B 2 H 6 - BH 3

97. What are structural formulas?

98. Structural formulas show which atoms are bonded to each other in the molecule.

99. What are some examples of structural formulas? Lewis structures Perspective drawing Ball and stick Space filling models

100. What is an ion?

101. When electrons are gained or lost from an atom, the atom becomes an ion.

102. What is a cation?

103. When electrons are lost the atom becomes a positively charged ion or a cation.

104. What is an anion?

105. When electrons are gained the atom becomes a negatively charged ion or an anion.

106. Which elements form cations? The metals tend to form cations because they tend to lose electrons.

107. Which elements form anions? The nonmetals tend to form anions because they tend to gain electrons.

108. How can you predict the charge that an ion will have?

109. Look at the number of valence electrons the atom has. Then determine the number of electrons that would need to be lost or gained to have a full valence shell.

110. What is a polyatomic ion?

111. An ion composed of more than one atom bonded together covalently. The entire group has a charge.

112. What is a monatomic ion? An ion that originated from a single atom. “ A single atom ion”

113. Define an ionic compound.

114. A compound consisting of ions. Ionic compounds are typically combinations of metals and nonmetals

115. What type of formula do we use to describe ionic compounds?

116. The empirical formula Ionic compounds tend to have large numbers of ions bonded together in the crystal lattice. The empirical formula gives the ratio of ions

117. What is the criss cross method?

118. A method used to determine the formula for ionic compounds. The charge for one ion becomes the subscript for the other.

119. How can you predict if a compound is ionic or covalent? If the substance has a metal and a nonmetal it is probably ionic If the substance has two nonmetals it is probably covalent.

120. Which of the following would you expect to be ionic? N 2 ONa 2 OCaCl 2 SF 4 CBr 4 FeS P 4 O 6 PbF 2

121. Which of the following would you expect to be ionic? N 2 ONa 2 OCaCl 2 Covalentionicionic SF 4 CBr 4 FeS Covalentcovalentionic P 4 O 6 PbF 2 Covalentionic

122. What is the formula for the following compounds? Aluminum oxide Magnesium nitrate Zinc sulfate Iron III Carbonate Sodium phosphate Iron II chloride

123. What is the formula for the following compounds? Aluminum oxide – Al 2 O 3 Magnesium nitrate – Mg(NO 3 ) 2 Zinc sulfate- ZnSO 4 Iron III Carbonate- Fe 2 (CO 3 ) 3 Sodium phosphate- Na 3 PO 4 Iron II chloride – FeCl 2

124. Naming Inorganic ionic compounds Name the cation first. * The cation is always named before the anion. *cations named from a metal have the same name as the metal ( Al +3 is an aluminum ion)

125. Naming Inorganic ionic compounds * Ions formed from a single atom are called monatomic ions. * If the ion can have more than one charge, a roman numeral must be used to indicate charge.

126. Naming Inorganic ionic compounds For example: Iron II – Fe +2 Iron III – Fe +3

127. Naming Inorganic ionic compounds If the ion is formed from several atoms covalently bonded to each other, it is a polyatomic ion. Ammonium – NH 4 + Sulfate – SO 4 -2

128. Naming Inorganic ionic compounds Name the anion Monatomic ions are named by replacing the ending with –ide. Hydrogen becomes hydride Oxygen becomes oxide

129. How do you identify polyatomic ions with oxygen? They end in –ate for the most common form, and –ite for the anion that has the same charge but one less oxgen.

130. With respect to polyatomic ions, what do the following prefixes indicate? Per- indicates one more oxygen than the oxyanion with the –ate ending. Hypo- one less oxygen than the -ite oxyanion

131. With respect to polyatomic ions, what do the following prefixes indicate? ClO 4 - perchlorate ClO 3 - chlorate ClO 2 - chlorite ClO - - hypochlorite

132. How are anions derived by adding a H + named?

133. By adding as a prefix the word hydrogen for one hydrogen or dihydrogen for two hydrogen atoms.

134. How are anions derived by adding a H + named? For every hydrogen that is added the negative charge on the anion is decreased by one.

135. examples CO 3 -2 Carbonate HCO 3 - hydrogen carbonate PO 4 -3 Phosphate H 2 PO 4 - dihydrogen Phosphate

136. The formula for selenate is SeO 4 2-. Write the formula for the selenite ion.

137. -ate is changed to -ite so one less oxygen is present. SeO 3 2-

138. The formula for the bromate ion is BrO 3 -. Write the formula for the hypobromite ion.

139. BrO -

140. Name the following compounds a.) K 2 SO 4 b.) Ba(OH) 2 c.) FeCl 3

141. Name the following compounds a.) K 2 SO 4 –Potassium sulfate b.) Ba(OH) 2 – Barium hydroxide c.) FeCl 3 – Iron III chloride

142. Name the following compounds a.) NH 4 Br b.) Cr 2 O 3 c.) Co(NO 3 ) 2

143. Name the following compounds a.) NH 4 Br- Ammonium bromide b.) Cr 2 O 3 – Chromium III oxide c.) Co(NO 3 ) 2 – cobalt II nitrate

144. Write the chemical formula for the following compounds Potassium sulfide Calcium hydrogen carbonate Nickel II perchlorate

145. Write the chemical formula for the following compounds Potassium sulfide K 2 S Calcium hydrogen carbonate Ca(HCO 3 ) 2 Nickel II perchlorate Ni(ClO 4 ) 2

146. What is the name for the following compounds? MgSO 4 AgS Pb(NO 3 ) 2

147. What is the name for the following compounds? MgSO 4 – Magnesium sulfate Ag 2 S – silver sulfide Pb(NO 3 ) 2 - lead II nitrate

148. Define an acid.

149. A substance that has hydrogen ions as the cation and that yields H + ions when dissolved in water.

150. How do you name an acid formed from a monatomic anion? Change the –ide ending of the anion to –ic and add the prefix hydro.

151. For example HCl H 2 S HBr H 3 N

152. For example HCl hydrochloric acid H 2 S hydrosulfic acid ( May also be hydrosulfuric acid) HBr hydrobromic acid H 3 N hydronitric acid

153. Exception to the rule: When the cyanide ion is used the acid is named as if it were a monatomic ion. HCN is hydrocyanic acid

154. How do you name acids formed from polyatomic ions that have the –ate ending?

155. Use the name of the polyatomic anion but change the –ate ending to –ic and add the word acid.

156. Name H 2 CO 3

157. You know it is an acid b/c the cation is hydrogen. Take the carbonate name change -ate to -ic and add the word acid. Carbonic acid

158. Name H 3 PO 4 You know it is an acid b/c the cation is hydrogen. Take the phosphate name change -ate to -ic and add the word acid. Phosphoric acid

159. Name H 2 SO 4 You know it is an acid b/c the cation is hydrogen. Take the sulfate name change -ate to -ic and add the word acid. Sulfuric acid

160. For all acids, the number of hydrogen atoms is determined by the charge on the anion.

161. How do you name acids formed from polyatomic ions that have the –ite ending?

162. Change the –ite ending to –ous and add the word acid. HNO 2 – nitrous acid H 3 PO 3 phosphorous acid H 2 SO 3 sulfurous acid

163. Name the following acids HCN HNO 3 H 2 SO 4 H 2 SO 3

164. Name the following acids HCN hydrocyanic acid HNO 3 nitric acid H 2 SO 4 sulfuric acid H 2 SO 3 sulfurous acid

165. Naming molecular compounds 1.) The name of the element furthest to the left on the periodic table is usually written first.

166. Naming molecular compounds 2.) If both elements are in the same group, the lower one is named first.

167. Naming molecular compounds 3.) The name of the second element is given the suffix -ide.

168. Naming molecular compounds 4. Greek prefixes are used to indicate the number of atoms for each element. If the first element has only one atom, then a prefix is not used.

169. What are the prefixes that are used to indicate the number of atoms? 1- mono6- hexa 2- di7- hepta 3- tri8- octa 4- tetra9 – nona 5- penta10- deca

170. Name the following SO 2 PCl 5 N 2 O 3

171. Name the following SO 2 – Sulfur dioxide PCl 5 – phosphorus pentachloride N 2 O 3 - dinitrogen trioxide

172. Give the formula for the following A.) silicon tetrabromide B.) disulfur dichloride

173. Give the formula for the following A.) silicon tetrabromide – SiBr 4 B.) disulfur dichloride – S 2 Cl 2

174. What are organic compounds?

175. Compounds that contain mainly hydrogen and carbon and often oxygen, nitrogen or other elements.

176. What are organic compounds? Glucose – C 6 H 12 O 6 Propane – C 3 H 8

177. What are hydrocarbons?

178. Compounds that contain only hydrogen and carbon for example :C 4 H 10 butane

179. What are alkanes?

180. A hydrocarbon in which carbon is bonded to four other atoms and all bonds are single bonds.

181. What are alkenes?

182. A hydrocarbon in which carbon is bonded to other carbon atoms and one or more of the bonds for carbon is a double bond

183. What are alkynes?

184. A hydrocarbon in which carbon is bonded to other carbon atoms and one or more of the bonds for carbon is a triple bond

185. What are the prefixes that are used to indicate the number of carbon atoms? 1- meth6- hexa 2- eth7- hepta 3- prop8- octa 4- but9- nona 5- pent10 - deca

186. when naming hydrocarbons… Alkanes end in –ane i.e.,Methane, propane, heptane Alkenes end in –ene i.e., ethene, butene Alkynes end in –yne i.e., propyne, pentyne

187. Hydrocarbons that have all single bonds are called saturated. If the hydrocarbon has one or more multiple bonds it is unsaturated.

188. what is an alcohol? An alcohol is formed when a hydrogen on an alkane is replaced by an –OH group ( an hydroxyl group)

189. How are alcohols named. Use the name of the alkane the alcohol was derived from and change the ending to -ol

190. what is an alcohol? Methane becomes methanol Ethane become ethanol Butane become butanol

191. what is an alcohol? The properties of the alcohol are very different than the alkane they were formed from.