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Unit 6 Test Review (Chemical Reactions)

Total questions: 50

Worksheet time: 1hrs 15mins

Name
Class
Date
1.

What do you call the solid formed when you react two aqueous solutions?

a)

a precipitate

b)

a olid

c)

Displaced

d)

Decomposed

2.

Identify the following type of reaction.

a)

synthesis

b)

decomposition

c)

single-displacement

d)

combustion

3.

Identify the following the type of reaction.

a)

combustion

b)

double-replacement

c)

synthesis

d)

decomposition

4.
A neutralization reaction will (almost) always produce...
a)
water & salt
b)
water
c)
salt
d)
water & carbon
5.

A type of chemical that forms solutions that taste sour, due to high concentrations of positive hydrogen ions

a)

acid

b)

base

c)

salt

d)

pH

6.
H3PO4 is an example of a ...
a)
acid
b)
base
c)
salt
7.
Zn(OH)2 is an example of a...
a)
acid
b)
base
c)
salt
8.

Complete the following reaction:

HCl + Mg(OH)2 -->

a)

MgCl2 + H2O

b)

Mg +H2O

c)

MgCl2 + H2

d)

MgCl2 + H2O + CO2

9.

What is the equivalence point of a titration?

a)

Where the amount of acid and base are equal as shown by a color change

b)

Where there is no base

c)

When the volume of base in the burette is used up

d)

When there is no acid

10.
A solution with a pH of 3.6 would be...
a)
Acid
b)
Base
c)
Neutral
d)
Acid and Base
11.
A solution with a pH of 8.6 would be...
a)
Acid
b)
Base
c)
Neutral
d)
Acid and Base
12.
A solution with a pH of 7.0 would have...
a)
more H ions than OH ions
b)
more OH ions than H ions
c)
equal number of H and OH ions
d)
None of these.
13.

Which of the following is the strongest acid?

a)

1

b)

5

c)

3

d)

8

14.

How does a catalyst work in speeding up a reaction?

a)

By lowering the activation energy or reaction

b)

by giving them more energy

c)

by making them more available

15.
During an endothermic reaction in a beaker if we are part of the surroundings and touched the beaker, it would feel _______. 
a)
Warm
b)
Cold
16.
If a chemical reaction is EXOTHERMIC, the temperature would....
a)
Stay the same
b)
Increase
c)
Decrease
17.
Is this reaction endothermic or exothermic?
a)
endothermic 
b)
exothermic
18.

A solid substance was tested in the laboratory. The test results are listed below.

• dissolves in water

• is an electrolyte

• melts at a high temperature

Based on these results, the solid substance could be

a)

Cu

b)

CuBr2

c)

C

d)

C6H12O6

19.

A substance that conducts an electrical current when dissolved in water is called

a)

catalyst

b)

metalloid

c)

electrolyte

d)

nonelectrolyte

20.

Which of the following is not an electrolyte?

a)

KBr

b)

LiOH

c)

RbNO3

d)

CH4

21.

What precipitate forms when you mix Pb(NO3)2 with NaCl?

a)

sodium nitrate 

NaNO3

b)

lead (II) chloride 

PbCl2

c)

sodium lead

NaPb

d)

chloride nitrate 

ClNO3

22.

Which of the following is the correct definition for a strong acid?

a)

Partially dissociates into ions when dissolved in water and the change is not reversible

b)

Fully dissociates into ions when dissolved in water and the change is not reversible

c)

Fully dissociates into ions when dissolved in water and the change is reversible

d)

Partially dissociates into ions when dissolved in water and the change is reversible

23.

The amount of solute dissolved in a measure of solvent is______

a)

dilute

b)

concentration

c)

volume

d)

density

24.
What element is being Oxidized?
a)
N
b)
H
c)
O
d)
S
25.
Is calcium oxidized or reduced in the following reaction? 
2 CaO--> 2 Ca + O2
a)
Oxidized
b)
Reduced
26.
Which of the following half reactions correctly represents a reduction half reaction?
a)
Fe →Fe2+ + 2e-
b)
Pb4+ + 2e- →Pb2+
c)
2O-2 →O2 + 4e-
d)
Fe + 3e- →Fe3+
27.

In a redox reaction, spectator ions...

a)

become oxidised

b)

become reduced

c)

remain unchanged

28.
What is oxidation number of Cr in Cr2O72-?
a)
-2
b)
+2
c)
+6
d)
+12
29.
What is oxidation number of O in O2 ?
a)
0
b)
-2
c)
+1
d)
+2
30.
What is the oxidation number of N in NO2-1?
a)
-3
b)
+4
c)
-2
d)
+3
31.

Which is oxidized and which is reduced?

Ca + Na2O → Na + CaO

a)

Oxidized: Na Reduced: O

b)

Oxidized: Ca Reduced: O

c)

Oxidized: Na Reduced: Ca

d)

Oxidized: Ca Reduced: Na

32.

Which reaction is an example of a neutralization reaction?

a)

AgNO3(aq) + KI(aq) --> AgI(s) + KNO3(aq)

b)

Cu + 2 AgNO3 --> Cu(NO3)2 + 2 Ag

c)

2 KOH + H2SO4 -> K2SO4 + 2 H2O

d)

Ba + 2 HCl --> BaCl2 + H2

33.

Which reaction is an example of a displacement reaction?

a)

AgNO3(aq) + KI(aq) --> AgI(s) + KNO3(aq)

b)

Cu + 2 AgNO3 --> Cu(NO3)2 + 2 Ag

c)

2 KOH + H2SO4 -> K2SO4 + 2 H2O

d)

Ba(OH)2 + 2 HCl -> BaCl2 + 2H2O

34.

Which reaction is an example of a precipitation reaction?

a)

AgNO3(aq) + KI(aq) --> AgI(s) + KNO3(aq)

b)

Cu + 2 AgNO3 --> Cu(NO3)2 + 2 Ag

c)

2 KOH + H2SO4 -> K2SO4 + 2 H2O

d)

Ba(OH)2 + 2 HCl -> BaCl2 + 2H2O

35.
What is the molarity of 4 grams of sodium chloride in 3,800 mL of solution?
a)
0.018 M
b)
0.018 mol
c)
1.052 M
d)
1.052 mol
36.
How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?
a)
0.625 g NaCl
b)
625 g NaCl
c)
36.5 g NaCl
d)
0.04 mol NaCl
37.
The substance being dissolved in a solution.
a)
sands
b)
solute
c)
solvent
d)
alloy
38.
The substance in which a solute is dissolved
a)
sands
b)
solvent
c)
alloy
d)
negative particles
39.
An indicator will ______________ when it is in contact with an acid or base
a)
Bubble
b)
Form a new substance
c)
Change color
d)
Stay the same color
40.

When carbonates react with acids, which gas is produced?

a)

Hydrogen

b)

Carbon dioxide

c)

Oxygen

d)

Nitrogen

41.
Acid + Metal --> ?
a)

Salt + Water

b)

Salt + Hydrogen gas

c)

Salt + CO2 gas

d)

a Precipitate

42.
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)
43.

____________ is the process whereby particles of a solvent completely surround the particles of a solute, disperse them throughout the solvent particles, and hold them in solution.

a)

solvation

b)

immisciblation

c)

dissolution

d)

saturation

44.

A non-electrolyte is composed of __________in solution

a)

molecules

b)

molecules and ions

c)

ions

d)

none of the above

45.

Which of the following shows the solvation of Na2CO3 in water?

a)

2Na+ + CO3-2

b)

2Na + CO3

c)

Na+1 + C-4 + O-2

d)

Na2CO3(l)

46.

Which of the following shows the solvation of C2H6O in water?

a)

2C-4 + H2O

b)

C2H6O(aq)

c)

2C-4 + 6H+1 + O-2

d)

C2H6O(l)

47.

Which of the following substances is an organic acid?

a)

HCl

b)

CH3COOH

c)

C2H5OH

d)

C2H5NH2

48.

A basic substance:

a)

is a proton donor

b)

is a proton acceptor

49.

What is the oxidation number of carbon in carbon dioxide CO2?

a)

-1

b)

-2

c)

-4

d)

+4

e)

+2

50.

Batteries create electrical energy by a controlled redox reaction while humans also generate energy through redox via oxidizing carbon compounds (in aerobic respiration).

a)

True

b)

False

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