1. Exam Review
2019 Ch. 1-9

2. What is the following and what is it used for?
A. test tube holder, holding test tubes
B. double buret clamp, holding burets
C. forceps, picking up small objects
D. crucible tongs, holding crucibles

3. Which of these would be  best  to measure 14.2 mL of liquid water?
A 25 mL volumetric flask
B 25 mL graduated cylinder
C 25 mL Erlenmeyer flask
D 25 mL beaker

4. The figure shows an experimental setup  used to sep arate the components of a  colored ink sample. Wh ich of the  following describes this laboratory techniq ue?
A Filtration
B Decanting
C Chromatography
D Distillation

5. The volume of the hammer  is approximately—
A 5 mL
B 64 mL
C 4 mL
D 69 mL

6. What is the following and what is it used for?
A. test tube holder, holding test tubes
B. double buret clamp, holding burets
C. forceps, picking up small objects
D. crucible tongs, holding crucibles

7. Convert 456 mL to dL
A. 45,600 dL
B dL
C dL
D dL

8. Why should excess chemicals never be returned to reagent bottles?
A.The entire stock bottle of the chemical would be contaminated  if the container holding the excess chemicals has some  contamination.
B.A spill could be created if excess chemicals  are poured from   the retaining bottle to the original  chemical stock bottle.
C.The excess of chemicals would be shaken  when placed back in to the original chemical stock,  thus creating an explosive  environment.
D.The excess chemical would spoil because it was exposed to  additional oxygen when placed in a  retaining bottle.

9. What is the following and what is it used for?
A. crucible, heating to high temperatures
B. graduated cylinder, measuring volume
C. watch glass, covering evaporating dish
D. evaporating dish, evaporating

10. A student did not follow proper safety procedures while conducting a chemistry  experiment and forgot to  wear safety goggles. During the experiment an acidic  solution splashed into the student's eyes causing  severe  pain. What are the  correct  steps that the student should   have taken during this emergency?
A.The student should immediately begin rinsing his  eyes at  the eye wash station while his partner  notifies the   instructor.
B.the student should inform his partner that his eyes are  severely burned and go to the bathroom  for water. C.The student should quickly notify the instructor of the   problem and ask for permission to rinse  his eyes.
D.The student should ask the instructor for permission to  visit the school nurse.

11. What is the following and what is it used for?
A. crucible, heating to high temperatures
B. graduated cylinder, measuring volume
C. watch glass, covering evaporating dish
D. evaporating dish, evaporating

12. If a student's hand is accidentally exposed to an  acidic solution,  what should be done?
A Rinse the hand in cold running water
B Wrap the hand in paper towels
C Cover the hand with oil
D Rinse the hand in a concentrated base

13. What is the following and what is it used for?
A. test tube holder, holding test tubes
B. double buret clamp, holding burets
C. forceps, picking up small objects
D. crucible tongs, holding crucibles

14. What is the correct order to add water and acid  together?
A1. Acid is poured into a beaker.  2. Water and  salt are then  poured into the beaker with acid.
B1. Acid is poured into a beaker.  2. Water is then poured into  the beaker with acid.
C1. Water is poured into a beaker.  2. Acid is then poured into  the beaker with water.
D1. Water and salt are poured into a beaker.   Acid is the n poured into the beaker with  water.

15. If you dissolve sugar in different types of solvents to determine which solvent dissolves the sugar fastest, what is the independent variable.
A. amount of sugar
B. amount of solvent
C. time to dissolve
D. type of solvent

16. If you dissolve sugar in different types of solvents to determine which solvent dissolves the sugar fastest, what is the dependent variable.
A. amount of sugar
B. amount of solvent
C. time to dissolve
D. type of solvent

17. Why do experiments do many trials?
A. So the results can be averaged to give a more accurate result.
B. So the results can be published in multiple data tables.
C. So that each lab group has a chance to do the experiment
D. So that more material can be used up during experimentation

18. What is the following and what is it used for?
A. crucible, heating to high temperatures
B. graduated cylinder, measuring volume
C. watch glass, covering evaporating dish
D. evaporating dish, evaporating

19. What is the following and what is it used for?
A. test tube holder, holding test tubes
B. double buret clamp, holding burets
C. forceps, picking up small objects
D. crucible tongs, holding crucibles

20. What is the correct reading for significant figures?B C
D. 146

21. What is the following and what is it used for?
A. crucible, heating to high temperatures
B. graduated cylinder, measuring volume
C. watch glass, covering evaporating dish
D. evaporating dish, evaporating

22. 4.2089300 X 105 g expresses how many significant figures?
B. 6
C. 8
D. 9

23. A student measured the density of an object three times
A student measured the density of an object three times. He recorded the following  density measurements:  1.50 g/mL, 1.60 g/mL,  and 1.30 g/mL. 
The  actual density of this object is  1.49 g/mL. After finding the  average of the  student's  measurements, what was  the percent  error between the student's average  measurement of density an d the actual density of the object?
A. 2.37%
B %
C %
D %

24. Which of the following contains the greatest number of significant digits?
A g
B g
C g
D g

25. Add the following and choose the answer with the correct number of significant digits. 4.5 g g g=?
A. 22 g
B g
C g
D g

26. When the products of a reaction have different chemical properties than the reactants that formed them, it is an indication that
A. a chemical change has occurred
B. no change has occurred
C. the reactants are contaminated
C. a physical change has occurred

27. A chemical property would include
A. boiling point
B. crystalline structure
C. freezing point
D. decomposition

28. What is this a picture of?
A. heterogeneous mixture
B. homogeneous mixture
C. colloid
D. sublimation

29. Calculate the density with the correct number of significant figures if the volume is 6.7mL and the mass is 5.67 g.
A. 1.2 g/mL
B g/mL
C g/mL
D g/mL

30. How does ionization energy trend within a period?
A. it increases
B. it decreases
C. it plateaus
D. it stays constant

31. Which element has the smallest atomic radius?
A. Mg
B. P
C. Ca
D. Cl 

32. How does shielding trend across a period?
A. it increases
B. it decreases
C. it plateaus
D. it stays constant 

33. What is the electron configuration of Phosphorus?
A. 1s22s22p63s23p14s2
B. 1s22s22p63s23p3
C. 1s22s22p63s23d3
D. 1s22s22p63s23p64s3 

34. Which block are the alkali metals in?
A. s block
B. p block
C. d block
D. f block

35. Which block are the transition metals in?
A. s block
B. p block
C. d block
D. f block 

36. Which block are the inner transition metals in?
A. s block
B. p block
C. d block
D. f block 

37. Which block are the noble gases in?
A. s block
B. p block
C. d block
D. f block 

38. The atomic number is always equal to the number of
A. electrons
B. neutrons
C. protons and electrons
D. protons 

39. Nitrogen- 16 has ___ neutrons and ___ protons
A. 9,7
B. 7,9
C. 16,7
D. 7,16

40. A neutral atom of an element has the same number of ____ as protons.
A. neutrons
B. electrons
C. neutrons and electrons
D. particles 

41. Dalton speculated that atoms of the same element are _____________ to one another.
A. identical
B. larger
C. smaller
D. different
He was wrong!

42. Isotopes of an element differ in the number of
A. electrons
B. protons
C. neutrons
D. alpha particles 

43. Calculate the average atomic mass of a sample that is 80% Fe-55 and 20% Fe-56.
B. 55.8
C. 55.2
D. 55.0 

44. What particle has a negative charge and is 1/2000th the mass of a proton?
A. neutron
B. proton
C. electron
D. alpha particle 

45. How does electronegativity trend down a group?
A. it increases
B. it decreases
C. it plateaus
D. it stays constant 

46. How does electronegativity trend across a period?
A. it increases
B. it decreases
C. it plateaus
D. it stays constant

47. What did J.J. Thompson discover that were later called electrons?
A. positive particles he called corpuscles
B. negative particles he called corpuscles
C. neutral particles he called corpuscles
D. negative particles he called neutrons 

48.  Groups 1A-7A are called A. transition elements
B. representative elements
C. alkali metals
D. noble gases 

49.  Group 3-12 are called A. transition elements
B. representative elements
C. alkali metals
D. noble gases

50. Groups 3A-7A have incomplete __ sublevels.
A. s
B. p
C. d
D. f 

51. Transition metals have incomplete __ sublevels
A. s
B. p
C. d
D. f 

52. Horizontal rows are called ___ and vertical columns are called ___ on the periodic table.
A. periods, groups
B. groups, periods
C. transition, representative
D. representative, transition

53. Noble gases are ___ because they have ___ outer energy levels.
A. reactive, filled
B. inert, partially filled
C. inert, filled
D. reactive, partially filled 

54. Which of these has the highest electronegativity?
A. Be
B. N
C. Ne
D. Li 

55. Which of the following has the highest electronegativity?
A. O
B. S
C. Cs
D. Fr

56. Noble gases are in group
A. 1A
B. 7A
C. 2A
D. 8A 

57. Happy Thursday! Clicker Review today.
Exam Reviews will be turned in AFTER the test to save time or before you leave for lunch – up to you.
Computers will be on and at PowerTest ready to login when you get back from lunch. Your time will then be pretty much the same as other classes – we are only short 13 minutes and still have over two hours – schedule was revised!

58. Alkaline Earth Metals are in group
A. 1A
B. 7A
C. 2A
D. 6A 

59. Convert 456 dL to mL A. 456,000 mL B. 45,600 mL C. 0.456 mL
D mL

60. Alkali metals are in group
A. 1A
B. 7A
C. 3A
D. 6A

61. 80% of the periodic table is
A. non-metals
B. transition elements
C. metals
D. solid 

62. In general, ___ are on the left side of the metalloid “stair-step” and ___ are on the right side of the metalloid “stair-step”. 
A. metals, nonmetals
B. metalloids, gases
C. gases, solids
D. p orbitals, s orbitals

63. Which noble gas would be used to write a noble gas configuration for magnesium?
A. Ne
B. Ar
C. Kr
D. Xe

64. Elements in the same group have the same number of
A. neutrons in highest occupied energy level
B. protons in the highest occupied energy level
C. alpha particles in the highest occupied energy level
D. electrons in the highest occupied energy level 

65.  What is Hund’s Rule? A. All electrons are negative
B. One electron occupies each orbital in a sublevel before a second one is added.
C. Only two electrons are allowed in each orbital and they must have opposite spins.
D. Electrons fill lower energy levels before filling higher energy levels. 

66. What is the Pauli Exclusion Principle?
A. All electrons are negative
B. One electron occupies each orbital in a sublevel before a second one is added.
C. Only two electrons are allowed in each orbital and they must have opposite spins.
D. Electrons fill lower energy levels before filling higher energy levels. 

67. What is the Aufbau Principle?
A. All electrons are negative
B. One electron occupies each orbital in a sublevel before a second one is added.
C. Only two electrons are allowed in each orbital and they must have opposite spins.
D. Electrons fill lower energy levels before filling higher energy levels. 

68. Make sure you know orbital notation and can recognize if Hund’s Rule, Pauli Exclusion Principle or the Aufbau Principle is not followed!!

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

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

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

72. What is the shape of BF3? ☺ A. trigonal planar B. bent C. pyramidal
D. tetrahedral

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

88. 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 in metals ☺

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

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

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

92. 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 ☺

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

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

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

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

97. 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- ☺

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

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

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

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

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

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

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

105. 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 ☺

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

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

108. When nitrogen triple bonds with another nitrogen atom, there are
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 ☺

109. 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 ☺

110. Which of the following would be nonpolar?
A BF3
B. H2Se
C. SiH4
D. H2Se ☺

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

112. The lewis dot structure for a molecule of C2H4 would have
A. five single bonds
B. four single bonds and one double bond
C. 3 single bonds and two double bonds
D. 2 single bonds and 2 double bonds ☺

113. 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 ☺

114. 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

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

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

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

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

119. 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 ☺

120. 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

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

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

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

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

125. 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 ☺ ☺

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

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

128. 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 ☺

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

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

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

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

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

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

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

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

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

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

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

140. 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 ☺

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

160. 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 ☺

161. 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