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Honors Chemistry Final

Total questions: 263

Worksheet time: 6hrs 20mins

Name
Class
Date
1.
What is the molar mass of C6H12O6?
a)

180.18 g/mol

b)

180.12 g/mol

c)

180.24 g/mol

d)

180.06 g/mol

2.
Cl2 + 2 KBr → Br2 + 2 KCl
How many grams of potassium chloride can be produced from 356 g of chlorine and 356 g of potassium bromide?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
3.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
4.
A chemist interested in the efficiency of a chemical reaction would calculate the
a)
mole ratio
b)
rate of reaction
c)
percent yield
d)
energy released
5.
What is a Excess Reagent?
a)
amount you end with
b)
what you run out of first
c)
what you have left over
d)
what you start with
6.
"Everything is composed of atoms" was stated by:
a)
Democritis
b)
Dalton
c)
Moseley
d)
Einstein
7.
John Dalton stated:
a)
elements are made of atoms
b)
atoms of a given element are identical
c)
atoms cannot be subdivided, created, nor destroyed
d)
all of the above
8.
The scientist responsible for "discovering" the nucleus is:
a)
Bohr
b)
Rutherford
c)
Schroedinger
d)
Einstein
9.
The nucleus of an atom can be described as:
a)
spacious and negatively charged
b)
dense and positively charged
c)
spacious and positively charged
d)
dense and negatively charged
10.
Electrons are not factored into atomic mass because:
a)
They are so small their mass is negligible
b)
They're not in the nucleus
c)
They're too big
d)
They move so quickly their mass is zero
11.
How did Rutherford discover the proton?
a)
Cathode tube ray experiment
b)
Gold Foil Experiment
c)
Planetary Model
d)
Plum Pudding Model
12.
True or False: The majority of an atom is made up of empty space
a)
True
b)
False
13.
The word "atom" comes from a Greek word that means
a)
Invisible
b)
Indivisible
c)
Undivided
14.

Which part of the atomic theory did Niels Bohr prove?

a)

there are electrons

b)

there is a nucleus

c)

electrons are in energy levels

d)

gold foil experiment

15.

Which part of the atomic theory did JJ Thomson prove?

a)

there are electrons

b)

electrons are in energy levels

c)

there is a nucleus

d)

cathode ray tube

16.

What experiment did JJ Thomson use?

a)

gold foil experiment

b)

cathode ray tube experiment

17.

John Dalton wrote postulates to make the idea of the atom useful. Which postulate below was proven wrong?

a)

All elements are made up of tiny indivisible particles called atoms.

b)

The atoms of one element are different from the atoms of another element.

c)

Atoms of different elements chemically combine to form chemical compounds.

d)

During chemical reactions, atoms are rearranged.

18.

JJ Thomson came up with which model for the atom?

a)

planetary model

b)

electron cloud model

c)

plum pudding model

d)

nuclear model

19.

Which statement is incorrect?

a)

The nucleus is very dense.

b)

The nucleus contains protons and neutrons.

c)

The nucleus is positively charged.

d)

The nucleus is involved in chemical reactions.

20.

What determines chemical reactivity?

a)

protons

b)

neutrons

c)

electrons

d)

isotopes

21.

What determines the identity of the atom?

a)

protons

b)

neutrons

c)

electrons

d)

isotopes

22.

What are atoms with the same number of protons but different numbers of neutrons?

a)

electrons

b)

protons

c)

neutrons

d)

isotopes

23.

When an atom loses or gains electrons to become more stable it becomes an:

a)

ion

b)

isotope

c)

atom

d)

average

24.

After Rutherford discovered the nucleus, which model is believed to be true?

a)

protons, neutrons, and electrons are evenly distributed

b)

the nucleus is made of protons, neutrons, and electrons

c)

the nucleus is made of protons and electrons

d)

the model is mostly empty space with a central nucleus

25.

Which describes the same atomic number but different numbers of neutrons?

a)

ions

b)

isotopes

c)

atoms

d)

neutrons

26.

Which particles form the nucleus of the atom?

a)

protons and electrons

b)

protons and neutrons

c)

electrons and ions

d)

electrons and neutrons

27.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
28.
How many neutrons in C-14?
a)
6
b)
7
c)
14
d)
8
29.
How many neutrons does the isotope below have?     89 36Kr
a)
53
b)
36
c)
89
d)
125
30.
How many neutrons does an atom of the isotope Neon-22 have?
a)
12
b)
10
c)
22
d)
20
31.

Isotopes of an element have a different number of...

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

32.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
33.
In a correctly written symbol what would be located in the "A" position?
a)
number of neutrons
b)
atomic number
c)
number of electrons 
d)
mass number
34.
What quantities vary between isotopes of an element?
a)
protons, electrons, and atomic mass
b)
protons, electrons, and atomic number
c)
neutrons and electrons
d)
neutrons and atomic mass
35.
Isotopes are atoms of the same element with different #’s of __________ & therefore different __________.
a)
n0 ;  atomic #’s
b)
p+ ; atomic #’s
c)
e- ; atomic masses
d)
n0 ; atomic masses
36.
Four isotopes of lead include lead-204, lead-206, lead-207, and lead-208.  The average atomic mass of lead is 207.2.  Which isotope of lead is likely to be the most abundant.
a)
204
b)
206
c)
207
d)
208
37.
Two isotopes of carbon are carbon-12 and carbon-14.  These isotopes differ from one another by two protons.
a)
true
b)
false
38.

The region inside an atom where electrons are likely to be found

a)

Proton

b)

Atom

c)

Electron Cloud

d)

Neutron

39.

A horizontal row of elements in the periodic table

a)

Molecule

b)

Period

c)

Family

d)

Atom

40.

A substance that cannot be broken down into other substances by chemical or physical means.

a)

Covalent bond

b)

Atom

c)

Element

41.

A chemical bond where electrons are shared between two atoms. In this type of bond no ions are. You will find these bonds when carbon bonds to other elements.

a)

Covalent bond

b)

Element

c)

Hydrogen bond

42.

A chemical bond that has hydrogen covalently bonded to an electronegative atom. It happens when oxygen bonds to hydrogen.

a)

Ionic bond

b)

Hydrogen bond

c)

Molecule

43.

A physical model that depicts the atom as a small positively charged nucleus with electrons in orbit at different levels.

a)

Covalent bond

b)

Ionic bond

c)

Bohr Model

d)

Electron dot diagram

44.

A diagram that shows the bonding between atoms of a molecule and the lone pair of electrons that may exists in the molecule

a)

Hydrogen bond

b)

Bohr Model

c)

Electron dot diagram

d)

Element

45.

A chemical bond between two atoms where one or more electrons are passed from one atom to another. When they give up electrons, each of the atoms should have a filled shell. An example is the sodium chloride bond.

a)

Ionic bond

b)

Hydrogen bond

c)

Element

d)

Covalent bond

46.

Elements in the same vertical column of the periodic table; also called group

a)

Family

b)

Atom

c)

Element

d)

Metals

47.
An element has two naturally occurring isotopes. One is 10.013 amu and is 19.9% abundant. The other is 11.01 amu and is 80.1% abundant. What is the average atomic mass? What element is it?
a)
9.012, Beryllium
b)
12.011, Carbon
c)
6.941, Lithium
d)
10.812, Boron
48.

Calculate the average atomic mass of silver.

a)

106.38649amu

b)

111.91896amu

c)

107.8677amu

d)

121

49.
Compute the average atomic mass for silicon:
a)
27.977
b)
28.09
c)
28.976
d)
The average mass cannot be determined from provided information.
50.

To calculate average atomic mass, you need

a)

the atomic mass of each isotope

b)

the percent abundance of each isotope

c)

the atomic mass and percent abundance of each isotope

d)

to find the average of the atomic masses of each isotope

51.

Element Z has 2 natural isotopes. One isotope has a mass of 15.0 amu and a relative abundance of 30%. The other isotope has a mass of 16.0 amu and a relative abundance of 70%. Estimate the average atomic mass for this one element.

a)

15.0 amu

b)

16.0 amu

c)

15.7 amu

d)

16.9 amu

52.
What is the mass number defined as?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
53.

The number in Kr-84 represents what about Krypton?

a)

The number of electrons

b)

The number of protons

c)

The mass number

54.

Which pair of atoms will form ionic bonds?

a)

S and F

b)

Mg and O

c)

F and Cl

d)

H and Ne

55.

The force between electric charges depends on...

a)

both the mass and the distance between charges

b)

the distance between charges

c)

the amount of charge

d)

both the distance between and the amount of charge

56.

A material through which electrons (and therefore charge) move easily.

a)

insulator

b)

conductor

c)

static electricity

d)

ions

57.

A material through which electrons (and therefore charge) do not move easily.

a)

insulator

b)

conductor

c)

static electricity

d)

ions

58.

I touched a negatively charged rod to a neutral object, and some negative charge was transferred to the object. This is an example of...

a)

charging by induction

b)

charging by polarization

c)

charging by contact

d)

not being smart - you should never do that

59.

I bring a positively charged rod near a neutral metal sphere, which causes the negative charge within the sphere to move toward the rod, and the positive charge to move away from the rod. This is an example of...

a)

charging by induction

b)

charging by polarization

c)

charging by contact

d)

charging by friction

60.

I bring a positively charged rod near a neutral metal sphere, which causes the negative charge within the sphere to move toward the rod, and the positive charge to move away from the rod. This is an example of...

a)

charging by induction

b)

charging by polarization

c)

charging by contact

d)

charging by friction

61.

what is the name of CCl4?

a)

carbon tetrachloride

b)

monocarbon tetrachloride

c)

tetracarbon monochloride

d)

carbon chloride

62.

what is the name of CCl4?

a)

carbon tetrachloride

b)

monocarbon tetrachloride

c)

tetracarbon monochloride

d)

carbon chloride

63.

What is the name of the compound SO2

a)

Monosulfate oxide

b)

Sulfur Dioxide

c)

Monosulfur dioxide

64.

What is the name of the compound P2O5

a)

Pentaphosphorus dioxide

b)

Phoshphide dioxide

c)

Diphosphorus pentoxide

65.

What is the name for MgF2 ?

a)

magnesium fluoride

b)

manganese Phosphide

c)

magnesium(III) fluoride

d)

magnesium fluoride(II)

66.
What is the charge on the calcium ion?
a)
1+
b)
2+
c)
2-
d)
1-
67.
Which is a transition metal?
a)
cesium
b)
iron
c)
helium
d)
tellurium
68.
Select the correct formula for sulfur hexachloride
a)
S2Cl6
b)
S6Cl
c)
SCl6
d)
SF6
69.
Name the compound CaF2
a)
calcium difluoride
b)
calcium (II) fluoride
c)
calcium fluorite
d)
calcium fluoride
70.

NaBr

a)

Bromide sodide

b)

Sodium bromide

c)

Sodium bromate

d)

Sodium bromite

71.
What is the formula for Potassium Fluoride? 
a)
KF
b)
K2F
c)
KF2
d)
none of the above
72.
C3O8
a)
Tricarbon Octoxide
b)
Carbon Octoxide
c)
Carbon Oxide
d)
Carbon (VIII) Oxide
73.
H2O
a)
Dihydrogen Monoxide
b)
Hydrogen Oxide
c)
Hydrogen Monoxide
d)
Water
74.
Zn3P2
a)
Zinc Phosphide
b)
Zinc (II) Phosphide
c)
Trizinc Diphosphide
d)
Zinc Phosphate
75.
What kind of bond forms between a cation and an anion?
a)
Chemical bond
b)
Ionic bond
c)
Covalent bond
d)
Electron bond
76.
What kind of bond forms between two nonmetals?
a)
Chemical bond
b)
Ionic bond
c)
Covalent bond
d)
Electron bond
77.
What kind of bond forms between two nonmetals?
a)
Chemical bond
b)
Ionic bond
c)
Covalent bond
d)
Electron bond
78.
Name the following compound: SnO2
a)
tin(II) oxide
b)
tin(IV)oxide
c)
tin(II)oxygen 
d)
tin oxide
79.
Name the following ionic compound: Cs2S
a)
cesium sulfide
b)
cesium sulfate
c)
cesium (II) sulfate
d)
cesium (II) sulfide
80.
SeF4
a)
Tetraselenium fluoride
b)
Selenium Fluoride
c)
Selenium tetraflouride
d)
Selenium (IV) Fluoride
81.
P2O5
a)
Phosphorus Oxide
b)
Pentaphosphorus Dioxide
c)
Diphosphorous pentoxide
d)
Phosphoric Oxygen
82.
Name Al2S3
a)
Aluminum sulfide
b)
Dialuminum trisulfide
c)
ammonium sulfide
d)
aluminum (II) sulfice
83.
Identify the phosphide ion
a)
P5+
b)
P3+
c)
P3-
d)
P4-
84.
Name the compound NH4OH
a)
ammonium hydroxide
b)
ammonia oxyhydride
c)
mononitrogen tetraoxihydride
d)
hydrogen nitrate
85.
What is the formula for lead (II) carbonate?
a)
PbCO3
b)
Pb2CO3
c)
Pb(CO3)2
d)
Pb(CO)4
86.
What is the metallic ion in the compound CuCl?
a)
Cu1+
b)
Cu2+
c)
Cu1-
d)
Cu2-
87.
What is the formula for aluminum sulfite?
a)
Al3S2
b)
AlSO4
c)
Al3(SO4)2
d)
Al2(SO3)3
88.
What is the formula for tin (II) chromate 
a)
Sn2(CrO4)4
b)
Sn(CrO4)2
c)
Sn4(CrO4)2
d)
SnCrO4
89.
What is the formula for barium hydride?
a)
BaOH2
b)
Ba(OH)2
c)
BaH2
d)
BaOH
90.
Name the compound Fe(NO2)3
a)
iron nitrite
b)
iron (III) nitrate
c)
iron (III) nitrite
d)
ferric nitrite
91.
Name the compound NO3
a)
nitrogen trioxide
b)
nitrate
c)
nitrite
d)
dinitrogen pentoxide
92.
Name the compound CuO
a)
copper (II) oxide
b)
copper oxide
c)
copper (I) oxide
d)
carbon uranium oxide
93.

WHAT'S THE NAME FOR P2O4?

a)

PHOSPHORUS OXIDE

b)

PHOSPHORUS(II) OXIDE

c)

DIPHOSPHORUS TETROXIDE

d)

DIPHOSPHORUS TETROXYGEN

94.

WHAT IS THE NAME FOR Sr3N2?

a)

STRONTIUM NITRIDE

b)

TRISTRONTIUM DINITRIDE

c)

STRONTIUM(III) NITRIDE

d)

STRONTIUM NITRATE

95.

WHAT IS THE NAME FOR XeF4?

a)

XENON FLUORIDE

b)

XENON(IV) TETRAFLUORIDE

c)

XENON TETRAFLUORINE

d)

XENON TETRAFLUORIDE

96.

WHAT IS THE FORMULA FOR TRIPHOSPHORUS HEXASULFIDE?

a)

P3(SO3)6

b)

P3S6

c)

P3SO

d)

P3SO6

97.

WHAT IS THE FORMULA FOR DINITROGEN PENTASULFIDE?

a)

N2SO5

b)

N2(SO4)5

c)

N2S5

d)

N2S(O)5

98.
The chemical formula for an ionic compound of potassium and oxygen is
a)
KO.
b)
K2O.
c)
K2O2.
d)
KO2.
99.
What formula results when Ca+2  and  Br- ions bond?
a)
Ca2Br2
b)
CaBr
c)
Ca(br)2
d)
CaBr2
100.
If an element has 3 valence electrons, what charge will likely form on its ion ?
a)
+3
b)
+5
c)
-3
d)
-5
101.

Hector claims that a single sodium ion and a single oxygen ion do not bond together to form a stable binary ionic compound. Is he correct? Why or why not?

a)

Hector is incorrect. The two ions have opposite charges, so they will bond together in a binary ionic compound.

b)

Hector is incorrect. The two ions have more than eighteen protons, so they will bond together in a binary ionic compound.

c)

Hector is correct. The sum of the charges of the two ions must be zero in order for them to form a stable ionic compound.

d)

Hector is correct. The sum of the protons of the two ions must be divisible by eight in order for them to form a stable ionic compound.

102.

Potassium (K), an alkali metal, and magnesium (Mg), an alkaline earth metal, both combine readily with bromine (Br), a halogen. What compound will each element (K and Mg) most likely form with bromine?

a)

KBr and Mg2Br

b)

KBr and MgBr

c)

K2Br and Mg2Br

d)

KBr and MgBr2

103.

Unknown element W has 2 valence electrons. Unknown element X has 7 valence electrons. Which formula shows the most likely outcome when elements W and X react?

a)

WX

b)

WX2

c)

W2X

d)

W2X2

104.

Which of the following have a possible 4+ charge?

a)

Silver

b)

Manganese

c)

Cobalt

d)

Tin

105.

Which of the have a possible 1+ charge?

a)

Copper

b)

Iron

c)

Manganese

d)

Nickel

106.

Which of the have a possible 3+ charge?

a)

Zinc

b)

Silver

c)

Mercury

d)

Gold

107.

Which elements both of the have a possible 3+ charge?

a)

Silver and Gold

b)

Copper and Iron

c)

Chromium and Cobalt

d)

Iron and Tin

108.

What are the possible charges of Gold?

a)

Au+ and Au3+

b)

Au2+ and Au3+

c)

Au+ and Au2+

d)

Au2+ and Au4+

109.

What are the possible charges of Tin?

a)

Sn+ and Sn3+

b)

Sn2+ and Sn4+

c)

Sn2+ and Sn3+

d)

Sn+ and Sn2+

110.

What are the possible charges of copper?

a)

Cu+ and Cu2+

b)

Cu+ and Cu3+

c)

Cu+ and Cu4+

d)

Cu2+ and Cu3+

111.

What are the possible charges of mercury?

a)

Hg+ and Hg2+

b)

Hg2+ and Hg3+

c)

Hg+ and Hg4+

d)

Hg3+ and Hg4+

112.

What are the possible charges of iron?

a)

Fe+ and Fe2+

b)

Fe2+ and Fe3+

c)

Fe3+ and Fe4+

d)

Fe+ and Fe3+

113.

What are the possible charges for Nickel?

a)

Ni2+ and Ni3+

b)

Ni+ and Ni3+

c)

Ni2+ and Ni4+

d)

Ni3+ and Ni4+

114.

What are the possible charges for chromium?

a)

Cr2+ and Cr3+

b)

Cr+ and Cr3+

c)

Cr2+ and Cr4+

d)

Cr2+ and Cr4+

115.

What is the possible charge of zinc?

a)

Zn2+

b)

Zn+

c)

Zn3+

d)

Zn4+

116.
NH4+
a)
nitrogen hydride
b)
ammonium
117.
CN-
a)
cyanide
b)
carbon nitride
118.
SO42-
a)
sulfate
b)
sulfite
119.
PO43-
a)
phosphate
b)
phosphorus oxide
120.
CO32-
a)
carbon oxide
b)
carbonate
121.
C2H3O2-
a)
acetate
b)
carbon hydroxide
122.
The elements on the left side of the periodic table are generally always ______ and the elements on the right side of the periodic table are generally always ______.
a)
cations; anions
b)
anions; cations
c)
reactive; non-reactive
d)
non-reactive; reactive
123.

Which of the following is nitrate?

a)

NO-

b)

NO2-

c)

NO3-

d)

NO4-

124.

Which of the following is sulfate?

a)

S2O3-2

b)

O2-2

c)

SO4-2

d)

SO3-2

125.
Ammonium and oxygen would combine to form:
a)
(NH4)2O
b)
NH4O2
c)
(NH4)O2
d)
NH6O3
126.
Name the acid: HC2H3O2
a)
Acetic Acid
b)
Acetous Acid
c)
Hydrogen Acetate
d)
Hydrogen Dicarbon Trihydrogen Dioxygen
127.
What is the formula for Hydrosulfuric Acid?
a)
H2(SO3)
b)
H2S
c)
H2(SO2)
d)
H2(SO4)
128.
Name the acid: H3PO3
a)
hydrophosphoric acid
b)
phosphorous acid
c)
phosphoric acid
d)
phosphoric hydroxide
129.
HNO2
a)
hydronitrogen
b)
hydrogen nitrogen oxygen
c)
nitrous acid
d)
nitric acid
130.
carbonic acid
a)
H2CO3
b)
H2CrO4
c)
H2C2O4
d)
HCO3
131.
chlorous acid
a)
HClO3
b)
HClO2
c)
HClO
d)
HCl
132.

When naming oxyacids, change "-ite" to:

a)

-ate

b)

-ic

c)

-ous

d)

-ite

133.

When naming oxyacids, change "-ate" to:

a)

-ate

b)

-ic

c)

-ous

d)

-ite

134.
What is the name of this compound:  N2O5
a)
Nitrogen Oxide
b)
Dinitrogen pentaoxide
c)
Nitrate pentaoxide
d)
Dinitrate pentaoxide
135.
What is the name of HI? 
a)
iodic acid
b)
hydroiodic acid
c)
iodous acid
d)
hypoiodous acid
136.
What element do all acids contain?
a)
H
b)
O
c)
C
d)
He
137.
What is the formula for perchloric acid?
a)
H3ClO3
b)
H3ClO4
c)
HClO3
d)
HClO4
138.
H2C2O4
a)
carbonic acid
b)
chromic acid
c)
chloric acid
d)
oxalic acid
139.

What is the name of HCN?

a)

Hydrogen cyanide acid

b)

Hydrocyanide acid

c)

Hydrocyanic acid

d)

cyanic acid

140.
How many atoms of iodine are in a mole of iodine?
a)
53
b)
63.55g
c)
126.9
d)
6.02 x 1023
141.
The number 6.02 x 1023 is called...
a)
Obama's number
b)
Bohr's number
c)
Trump's number
d)
Avogadro's number
142.
What is the mass of 0.75 moles of (NH4)3PO4?
a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g
143.
How many particles would be in 8.4 moles of Octane (C8H18)?
a)
5.77 x 1023
b)
5.04 x 1024
c)
5.77 x 1026
d)
5.04 x 1023
144.
Which has more molecules?
a)
1 mole H2O
b)
1 mole Al(OH)3
c)
1 mole NaCl
d)
There are all the same
145.
What is the mass of 54.3x1045molecules of BeO?
a)
3.27x1070 g
b)
9.01 x1022g
c)
2.25 x1024 g
d)
1.31 x1069g
146.
The molar mass of an element is equal to its...
a)
Atomic mass
b)
Atomic number
c)
Oxidation number
d)
Valence electrons
147.
What is the mass of one mole of aluminum chloride (remember to determine the correct formula first)?
a)
62.435g
b)
116.399g
c)
133.341g
d)
97.888g
148.

Carbon monoxide, a deadly gas, has a chemical formula of CO (one carbon atom with one oxygen atom). If you look at the total atomic mass of CO, does carbon or oxygen make up more of the mass?

a)

carbon

b)

oxygen

c)

they are exactly the same

d)

it is impossible to tell

149.

What percentage of the total atomic mass of magnesium bromide (MgBr2) is composed of magnesium?

a)

13%

b)

43%

c)

63%

d)

87%

150.

What percentage of the total atomic mass of magnesium bromide (MgBr2) is composed of bromine? Hint - consider the mass of both atoms of bromine in your calculation.

a)

13%

b)

43%

c)

63%

d)

87%

151.

What percentage of the total atomic mass of calcium nitrate (Ca(NO3)2) is composed of nitrogen? Hint - another way to think of calcium nitrate is Ca(NO3)(NO3).

a)

17%

b)

24%

c)

29%

d)

59%

152.

What is the percent by mass of oxygen in MgO? Hint: The attached image is an example of a worked problem other than this one.

a)

20%

b)

40%

c)

50%

d)

60%

153.
What is the percent by mass of fluorine in CaF2 (gram-formula mass = 78 g/mol)?
a)
24%
b)
49%
c)
51%
d)
65%
154.
What is the percent composition by mass of sulfur in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
155.
In which compound is the percent composition by mass of Cl equal to 42%?
a)
HClO (gram formula mass = 52 g/mol)
b)
HClO2 (gram formula mass = 68 g/mol)
c)
HClO3 (gram formula mass = 84 g/mol)
d)
HClO4 (gram formula mass = 100 g/mol)
156.
What is the empirical formula for the following:
Pb5Cr5O20
a)
Pb2Cr2O10
b)
PbCr2O7
c)
Pb9Cr4O2
d)
PbCrO4
157.

Which element has an abundance of 39.03% in the compound sodium phosphate, Na3PO4

a)

Na

b)

P

c)

O

d)

None of the above

158.

How close a set of measurements are to each other...

a)

accuracy

b)

precision

c)

% error

d)

luminous intensity

159.

How close a measurement is to the accepted value...

a)

accuracy

b)

precision

c)

electric current

d)

adaptability

160.

SI base unit for electric current:

a)

candela

b)

kilogram

c)

ampere

d)

mole

161.

SI base unit for mass:

a)

gram

b)

kilogram

c)

pound

d)

newton

162.

A substance has a mass of 400 grams and a volume of 100 mL. What is the density in g/mL?

a)

40000

b)

.25

c)

4

d)

40

163.

What can be calculated by comparing the accuracy of an experimental measurement to the accepted value?

a)

percent composition

b)

percent error

c)

percent daily value

d)

percent by mass

164.

How many significant digits: 405 m

a)

1

b)

2

c)

3

d)

4

165.

How many significant digits: .0090 mL

a)

1

b)

2

c)

3

d)

4

166.

How many significant digits: 10.01 kg

a)

1

b)

2

c)

3

d)

4

167.

How many sig figs allowed in the answer...Volume of a box with a length of 10 meters, width 456 meters, height 35 meters?

a)

1

b)

2

c)

3

d)

4

168.

How many decimal places allowed in the answer...Perimeter of a triangle with sides of 5.444 cm, 6.02 cm, and 5.9857 cm?

a)

0

b)

1

c)

2

d)

3

e)

4

169.

25 mL = ________ cm3

a)

25000

b)

2500

c)

250

d)

25

170.

1 dm3 = _________ cm3

a)

1

b)

10

c)

100

d)

1000

171.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
172.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.
a)
SO
b)
SO2
c)
SO3
d)
SO4
173.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
174.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
175.

2.40 g of an explosive, J, contains 0.473 g of nitrogen. J also contains 33.8% carbon and 1.41% hydrogen by mass. The remainder of J is oxygen.


What is the empirical formula of J?

a)

C4HNO2

b)

CH2N2O

c)

C2HNO2

d)

CHNO

176.
What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?
a)
CH2O
b)
C2H4O2
c)
C4H8O4
d)
C6H12O6
177.
What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.
a)
K2SO4 
b)
K8SO16
c)
K8S4O8 
d)
K8S4O16 
178.
When calculating the EF the mole ratio is given as follows:
H1O3.5
What will the EF be?
a)
H1O3.5
b)
HO3.5
c)
HO4
d)
H2O7
179.
Which of the following shows the correct way to balance the chemical equation?
Fe + O2 -> Fe2O3
a)
4Fe + 3O2 -> 2Fe2O3
b)
2 Fe + 3O2 -> Fe2O6
c)
4 Fe + O6 -> 2Fe2O3
d)
None of the options are correctly balanced.
180.
Which of the following reactions is balanced?
a)
2CH4 + O2 -> CO2 + H2O
b)
CH4 + 2O2 -> CO2 + H2O
c)
CH4 + 2O2 -> CO2 + 2H2O
d)
None of the chemical equations are balanced.
181.
Balance this equation.
_CF4 + _Br2 -- _CBr4 + _F2
a)
2,1,2,1
b)
1,2,2,1
c)
1,2,1,2
d)
2,2,2,2
182.
Balance this equation
_Al +_HCl --> _H2 +_AlCl3
a)
2, 6, 3, 2
b)
it is already balanced
c)
4, 12, 3, 4
d)
2, 1, 4, 5
183.
In chemical reactions, what does the principle of conservation of mass mean?
a)
Matter is not created or destroyed.
b)
The total mass of the reactants is greater than the total mass of the products.
c)
The total mass of the reactants is less than the total mass of the products.
d)
Matter is not changed.
184.

What law governs the balancing of chemical equations?

a)

Law of Energy

b)

Law of Conservation of Matter/Mass

c)

Law of Gravity

d)

Law of Matter Movement

185.
Which of the following equations are correctly balanced?
a)
12CO2 +H2O --> C6H12O6 + O2
b)
CO2 + 9H2O --> C6H12O6 + O2
c)
CO2 + H2O --> 3C6H12O6 + O2
d)
6CO2 + 6H2O --> C6H12O6 + 6O2
186.

Balance the following equation:

___ SeCl6+ ___ O2→___ SeO2+____Cl2

a)

1, 1, 1, 3

b)

2, 1, 2, 1

c)

1, 2, 1, 2

d)

2, 2, 2, 4

187.
A sealed test tube containing 8 grams of iron filings and 5 grams of sulfur is heated until the material in the test tube glows bright red.  What is the mass of products? 
a)
Mass is less than 13 grams
b)
Mass is equal to 13 grams
c)
Mass is greater than 13 grams
d)
Mass cannot be measured
188.

Which type of reaction is:

C7H16 + 10 O2 → 7 CO2 + 8 H2O

a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Combustion
189.

Which type of reaction is:

3 Pb + 2 H3PO4 → 3 H2 + Pb3(PO4)2

a)
Synthesis
b)
Single Displacement
c)
Double Displacement
d)
Combustion
190.
The following reaction is an example of what reaction type? 
CoCO3 → CoO + CO2
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
191.

In decomposition reactions, for compounds with ions, most anions decompose into what? What is the exception that produces CO2 gas?

a)

the individual elements; ClO3 1-

b)

Oxygen (O2) gas; CO3 2-

c)

they remain anions; CO3 2-

192.

In single displacement, if A is a metal how does the example equation go?

a)

A + BC-> B +AC

b)

A + BC-> C +BA

c)

A + BC-> AC + B

193.

Which elements from the activity series displace hydrogen from cold water, steam, and acids? (Page 167 in textbook)

a)

K, Ca, Na

b)

H, Cl, I

c)

O, F, Ne

d)

Br, Li, Ar

194.

What elements from the activity series displace hydrogen from steam and acids? (page 167 in textbook)

a)

K, Ca, Na

b)

Mg, Al, Zn, Fe

c)

Cl, I, Br

d)

H, Ag, Hg, Sn

195.

What elements from the activity series displace hydrogen only from acids? (page 167 in textbook)

a)

H, Ag, N, O

b)

Cl, Fe, S

c)

Cu, Al, Br

d)

Ni, Sn, Pb

196.

What elements from the activity series do not displace hydrogen? (page 167 in textbook)

a)

Cu, Ag, Hg, Au

b)

I, Zn, F, Fe

c)

Cu, Pb, Al, Mg

d)

K, Cl, Br, Na

197.

Evidence of a double displacement reaction are... (mark all that apply)

a)

gas

b)

heat

c)

precipitate

d)

water

e)

both reactants are aqueous

198.

exothermic reactions...

a)

release heat

b)

absorb heat

c)

have energy as a product

d)

have energy as a product

199.

endothermic reactions...

a)

absorb heat

b)

have energy as a product

c)

release heat

d)

have energy as a reactant

200.

C3H8 +5O2->3CO2 + 4H2O + energy

a)

is a combustion reaction

b)

is single displacement

c)

is analysis

d)

is a double displacement reaction

201.

HCl + NaOH-> NaCl + H2O

a)

is a neutralization reaction

b)

is a combustion reaction

c)

is a double displacement reaction

d)

is single displacement

202.

One of Dalton's three laws is the law of (a)  

203.

Dissassociation is (a)  

204.

sublimation is (a)  

205.

Who discovered the electron?

(a)  

206.

who created the charge to mass ratio?

(a)  

207.

What were electrons called before they were called electrons and by who?

a)

corpuscules

b)

particles

c)

J. J. Thomson

d)

William Crookes

208.

In alpha decay elements....

a)

lose two electrons and 2 neutrons

b)

gain 3 electrons and 3 neutrons

c)

lose two protons and 2 neutrons

d)

gain 3 protons and 3 neutrons

209.

Who did the goldfoil experiment?

a)

Ernest Rutherford

b)

Niels Bohr

c)

J.J. Thomson

d)

Erwin Schrödinger

210.

Who created the plum pudding model?

a)

John Dalton (1803)

b)

J. J. Thomson (1904)

c)

Niels Bohr (1913)

d)

Ernest Rutherford (1911)

211.

who created the billiard ball model?

a)

John Dalton (1803)

b)

Ernest Rutherford (1911)

c)

J.J. Thomson (1904)

d)

Niels Bohr(1913)

212.

Who discovered the mass of the electron?

a)

Robert Milikan

b)

Ernest Rutherford

c)

J.J. Thomson

d)

George Stoney

213.

who named the electron the "electron"?

a)

George Stoney

b)

Robert Millikan

c)

J. J. Thomson

d)

William Crookes

214.

_____ ____ is called the "Father of Quantum Mechanics"

(a)  

215.

Who created the nuclear model?

a)

J. J. Thomson (1904)

b)

Ernest Rutherford (1911)

c)

Niels Bohr (1913)

d)

Erwin Schrödinger (1926)

216.

Who created the planetary model?

a)

Niels Bohr (1913)

b)

Ernest Rutherford (1911)

c)

Erwin Schrödinger (1926)

d)

J. J. Thomson (1904)

217.

Who created the Quantum model?

a)

Erwin Schrödinger (1926)

b)

J. J. thomson (1904)

c)

Niels Bohr (1913)

d)

Ernest Rutherford (1911)

218.

What is this: "It is impossible to know both the exact location and velocity of an electron at the same time"

a)

Heisenberg Uncertainty principle

b)

Pauli exclusion principle

c)

Hund's rule of maximum multiplicity

219.

What is this: "only two electrons can exist in an orbital at a time"

a)

Pauli exclusion principle

b)

Hund's rule of maximum multiplicity

c)

Heisenberg Uncertainty principle

220.

What is this: "...electron pairing in p, d and f orbitals cannot occur until each orbital of a given subshell contains one electron each or is singly occupied."

a)

Hund's rule of maximum multiplicity

b)

pauli exclusion principle

c)

Heisenberg uncertainty principle

221.

Name this SCN 1-

(a)  

222.

The traditional naming system uses ________ and the stock naming system uses _____ numerals and ___________

(a)  

223.

Per ____ one oxygen to the -ate root and Hypo _________ one oxygen from the -ite root

a)

adds, subtracts

b)

subtracts, adds

c)

gives, takes

d)

takes, gives

224.

The mass of an element or compound in grams which contains Avogadro's number of particles is the _____ ____

(a)  

225.

STP stands for

a)

standard temperature pressure

b)

specialized transcription postulate

c)

sub total points

226.

1 mol of any gas at STP will occupy a volume of?

a)

4L

b)

24 mL

c)

22.4L

d)

444mL

227.

The smallest whole number ratio of atoms in a compound is the _________ _______

(a)  

228.

The actual formula of a covalent compound or the total # of atoms in one formula unit of the compound is the _________ _______

(a)  

229.

T or F: Compounds with the same empirical formula have the same percent composition

a)

true

b)

false

230.

T or F: ionic compounds are usually solids

a)

false

b)

true

231.

total mass of substances in a reaction remains constant is the law of (a)  

232.

metal plus acid yields...

(a)  

233.

metal plus water yields...

(a)  

234.

metal or halogen plus salt yields

(a)  

235.

acid plus base yields

(a)  

236.

T or F: solid metal oxide and acid can perform a double displacement reaction

a)

true

b)

false

237.

The energy needed to remove electrons from atoms is called the __________ ______

(a)  

238.

The measure of how strongly an atom attracts a pair of electrons in a chemical bond is (a)  

239.

Tor F: anions have a smaller radius than the radius of the neutral form of the same element

a)

true, it's smaller

b)

false, it's larger

240.

T or F:cations have a smaller radius than the radius of the neutral form of the same element

a)

true, it's smaller

b)

false, it's larger

241.

T or F:when metals make covalent bonds they almost always end up short on electrons

a)

true

b)

false

242.

T or F: when several nonmetals in a compound, the lowest electronegativity is usually in the middle of the lewis structure

a)

true

b)

false

243.

T or F: if carbon exists in a compound it is never in the middle of a lewis structure

a)

false, it's usually in the middle

b)

true, it is never in the middle

244.

VSEPR stands for

(a)  

245.

quantitative relationships between products and reactant in chemical reactions is (a)  

246.

Ratio between any two species in a chemical reaction is ____ _____

(a)  

247.

calculated amount of product that can be obtained from a given amount of a reactant is ________ _____

(a)  

248.

amount of product actually obtained in reaction is _______ _____

(a)  

249.

T or F: to find percent yield you use actual yield over theoretical yield times 100

a)

true

b)

false

250.

the chemical bond between opposite charge ions is (a)  

251.

T or F: a formula unit has a polar structure and a negative charge of 1

a)

true the formula unit is created and there is a negative charge of 1

b)

false, the formula unit is created but the charge is 0

c)

false a formula unit is not creates

252.

T or F: polyatomic ions usually have 3 or 4 cations to 2 anions

a)

true, it is 3 or 4 cations for 2 anions

b)

false, it is usually 1 or 2 cations for one anion

253.

the chemical bond formed by 2 atoms sharing electrons is (a)  

254.

T or F: in a covalent bond the sharing of electrons can be equal or not equal depending on the atoms' electronegativity

a)

true

b)

false

255.

T or F: δ+ stand for slightly negative

a)

false

b)

true

256.

T or F: δ− stands for slightly negative

a)

false

b)

true

257.

T or F: as the difference between electronegativity decreases, the bond becomes less covalent

a)

true, it is less covalent

b)

false, it is more covalent

258.

T or F: Hydrogen bonds are not permanent, break and reform constantly, occur only between atoms, occurs between any atoms

a)

false, hydrogen bonds only occur between molecules and only occur w/molecules that have highly electronegative atoms

b)

true, Hydrogen bonds are not permanent, break and reform constantly, occur only between atoms, occurs between any atoms

259.

4.0 mol of H2 and 3.5 mol Cl2 are reacted (H2 plus Cl2-> 2HCl), which compound is the limiting reactant?

a)

H2

b)

Cl2

260.

What speed (in a vacuum) does all electromagnetic radiation travel at?

a)

3.00 x10^8 m/s

b)

2.00 X 10^5 m/s

c)

4.00 x10^6 m/s

d)

1.37 X10^9 m/s

261.

(Mark all that apply) electromagnetic waves have three basic characteristics

a)

wavelength-the distance between consecutive peaks

b)

density- tells how much of the wave exists in the given space

c)

frequency-tells how many waves pass a particular point per second

d)

speed-tells how fast a wave moves through space

262.

A minute energy packet of electromagnetic radiation is a (a)  

263.

You should

a)

take the chapter 10 and labs quiz

b)

not study and fail chem

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