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Unit 4 Test Review: Ionic Compounds and Thermochemistry

Total questions: 50

Worksheet time: 1hrs 2mins

Name
Class
Date
1.
Ionic compounds are bonds between
a)
Metals and Metals
b)
Metals and Nonmetals
c)
Nonmetals and Nonmetals
d)
None of the above
2.
Name this compound: 
NaBr
a)
Bromide sodide
b)
Sodium bromide
c)
Sodium bromate
d)
Sodium bromite
3.
Name this compound: 
KF
a)
Potassium fluoride
b)
Potassium fluorite
c)
Fluorine potasside 
d)
Potassium fluorate
4.
Name MgO
a)
Magnesium Oxygen
b)
Magnesium Oxide
c)
Magnesium Monoxide
d)
Magnesium Dioxide
5.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

6.

Which of the following combinations would need roman numerals in the name?

a)

potassium + fluorine

b)

beryllium + oxygen

c)

boron + iodine

d)

lead + oxygen

7.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

8.
What is the correct formula for Sodium Oxide?
a)
NaO
b)
NaO2
c)
Na2O
d)
Na2O2
9.

What is the correct molecular formula for barium hydroxide?

a)

Ba(OH)2

b)

Ba2OH

c)

BaOH

d)

Ba2OH

10.
What is the formula for copper(I) sulfate?
a)
CuSO3
b)
CuSO4
c)
Cu2SO3
d)
Cu2SO4
11.
PbS2
a)
lead sulfide
b)
lead sulfur
c)
lead II sulfide
d)
lead IV sulfide
12.
When a nonmetal gains electrons, it becomes this type of ion.
a)
Anion
b)
Cation
13.
When a metal loses electrons, it becomes this type of ion.
a)
anion
b)
cation
14.

What is the correct name for this polyatomic ion: OH–

a)

hydrogen carbonate

b)

oxonium

c)

hydroxide

d)

acetate

15.

What is the correct name for this polyatomic ion: NO3–

a)

carbonate

b)

hydroxide

c)

nitrite

d)

nitrate

16.

What is the correct name for this polyatomic ion: PO43–

a)

phosphorus tetroxide

b)

phosphate

c)

sulphate

d)

hydroxide

17.

What is the correct formula for the polyatomic ion called hydrogen carbonate?

a)

HCO3–

b)

CO32–

c)

CrO42–

d)

CN–

18.

What is the correct formula for the polyatomic ion called sulphate?

a)

SO32–

b)

HSO4–

c)

SO42–

d)

CH3COO–

19.

What is the correct formula for the polyatomic ion called ammonium?

a)

NH3+

b)

NH3

c)

CN+

d)

NH4+

20.

What is NO3- ?

(a)  

21.
What is the name of K3PO4?
a)
Tripotassium Phosphate
b)
Tripotassium Phosphite
c)
Potassium phosphide
d)
Potassium phosphate
22.
What is the name of Al(NO3)3?
a)
Aluminum trinitrate
b)
Monoaluminum nitrate
c)
Aluminum (III) nitrate
d)
Aluminum Nitrate
23.
What is the name of Mg(OH)2?
a)
Magnesium Hydride
b)
Magnesium Dihydride
c)
Magnesium Dihydroxide
d)
Magnesium Hydroxide
24.

The phosphate ion is written as

a)

PO-3

b)

PO3-4

c)

PO4-3

d)

PO4+3

25.

Which polyatomic ion is acetate?

a)

C2H3O21-

b)

C3H2O31-

c)

C2H2O31-

d)

C3H3O21-

26.

The potential energy diagram of a reaction is shown. Which statement below is correct relating to this reaction?

a)

#1 represents the enthalpy change for this exothermic reaction.

b)

#2 represents the enthalpy change for this endothermic reaction.

c)

#3 represents the enthalpy change for this endothermic reaction.

d)

#4 represents the enthalpy change for this exothermic reaction.

27.

During an exothermic reaction, heat content in the surroundings increases because

a)

heat energy is destroyed during reactions

b)

the reaction absorbs heat energy

c)

the energy contained in the reactants is lower then the products

d)

the energy contained in the products is lower than the reactants

28.

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)

29.

A cast iron skillet is used to fry bacon. For optimal frying, the pan must be heated to about 178 oC from a room temperature of 22.0 oC. It is known that 1.58 x 105 J of heat energy are absorbed by the pan to reach the desired temperature and the specific heat of iron is 0.450 J/g oC. What must the mass of the skillet be?

a)

12.7 kg

b)

2.25 kg

c)

110 kg

d)

1.97 kg

30.

The energy level diagram represents:

a)

exothermic reaction

b)

endothermic reaction

31.
How much heat does an aluminum block absorb if 10.00 grams ae heated from 25.0oC to 50.0oC? the specific heat of aluminum is .900J/goC
a)
450
b)
-450
c)
225
d)
-225
32.
The diagram represents which type of reaction
a)
endothermic
b)
exothermic
33.
A measure of the average kinetic energy of a substance.
a)
heat
b)
temperature
c)
enthalpy
d)
entropy
34.

What is the Heat of Reaction ΔH\Delta H  for this reaction?

a)

-200 KJ

b)

200 KJ

c)

400 KJ

d)

-300 KJ

35.

What type of reaction is this?

a)

Exothermic

b)

Endothermic

c)

Energy Producing

d)

No way to tell

36.

if more heat energy is released in making bonds in the products than is taken in when breaking bonds in the reactants

a)

Exothermic

b)

Endothermic

c)

Exotermic

d)

Endotermic

37.
H2 + 2 C + N2 + 270.3 kJ --> 2 HCN
Is this reaction endothermic or exothermic?
a)
Endothermic 
b)
Exothermic
38.

Calculate the amount of heat needed to increase the temperature of 2.0 g of iron (Fe) by  2 oC2\ ^oC  .

Given the specific heat capacity of iron is  0.44 Jg−1 oC−10.44\ Jg^{-1}\ ^oC^{-1}  

a)

0.88 J

b)

1.76 J

c)

0.44 J

d)

0.66 J

39.

Which of the following thermochemical equations illustrates an endothermic reaction?

a)
b)
c)
d)
40.
Refer the the following question:
2N2 + 3H2 --> 2NH3 + 46 kJ
How much energy would be produced if only 1 mol of nitrogen was reacted?
a)
92 kJ
b)
0.143 kJ
c)
23 kJ
d)
15 kJ
41.

the energy required to melt a solid at its melting point

a)

heat of reaction

b)

heat of formation

c)

Hess's law of heat summation

d)

heat of fusion

e)

heat of solution

42.

Which of these phase changes is an endothermic process?

a)

condensation

b)

evaporation

c)

freezing

d)

all phase changes are endothermic

43.

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

a)

endothermic process

b)

polythermic process

c)

exothermic process

d)

ectothermic process

44.

How much ammonia (NH3) can be melted by the addition of 2 kJ of heat (ΔHfus = 5.66 kJ/mol)

a)

.66 g

b)

3.6 g

c)

79.2 g

d)

6.0 g

45.

During a phase change temperature...

a)

may increase or decrease

b)

increase

c)

decreases

d)

stays the same

46.

How much energy must be removed to make 150.0 grams of water at 0.0 C freeze? ( °\degree Hfus = 6.00kJ/mol)

a)

900. J

b)

49.9 J

c)

900. kJ

d)

49.9 kJ

47.

Predict the products for the this Single Replacement reaction:

K + HCl →

a)

KCl + H2

b)

KHCl

c)

KH + Cl2

d)

HCl + K2

48.

Predict the products for the this Double Replacement reaction:

AgNO3 + KCl →

a)

AgCl + KNO3

b)

AgK + ClNO3

c)

KAg + NO3Cl

d)

AgCl + 3 KNO

49.

Predict the products for the this Single Replacement reaction: (Copper has a charge of 1+)

Mg + CuCl →

a)

MgCl2 + Cu

b)

Mg + Cu

c)

MgCu + Cl2

d)

MgCl + Cu2

50.

Given the equation Al2O3+3K2CO3+832kJ  →  Al2(CO3)3+3K2OAl_2O_3+3K_2CO_3+832kJ\ \ \rightarrow\ \ Al_2\left(CO_3\right)_3+3K_2O  , how much energy would be required to react 5 mol of potassium carbonate?

a)

1390 kJ

b)

499 kJ

c)

847 kJ

d)

838 kJ

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