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Midterm Review Units 1-7

Total questions: 150

Worksheet time: 2hrs 19mins

Name
Class
Date
1.
A mixture that is NOT evenly distributed is called ....
a)
Compounded
b)
Homogenous
c)
Heterogenous
d)
Salty
2.
What kind of properties can only be observed when a substance changes into a different substance?
a)
physical properties
b)
chemical properties
3.
Example for chemical property
a)
malleability
b)
texture
c)
combustion
d)
sour taste
4.
Isotopes of the same element have different ____________. 
a)
 numbers of protons  
b)
numbers of electrons
c)
 symbols 
d)
numbers of neutrons
5.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
6.

When compared, a mole of carbon and a mole of sulfur, how many atoms each has?

a)

carbon has 12.01 grams of atoms

b)

sulfur has 32.06 grams of atoms

c)

both contains 6.02 x 1023 atoms

d)

need more information

7.
What is the name of this element?
a)
Lithium
b)
Boron
c)
Carbon
d)
Neon
8.

When can atoms emit photons?

a)

When the electron is in the ground state

b)

When the electron is in the excited state

c)

When an electron is going from the ground state to the excited state

d)

When an electron is going from the excited state to the ground state

9.
What did Bohr add to the model of the atom?
a)
electrons found in specific orbits around nucleus 
b)
 electrons found in nucleus
c)
discovered electron
d)
neutrons found in nucleus
10.

What is the goal of the Lewis Dot Structure?

a)

To determine the electron position.

b)

To show the element's valence electrons & bonding capabilities.

c)

To find the atomic mass of an element.

d)

To search for the number of electrons in an individual atom.

11.
Ionic bonds form between metals and ____.
a)
metalloids
b)
metals
c)
nonmetals
12.
Which three nonmetals exist only as diatomic molecules?
a)
H, C, Br
b)
N, O, S
c)
I, F,N
d)
H, O, P
13.
The red numbers in the image below represent ________
a)
subscripts
b)
coefficients
c)
I don't know, and don't want to try
d)
None of the answers are correct
14.

4Ag + O2 --> ___Ag2O

a)

1

b)

2

c)

3

d)

4

15.
How would you describe reactivity on the periodic table?
a)
Elements in the same group are most likely to react.
b)
Elements in the same Periodic are most likely to react.
c)
Elements on opposite sides of the Periodic Table are most likely to react.
d)
There is no trend of reactivity.
16.

An element with the lowest electronegativity would be found in of the periodic table.

a)

Group 1, Period 7

b)

Group 3, Period 4

c)

Group 5, Period 3

d)

Group 17, Period 2

17.
Which conversion factor should be used to solve the following, "Find the mass in grams of 2.00 x 1023 molecules of F2."
a)
1 mol = 22.4 L 
b)
1 mol = 38.00 g
c)
1 mol = 6.02x1023 atoms
d)
more than one
18.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)  
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
19.
in a reaction, aqueous barium chloride reacts with aqueous potassium carbonate to produce solid barium carbonate and aqueous potassium chloride. what is the correct balanced equation.
a)
Ba2Cl(aq) + KCO3(aq) --> BaCO3(s) + KCl(aq)
b)
BaCl2(aq) + K2CO3(aq) --> BaCO3(s) + 2KCl(aq)
c)
BaCl(aq) + K2CO3(aq) --> BaCO3(s) + K2Cl(aq)
d)
Ba2Cl2(aq) + KCO3(aq) --> Ba2CO3(s) + KCl2(aq)
20.
If Nitrogen and Silver chemically bond, which will be named first?
a)
Silver
b)
Nitrogen
c)
Unknown
d)
Iodine
21.
How do the following two elements bond together?
Pb4+  O2-       
a)
PbO
b)
Pb2O3
c)
PbO2
d)
Pb3O2
22.
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
23.

A student measures the pressure and volume of an empty water bottle to be 1.4 atm and 2.3 L. She then decreases the pressure to 0.65 atm. What is the new volume?

a)

2.1 L

b)

5.0 L

c)

8.2 L

d)

3.9 L

24.
Which of the following is NOT a value for standard pressure?
a)
101.3 kPa
b)
760 mm Hg
c)
1 atm
d)
1 torr
25.
A gas of volume V is placed in a balloon.  Determine the new volume of the balloon if the pressure is tripled. The new volume will be ____ what it was originally.  
a)
1/3 of
b)
1/6 of
c)
1/9 of
d)
 9 times
26.

Which travels faster? CO2 or Ar?

a)

CO2

b)

Ar

27.
A compound reactant splits up to make 2 or more new products.
a)
Syntheiss
b)
Decomposition
c)
Double Replacement
d)
Single Replacement
28.

Which energy state has more energy?

a)

Ground State

b)

Excited State

29.
The atomic number of an atom or ion refers to the number of:
a)
neutrons
b)
protons
c)
nucleons
d)
electrons
30.
Are made from a combination of 2 or more elements in a constant ratio...
a)
Atome
b)
Mixture
c)
Compounds
d)
Elements
31.

How much faster will He(g) travel than O2(g)?

a)

4 times faster

b)

2.8 times faster

c)

0.35 times faster

d)

0.125 times faster

32.
The blue numbers in the image below represent ________
a)
I don't know, and don't want to try
b)
coefficients
c)
subscripts
d)
none of the answers are correct
33.
Why did the alpha particle (positively charged particle) sometimes bounce back when hitting the gold foil.
a)
hit neutron in nucleus and they repelled alpha particle
b)
hit proton in nucleus and they repelled alpha particle
c)
hit electrons in electron shells and they repelled alpha particle
34.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
35.
Properties that can be observed without changing the identity of the substance.
a)
Physical
b)
Chemical
36.
A bar of copper has a mass of 216g and a volume of 24cm3. What is the density of copper?  
a)
9g/cm3
b)
.11g/cm3
c)
5184g/cm3
d)
322mL
37.
Which of the following is the correct formula for Cesium sulfate?
a)
CsS2
b)
Cs(SO4)2
c)
Cs2SO4
d)
Cs2S
38.
Which container will have a lower pressure?
a)
left
b)
right
c)
they both have the same pressure
d)
I don't know
39.
What units can be used to express density?
a)
g/mL
b)
grams
c)
millimeters
d)
milliliters
40.
How many electrons does potassium K contain? (click to see image)
a)
19
b)
39
c)
20
d)
40
41.
A molecule with a double covalent bond is....
a)
HCl
b)
SO
c)
I2
d)
N2
42.

How many molecules of water are in a 821.3 g sample?

a)

45.58 molecules

b)

8.232 x 1025 molecules

c)

8.909 x 1027 molecules

d)

2.744 x 1025 molecules

43.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
44.
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
45.

Usuing Graham's Law: If you had 2 identical balloons filled with Nitrogen gas (N2) and Helium gas (He), which balloon will deflate the fastest?

a)

Helium balloon

b)

nitrogen balloon

c)

they will both deflate at the same rate

d)

the balloons will both pop

46.
Example for chemical property
a)
color
b)
hardness
c)
toxicity
d)
solubility
47.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
48.

Rutherford discovered what through his experimentation?

a)

The nucleus

b)

The orbitals

c)

The electron

d)

The quark

49.

A water bottle at STP is cooled to -155°C. What is the new pressure?

a)

3.2 atm

b)

0.43 atm

c)

1.8 atm

d)

0.27 atm

50.
In Charles' Law the pressure remains constant.
a)
True
b)
False
51.
Which of the following describes covalent bonds?
a)
Bonds form because of opposite charges
b)
Bonds form to fill outer electron shells
c)
Electrons are transferred between atoms
d)
Covalent bonds are magical
52.
Where are the nonmetals on the Periodic Table?
a)
To the left
b)
In the upper right hand corner
c)
On the zigzag line
d)
At the bottom
53.
Which of the following dimensional analysis setups will correctly convert 27.76g of Li to atoms of Li?
a)
A
b)
B
c)
C
d)
D
54.

A 5.018 gram sample of a certain hydrate of magnesium sulfate, MgSO4•xH2O, is heated until all the water is driven off. The resulting anhydrous compound weighs 2.449 grams. What is the formula of the hydrate?

a)

MgSO4•9H2O

b)

MgSO4•8H2O

c)

MgSO4•7H2O

d)

MgSO4•6H2O

55.

If an atom has no charge, which of the following must be true?

a)

It has more neutrons than protons or electrons.

b)

There are only neutrons inside the atom.

c)

Its number of protons is equal to its number of electrons.

d)

The neutrons in the atom outnumber the electrons and protons.

56.
What is the mass of 3.01 x 1022 atoms of magnesium?
a)

1.22 grams

b)

0.0500 grams

c)


4.41x10474.41x10^{47} grams

d)

3.22x1046 grams

57.

___AlBr3 + 3Cl2 --> 2AlCl3 + 3Br2

a)

1

b)

2

c)

3

d)

4

58.
2H2  +   O2  →  2H2O
How many moles of oxygen are consumed if 8 moles H2 are used?
a)
2
b)
4
c)
6
d)
8
59.
What is the formula for Copper (III) fluoride?
a)
Cu3F
b)
CuF3
c)
Cu3F3
d)
Cu2F3
60.
An element with five valence electrons is
a)
phosphorus
b)
oxygen
c)
beryllium
d)
rubidium
61.

What is happening in the picture

a)

An atom is absorbing energy to go to a higher state

b)

An atom is emitting a photon to go to a lower state

c)

The atom is losing an electron

d)

The atom is losing a proton

62.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
63.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
64.

Which of the following is NOT a property of ionic compounds?

a)

They conduct electricity when molten

b)

They conduct electricity when in solution

c)

They have high boiling points

d)

They are insoluble in water

65.
Which of the following is a characteristic property of ionic compounds?
a)
They form hard, brittle crystals with characteristic shapes
b)
They have low melting points
c)
They have low boiling points
d)
They contain no charged particles
66.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
None
d)
conduct electricity
67.

Which of the compounds below contains a single covalent bond?

a)

A. Br2

b)

B. SO

c)

C. HCl

d)

Both a and c

68.

Which is stronger...

a)

N − N

b)

N = N

c)

N ≡ N

69.

What is the volume of a balloon that contains 3.7 moles of helium at 75°C and 5.1 atm?

a)

37 L

b)

13 L

c)

45 L

d)

21 L

70.
When an atom loses an electron, it becomes a:
a)
positive ion
b)
negative ion
c)
neutral ion
d)
neutral atom
71.
Why did the alpha particle (positively charged particle) sometimes bounce back when hitting the gold foil.
a)
hit neutron in nucleus and they repelled alpha particle
b)
hit proton in nucleus and they repelled alpha particle
c)
hit electrons in electron shells and they repelled alpha particle
72.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
73.
Which expression below show the correct method of determining the percent composition of Sodium in Na2CO3?
a)
%Na = (22.99g/106g) x 100
b)
%Na = (22.99g/106) / 100
c)
%Na = (45.98g/106g) x 100
d)
%Na = (106/45.98g) x 100
74.

What would be the mass of 9.76 x 1022 formula units of SrCl2?

a)

.1622 g

b)

25.7 g

c)

20.0 g

d)

.3589 g

75.
Which of the following would increase the (gas) pressure of a system?
a)
Increase the Temperature
b)
Pump in more gas
c)
Decrease the volume
d)
All of these
76.

What is the pressure of a car tire that had an initial pressure of 1.8 atm but was heated from 38°C to 123°C?

a)

0.9 atm

b)

2.1 atm

c)

1.6 atm

d)

3.4 atm

77.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
78.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
79.
What is the name for FeO?
a)
Iron oxide
b)
Iron monoxide
c)
Iron (II) oxide
d)
Iron (III) oxide
80.
Which group of elements are most likely to need a Roman numeral in an ionic compound name?
a)
alkaline earth metals
b)
transition metals
c)
halogens
d)
noble gases
81.

Predict the products for the this reaction: [Ag has an oxidation number of 1+]

Ag3N + KCl →

a)

AgCl + K3N

b)

AgK + ClN3

c)

AgN3 + KCl

d)

KAg + N3Cl

82.

What are the products for this reaction:
C2H4 + 2 O2 -->

a)

C2O2 + H4

b)

CO2 + HOH

c)

CO + H

d)

2 CO2 + 2H2O

83.

What is the mass of one mole of silver?

a)

32.06 g

b)

107.87 g

c)

14.01 g

d)

22.99 g

84.

Across a period in the periodic table, atomic radii generally

a)

decrease

b)

decrease, then increase.

c)

increase.

d)

increase, then decrease.

85.
What is the name of Groups 17?
a)
Alkali Metals
b)
Alkali Earth Metals
c)
Transition Metals
d)
Halogens
86.
Where are the metals on the Periodic Table?
a)
To the left
b)
In the upper right hand corner
c)
On the zigzag line
d)
At the bottom
87.
When two reactant compounds switch partners to make two new products.
a)
Syntheiss
b)
Decomposition
c)
Double Replacement
d)
Single Replacement
88.
 H2 + 2O2  -->  2H2O 
a)
Syntheiss
b)
Decomposition
c)
Double Replacement
d)
Single Replacement
89.
Polar, nonpolar, or ionic?
a)
Nonpolar
b)
Polar
c)
Ionic
d)
Pizza
90.
What do we call a covalent bond where electrons are shared UNEVENLY or UNEQUALLY?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
91.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

92.
A(n) _________ is an ion with a positive (+) charge.
a)
anion
b)
cation
c)
ion
d)
solute
93.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
94.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
95.

What element is represented in this Bohr Model?

a)

Carbon

b)

Hydrogen

c)

Aluminum

d)

Lithium

96.

Which statement is INCORRECT use of mole measurement?

a)

one mole of calcium is 40.01 grams.

b)

one mole of calcium is equals to 6.02 x 1023 atoms

c)

two moles of CaCl2 is equal to 6.02 x 1023 molecules

d)

two moles of KI is equals to 166g

97.

What do these isotopes of lithium 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

98.
which explanation of this notation is correct?
a)
 12 is proton #
b)
6 tells you there are 6 neutrons
c)
6 tells you there are 6 protons
d)
12 is not a mass # here
99.

In his experiment, Rutherford concluded that atoms have a nucleus because

a)

most of the particles went straight through the foil.

b)

some of the particles were deflected near the front of the screen.

c)

some of the particles were deflected back towards the alpha source.

d)

not enough information is given.

100.

Thomson concluded that cathode rays have a negative charge. Why did his experiment lead him to this conclusion?

a)

Opposite charges attract

b)

Like charges attract

c)

Opposite charges repel

d)

Like charges repel

101.
Example for physical property
a)
melting point
b)
flammability
c)
reactivity 
d)
combustion
102.

Down a group in the periodic table, atomic radii generally

a)

decrease.

b)

remain constant.

c)

increase.

d)

vary unpredictably.

103.

how many atoms are contained in a 456 g sample of carbon dioxide?

a)

10.34 atoms

b)

6.237 x 1024 atoms

c)

1.871 x 1025atoms

d)

2.079 x 1024 atoms

104.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)
124 g O2
105.

Directly proportional means that as one value increases ...

a)

the other stays the same

b)

the other increases as well

c)

the other decereases

d)

the other goes to zero

106.

Inversely proportional means as one value increases the other...

a)

increases

b)

decreases

c)

stays the same

d)

goes to zero

107.
Temperature describes  the ______________ of particles.
a)
volume
b)
mass
c)
motion
d)
conductivity
108.

If the temperature of a gas increase, the pressure... (volume is constant)

a)

Decreases

b)

Increases

c)

Does not change

109.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
110.
Which container will have lower pressure?
a)
left
b)
right
c)
they both have the same pressure
111.

Pressure is

a)

defined as the mass that an object exerts when at rest.

b)

not a measurable in gases.

c)

defined as the number of moles of substance divided by the mass of the substance.

d)

created by the force of the gas particles impacting the walls of the container.

112.

When using Charles' Law if you double volume, what happens to temperature?

a)

it remains constant

b)

it triples

c)

it is divided by 2

d)

it is doubled also

113.

What temperature scale must we use in the Gas Laws?

a)

Rankine

b)

Fahrenheit

c)

Kelvin

d)

Celsius

114.

How do we measure an increase in kinetic energy?

a)

volume

b)

temperature

c)

Liters

d)

none of the above

115.

In the picture when the pistons rise the volume of the cylinder decreases. What happens to the pressure and temperature?

a)

The temperature will decrease and, therefore, the pressure will decrease.

b)

The collisions between molecules and the container walls will increase causing an increase in pressure. The temperature will decrease because the kinetic energy decreases.

c)

The collisions between molecules and the container walls will increase causing an increase in pressure. The temperature will because the kinetic energy will increase.

d)

The temperature and pressure are not related.

116.

What causes a hot air balloon to rise?

a)

An increase in temperature causes an increase in pressure that causes an increase in volume which causes the air in the balloon to be more dense than the air around it.

b)

An increase in temperature causes an increase in pressure that causes an increase in volume which causes the air in the balloon to be less dense than the air around it.

c)

As the temperature of the gas increases it escapes the balloon similarly to the gas leaving a rocket. This forces the balloon into the air.

d)

The increase in kinetic energy due to a temperature increase causes the atoms to lose protons and become helium. Helium is lighter than the air surrounding the balloon and this causes it to rise.

117.

Drag the values to the correct labels in the problem on the left

a)4.38L
b)5.36L
c)705.0 K
d)Unknown Value
1
2
3
4
1)
2)
3)
4)
118.

What would happen to the volume of a gas in balloon if the temperature is DOUBLED? (multiplied by 2)

a)

The balloon will be twice as big

b)

The balloon will shrink to half its size

c)

The volume of the balloon does not change

d)

Not enough information

119.

The relationship between volume and temperature is

a)

inverse

b)

direct

c)

indirect

d)

they are unrelated

120.

The relationship between pressure and volume is

a)

inverse

b)

direct

c)

indirect

d)

they are unrelated

121.

Which of the following is NOT a property of gasses?

a)

they expand to fill their container

b)

they take the shape of their container

c)

they exert pressure on the walls of their container

d)

their particles interact with each other

122.

The amount of space particles of a gas occupy

a)

Temperature

b)

Pressure

c)

Volume

d)

Mass

123.

What would happen to the pressure of a gas if the temperature decreases by half?

a)

it is halved

b)

It doubles

c)

It doesn't change

d)

Not enough information

124.

What would happen to the pressure in a piston if the piston is depressed (pushed in) halfway?

a)

The pressure doubles

b)

The pressure is halved

c)

The pressure does not change

d)

Not enough information

125.

Which conversion factor would be needed?

a)
b)
c)
d)
126.

 Convert 2.5 grams into milligrams.

a)
25 mg
b)
25,000 mg
c)
250 mg
d)
2500 mg
127.

How many inches are in 1 mile? (5280ft = 1mi; 12in = 1ft)

a)

66330in

b)

63360in

c)

63660in

d)

63066in

128.

How many yards are in 1 mile? (3 ft = 1 yd) (5280 ft = 1 mi)

a)

1670yds

b)

5280yd

c)

1760yds

d)

5820yds

129.

How many kilograms of calcium are there in 173 pounds of calcium? (1 pound = 454 grams; 1 kg = 1000 g)

a)

1.10 kg

b)

78.5 kg

c)

110 kg

d)

78500 kg

130.
What unit should be in the denominator of the conversion factor?
a)
yards
b)
leagues
c)
feet
d)
fathoms
131.
What is the measurement using the correct number of sig. figs.?
a)
39.5 mL
b)
40 mL
c)
39 mL
d)
40.0 mL
132.
This bullseye demonstrates...
a)
High Accuracy & High Precision
b)
High Accuracy & Low Precision
c)
Low Accuracy & High Precision
d)
Low Accuracy & Low Precision
133.

Which of the following numbers have two significant figures?

a)

21

b)

4900.

c)

0.000210

d)

0.023

134.
Which has more molecules?
a)
1 mole H2O
b)

1 mole NH3

c)

1 mole CCl4

d)
There are all the same
135.

When balancing a chemical equation, you can only change _________, you can never change _______!

a)

coefficients, subscripts

b)

subscripts, coefficients

c)

formulas, subscripts

d)

coefficients, formula units

136.

Mole Ratios used for conversions are derived from:

a)

the molar mass of the reactants in the balanced chemical equation

b)

the coefficients of the balanced chemical equation

c)

the subscripts of the products in the balanced chemical equation

d)

the group number of each element in the balanced chemical equation

137.

If there are 2 moles of oxygen available, which mole ratio will tells how much water is produced?


C3H8 +5O2 → 3CO2 + 4H2O

a)

4 mol H2O/ 5 mol O2

b)

5 mol O2/ 4 mol H2O

c)

2 mol O2/ 4 mol H2O

d)

4 mol O2/ 2 mol H2O

138.
If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
a)
theoretical yield
b)
mole ratio
c)
actual yield
d)
percentage yield
139.
When does a chemical reaction stop?
a)
When the lab is finished
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
140.
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
141.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)

6 mol H

b)

2 mol H

c)

3 mol H

d)

1 mol H

142.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)  
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
143.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
144.
Using the following equation:
4NH3(g) + 5O2(g) --> 4NO(g) + 6H2O(l)
How many grams of oxygen gas are needed to react with 56.8 grams of ammonia?
a)
45.08 g O2
b)
133.33 g O2
c)
260.77 g O2
d)
75.92 g O2
145.
  In a Chemical Reaction, the Law of Conservation of Mass states? 
a)
Matter is present.
b)
Matter is NOT created or destroyed.
c)
Matter is created and destroyed. 
146.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)
125.2 g O2
147.
If Nitrogen and Silver chemically bond, which will be named first?
a)
Silver
b)
Nitrogen
c)
Unknown
d)
Iodine
148.

A theory that states atoms tend to combine in such a way that they each have 8 electrons in their valence shell is known as

a)

The Atomic Theory

b)

The Octet Rule

c)

The Valence Electron Rule

d)

The Law of Conservation of Mass

149.

What is the following shape?

a)

Bent

b)

Trigonal Planar

c)

Tetrahedral

d)

Trigonal Pyramidal

150.

2 Atoms Bonded to Central Atom and 1 Unshared Pair

a)

Linear

b)

Bent

c)

Trigonal Planar

d)

Tetrahedral

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