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Final Exam Review

Total questions: 166

Worksheet time: 1hrs 29mins

Name
Class
Date
1.

Chemical equations must be balanced to satisfy ____.

a)

The law of definite proportions

b)

The law of multiple proportions

c)

The law of conservation of mass

d)

Avogadro's principle

2.

What are the coefficients that will balance the skeleton equation below?

AlCl3 + NaOH → Al(OH)3 + NaCl

a)

1,3,1,3

b)

3,1,3,1

c)

1,1,1,3

d)

1,3,3,1

3.

How many moles of aluminum are needed to react completely with 1.2 mol of FeO?

2Al(s) + 3FeO(s) → 3Fe(s) + Al2O3(s)

a)

1.2 mol

b)

0.8 mol

c)

1.6 mol

d)

2.4 mol

4.

What is the name of H2SO4?

a)

hyposulfuric acid

b)

hydrosulfuric acid

c)

sulfuric acid

d)

sulfurous acid

5.

When an equation is used to calculate the amount of product that could form during a reaction, then the value obtained is called the ____.

a)

Actual yield

b)

Percent yield

c)

Minimum yield

d)

Theoretical yield

6.

The equation 2C3H7OH + 9O2 → 6CO2 + 8H2O is an example of which type of reaction?

a)

Combustion reaction

b)

Single replacement reaction

c)

Double replacement reaction

d)

Decomposition reaction

7.

A process that absorbs heat is a(n) _________.

a)

Exothermic process

b)

Polythermic process

c)

Endothermic process

d)

Ectothermic process

8.

Which is the most likely ∆H for an endothermic reaction?

a)

0 kJ

b)

-16 kJ

c)

+16 kJ

d)

There is no such thing as an endothermic reaction

9.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
10.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more neutrons
11.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
12.
 Which of the following is the correct formula for these two ions:
Al+3 +  S-2
a)
AlS3
b)
Al2S3
c)
Al3S2
d)
Al3S
13.
What is the name of K3PO4?
a)
Tripotassium Phosphate
b)
Tripotassium Phosphite
c)
Potassium phosphide
d)
Potassium phosphate
14.

Covalent bonding occurs between which two types of elements?

a)

metals and metals

b)

nonmetals and metals

c)

nonmetals and nonmetals

d)

metalloids and metalloids

15.
In chemistry, a "mole" is:
a)
The mass of an atom
b)
a large number used to count particles
c)
based on the volume of a substance
16.
Rank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attraction
a)
dipole-dipole>covalent bond>hydrogen bond>London
b)
London>dipole-diple>hydrogen bond>covalent bond
c)
covalent bond>hydrogen bond>dipole-dipole>London
d)
hydrogen bond>dipole-dipole>London>covalent bond
17.
The number 6.02 x 1023 is called...
a)
Obama's number
b)
Bohr's number
c)
Trump's number
d)
Avogadro's number
18.
What is the molar mass of NaCl?
a)
58.45g/mol
b)
28g/mol
c)
12g/mol
d)
6.02 x 1023
19.
What would be the mass of 1.5mol H2O
a)
20
b)
27
c)
32
d)
40
20.
T/F
If 2 compounds have the same empirical formula, they are the same (same properties, structure, etc.)
a)
True
b)
False
21.
Find the percent composition of N2S2.
a)
N: 69.6%  S: 30.4%
b)
N:36% S: 75.6%
c)
N: 96.6% S: 3.4%
d)
N: 30.4% S: 69.6%
22.
Balance this reaction: ____ Na3PO4 + ____ KOH ---> ____ NaOH + ____ K3PO4
a)
1,3,3,1
b)
1,3,2,1
c)
2,3,3,1
d)
1,1,3,1
23.

In a balanced chemical equation, the mass of the reactant is equal to the

a)

atoms in a molecule.

b)

atomic mass of the elements.

c)

volume of the reactacts.

d)

mass of the products.

24.

A solid that is deposited from a solution

a)

Solid

b)

Liquid

c)

Product

d)

Precipitate

25.

Predict the products for the this Single Replacement reaction:

K + HCl →

a)

KCl + H2

b)

KHCl

c)

KH + Cl2

d)

HCl + K2

26.
In Charles' Law the pressure remains constant.
a)
True
b)
False
27.
Which has more molecules?
a)
1 mole H2O
b)
1 mole Al(OH)3
c)
1 mole NaCl
d)
There are all the same
28.
Which of the following is NOT a diatomic element?
a)
neon
b)
hydrogen
c)
oxygen
d)
chlorine
29.
  What is the name of NO2?
a)
nitrogen monoxide
b)
nitrogen oxide
c)
nitrogen dioxide
d)
nitrogen oxygen
30.
How many moles of oxygen are present in 16 g of O2?
a)
1 mole
b)
2 moles
c)
0.5 moles
d)
6.02 x 1023 moles
31.
What is the molar mass of Zn(NO3)2?
a)
159.41 g
b)
189.41 g
c)
173.41 g
d)
254.81 g
32.
How many total oxygen atoms are on the reactant side of the equation?
a)
5
b)
6
c)
10
d)
14
33.
What temperature is equal to -50 0C?
a)
-223 K
b)
223 K
c)
0 K
d)
-323 K
34.
How many moles of carbon are present in 36 g of carbon?
a)
6.02 x 1023 moles
b)
1 mole
c)
22.4 moles
d)
3 moles
35.
In the symbol C-14, 14 refers to the particle's ____.
a)
mass number
b)
atomic mass
c)
atomic number
d)
charge
36.
Cu2S
a)
copper sulfide
b)
copper (I) sulfide
c)
copper (II) sulfide
d)
copper sulfate
37.
Which of the following is the general formula for a decomposition reaction?
a)
A + B  → AB
b)
AB → A + B
c)
AB + C → AC + B
d)
AB + CD → AC + BD
38.
Balance this equation
_N2 + _H2 --> _NH3
a)
1,2,3
b)
1,3,2
c)
1,1,2
d)
2,1,1
39.
As a reaction is taken place,  the student notices that the temperature has dropped. This indicates that the system has increased in energy. What type of process is this?
a)
Endothermic
b)
Exothermic
40.
All atoms of the same element have the same ____.
a)
number of neutrons
b)
number of protons
c)
mass numbers
d)
mass
41.
What is the chemical formula for magnesium bromate?
a)
MgBr
b)
MgBr2
c)
MgBrO3
d)
Mg(BrO3)2
42.

The amount of heat energy required to change the temperature of 12 g of gold from 45°C to 15°C is -47 J. What is the specific heat capacity of gold?

a)

0.13 J/(g°C)

b)

17,000 J/(g°C)

c)

1600 J/(g°C)

d)

0.065 J/(g°C)

43.
Energy can be _____________ or changed from one type to another.
a)
destroyed
b)
transferred
c)
created
d)
ignored
44.

An electron is

a)

positively charged

b)

neutral

c)

negatively charged

45.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
46.

How many valence electrons are found in atoms of group 4?

a)

4

b)

3

c)

14

d)

16

47.

How do electrons of an element determine that element's reactivity?

a)

If the valence shell has missing electrons it is very reactive to attract or lose more electrons.

b)

If the valence shell has a full ring of electrons it is very reactive because it needs more.

c)

If the valence shell has a full shell of electrons it is very reactive because it is already full.

d)

If the valence shell has missing electrons it is not reactive because it is missing electrons.

48.

Which has the greater Electronegativity?

a)

Ca

b)

O

c)

S

d)

B

49.

Which of the following is the correct Lewis structure for a molecule of fluorine?

a)

A

b)

B

c)

C

d)

D

50.

Formula for barium sulfide

a)

B2S3

b)

BaS

c)

Ba2S

d)

BaS2

51.

Carbon monoxide is a deadly gas produced from incomplete combustion. What type of compound is it?

a)

covalent

b)

ionic

52.
What is represented by the dots in a Lewis electron-dot diagram of an atom of an element in Period 2 of the Periodic Table?
a)
a. the number of neutrons in the atom
b)
b. the number of protons in the atom
c)
c. the number of valence electrons in the atom
d)
d. the total number of electrons in the atom
53.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
54.

A diatomic molecule like O2 is always _____ because electrons are shared _____

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

55.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
56.

Does NH3 or PH3 have a higher boiling point?

a)

NH3 because it has the strongest intermolecular forces

b)

PH3 because it has the strongest intermolecular forces

c)

NH3 because it has the weakest intermolecular forces

d)

PH3 because it has the weakest intermolecular forces

57.

What is the correct coefficents for the unbalanced equation:

__Al + __O2--> __Al2O3

a)
4,1 --> 2
b)
4,3 --> 4
c)
3,4 --> 1
d)
4,3 --> 2
58.

Predict the products of this synthesis reaction: H2 + Cl2 →

a)

HCl

b)

H2Cl2

c)

H2Cl

d)

HCl2

59.

How many moles are in 98.3 grams of aluminum hydroxide, Al(OH)3?

a)

1.26 moles

b)

0.8 moles

c)

7,670 moles

d)

1.63 x 10-22 moles

60.
If a 8.50g ice cube at -10o C sits out on the counter, completely melts, and then warms to room temperature (25o C) how much energy did the ice cube absorb? Use C = 2.108 J/goC for ice, C = 4.184 J/goC for water, and Hf = 334 J/g.
a)
179.18 J
b)
2839 J
c)
889.1 J
d)
3907.3 J
61.
What kelvin temperature is equivalent to -24 0C?
a)
a. 226 K
b)
b. 249 K
c)
c. 273 K
d)
d. 297 K
62.
The atomic mass of titanium is 47.88 atomic mass units. This atomic mass represents the 
a)
a. total mass of all of the protons and neutrons in the atom of Ti
b)
b. total mass of all the protons, neutrons, electrons in an atom of Ti
c)
c.  weighted average mass of the most abundant isotope of Ti
d)
d. weighted average mass of all the naturally occurring isotopes of Ti
63.
Which element has chemical properties that are most similar to the chemical properties of sodium?
a)
a. Mg
b)
b. K
c)
c. Se
d)
d. Cl
64.
All the elements in Period 3 have the same number of 
a)
a. occupied sublevels
b)
b. principal energy levels
c)
c. electrons
d)
d. protons
65.
Which gas has properties that are most similar to those of an ideal gas?
a)
a. N2
b)
b. O2
c)
c. He
d)
d. Xe
66.
Which two substances can not be broken down by chemical change?
a)
a. C & CuO
b)
b. C and Cu
c)
c. CO2 & CuO
d)
d. CO2 & Cu
67.
What is the mass number of an atom which contains 21 electrons, 21 protons, and 24 neutrons?
a)
a. 21
b)
b. 42
c)
c. 45
d)
d. 66
68.
What is the total number of electrons in a Mg2+ ion?
a)
a. 10
b)
b. 2
c)
c. 12
d)
d. 24
69.
How many significant figures: 216 m
a)
1
b)
2
c)
3
d)
0
70.
Write 0.00000707 in scientific notation.
a)
7.07 x 10-6
b)
7.07 x 106
c)
707 x 108
d)
707 x 10-8
71.
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
72.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

73.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
74.
Atomic Radius is...
a)
the relative size of the atom's nucleus
b)
the relative size of the atom's electron cloud
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
75.
How do the following two elements bond together?
Na1+  F1-         
a)
NaF
b)
NaF3
c)
Na3F
d)
Na1F2
76.
How many significant figures: 0.012 km
a)
1
b)
2
c)
3
d)
4
77.

Which SI unit is used to measure length?

a)

mol

b)

m

c)

kg

d)

m2

78.
Which orbital has the least amount of energy? 
a)
p orbital
b)
d orbital
c)
s orbital 
d)
What is an orbital?
79.

What is the electronic configuration of sodium?

a)

1s22s22p63s1

b)

1s22s22p7

c)

1s22s22p63s2

80.
Calculate 1.23 m x 0.89 m and give your answer with the appropriate number of significant figures.
a)
1.0 m2
b)
1.1 m2
c)
1.0947 m2
d)
1.09 m2
81.

Which is an example of a mixture?

a)

iron filings (Fe)

b)

copper wire (Cu)

c)

bronze pipe (Cu, Sn)

d)

carbon dioxide (CO2)

82.

What type of bond does NO2 have?

a)

Ionic

b)

Covalent

83.

How many atoms of oxygen are in the compound Al2(SO4)3

a)

2

b)

3

c)

4

d)

7

e)

12

84.

What is the correct molecular geometry AND molecular polarity of HCN?

a)

Tetrahedral, nonpolar

b)

Tetrahedral, polar

c)

Bent, polar

d)

Linear, polar

e)

Linear, nonpolar

85.

Which of the following bonds is the most polar?

a)

O-F

b)

N-F

c)

H-F

d)

S-F

86.

An atomic orbital can at most hold how many electrons, according to the Pauli Exclusion Principle?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

87.
As you move from Aluminum to Gallium, the atomic radius will ....
a)
decrease
b)
increase
c)
stay the same
88.

What is the formula for iron(III) chloride?

a)

FeCl

b)

Fe3Cl

c)

FeCl2

d)

FeCl3

89.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
90.
4.35% of all X atoms have a mass of 39.946 amu. 83.79% have a mass of 41.941 amu, 9.50% have a mass of 42.941 amu, and 2.36% have a mass of 43.939 amu. What is the average atomic mass of atom X?
a)
41.97 amu
b)
42.19 amu
c)
10.43 amu
d)
40.04 amu
91.

What is the electron configuration of the calcium ion?

a)

1s22s22p63s23p64s2

b)

1s22s22p63s23p64s23d104p6

c)

1s22s22p63s23p64s24p6

d)

1s22s22p63s23p6

e)

1s22s22p63s23p64s1

92.

What is the name of the ionic compound K3N?

a)

potassium nitride

b)

potassium (III) nitride

c)

potassium (I) nitride

d)

potassium nitrogen

e)

potassium+3 nitride-1

93.
What is the volume of 5 moles of oxygen gas at STP? 
a)
112 L 
b)
22.4 L
c)
78.8 L 
d)
114.24 L
94.
What is the percentage of iron in iron(III)oxide?
a)
30%
b)
70%
c)
40%
d)
60%
95.
What is the mass in grams of 5.90 mol C8H18?
a)
.0512 g
b)
19.4 g
c)
673 g
d)
389 g
96.

How many moles of magnesium are added to a test tube if Micah and his lab partner could count the number of atoms in the piece of magnesium ribbon to be 1.50 X 1023?

a)

2.40 X 10-1 mol Mg

b)

2.49 X 10-1 mol Mg

c)

4.03 X 101 mol Mg

d)

9.03 X 101 mol Mg

97.
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
98.

If the nitrogen gas is collected in a rigid 2.00 liter metal cylinder at 22oC at 2.00 X 103 kPa pressure, how many moles of nitrogen gas does the cylinder contain? (R = 8.31)

a)

1.63 moles

b)

1.42 X 102 moles

c)

1.82 X 102 moles

d)

1.35 X 10 moles

99.
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
100.
A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC.  What is the new volume of the gas?
a)
60.0 mL
b)
15.0 mL
c)
27.5 mL
d)
32.5 mL
101.

When sodium fluoride dissolves and dissociates in water, a solvation sphere of water molecules forms around the ions. The solute solvent interaction ____________ and makes the beaker warm.

a)

absorbs energy from the surroundings

b)

absorbs energy into the surroundings

c)

releases energy from the surroundings

d)

releases energy into the surroundings

102.
What is the molality of a solution containing 1.3 mol in 13.4 kg of solution?
a)
9.7 m
b)
17.42 m
c)
0.097 m
103.

How many grams of AgNO3 are needed to prepare 0.125M solution in 250 mL of water?

a)

.03g

b)

0.5g

c)

5.3g

d)

84.9g

104.
What characterizes a strong acid or base?
a)
ionic bonding
b)
presence of a hydroxide or hydrogen ion
c)
complete ionization in water
d)
polar covalent bonding
105.

What charge will barium (Ba) form when becoming an ion?

a)

6+

b)

6-

c)

2+

d)

2-

e)

0

106.
What is the name of C3Cl8 ?
a)
Carbon octachloride
b)
Tricarbon octachloride
c)
Carbon trichloride
d)
Octacarbon trichloride
107.

What is the molar mass of ammonium sulfide - (NH4)2S?

a)

68.17 g/mol

b)

40.02 g/mol

c)

54.16 g/mol

108.

According to the following equation, how many grams of water could be created by combusting 100.5 g of ethane?

2 C2H6+ 5 O2-> 4 CO2+ 6H2O

a)

180.6 g H2O

b)

108.1 g H2O

c)

201.2 gH2O

109.

As 120 g of copper piping heated to a temperature of 120.50C cools to 50.80C . How much heat did the copper lose in the process?

a)

3220 J

b)

69.7 0C

c)

8364 J/0C

110.

Which is an example of an endothermic change?

a)

Ice melting

b)

Combustion

c)

Steam condensing

111.

10 L of a gas is collected at 100 K and allowed to expand to 30.0 L. What is the new temperature?

a)

400 K

b)

300 K

c)

275 K

112.
To form a charge of +2 an atom must _ electrons.  To form -3 it must _ electrons.
a)
Gain 2; Lose 3
b)
Gain 3; Lose 2
c)
Lose 2; Gain 3
d)
Lose 3; Gain 2
113.

Ions that end in -ate or -ite are...

a)

polyatomic

b)

monoatomic

c)

do not exist

d)

are always cations

114.
P2O5
a)
Phosphorus Oxide
b)
Pentaphosphorus Dioxide
c)
Diphosphorous pentoxide
d)
Phosphoric Oxygen
115.
How many atoms of iodine are in a mole of iodine?
a)
53
b)
63.55g
c)
126.9
d)
6.02 x 1023
116.
What is the volume occupied by 1 mole of any gas?
a)
44.8 L
b)
22.4 L
c)
16.8 L 
d)
20.4 L 
117.

Empirical Formula = CF2 , Molecular formula mass = 192. What is the molecular formula?

a)
C4F8
b)
C4F
c)
CF8
d)
C2F4
118.
Is this balanced?...
Al + O2 --> 2Al2O3
a)

yes

b)

no

119.

Exothermic reactions...

a)

Absorb energy and have a positive ΔH

b)

Release energy and have a negative ΔH

c)

Release Color and have a positive ΔH

d)

Absorb Color and have a negative ΔH

120.
N2 + 3H2 --> 2NH3
What is the total number of moles of NH3 produced when 10 moles of H2 reacts completely with N2?
a)
6.7
b)
2.0
c)
3.0
d)
15.0
121.

P4 + 6Cl2 --> 4PCl3

75.0g P4 reacts with excess chlorine gas, and 110g PCl3 is collected in the lab. What is the percent yield of this reaction?

a)

78%

b)

64%

c)

27%

d)

33%

122.

CH4 + 2H2O --> CO2 + 4H2

What reactant will be used up first when 20g CH4 react with 15g H2O?

a)

CH4

b)

H2O

c)

CO2

d)

H2

123.

Calculate the molar mass of Ba(C2H3O2)2

a)

255.3 g/mol

b)

237.3 g/mol

c)

228.3 g/mol

d)

196.3 g/mol

124.

How much energy is required to completely boil away 150g of 10o C water? Use c = 4.184 J/goC for liquid water, and Hv = 40.6 kJ/g.

a)

56,484 kJ

b)

394,400 kJ

c)

394.4 kJ

d)

337,900 kJ

125.
The ___ is the thing being dissolved
a)
solute
b)
solvent
126.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
127.
(Hess's Law)Calculate the ∆H for the following reaction: 2H2O2 →  2H2O  + 1 O2 
You are given these two equations:
2H2  +  O2 → 2H2O            ∆H  =  -572 kJ
 H2  +  O2  →  H2O2            ∆H  =  -188 kJ 
a)
∆H  =  -948 kJ 
b)
∆H  =  -196 kJ 
c)
∆H  =  -384 kJ 
d)
∆H  =  -188 kJ 
128.
A sample of iron receives 50.J of heat energy that raises the temperature of the iron 25.0°C. If iron has a specific heat of  0.10 J/g°C, what is the mass of the iron sample?
a)
25 g
b)
30 g
c)
20 g
d)
50 g
129.
You have a gas that has a pressure of 2 ATM and a volume of 10L.  What would be the new volume if the pressure was changed to 1 ATM?
a)
5 L
b)
20 L
c)
It would stay at 10L
d)
1 L
130.

2Al + 6HCl --> 2AlCl3 + 3H2

Aluminium reacts with hydrochloric acid. How many grams of aluminum are necessary to produce 11 L of hydrogen gas at STP?

a)

13

b)

8.8

c)

0.99

d)

1.0

131.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
132.

When 4.7 x 10^11 atoms of sodium are put into excess water, how many grams of NaOH are made?

Reaction: Na + H2O → NaOH + H2

a)

1.13 x 10^46 gram

b)

1.13 x 10^-11 gram

c)

3.12 x 10^-11 gram

d)

6.02 x 10^23 gram

133.
How would you write 0.0005 in scientific notation?
a)
50 x 105
b)
5 x 10^-4 
c)
5 x 103
d)
.5 x 103
134.
What is the measurement using the correct number of sig. figs.?
a)
89cm
b)
88.9cm
c)
88.90cm
d)
88cm
135.
the central region of an atom where its neutrons and protons are is its 
a)
nucleus 
b)
electron cloud
c)
core 
d)
center 
136.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
137.
What is the name of Si2Cl6?
a)
disilicon hexachlorine
b)
disilicon hexachloride
c)
silicon hexachloride
d)
silicon chloride
138.

What is the bond angle around the central carbon atom?

a)

180

b)

120

c)

109.5

d)

90

139.

What is the coefficient of H2O after balancing the chemical reaction below?


___ C3H8 + ___ O2 → ___ CO2 + ___ H2O

a)

4

b)

1

c)

2

d)

3

e)

5

140.

If the reactants on the left side of a chemical equation are C₃H₈ + 5 O₂, the products in a balanced equation could be

a)

4 CO₂ + 3 H₂O

b)

3 CO₂ + 4 H₂O

c)

2 CO₂ + 3 H₂O

d)

3 CO + 4 H₂O

141.

How many significant figures?

1001.00

a)

2

b)

4

c)

6

142.

Which is a diatomic molecule?

a)

bromine

b)

hydroxide

c)

carbon

d)

gallium

143.

Convert 2.3 m/s to km/hr

a)

8.3

b)

3.68

c)

0.061

d)

221

144.

How would you write 340,000 in scientific notation?

a)

3.4 x 10^5

b)

.34 x 10^6

c)

3.4 x 10^-5

d)

3.4 x 10^6

145.

Which is a polyatomic molecule?

a)

bromine

b)

hydroxide

c)

oxygen

d)

carbon

146.

Predict the shape:

a)

bent

b)

trigonal pyramidal

c)

tetrahedral

d)

trigonal planar

147.

How many grams of beryllium are needed to produce 36.0 g of hydrogen? (Assume an excess of water)

Be + 2H2O → Be(OH)2 + H2

a)

161

b)

4.00

c)

648

d)

36

148.

Identify the limiting reactant when 11 mol CS2 reacts with 18 mol O2.

CS2 + 3O2 → CO2 + 2SO2

a)

CS2

b)

O2

c)

CO2

d)

SO2

149.

What would be your percent yield if only 12 grams of water were produced in the lab, and the reaction started with 30 g of oxygen with an excess of hydrogen?

2H2 + O2 --> 2H2O

a)

36%

b)

14%

c)

55%

d)

5%

150.

1 mole of sodium has the same number of particles as 1 mole of calcium.

a)

true

b)

false

151.

Find the molar mass of calcium hydroxide.

a)

57.1 g/mol

b)

74.1 g/mol

c)

641.2 g/mol

152.

The correct electron configuration for iron is:

a)

1s22s22p63s23p64s23d6

b)

1s22s22p63s23p64s23d4

c)

1s22s22p63s23p6

d)

1s22s22p63s23p64s2

153.

If you dilute 175 mL of a 1.6 M solution of LiCl to 1.0 L, determine the new concentration of the solution.

a)

2.1 M

b)

3.6 M

c)

280 M

d)

0.28 M

154.
P4 + 3O2 --> P4O6 
What is the limiting reactant is 12 moles of P4 react with 15 moles of O2?
a)
P4
b)
O2
c)
P4O6 
d)
none of the above
155.
Which of the following does NOT form a precipitate?
a)
Pb(NO3)2(aq) + 2KI(aq) →
b)
Sr(NO3)2 (aq) + K2SO4(aq) →
c)
AgNO3(aq) + Na2S(aq) →
d)
 Pb(NO3)2(aq) + AgNO3(aq) →
156.

11. LiOH + KCl → LiCl + KOH ; the reaction was done with 20 grams of lithium hydroxide.  What is my theoretical yield of lithium chloride? 

a)
35.5 grams
b)
11.3 grams
c)
0.03 grams
d)
0.09 grams
157.

if a balloon is heated, what happens to the volume of the air inside the balloon if the pressure remains constant?

a)

it increases

b)

it stays the same

c)

it decreases

d)

the change cannot be predicted

158.

Na + Cl2 --> NaCl

what is the oxidation number of chlorine in NaCl?

a)

-2

b)

-1

c)

0

d)

+1

159.
What is the mole ratio of H2O to H3PO4 in the following chemical equation?   P4O10 + 6 H2O --> 4 H3PO4 
a)
6:4
b)
4:6
c)
1:3
d)
3:1
160.
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
161.
How many grams are in 7.8 moles of NaCl?
a)
476grams
b)
460 grams
c)
452 grams
d)
462 grams
162.

Consider this equation: 2 Al + 3Cl2 → 2AlCl3

How many grams of Cl2 are needed to react with 36 grams of Al?

a)

141.9 g of Cl2

b)

2.00 g of Cl2

c)

0.789 g of Cl2

d)

94.6 g of Cl2

163.
what is the molarity of a solution that contains 125 g NaCl in 4.00 L of solution?
a)
0.535 M NaCl
b)
2.14 M NaCl
c)
8.56 M NaCl
d)
31.3 M NaCl
164.

HNO2 is a __________

a)

a base

b)

a salt

c)

an acid

d)

an ionic compound

165.
Predict the following reaction 
NaCl   +   Ca(NO3)2 --> 
a)
no reaction both products are aqueous 
b)
Calcium chloride and sodium nitrate are produced  
c)
sodium nitrate is a solid formed 
d)
calcium chloride is the solid formed
166.
Identify the limiting reagent when 6.00 moles HCl combines with 5.00 moles Mg to form MgCl2.
 
1 Mg +  2 HCl --> 1 MgCl2  +  1 H2   
 
a)
Mg
b)
H2
c)
MgCl2
d)
HCl

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