Test II
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
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1. Which of the following is true of a cation?
a. it has equal numbers of protons and electrons
b. it has fewer protons than electrons
c. it has more protons than electrons
d. the relationship between protons and electrons depends on the specific cation
2. Which of the following is true of an anion?
a. it has equal numbers of protons and electrons
b. it has fewer protons than electrons
c. it has more protons than electrons
d. the relationship between protons and electrons depends on the specific anion
3. Which is most likely true for an atom with six valence electrons?
a. it will gain one electron
b. it will gain two electrons
c. it will lose one electron
d. it will lose two electrons
4. Which is most likely true for an atom with one valence electron?
a. it will gain one electron
b. it will gain two electrons
c. it will lose one electron
d. it will lose two electrons
5. Which of the following atoms is least likely to form an ion?
a. fluorine
b. magnesium
c. silicon
d. sodium
6. For which of the following atoms do we not try to apply the octet rule?
a. oxygen
b. nickel
c. sodium
d. xenon
7. Which of the following is likely to form an ion with the largest positive charge?
a. potassium
b. calcium
c. aluminum
d. silicon
8. Which of the following is likely to form an ion with the most negative charge?
a. aluminum
b. sulfur
c. chlorine
d. argon
9. Which of the following ions has the same electronic configuration as neon?
a. Mg2+
b. F
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____ 19.
c. both (a) and (b)
d. neither (a) nor (b)
What is the name of the species formed when a sodium atom loses an electron?
a. sodate
b. sodide
c. sodium
d. sodium ion
What is the name of the species formed when a bromine atom gains an electron?
a. bromate
b. bromide
c. bromine
d. bromine ion
For which types of elements do we sometimes use the "ous/ic" system in naming ions?
a. alkali metals
b. halogens
c. noble gases
d. transition metals
In the "ous/ic" system which species is named with the "ic" ending?
a. the less negative anion
b. the more negative anion
c. the less positive cation
d. the more positive cation
Which of the following endings is generally associated with a monatomic anion?
a. ...ade
b. ...ate
c. ...ic
d. ...ide
If the name of an ion ends in "ate" what type of ion is it most likely to be?
a. a monatomic anion
b. a monatomic cation
c. a polyatomic anion
d. a poly atomic cation
The preferred name for HSO4- is hydrogen sulfate. What is the common name for this ion?
a. bisulfate
b. disulfate
c. bisulfide
d. disulfide
The "ide" ending is usually, but not always, associated with monatomic anions. Which of the following
polyatomic ions has a name which ends in "ide"?
a. C2H3O2b. HPO42 c. OH d. SO42 Which pair of species is most likely to form an ionic bond?
a. two electrically neutral species
b. two electrically charged species, one positive and one negative
c. two negatively charged species
d. two positively charged species
Which of the following situations is most likely to result in formation of a covalent bond?
____ 20.
____ 21.
____ 22.
____ 23.
____ 24.
____ 25.
____ 26.
____ 27.
____ 28.
a. when an electrically positive species interacts with an electrically negative species
b. when two nonmetallic elements interact to form a compound
c. when two electrically negative species interact
d. when two electrically positive species interact
Which of the following statements is generally true about electronegativity?
a. electronegativity decreases as we move left to right and decreases as we move top to
bottom
b. electronegativity decreases as we move left to right and increases as we move top to
bottom
c. electronegativity increases as we move left to right and decreases as we move top to
bottom
d. electronegativity increases as we move left to right and increases as we move top to
bottom
Which halogen atom is most electronegative?
a. bromine
b. chlorine
c. fluorine
d. iodine
For which of the following pairs are the atoms most likely to form an ionic bond with each other?
a. carbon and oxygen
b. calcium and chlorine
c. chlorine and oxygen
d. sodium and magnesium
What is the formula of the compound formed by aluminum and chlorine?
a. AlCl
b. AlCl2
c. AlCl3
d. Al3Cl
What is the formula of the compound formed by sodium and bromine?
a. NaBr
b. NaBr2
c. NaBr3
d. Na2Br
What is the formula of the compound formed by magnesium and iodine?
a. MgI
b. MgI2
c. MgI3
d. Mg2I
What is the formula of the compound formed by lithium and oxygen?
a. LiO
b. LiO2
c. LiO3
d. Li2O
What is the formula of the compound formed by calcium and oxygen?
a. CaO
b. CaO2
c. Ca2O2
d. Ca2O
What is the formula of the compound formed by iron (in its ferric form) and oxygen?
____ 29.
____ 30.
____ 31.
____ 32.
____ 33.
____ 34.
____ 35.
____ 36.
____ 37.
a. FeO
b. FeO2
c. Fe2O3
d. Fe3O2
What is the formula of the compound formed between the ammonium ion and the carbonate ion?
a. NH4CO3
b. NH4(CO3)2
c. (NH4)2CO3
d. (NH4)3CO3
What is the formula of the compound formed between the magnesium ion and the acetate ion?
a. MgC2H3O2
b. Mg2C2H3O2
c. Mg(C2H3O2)2
d. Mg(C2H3O2)3
What is the correct name for KI?
a. monopotassium monoiodide
b. potassium iodine
c. potassium iodide
d. potassium ion iodine ion
CaO, commonly called lime was once heated in theaters to give a bright light, hence the term "limelight."
What is the correct name for CaO?
a. calcium oxide
b. calcium oxygen
c. california oxide
d. monocalcium monoxide
AgCl is a chemical commonly used in photography. What is the correct name for AgCl?
a. monosilver monochloride
b. silver chloride
c. silver chlorine
d. silver monochlorine
The tin compound used to strengthen teeth has the formula SnF2. Which of the following is an accepted name
for this compound?
a. stannic fluoride
b. stannous fluoride
c. tin fluoride
d. tin fluorine
FeSO4 is commonly used to treat iron deficiency. Which of the following is the correct for this compound?
a. iron sulfate
b. iron(II) sulfate
c. iron(III) sulfate
d. iron sulfur tetroxide
A compound used to treat manic depressives has the formula Li2CO3. Which of the following is the correct
name for this compound?
a. dilithium carbonate
b. lithium carbon trioxide
c. lithium carbonate
d. lithium carboxide
What is the correct name for NH4NO3?
a. ammonia nitrate
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____ 39.
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____ 45.
____ 46.
b. ammonium nitrate
c. ammonia nitrite
d. ammonium nitrite
What electronegativity difference is associated with a nonpolar covalent bond?
a. exactly 0
b. less than 0.5
c. between 0.5 and 1.9
d. greater than 1.9
Which of the following bonds is the most polar?
a. H__F
b. H__Cl
c. H__Br
d. H__I
In which of the following cases is a polar covalent bond formed?
a. when an electron is transferred from one atom to another
b. when the electrons of a bond are shared equally by the two atoms
c. when the electrons of a bond are shared unequally by the two atoms
d. when a metallic element forms a bond with a non-metallic element
Which of the following statements is true about elements which exist as diatomic molecules?
a. the bond in the molecule is nonpolar covalent
b. the bond in the molecule is polar covalent
c. the bond in the molecule is ionic
d. the type of bond depends on the specific molecule
Which Greek letter is used in denoting the spatial distribution of charge in a polar bond?
a. alpha, 
b. beta, 
c. gamma, 
d. delta, 
How many electrons are associated with a single bond?
a. 1
b. 2
c. 4
d. 6
How many electrons are associated with a double bond?
a. 1
b. 2
c. 4
d. 6
How many electrons are associated with a triple bond?
a. 2
b. 3
c. 4
d. 6
Formaldehyde has the chemical formula CH2O. How many electrons must be shown in the Lewis structure of
formaldehyde?
a. 4
b. 8
c. 12
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____ 51.
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____ 54.
____ 55.
____ 56.
d. none of these
The ammonium ion has the formula NH4+. How many electrons must be shown in the Lewis structure of the
ammonium ion?
a. 4
b. 8
c. 9
d. 10
Which of the following statements is true of Lewis structures?
a. we can write Lewis structures for anions
b. we can write Lewis structures for cations
c. we can write Lewis structures for molecules
d. all of the above are true
How many bonds does a carbon atom typically form?
a. 2
b. 4
c. 6
d. 8
In a Lewis structure, which of the following atoms can have more than eight electrons associated with it?
a. C
b. O
c. S
d. none of these
The active ingredient in household bleach is sodium hypochlorite, NaClO2. What is the formula weight
sodium hypochlorite?
a. 74.5 amu
b. 90.5 amu
c. 110 amu
d. 149 amu
Formic acid, HCOOH, is what causes the sting of bee stings. What is the formula weight of formic acid?
a. 29 amu
b. 46 amu
c. 50 amu
d. 58 amu
Hospital ether, diethyl ether, has the formula (C2H5)2O. What is the formula weight of diethyl ether?
a. 28 amu
b. 45 amu
c. 74 amu
d. 90 amu
Which of the following compounds has the largest formula weight?
a. KCl
b. NaCl
c. MgF2
d. BF3
Which of the following compounds has the largest formula weight?
a. aluminum acetate
b. calcium acetate
c. potassium acetate
d. sodium acetate
When comparing one mole of water with one mole of carbon dioxide which of the following is true?
____ 57.
____ 58.
____ 59.
____ 60.
____ 61.
____ 62.
____ 63.
____ 64.
____ 65.
a. they contain the same number of atoms
b. they contain the same number of molecules
c. both (a) and (b) are true
d. both (a) and (b) are false
When comparing one mole of water with one mole of ammonia which of the following is true?
a. they contain the same number of atoms
b. they contain the same number of molecules
c. both (a) and (b) are true
d. both (a) and (b) are false
How much does one mole of oxygen gas weigh?
a. 16 amu
b. 32 amu
c. 16 g
d. 32 g
How many atoms are in a mole of sodium chloride, NaCl?
a. 1
b. 2
c. 6.02  1023
d. 12.04  1023
How many molecules are in a mole of ammonia, NH3?
a. 1
b. 4
c. 6.02  1023
d. 24.08  1023
What is the weight of 300. moles of KCl?
a. 22.4 amu
b. 22.4 g
c. 74.5 amu
d. 74.5 g
What is the weight of 2.50 moles of Al2O3?
a. 102 amu
b. 102 g
c. 255 amu
d. 255 g
2.90 moles of a particular substance weighs 81.2 g. What is the weight of one mole of the substance?
a. 0.0357 amu
b. 0.0357 g
c. 28.0 amu
d. 28.0 g
How many hydrogen atoms are in a mole of acetic acid, HC2H3O2?
a. 4
b. 1.51  1023
c. 6.02  1023
d. 2.408  1024
The atomic weight of gold is approximately 197 g/mole. What is the approximate weight of one atom of
gold?
a. 3.3  10-22 amu
b. 3.3  10-22 g
c. 197 amu
d. 197 g
____ 66. Which of the following is true of all chemical reactions?
a. there are equal numbers of atoms on the reactant and product sides
b. there are equal numbers of molecules on the reactant and product sides
c. both (a) and (b) are true
d. both (a) and (b) are false.
____ 67. When we balance a chemical equation which of the following is permitted?
a. we may adjust chemical formulas as is necessary
b. we may coefficients as is necessary
c. we may adjust both chemical formulas and coefficients as is necessary
d. we may change the physical states of the reactants or products as necessary
____ 68. The balanced equation 2H2 + O2  2H2O means which of the following?
a. two grams of hydrogen react with one gram of oxygen to form two grams of water
b. two moles of hydrogen react with one mole of oxygen to form two mole of water
c. the equation represents both (a) and (b)
d. the equation represents neither (a) nor (b)
____ 69. What do we call the chemicals which appear to the right of the arrow in a balanced chemical equation?
a. products
b. reactants
c. reagents
d. none of the above
____ 70. What do we call the chemicals which appear to the left of the arrow in a balanced chemical equation?
a. reactants
b. reagents
c. starting materials
d. all of the above
____ 71. When we write a balanced chemical equation there are some things which we must absolutely know and some
things which it is desirable to know. Which of the following statements is true?
a. we must definitely know the chemical formulas of the reactants and products
b. we must definitely know the physical states of the reactants and products
c. we must definitely know both the chemical formulas and physical states of the reactants
and products
d. none of the above statements is true
____ 72. Which of the following is true about a conventionally balanced chemical equation?
a. the number of molecules on the left equals the number of molecules on the right
b. the coefficients are all integers
c. both (a) and (b) are true
d. both (a) and (b) are false
____ 73. Which of the following is the correctly balanced equation for the complete combustion of methane, CH4?
a. CH4(g) + O2(g)  H2O(g) + CO(g)
b. CH4(g) + O2(g)  H2O(g) + CO2(g)
c. 2CH4(g) + 5O2(g)  4H2O(g) + 2CO(g)
d. CH4(g) + 2O2(g)  2H2O(g) + CO2(g)
____ 74. Nitrogen dioxide, NO2, is a brown gas found in smog. It can produced by the reaction of nitric oxide, NO,
with molecular oxygen in the air Which of the following is the correctly balanced chemical equation for the
reaction?
a. NO(g) + O(g)  NO2(g)
b. NO(g) + O2(g)  NO2(g)
c. 3NO(g) + O3(g)  3NO2(g)
d. 2NO(g) + O2(g)  2NO2(g)
____ 75. A classic method for generating molecular oxygen is the decomposition of potassium chlorate, KClO3. The
other product of this reaction is potassium chloride. Which of the following is the correctly balanced chemical
equation for this reaction?
a. KClO3(s)  KCl(s) + 3O(g)
b. 2KClO3(s)  2KCl(s) + 3O2(g)
c. KClO3(s)  KCl(s) + O3(g)
d. 2KClO3(s)  K2Cl2(s) + 3O2(g)
____ 76. For the reaction 2H2 + O2  2H2O which of the following can be answered only using the coefficients of the
balanced equation?
a. What weight of water is produced when 2.5 grams of hydrogen react completely?
b. What weight of water is produced when 2.5 moles of hydrogen react completely?
c. How many moles of water are produced from 4.0 grams of hydrogen and 32.0 grams of
oxygen?
d. How many moles of water are produced when 2.5 moles of hydrogen react completely?
____ 77. For the reaction 2H2 + O2  2H2O how much water is produced when 2.5 moles of hydrogen react
completely?
a. 2.5 grams
b. 18.0 grams
c. 2.0 moles
d. 2.5 moles
____ 78. For the reaction 2KClO3(s)  2KCl(s) + 3O2(g), how much oxygen is produced when 5.00 moles of starting
material is completely decomposed?
a. 3.33 moles
b. 3.00 moles
c. 5.00 moles
d. 7.50 moles
____ 79. When we see the equation CH4(g) + 2O2(g)  2H2O(g) + CO2(g), we understand it to mean which of the
following?
a. we cannot carry out the reaction if we do not have exactly 1 mole of CH4(g) and 2 moles
of O2(g)
b. if we have a certain weight of CH4(g) we need twice that weight of O2(g)
c. if we have 16.0 grams of CH4(g) we need 64.0 grams of O2(g) to completely react with the
CH4(g)
d. none of the above
____ 80. What is the weight of the KCl residue when 3.00 grams of KClO3(s) is decomposed according to the reaction
2KClO3(s)  2KCl(s) + 3O2(g)?
a. 0.193. g
b. 1.37 g
c. 1.83 g
d. 2.74 g
____ 81. What weight of oxygen is produced when 3.00 grams of KClO3(s) is decomposed according to the reaction
2KClO3(s)  2KCl(s) + 3O2(g)?
a. 0.392 g
b. 0.587 g
c. 0.783 g
d. 1.17 g
____ 82. Ammonia can be produced industrially by the Haber process. The chemical reaction for this process is
3H2(g) + N2(g)  2NH3(g)
What weight of nitrogen is needed to produce 51.0 grams of ammonia?
a. 14.0 g
b. 21.0 g
c. 28.0 g
d. 42.0 g
____ 83. Ammonia can be produced industrially by the Haber process. The chemical reaction is
3H2(g) + N2(g)  2NH3(g)
What weight of hydrogen is needed to produce 51.0 grams of ammonia?
a. 3.00 g
b. 4.50 g
c. 6.00 g
d. 9.00 g
____ 84. The balanced equation for the complete combustion of propane is
C3H8(g) + 5O2(g)  4H2O(g) + 3CO2(g)
If 2 moles of propane and 10 moles of oxygen are placed in container, what will be left in the container after
the reaction is complete?
a. 1 mole of propane, 5 moles of oxygen, 4 moles of water vapor, 3 moles of CO2
b. no propane, no oxygen, 4 moles of water vapor, 3 moles of CO2
c. no propane, no oxygen, 8 moles of water vapor, 6 moles of CO2
d. none of the above combinations is correct
____ 85. The balanced equation for the complete combustion of propane is
C3H8(g) + 5O2(g)  4H2O(g) + 3CO2(g)
If 1 mole of propane and 10 moles of oxygen are placed in container, what will be left in the container after
the reaction is complete?
a. no propane, 5 moles of oxygen, 4 moles of water vapor, 3 moles of CO2
b. no propane, no oxygen, 4 moles of water vapor, 3 moles of CO2
c. no propane, no oxygen, 8 moles of water vapor, 6 moles of CO2
d. none of the above combinations is correct
____ 86. If a sample of sodium is dropped into a container of water the reaction is
2Na(s) + 2H2O(l)  2NaOH(aq) + H2(g)
What weight of hydrogen is produced when 2.3 grams of sodium is dropped into 100 mL of water?
a. 0.10 g
b. 0.20g
c. 0.23 g
d. 0.40 g
____ 87. If a sample of sodium is dropped into a container of water the reaction is
2Na(s) + 2H2O(l)  2NaOH(aq) + H2(g)
What weight water is consumed when 2.3 grams of sodium is dropped into 100 mL of water?
a. 0.90 g
b. 1.8 g
c. 2.3 g
d. 3.6 g
____ 88. Among the ingredients for a particular cake recipe are 2 eggs, 2 cups of flour, 3 ounces of unsweetened
chocolate, 8 one-ounce squares of semisweet chocolate. In your kitchen you have a dozen eggs, a 16 cups of
flour, 9 ounces of unsweetened chocolate, and 16 ounces of semisweet chocolate. How many of these cakes
can you bake?
a. 2
b. 3
c. 6
d. 8
____ 89. When ammonia gas comes in contact with hydrogen chloride gas the reaction is
NH3(g) + HCl(g)  NH4Cl(s)
What weight of ammonium chloride, NH4Cl(s), is produced by the reaction of 34.0 grams of NH3(g) with
75.0 grams of HCl(g)?
a. 34.0 g
b. 75.0 g
c. 107 g
d. 109 g
____ 90. When ammonia gas comes in contact with hydrogen chloride gas the reaction is
NH3(g) + HCl(g)  NH4Cl(s)
What weight of ammonium chloride, NH4Cl(s), is produced by the reaction of 34.0 grams of NH3(g) with
36.5 grams of HCl(g)?
a. 34.0 g
b. 36.5 g
c. 53.5 g
d. 70.5 g
____ 91. When ammonia gas comes in contact with hydrogen chloride gas the reaction is
NH3(g) + HCl(g)  NH4Cl(s)
What weight of ammonium chloride, NH4Cl(s), is produced by the reaction of 17.0 grams of NH3(g) with
60.0 grams of HCl(g)?
a. 34.0 g
b. 53.5 g
c. 60.0 g
d. 94.0 g
____ 92. When ammonia gas comes in contact with hydrogen chloride gas the reaction is
NH3(g) + HCl(g)  NH4Cl(s)
What weight of ammonium chloride, NH4Cl(s), is produced by the reaction of 50.0 grams of NH3(g) with
73.0 grams of HCl(g)?
a. 50.0 g
b. 73 g
c. 107 g
d. 123 g
____ 93. A particular recipe can make 225 grams of chocolate frosting. However, the cook cannot get the last 5.00
grams out of the mixing bowl. What is the percentage yield of usable frosting?
a. 2.22%
b. 5.00 %
c. 97.8%
d. 99.1%
____ 94. When a hydrocarbon such as octane is burned in an automobile engine most of the carbon is converted to
carbon dioxide but some carbon monoxide is also produced. The reaction for the complete combustion of
octane is
2C8H18(g) + 25O2(g)  18H2O(g) + 16CO2(g)
In a particular engine it is observed that when 114.0 grams of octane is burned 334 grams of CO2(g) is
produced. What is the percent yield of CO2(g)?
a. 16.0%
b. 44.0 %
c. 94.9 %
d. 98.9%
____ 95. Aspirin can be made by the following reaction:
C7H6O3(s) +
Salicylic
acid
2C4H6O3(l)
acetic
anhydride

C9H8O4(s)
aspirin
+
C2H4O2(l)
acetic
acid
If this reaction is carried out with a 95.0% yield, how much salicylic acid is needed to produce 90.0 grams of
aspirin?
a. 65.6 g
b. 69.0 g
c. 72.6 g
d. 138 g
Test II
Answer Section
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ATOMS AND THEIR IONS
ATOMS AND THEIR IONS
ATOMS AND THEIR IONS
ATOMS AND THEIR IONS
ATOMS AND THEIR IONS
ATOMS AND THEIR IONS
ATOMS AND THEIR IONS
ATOMS AND THEIR IONS
ATOMS AND THEIR IONS
NAMING IONS
NAMING IONS
NAMING IONS
NAMING IONS
NAMING IONS
NAMING IONS
NAMING IONS
NAMING IONS
FORMATION OF CHEMICAL BONDS
FORMATION OF CHEMICAL BONDS
FORMATION OF CHEMICAL BONDS
FORMATION OF CHEMICAL BONDS
IONIC COMPOUNDS
IONIC COMPOUNDS
IONIC COMPOUNDS
IONIC COMPOUNDS
IONIC COMPOUNDS
IONIC COMPOUNDS
IONIC COMPOUNDS
IONIC COMPOUNDS
IONIC COMPOUNDS
NAMING IONIC COMPOUNDS
NAMING IONIC COMPOUNDS
NAMING IONIC COMPOUNDS
NAMING IONIC COMPOUNDS
NAMING IONIC COMPOUNDS
NAMING IONIC COMPOUNDS
NAMING IONIC COMPOUNDS
COVALENT MOLECULAR COMPOUNDS
COVALENT MOLECULAR COMPOUNDS
COVALENT MOLECULAR COMPOUNDS
COVALENT MOLECULAR COMPOUNDS
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84.
85.
86.
87.
ANS:
ANS:
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ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
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D
B
C
D
C
B
D
B
C
B
B
C
A
A
C
B
D
D
C
B
D
D
D
B
A
B
B
A
D
A
B
D
D
B
D
D
D
C
C
D
D
D
C
A
A
B
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COVALENT MOLECULAR COMPOUNDS
COVALENT MOLECULAR COMPOUNDS
COVALENT MOLECULAR COMPOUNDS
COVALENT MOLECULAR COMPOUNDS
COVALENT MOLECULAR COMPOUNDS
COVALENT MOLECULAR COMPOUNDS
COVALENT MOLECULAR COMPOUNDS
COVALENT MOLECULAR COMPOUNDS
COVALENT MOLECULAR COMPOUNDS
FORMULA WEIGHT
FORMULA WEIGHT
FORMULA WEIGHT
FORMULA WEIGHT
FORMULA WEIGHT
THE MOLE
THE MOLE
THE MOLE
THE MOLE
THE MOLE
THE MOLE
THE MOLE
THE MOLE
THE MOLE
THE MOLE
CHEMICAL EQUATIONS
CHEMICAL EQUATIONS
CHEMICAL EQUATIONS
CHEMICAL EQUATIONS
CHEMICAL EQUATIONS
CHEMICAL EQUATIONS
CHEMICAL EQUATIONS
CHEMICAL EQUATIONS
CHEMICAL EQUATIONS
CHEMICAL EQUATIONS
MASS RELATIONSHIPS IN CHEMICAL REACTIONS
MASS RELATIONSHIPS IN CHEMICAL REACTIONS
MASS RELATIONSHIPS IN CHEMICAL REACTIONS
MASS RELATIONSHIPS IN CHEMICAL REACTIONS
MASS RELATIONSHIPS IN CHEMICAL REACTIONS
MASS RELATIONSHIPS IN CHEMICAL REACTIONS
MASS RELATIONSHIPS IN CHEMICAL REACTIONS
MASS RELATIONSHIPS IN CHEMICAL REACTIONS
MASS RELATIONSHIPS IN CHEMICAL REACTIONS
MASS RELATIONSHIPS IN CHEMICAL REACTIONS
MASS RELATIONSHIPS IN CHEMICAL REACTIONS
MASS RELATIONSHIPS IN CHEMICAL REACTIONS
88.
89.
90.
91.
92.
93.
94.
95.
ANS:
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ANS:
ANS:
ANS:
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ANS:
A
C
C
B
C
C
C
C
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MASS RELATIONSHIPS IN CHEMICAL REACTIONS
MASS RELATIONSHIPS IN CHEMICAL REACTIONS
MASS RELATIONSHIPS IN CHEMICAL REACTIONS
MASS RELATIONSHIPS IN CHEMICAL REACTIONS
MASS RELATIONSHIPS IN CHEMICAL REACTIONS
MASS RELATIONSHIPS IN CHEMICAL REACTIONS
MASS RELATIONSHIPS IN CHEMICAL REACTIONS
MASS RELATIONSHIPS IN CHEMICAL REACTIONS