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General Chemistry Reviewer

Total questions: 115

Worksheet time: 2hrs 57mins

Name
Class
Date
1.

Which scientist discovered the electrons?

a)

Dalton

b)

Thomson

c)

Atristotle

d)

Bohr

2.

Bohr discovered that electrons are located in

a)

the nucleus

b)

inside protons

c)

electron cloud

d)

circular orbits around the nucleus

3.

The smallest particle of an element that still represents that element.

a)

Nucleus

b)

electron

c)

proton

d)

atom

4.

What is a particle with one positive charge called?

a)

proton

b)

electron

c)

neutron

d)

quark

5.

What is the center of an atom called?

a)

nucleus

b)

electron cloud

c)

proton center

d)

photon center

6.

All matter is made of

a)

energy

b)

atoms

c)

electrons

d)

compounds

7.
In Dalton's Atomic Theory, all elements consist of __________ that cannot be divided.
a)
Atoms
b)
Parts
c)
Molecules
d)
Hydrogen
8.

Who was the Greek philosopher who called the smallest particle of matter an "atom"?

a)

Democritus

b)

Aristotle

c)

J.J Thompson

d)

Einstein

9.
Who is the scientist who proposed the "solar system" model of an atom where the electrons orbit around the nucleus?
a)
Democritus
b)
Niels Bohr
c)
Ernest Rutherford
d)
Chadwick
10.
What is the number of protons that the element in this image contain?
a)
14
b)
7
c)
15
d)
18
11.
What number indicates the nucleus?
a)
1
b)
2
c)
3
d)
4
12.
J.J. Thomson provided evidence that an atom...
a)
is the smallest particle of matter
b)
contains negatively charged particles
c)
has an overall negative charge
d)
has an overall positive charge
13.

The majority of an atom's mass exists where?

a)

In the nucleus

b)

In the electron cloud

c)

In the space between the nucleus and the electrons

d)

In the neutrons

14.
What did James Chadwick discover?
a)
neutrons
b)
electrons
c)
the atomic theory
d)
protons
15.
When phosphorus combines with oxygen to form diphosphorus pentoxide the skeleton equation is...
a)
P+O2 -> PO2
b)
P+O -> P5O2
c)
P+O2 -> P2O5
d)
P2O5 -> P2+O2
16.

In a combustion reaction one of the products is

a)

a hydrocarbon

b)

carbon dioxide

c)

oxygen

d)

nitrogen

17.
What must be balanced in a chemical reaction?
a)
moles
b)
molecules
c)
coefficients
d)
atoms
18.
When one element reacts with a compound, that type of reaction is...
a)
combination
b)
decompostion
c)
single replacement
d)
double replacement
19.
When one compound is broken up into multiple products, that type of reaction is...
a)
combination
b)
decomposition
c)
single replacement
d)
double replacement
20.
What are the products of the reaction between CsOH and H3PO4?
a)
Cs(PO4)3 and H2O
b)
CsPO4 and H2O
c)
Cs3PO4 and H2O
d)
H3Cs and PO4OH
21.
If a combination reaction reacts sodium and iodine, the formula of the product is...
a)
NaI
b)
Na2I
c)
NaI2
d)
SI
22.
Which compound is a solid?
a)
NaCl
b)
KNO3
c)
SrSO4
d)
BaCl2
23.
The products when Cl2 and reacts with MgBr2 is...
a)
Mg and ClBr
b)
MgCl2 and Br2
c)
None of these
24.
Name one diatomic molecule
a)
hydrogen
b)
neon
c)
carbon
d)
sodium
25.
What are the products for: Al+BaO?
a)
Ba+Al2O3
b)
Ba+AlO3
c)
Ba+AlO
d)
Al+BaO
26.
Which of the following represents a balanced equation when mercury (IV) oxide decomposes?
a)
HgO2->Hg+2O
b)
HgO2->Hg+O2
c)
Hg2O->2Hg+O
d)
HgO->Hg+O2
27.
What color light did magnesium give off in lab?
a)
yellow
b)
white
c)
red
d)
blue
28.
Balance: Fe+Co(NO3)2→Fe(NO3)3+Co
a)
1,3,1,3
b)
4,6,2,6
c)
2,3,3,2
d)
2,3,2,3
29.

How many single bonds will carbon look to make when it bonds covalently?

a)

2

b)

3

c)

4

d)

5

30.

Which of the following elements does NOT form an ion with a charge of 2+?

a)

Beryllium

b)

Strontium

c)

Magnesium

d)

fluorine

31.

When Alkali metals (Group 1) form ions, they ____.

a)

lose 1 proton

b)

gain 1 proton

c)

lose 1 electron

d)

gain 1 electron

32.

Which of the following pairs of elements is most likely to form an ionic compound?

a)

magnesium and fluorine

b)

manganese and iron

c)

oxygen and chlorine

d)

sodium and aluminum

33.

Which of the following shows correctly an ion pair and the ionic compound the two ions form?

a)

Sn4+ and N3- form Sn4N3

b)

Cu2+ and O2- form Cu2O2

c)

Cr3+ and I- form CrI

d)

Cr2+ and I- form CrI2

34.

How many valence electrons are transferred from the sodium atom to fluoride in the formation of the compound sodium fluoride?

a)

0

b)

1

c)

2

d)

3

35.

What is the chemical formula of sodium nitride?

a)

NaN

b)

Na2N

c)

Na3N

d)

NaN3

36.

What is the balanced chemical formula of iron (II) oxide?

a)

FeO

b)

FeO2

c)

Fe2O2

d)

Fe2O

37.

Select the correct formula for boron trichloride.

a)

B2Cl

b)

B3Cl

c)

BCl3

d)

BCl2

38.

AlCl3 + Na(OH) → Al(OH)3 + NaCl


In the chemical equation above, NaCl is a ______.

a)

Catalyst

b)

Solvent

c)

Product

d)

Reactant

39.

MgCl2 + Na ---> NaCl + Mg


What type of reaction is shown by the equation?

a)

Combination/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

40.

___Fe + ___O2 ---> ___Fe2O3


Which set of coefficients will correctly balance the equation?

a)

Already Balanced (no coefficients needed)

b)

2, 3, 4

c)

4, 3, 2

d)

3, 2, 2

41.

How many chlorine (Cl) atoms are in 3MgCl2?

a)

2

b)

3

c)

5

d)

6

42.

What type of reaction is electrolysis if its formula is:


2H2O → 2H2 + O2

a)

Synthesis (Combination)

b)

Decomposition

c)

Single Replacement

d)

Combustion

43.

Branch of chemistry that deals with the quantitative measurements that can be determined using balanced chemical equations.

a)

Physics

b)

Inorganic Chemistry

c)

Organic Chemistry

d)

Stoichiometry

44.

Stoichion means?

a)

Element

b)

Compound

c)

Mixture

d)

Solution

45.

A unit of measurement for the quantity of a substance.

a)

Mass

b)

Density

c)

Pressure

d)

Mole

46.

6.02 x 1023

a)

Mole Day

b)

Avogadro's Number

c)

Avodagro's Number

d)

Mol Day

47.

The sum of the atomic masses of all the atoms represented in the chemical formula of a substance.

a)

Formula Mass

b)

Percent Composition

c)

Theoretical Yield

d)

Percent Yield

48.

Formula mass can also be called:

a)

Molar Mass

b)

Atomic Mass

c)

Molarity

d)

Atomic Weight

49.

Can tell how abundant the element is in the compound.

a)

Formula Mass

b)

Percent Composition

c)

Theoretical Yield

d)

Percent Yield

50.

Refers to the reactant that limits the yield of the product. It is also the reactant that runs out first and produced the LEAST amount of product.

a)

Limiting Reagents or Limiting Reactant

b)

Excess Reagent or Excess Reactant

51.

The reactant that is left over and produced the GREATEST amount of product.

a)

Limiting Reagents or Limiting Reactant

b)

Excess Reagent or Excess Reactant

52.

The amount that the limiting reactant produces.

a)

Formula Mass

b)

Percent Composition

c)

Percent Yield

d)

Theoretical Yield

53.

The reaction 2ICl(s) ⇌ I2I_2 (s) + Cl2Cl_2 (g) is at equilibrium. Which change will increase the yield of Cl2Cl_2

a)

removing some of the I2I_2 (s)

b)

adding more ICl(s)

c)

removing the Cl2Cl_2 as it is formed

d)

decreasing the volume of the container

54.

Consider the equilibrium: 2 NO2NO_2 (g) ⇌ N2O4N_2O_4 (g) + energy. The equilibrium will shift to the left as a result of

a)

adding a catalyst

b)

increasing the volume

c)

removing some N2O4N_2O_4

d)

decreasing the temperature

55.

The reaction CO(g) + 2 H2H_2 (g) ⇌ CH3OHCH_3OH (g) + energy produces methanol. What will maximize the equilibrium yield of CH3OHCH_3OH ?

a)

low temperature and low pressure

b)

high temperature and low pressure

c)

low temperature and high pressure

d)

high temperature and high pressure

56.

Consider the equilibrium: PCl5PCl_5 (g) ⇌ PCl3PCl_3 (g) + Cl2Cl_2 (g).  A 1 L flask contains 0,02 mol PCl5PCl_5 , 0,05 mol PCl3PCl_3 and 0,05 mol Cl2Cl_2 at equilibrium. The value of KcK_c is …

a)

0,125

b)

2,50

c)

5,00

d)

8,00

57.

Consider the equilibrium:

CH3COOHCH_3COOH (aq) + H2OH_2O (l) ⇌ CH3COO−CH_3COO^- (aq) + H3O+H_3O^+ (aq) + heat

A stress was applied at time t1 and the data was plotted …

The stress is the result of …

a)

the addition of  HCl

b)

decreasing the temperature

c)

the addition of NaCH3OONaCH_3OO

d)

increasing the volume of the container

58.

Consider the equilibrium:  C(s) + 2 H2H_2 (g) ⇌ CH4CH_4 (g).  The addition of H2H_2 will cause the equilibrium to shift to the …

a)

left and [CH4]\left[CH_4\right] will increase

b)

left and [CH4]\left[CH_4\right] will decrease

c)

right and [CH4]\left[CH_4\right] will increase

d)

right and [CH4]\left[CH_4\right] will decrease

59.

Of the following equilibria, only __ will shift to the left in response to a decrease in volume …

a)

4Fe(s) + 3 O2O_2 (g) ⇌ 2 Fe2O3Fe_2O_3 (s)

b)

H2H_2 (g) + Cl2Cl_2 (g) ⇌ 2HCl(g)

c)

2 SO3SO_3 (g) ⇌ 2 SO2SO_2 (g) + O2O_2 (g)

d)

2HI(g) ⇌ H2H_2 (g) + I2I_2 (g)

60.

The reaction is exothermic: 2 SO2SO_2 (g) + O2O_2 (g) ⇌ 2 SO3SO_3 (g). Le Chatelier  predicts that ____ will result in an increase in the number of moles of SO3SO_3 (g) in the reaction container.

a)

increasing the pressure

b)

increasing the temperature

c)

removing some oxygen

d)

increasing the volume of the container

61.
At a constant volume, the pressure increases.  What happens to the temperature?
a)
increases
b)
decreases
c)
stays the same
62.
At a constant temperature, the volume decreases.  What happens to the pressure?
a)
increases
b)
decreases
c)
stays the same
63.
A 2.00 L sample of pure oxygen gas (O2) is measured at STP.  How many moles of oxygen is this?
a)
24.4 mol
b)
0.007 mol
c)
1.44 mol
d)
0.09 mol
64.
A 7.00 L sample of argon gas at 420. K exerts a pressure of 625 kPa.  If the gas is compressed to 1.25 L and the temperature is lowered to 350 K, what will be its new pressure in atm?
a)
10.4 atm
b)
2920 atm
c)
2916.7 atm
d)
28.8 atm
65.
How many grams of N2O5 gas  are in a sample that has a volume of 2.00 Liters at 298 K and 100. kPa of pressure.  
a)
8.72 grams
b)
0.0807 grams
c)
12.3 grams
d)
883 grams
66.
Calculate the volume that a 0.323-mol sample of a gas will occupy at -8oC and a pressure of 0.900 atm.
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
67.
The volume of a gas is increased from 150.0 mL to 350.0 mL by heating it. If the original temperature of the gas was 25oC, what will its final temperature be (in oC)
a)
146 oC
b)
10.7 oC
c)
58.3 oC
d)
422 oC
68.
How many grams of potassium chlorate are needed to form
3.45 liters of oxygen gas at STP?
2KClO3 (s) --> 2KCl (s) + 3O2 (g) 
a)
113 g
b)
0.631 g
c)
12.6 g
d)
28.3 g
69.
At STP (Standard Temperature and Pressure), a gas has a volume of
3.0 L. What is the new volume if the pressure increases to 303.9 kPa? 
a)
9.0 L
b)
1.0 L
c)
9.0 kPa
d)
1.0 kPa
70.
Under which of the following conditions do REAL gases behave most like IDEAL gases?
a)
High pressure and high temperature
b)
High pressure and low temperature
c)
Low pressure and low temperature
d)
Low pressure and high temperature
71.

When CH3OH is dissolved in water, how many moles of particles does it put into solution?

a)

1

b)

3

c)

4

d)

5

e)

6

72.

At the same concentration, which of the following will depress (lower) freezing point the most?

a)

C2H4O2

b)

C12H22O11

c)

LiBr

d)

CaF2

73.

What happens to the boiling point of water as a solute is added to it?

a)

it increases (elevates)

b)

it decreases (depresses)

c)

it stays the same (constant)

74.

At the same concentration, which of the following will elevate (increase) boiling point the most?

a)

CH3OH

b)

C6H12O6

c)

KNO3

d)

SrCl2

75.

Rank the following solutes from least to greatest effect on freezing point:


KI, CH3OH, Li3PO4, CaCl2

a)

KI, CH3OH, Li3PO4, CaCl2

b)

Li3PO4, CaCl2, KI, CH3OH

c)

Li3PO4, CH3OH, CaCl2, KI

d)

CH3OH, KI, CaCl2, Li3PO4

76.

Examine the models below. Assuming the same concentration, which would affect colligative properties more?

a)

beaker A

b)

beaker B

77.
Colligative properties depend on the _________ of the solute but not the __________ of the solute.
a)
 concentration; identity
b)
identity; concentration
c)
reactivity; nature
d)
nature; reactivity
78.

What happens to vapor pressure when you add a solute to a solution?

a)

It lowers the vapor pressure.

b)

It has no effect.

c)

It raises the vapor pressure.

d)

It causes the reaction to reach equilibrium.

79.
Colligative properties depend on the _____ of solute particles in solution.
a)
type
b)
number
c)
pH
d)
nature
80.

Which of the following is an incorrect implication of the first law of thermodynamics?

a)

The change in energy of a system is equal to the heat absorbed by the system and the work done on it.

b)

It follows the law of conservation of energy.

c)

Net change in energy can either be positive or negative.

d)

Net change in energy is always negative.

81.

Which of the following professions make great use of the study of the thermochemistry of food and the biochemical processes to establish the food intake and energy requirement of an individual?

a)

Nutritionists and dieticians

b)

Physical and occupational therapists

c)

Physicians and Psychologists

d)

Astronomers and Astrologers

82.

Based on the formula q=mcΔT, what unit would specific heat have?

a)

g/J°C

b)

J/g°C

c)

kJ/g

d)

°C/gJ

83.

For a group of particles enclosed in space, what would be the effect if more heat is supplied to the system?

a)

They would slow down.

b)

They would speed up.

c)

They would stop moving.

d)

There would be no effect.

84.

In which way does heat flow?

a)

Cooler to warmer

b)

Warmer to warmer

c)

Cooler to cooler

d)

Warmer to cooler

85.

The transfer of thermal energy between objects of different temperatures is called…

a)

Heat

b)

Temperature

c)

Internal energy

d)

Internal pressure

86.

A chemical reaction that absorbs heat from the surroundings is said to be _____, and has a ______ ΔH at constant pressure.

a)

Endothermic; positive

b)

Exothermic; negative

c)

Endothermic; negative

d)

Exothermic; positive

87.

The temperature of a glass of cold water will eventually…

a)

Never change temperature.

b)

Become warmer than the surrounding environment.

c)

Always be colder than the surrounding environment.

d)

Match the temperature of the surrounding environment.

88.

Enthalpy is the energy absorbed or released during a chemical reaction as ___.

a)

Light

b)

Heat

c)

Temperature

d)

Sound

89.

During an endothermic reaction in a beaker if we are part of the surroundings and touched the beaker, it would feel _______.

a)

Warm

b)

Moist

c)

Cold

d)

Slippery

90.

4 PCl5 + 3438 kJ --> P4 + 10 Cl2

How much energy is required to produce each mole of chlorine?

a)

687.6kJ

b)

343.8kJ

c)

859.5kJ

d)

245.8kJ

91.

As someone is running on the track, they begin to perspire. If the runner is our system, are they endothermic or exothermic?

a)

Endothermic

b)

Exothermic

92.

H2 + 2C + N2 + 270.3 kJ --> 2 HCN

Is this reaction endothermic or exothermic?

a)

Exothermic

b)

Endothermic

93.

Electrons always flow from

a)

cathode to anode

b)

anode to cathode

94.

Oxidation occurs at the

a)

anode

b)

cathode

95.

Electrons are gained at the

a)

anode

b)

cathode

96.

Given their standard reduction potentials, which of the species is going to be oxidized?

Cu2+/Cu = 0.34V

Zn2+/Zn = -0.76V

a)

Cu

b)

Zn

c)

CuSO4

d)

ZnSO4

97.
An iron nail is put into a solution of copper nitrate, iron is above copper in the activity series of metals, what will happen?
a)
iron will be reduced
b)
bubbles of oxygen gas will form on iron nail
c)
the iron nail will become copper plated
d)
no reaction occurs
98.
If Al is above Co in the activity series of metals, which of the following will occur if Al metal is put into a solution of cobalt nitrate?
a)
a redox reaction takes place
b)
the Al strip dissolves
c)
the Al strip becomes coated with cobalt
d)
all of the above
99.

What occurs to the mass of copper electrode in the following reaction?

Zn/Zn2+ // Cu2+/Cu

a)

increases

b)

decreases

c)

remains the same

100.

Which metal is the negative electrode?

Zn/Zn2+ // Cu2+/Cu

a)

zinc

b)

copper

101.

What reaction occurs at the anode?

Ag+/Ag = 0.80V

Ni2+/Ni = -0.25V

a)

Ag+ + e- →Ag

b)

Ag → Ag+ + e-

c)

Ni2+ + 2e- → Ni

d)

Ni → Ni2+ + 2e-

102.

What would be the theoretical cell potential of the previous electrochemical cell?

Ag+/Ag = 0.80V

Ni2+/Ni = -0.25V

a)

1.05V

b)

-1.05V

c)

0.55V

d)

-0.55V

103.
How many carbon atoms are in propane
a)
1
b)
2
c)
3
d)
4
104.
If an alkane has 20 carbon atoms, how many hydrogen atoms will it have?
a)
20
b)
22
c)
40
d)
42
105.
Name this alkane
a)
Methane
b)
Ethane
c)
Propane
d)
Butane
106.
Name this alkane
a)
Methane
b)
Ethane
c)
Propane
d)
Butane
107.
The "ane" ending in "alkane" tells someone that they are dealing with _________-bonded carbons.
a)
single
b)
double
c)
triple
d)
quadruple
108.
Give the name of this compound...
C3H8
a)
Propene
b)
Butane
c)
Butene
d)
Propane
109.
The molecular formula for Heptane is
a)
C4H10
b)
C8H18
c)
C5H12
d)
C7H16
110.
General formula of Alkane is 
a)
CnH2n+2
b)
CnH2n
c)
CnH2n+1OH
d)
CnH2n+1COOH
111.
How many hydrogen atoms are in butane
a)
4
b)
6
c)
8
d)
10
112.
Hydrocarbons are compounds that contain
a)
Carbon, only
b)
Carbon and Hydrogen, only
c)
Carbon, Oxygen, and Hydrogen, only
d)
Carbon, Oxygen, Hydrogen, and Nitrogen, only
113.
Which one of the following is saturated?
a)
water
b)
C4H8
c)
C4H10
d)
C5H8
114.
Which of the following generally undergoes substitution reactions
a)
alkanes
b)
alkenes
c)
Alkanes and alkenes 
d)
algebras
115.

Hydrocarbons burning is an example of what type of chemical reaction ?

a)

neutralisation

b)

endothermic

c)

addition

d)

exothermic

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