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Unit 2 Exam Review

Total questions: 70

Worksheet time: 2hrs 25mins

Name
Class
Date
1.
When metals bond with non-metals they form what type of bonds
a)
covalent
b)
ionic
c)
cooperative
d)
lewis
2.
Which of the following is NOT an ionic compound:
a)
CaO
b)
NaOH
c)
BaCl2
d)
Br2
3.
How many valence electrons does a bromine atom have?
a)
1
b)
2
c)
6
d)
7
4.
The chemical formula of iron (III)bromide is
a)
FeBr
b)
Fe(III)Br
c)
FeBr₃
d)
Fe₂Br₃
5.
What would be the proper chemical formula for combining Al3+ and Cl- :
a)
AlCl3
b)
Al3Cl
c)
AlCl
d)
Al3Cl3
6.
Name the following ionic compound: BeCl2
a)
beryllium chlorine
b)
beryllium II chloride
c)
beryllium chloride
d)
beryllium dichloride
7.
Name the following ionic compound: MgSO4
a)
magnesium sulfoxide
b)
magnesium sulfide
c)
magnesium sulfate
d)
magnesium oxide
8.
If an atom becomes an ion with a 2+ charge, what does that mean?
a)
It has lost 2 electrons
b)
It has gained 2 electrons
c)
The atom is in period 2
d)
The atom has an atomic # of 2
9.
Atoms want _____ electrons in their valence (outermost) shell. 
a)
1
b)
2
c)
6
d)
8
10.
What is the correct term for "bond that forms when electrons are shared"?
a)
ionic bond
b)
metallic bond
c)
covalent bond
11.
Carbon has 4 valence electrons. How many electrons does carbon need to fill its shell?
a)
2
b)
4
c)
8
d)
0, it is already full
12.
Which compound contains covalent bonds?
a)
NaI
b)
K2O
c)
N2O3
d)
BeO
13.
Covalent bonds form between 
a)
nonmetal and metal
b)
metal and metal 
c)
nonmetal and nonmetal
14.
Which two elements would form an ionic bond?
a)
carbon and hydrogen
b)
oxygen and silicon
c)
cesium and iodine
d)
potassium and calcium
15.
Prefixes are used only for ________ compounds
a)
ionic
b)
covalent
16.

How many electrons are shared in a single covalent bond?

a)

1

b)

3

c)

2

d)

7

17.

Which of these would form a diatomic molecule with two atoms joined by a covalent bond?

a)

copper

b)

helium

c)

chlorine

18.
What does the prefix tetra mean?
a)
Three
b)
Four
c)
Six
19.
In covalent bonds, electrons are ___________.
a)
transferred
b)
gained
c)
lost
d)
shared
20.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
21.

An atom's ability to draw electrons toward their nucleus is referred to as____________

a)

ionization energy

b)

electronegativity

c)

reactivity

22.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

23.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

24.
What geometry will this molecular structure have?: PH3
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
25.
Will this molecule be polar or nonpolar? CCl4
a)
polar
b)
nonpolar
26.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms

b)

The difference in the electronegativities of the two atoms

c)

The charges of the atoms

d)

None of the Above

27.

What must the difference in electronegativity between two atoms be in order for the bond between them to be nonpolar covalent?

a)

less than 0.4

b)

greater than 1.7

c)

between 0.4 and 1.7

d)

exactly 0

28.
The most electronegative atom in the periodic table is:
a)
Fluorine
b)
Helium
c)
Neon
d)
Francium
29.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
30.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
31.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
32.

3Mg + N2 --> Mg3N2


What type of reaction is this?

a)

Synthesis

b)

Decomposition

c)

Single displacement

d)

Combustion

33.
Which chemical reaction breaks down into 2 substances?
a)
Double Replacement
b)
Single Replacement
c)
Synthesis
d)
Decomposition
34.
What type of reaction occurs between an element and a compound?
Zn + 2HCl --> ZnCl2 + H2
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
35.
The reaction below is an example of?
AgNO3 + NaCl → AgCl + NaNO3
a)
Single Replacement
b)
Double Replacement
c)
Decomposition
d)
Combustion
36.
What type of reaction is illustrated below?
2HI --> H2  +  I2
a)
synthesis
b)
decomposition
c)
single replacement
d)
double replacement
37.
Provides evidence that a chemical reaction has occurred. 
a)
dissolving 
b)
melting
c)
formation of a gas
d)
bending
38.

What type of reaction is CH3COOH + O2 yields CO2 + H2O ?

a)

synthesis

b)

decomposition

c)

combustion

d)

single replacement

e)

double replacement

39.
__NaClO3 --> __NaCl + __O2
a)
2,2,2
b)
2,2,3
c)
3,2,2
d)
1,2,3
40.
_AgNO3 + _Cu →_Cu(NO3)2 + _Ag
a)
2 AgNO3 + 2 Cu → 3 Cu(NO3)2 + 1 Ag
b)
2 AgNO3 + 1 Cu → 1 Cu(NO3)2 + 2 Ag
c)
1 AgNO3 + 2 Cu → 2 Cu(NO3)2 + 1 Ag
d)
3 AgNO3 + 2 Cu → 3 Cu(NO3)2 + 2 Ag
41.

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

42.
How many Hydrogen are in 4H2O?
a)
6
b)
8
c)
2
d)
4
43.
What is the left part of a chemical equation called?
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
44.
What is the right part of a chemical equation called...
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
45.

Write the formula of one spectator ion from the following reaction:

KCl (aq) + AgNO3 (aq) --> KNO3 (aq) + AgCl (s)

(a)  

46.
How many particles (atoms) 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
47.

Calculate the number of moles in 20.9 grams of N2N_2

a)

1.49 moles

b)

0.746 moles

c)

0.37 moles

d)

1.74 moles

48.
What is the definition for Avogadro's number?
a)
number of grams per one mole of a substance
b)
whole number ratio that is a multiple of a chemical formula
c)
simplest, whole number ratio of a chemical formula
d)
6.02 x 10^23 particles per one mole of a substance
49.
Molar mass is in units of ________.
a)
grams
b)
grams/mole
c)
mole
d)
moles/gram
50.
How many grams are in 88.1 moles of magnesium?
a)
2141 g
b)
0.3 g
c)
30 g
d)
3.6 g
51.

When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

52.
The ______________ yield is the maximum amount of product possible in a reaction. This determines the amount of product that should be produced in a perfect setting
a)
Percent
b)
actual
c)
stoichiometry
d)
theoretical
53.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
54.

Balance the following reaction: (You will use this for the next few questions so write it down.)

Mg(s) + HCl(aq) --> MgCl₂(aq) + H₂(g)

a)

1,2,1,2

b)

2,1,1,2

c)

1,2,1,1

d)

1,2,2,2

55.
Using the balanced equation in question 1,
Mg(s)   +   HCl(aq)  -->   MgCl₂(aq)   +   H₂(g)
How many grams of HCl are consumed by the reaction of 2.50 moles of magnesium?
a)
5.00 g
b)
7.29
c)
182 g
d)
218 g
56.

What mass of carbon dioxide will be produced when 29.9 g of butane reacts with an excess of oxygen in the following reaction?

2 C4H10 + 13 O2 ⟶ 8 CO2 + 10 H2O

a)

181.1 g CO2

b)

90.6 g CO2

c)

11.32 g CO2

d)

119.6 g CO2

57.
What is the first thing you must do to solve a stoichiometry problem?
a)
Write a Balanced Equation
b)
Panic
c)
Write an Unbalanced Equation
d)
Ask for help
58.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of MgO to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
59.

Calculate the molar mass of Cu2O.

a)

37 g/mol

b)

45 g/mol

c)

79.5 g/mol

d)

143 g/mol

60.

Calculate the molar mass of KOH.

a)

28 g/mol

b)

56 g/mol

c)

84 g/mol

d)

112 g/mol

61.

During the process of reduction, _________________

a)

protons are lost.

b)

protons are gained.

c)

electrons are lost.

d)

electrons are gained

e)

neutrons are lost.

62.

Find the oxidation number of Ca in CaH2

a)

-2

b)

-4

c)

+2

d)

+4

e)

0

63.

Oxidation is....

a)

Gain of electrons

b)

Loss of electrons

c)

Both the loss and gain of electrons

d)

None of these

64.

Reduction is....

a)

Gain of electrons

b)

Loss of electrons

c)

Both the loss and gain of electrons

d)

None of these

65.
In the reaction
2Ca(s) + O2(g) --> 2CaO(s), calcium is __________
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
66.

In a redox reaction, spectator ions...

a)

become oxidised

b)

become reduced

c)

remain unchanged

67.
What substance is oxidized in the following reaction?
4Fe + 3O2 --> 2Fe2O3
a)
Iron
b)
Fluorine
c)
Oxygen
68.

Identify the substance that is reduced in the reaction between copper(II) ion and magnesium.

Cu2+ + Mg → Cu + Mg2+

a)

Cu2+

b)

Mg

c)

Cu

d)

Mg2+

69.

What is the oxidation number of O in elemental O2 ?

a)

0

b)

-2

c)

+1

d)

+2

70.
What is the oxidation number of Fe in FeO?
a)
+1
b)
-1
c)
+2
d)
-2

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