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Solubility and Net Ionic equations

Total questions: 100

Worksheet time: 2hrs 35mins

Name
Class
Date
1.

Which of the following is MOST reactive?

a)

Magnesium

b)

Lead

c)

Tin

d)

Copper

e)

Zinc

2.

Which metal is more reactive than calcium?

a)

magnesium

b)

potassium

c)

silver

d)

aluminum

3.

Choose the least reactive metal

a)

calcium

b)

magnesium

c)

iron

d)

copper

4.

What does displacement mean?

a)

A chemical reaction where a less reactive metal takes the place of a more reactive metal in a compound.

b)

A chemical reaction where a more reactive metal takes the place of a less reactive metal in a compound.

c)

A more reactive metal is removed from a compound.

5.

Magnesium chloride + Sodium → ?

a)

Sodium chloride + Magnesium

b)

Magnesium chloride + Sodium (No change)

c)

Sodium magnesium + Chlorine

6.

Lithium chloride + Iron → ?

a)

Lithium chloride + Iron (No change)

b)

Iron chloride + Lithium

c)

Lithium oxide + hydrogen

7.

Zinc sulphate + Magnesium → ?

a)

Magnesium + Sulphur + Hydrogen

b)

Zinc sulphate + Magnesium

c)

Magnesium sulphate + Zinc

8.

Iron nails + copper oxide → ?

a)

Iron nails + copper oxide

b)

Iron oxide + copper oxide

c)

Iron oxide + copper

d)

Magic

9.
Which of the following is arranged according increasing reactivity?
a)
Mg > Li > Na > K
b)
Mg > Na > Li > K
c)
Na > Li > Mg > K
d)
K > Mg > Na > Li
10.
Which one of the following equations correctly represents the reaction of silver nitrate with copper metal?
a)
CuNO3(aq) + Ag(s) → Cu(s) + AgNO3(aq)
b)
Cu(s) + 2 AgNO3(aq) → Cu(NO3)2(aq) + 2 Ag(s)
c)
Cu(s) + AgNO3(aq) → CuNO3(aq) + Ag(s)
d)
Cu(s) + Ag(NO3)2(aq) → Cu(NO3)2(aq) + Ag(s)
11.
When scrap iron is added to blue copper sulphate solution, a pinky-brown deposit is formed and a pale green solution is left above it. The pale green solution is of?
a)
 iron oxide
b)
copper chloride
c)
sulphuric acid
d)
iron sulphate
12.
If the metal is more reactive than the metal in the compound it completes with the less reactive metal. Therefore, it can concluded that ...
a)
The less reactive metal repel the more reactive metal from its compound
b)
The more reactive metal bonded with  the less reactive metal from its compound
c)
The less reactive metal pushes out or displaces the more reactive metal from its compound
d)
The more reactive metal pushes out or displaces the less reactive metal from its compound
13.
What will be reaction if less reactive metal is added in a solution with more reactive metal compound?
a)
vigorous reaction
b)
fizzing gas produced
c)
burns moderately
d)
no reaction
14.
Which of the following will not undergo reaction?
a)
zinc metal  +  zinc oxide 
b)
iron metal  +  copper oxide
c)
zinc metal +  iron oxide
d)
magnesium  +  iron oxide
15.
When a metal reacts with oxygen gas, the product is ...
a)
metal hydroxide
b)
metal oxide
c)
metal oxide and oxygen
d)
metal hydroxide and hydrogen gas
16.

A more reactive metal will displace a less reactive metal from a metal compound. Which metal is more reactive - copper or iron?

a)

copper

b)

iron

17.

Copper is less reactive than iron. What do you expect to happen when copper is placed inside a solution of iron(II) sulfate?

a)

No reaction takes place.

b)

A reaction takes place. And a colour change is observed.

18.

Copper is less reactive than iron. What do you expect to happen when iron is placed inside a solution of copper(II) sulfate?

a)

No reaction takes place.

b)

A reaction takes place. And a colour change is observed on the iron nail.

19.
Acid + Metal --> ?
a)
Salt + Water
b)
Salt + Hydrogen
c)
Salt
d)
Hydrogen
20.

Iron + Hydrochloric acid --> ?

a)

iron(II) sulfate + water

b)

iron + hydrogen

c)

iron(II) chloride + hydrogen

d)

iron(II) chloride + water

21.

Which equation correctly shows the displacement of copper from copper(II) sulfate by zinc?

a)

copper + zinc sulfate --> copper(II) sulfate + zinc

b)

zinc sulfate + copper --> copper(II) sulfate + zinc

c)

copper(II) sulfate + zinc --> zinc sulfate + copper

d)

copper(II) sulfate + zinc --> zinc sulfate + water

22.

Which equation correctly shows magnesium displacing copper from it copper(II) sulfate?

a)

2Mg + O2 --> 2MgO

b)

Mg + CuSO4 --> MgSO4 + Cu

c)

Mg + MgSO4 --> MgSO4 + Mg

23.

A copper coil is placed inside a solution of silver nitrate. What would you expect to see after 5 minutes? Choose 2 options.

a)

There is no visible change because no displacement reaction took place. Copper, being less reactive than silver, cannot displace silver from silver nitrate.

b)
c)
d)

Silver crystals were formed on copper coil, because copper (being more reactive than silver) displaced silver from silver nitrate.

24.

Read the underlined words carefully. Rank the metals according to decreasing reactivity (most reactive to least reactive).

a)

Metal A, B, C, D

b)

Metal A, C, B, D

c)

Metal B, C, D, A

d)

Metal D, B, C, A

25.

In this reactivity series, which of these metals is the most reactive?

a)

Gold

b)

Zinc

c)

Potassium

26.

In the reactivity series, which metal is the least reactive?

a)

Gold

b)

Potassium

27.

Which gas is always produced when a metal reacts with water?

a)
Oxygen
b)
Carbon Dioxide
c)
Hydrogen
d)
Carbon Monoxide
28.

which of the following is the correct equation for when a metal reacts with acids ?

a)

metal + acid ➯ salt +hydrogen+nitrogen

b)

metal +acid ➯ salt + hydrogen

c)

metal + acid ➯hydrogen

d)

metal +acid ➯ salt

29.

if water only reacts with those metal/metals above hydrogen , then which metal/metals do not react with water ?

a)

gold

b)

silver

c)

copper

d)

all of the above

30.

if water only reacts with those metals above hydrogen , then which of the following will react with water ?

a)

potassium

b)

sodium

c)

gold

d)

copper

e)

hydrogen

31.

Magnesium chloride + Sodium → ?

a)

Sodium chloride + Magnesium

b)

Magnesium chloride + Sodium (No change)

c)

Sodium magnesium + Chlorine

d)

Magnesium sodium chloride

32.

Which of the following does not react with water?

a)

Lithium

b)

Magnesium

c)

Lead

d)

Calcium

33.

Which one of the following metals reacts most vigorously with cold water?

a)

Sodium

b)

Magnesium

c)

Copper

d)

Zinc

34.

What element rusts?

a)

Carbon

b)

Iron

c)

Manganese

d)

Potassium

35.

The student used measuring instruments to measure some of the variables.

Choose the correct measuring instrument used to measure the volume of metal sulfate.

a)

Measuring cylinder

b)

Ruler

c)

Balance

d)

Thermometer

e)

Test tube

36.

Use the results shown in table to place zinc, copper and magnesium in order of reactivity from most reactive to least reactive.

a)

zinc, copper, magnesium

b)

magnesium, zinc, copper

c)

magnesium, copper, zinc

d)

copper, zinc, magnesium

37.

Which metal is found in the Earth as the metal itself?

a)

calcium

b)

gold

c)

lithium

d)

potassium

38.

Iron is found in the Earth as iron oxide (Fe2O3).

Iron oxide is reduced to produce iron.

Which is the correct equation for the reaction.

a)

Fe2O3 + C → Fe + CO2

b)

Fe2O3 + C → 2Fe + CO3

c)

2Fe2O3 + 3C → 4Fe + 3CO2

d)

2Fe2O3 + 3C → Fe4 + 3CO2

39.

What is meant by reduction?

a)

Gain of iron

b)

Gain of oxide

c)

Loss of iron

d)

Loss of oxygen

40.
The alkali metals are in group 1, on the far left of the periodic table. Which of these is NOT an alkali metal?
a)
Lithium
b)
Iron
c)
Potassium
d)
Francium
41.
How can you tell that a metal is reacting with water?
a)
Colour change
b)
Bright light
c)
Fizzing
d)
It gets colder
42.
What else is produced when a metal reacts with water? (HINT: Water has the formula H2O)
a)
Metal Oxide
b)
Metal Carbonate
c)
Metal Hydride
d)
Metal Hydroxide
43.
When copper and magnesium sulphate are mixed together, there is no reaction. Why?
a)
Magnesium is more reactive than copper
b)
Copper is more reactive than magnesium
c)
Copper never reacts with metal salts
d)
Magnesium Sulphate never reacts with metals
44.
What is the correct equation when potassium reacts with water?
a)
2K (s) + H2O (l) -->  KOH (aq) + H2 (g)
b)
K (s) + 2H2O (l) -->  KOH (aq) + 2H2 (g)
c)
2K (s) + 2H2O (l) -->  2KOH (aq) + H2 (g)
d)
K (s) + H2O (l) -->  KOH (aq) + H2 (g)
45.
Which of the following is the correct equation when aluminum reacts with sulfuric acid?
a)
2Al (s) + 3H2SO4 (aq) -->  Al2(SO4)3 (aq) + 3H2 (g)
b)
2Al (s) + 3H2SO4 (aq) -->  Al2(SO4)3 (l) + 3H2 (s)
c)
2Al (s) + 3H2SO4 (l) -->  Al2(SO4)3 (l) + 3H2 (g)
d)
2Al (s) + 3H2SO4 (s) -->  Al2(SO4)3 (l) + 3H2 (g)
46.
Complete the following equation: 
2Cu (s)  +  O2 (g)  -->
a)
2CuO (s)
b)
2CuO (g)
c)
4CuO (s)
d)
2CuO (g)
47.
Complete the following equation: 
4Fe (s)  +  3O2 (g) -->
a)
4Fe2O3 (s)
b)
2FeO (s)
c)
2Fe2O3 (s)
d)
4FeO (s)
48.
Which of the following will not undergo reaction?
a)
zinc metal  +  zinc oxide 
b)
iron metal  +  copper oxide
c)
zinc metal +  iron oxide
d)
magnesium  +  iron oxide
49.

What is the most likely identity of the metal on the filter paper?

a)

Copper, because it is grey.

b)

Potassium, because it can be cut with a knife showing it is soft.

c)

Iron, because it looks grey and all iron looks grey.

50.

Complete the word equation below.


Magnesium + oxygen --> .....

a)

Magnesium

b)

Magnesium oxide

c)

Oxides

d)

Magnesium oxide + water

51.

Magnesium is more reactive towards oxygen compared to

a)

Calcium

b)

Zinc

c)

Sodium

d)

Potassium

52.

If carbon can remove oxygen from a metal oxide, it means carbon is ___________ reactive than the metal.

a)

more

b)

less

53.

The most reactive metal in the reactivity series of metals is ______________.

a)

Calcium

b)

Potassium

c)

Magnesium

d)

Aluminium

54.

Iron is located between ______________ and _______________ in the reactivity series.

a)

Zinc

b)

Oxygen

c)

Gold

d)

Copper

e)

Potassium

55.

What is the gas released when potassium manganate is heated?

a)

Hydrogen

b)

Oxygen

c)

Carbon dioxide

d)

Carbon monoxide

56.

Potassium is a metal that is ........ in the series

a)

low

b)

high

c)

very high

d)

very low

57.

Sodium does not exist as a free element in nature because it is a very reactive metal.

a)

TRUE

b)

FALSE

58.

Aluminum and Copper Sulfate produces

a)

Al(SO4)3 and Cu

b)

Al and CuSO4

c)

Al2(SO4)3 and Cu

d)

No reaction

59.

Iron and Plumbous Nitrate produces

a)

Fe + Pb(NO3)2 --> Pb + Fe(NO3)2

b)

Fe + PbNO3 --> Pb + Fe(NO3)2

c)

Fe + Pb(NO3)2 --> Pb + FeNO3

d)

no reaction

60.

Magnesium and hydrochloric acid produces

a)

Mg + HCIO --> H + MgCl2

b)

Mg + 2HCI --> H2 + MgCl2

c)

Mg + HCI --> H2 + MgCl2

d)

no reaction

61.

Copper and Ferrous Sulfate produces

a)

Cu + FeSO4 --> CuSO4 + Fe

b)

Cu + Fe2(SO4 )3--> CuSO4 + Fe

c)

Cu + Fe2SO4 --> CuSO4 + Fe

d)

no reaction

62.

Silver and Potassium nitrate produces

a)

K + AgNO3

b)

K + AgNO2

c)

K + Ag(NO3)2

d)

no reaction

63.

Calcium and magnesium nitrite produces

a)

2 Ca + Mg(NO3)2 --> 2 CaNO3 + Mg

b)

Ca + Mg(NO2)2 --> Ca(NO2)2 + Mg

c)

Ca + Mg(NO3)2 --> Ca(NO3)2 + Mg

d)

no reaction

64.

Copper (II) Bromide + Aluminum Chloride produces

a)

CuBr + AlCl --> CuCl + AlBr

b)

3 CuBr2 + 2 AlCl3 --> 3 CuCl2 + 2 AlBr3

c)

3 CuBr + 2 AlCl3 --> 3 CuCl2 + 2 AlBr

d)

No Reaction

65.

Calcium Hydroxide and Phosphoric acid

a)

CaOH + HPO4 --> CaPO4 + H2O

b)

2 Ca(OH)2 + 2 HPO4 --> 3 CaPO4 + 2 H2O

c)

3 Ca(OH)2 + 2 H3PO4 --> Ca3(PO4)2 + 6 H2O

d)

no reaction

66.
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)
67.
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) →
68.
What are the spectator ions in the reaction of sodium chloride with silver nitrate?
a)
silver and nitrate
b)
sodium and chloride
c)
sodium and nitrate
d)
silver and chloride
69.
What are the spectator ions in this reaction?
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
 
a)
Cu2+ and OH1-
b)
Na2+ and Cl2-
c)
Na1+ and Cl1-
d)
Na1+ and OH1-
70.
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)
71.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl1- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl1- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
72.
In the reaction Zn + H2O → ZnO2 + H2 which element is oxidized? 
a)
Zinc
b)
Hydrogen
c)
Oxygen
d)
None
73.
In the reaction
2Ca(s) + O2(g) → 2CaO(s), calcium is...
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
74.
What substance is oxidized in the following reaction? 
Fe+2 + MnO4  → Fe+3 + Mn+2   
a)
Fe+2
b)
Mn+3
c)
Mn+2
d)
MnO4
75.
What is the oxidation number of N in NO2-1?
a)
-3
b)
+4
c)
-2
d)
+3
76.
What is oxidation number of P in K3PO4?
a)
+1
b)
+5
c)
-2
d)
0
77.
Which of these lists contains only soluble substances? Don't forget that the halides (family 17) will form precipitates with Ag+, Pb2+ and Hg2+.
a)
sodium nitrate, potassium chloride, calcium carbonate
b)
lead nitrate, lead chloride, lead sulfate
c)
calcium nitrate, copper chloride, ammonium phosphate
d)
silver nitrate, barium sulfate, copper carbonate
78.
What element is being Oxidized?
a)
N
b)
H
c)
O
d)
S
79.

Give the oxidation number of Nitrogen and Oxygen in N2O molecule.

a)

Nitrogen +1, Oxygen -2

b)

Nitrogen -1, Oxygen -2

c)

Nitrogen +2, Oxygen -2

d)

Nitrogen -3, Oxygen -2

80.

Give the oxidation number for the underlined atoms below.

a)

+4

b)

-3

c)

-4

d)

0

81.

Identify ALL substances that CANNOT be broken apart in a net ionic equation.

a)

Solids

b)

Liquids

c)

Aqueous solutions

d)

Gases

82.

For the following complete ionic equation, identify the correct net ionic equation:

2 NH4+ (aq) + S2- (aq) + 2 H+ (aq) + 2 Cl- (aq) --> H2S (g) + 2 NH4+ (aq) + 2 Cl- (aq)

a)

S2- (aq) + 2 H+ (aq) --> H2S (g)

b)

2 NH4+ (aq) + 2 H+ (aq) --> H2S (g) + 2 NH4+ (aq)

c)

S2- (aq) + 2 Cl- (aq) --> 2 NH4+ (aq) + 2 Cl- (aq)

d)

2 NH4+ (aq) + 2 Cl- (aq) --> H2S (g) + 2 NH4+ (aq) + 2 Cl- (aq)

e)

None of the equations are correct

83.

Ba(OH)2

a)

strong electrolyte

b)

weak electrolyte

c)

non - electrolyte

84.

CO2

a)

strong electrolyte

b)

weak electrolyte

c)

non electrolyte

85.

What makes a solution a WEAK electrolyte?

a)

When the solute completely ionizes in water.

b)

When the solute doesn't dissolve in water.

c)

When the solute partially ionizes in water.

d)

When the solute is not added to the water.

86.

Four chemical solutions are shown above. Which of the following solutions would correspond to a weak electrolyte?

a)

IV

b)

III

c)

II

d)

I and II

87.

What is a Net Ionic Equation?

a)

a balanced chemical equation in which all the reactants and products are given by their chemical formulae.

b)

a chemical equation that shows all soluble species broken into their respective ions.

c)

a chemical equation showing only the species which are actively involved in the reaction.

88.

What is the correct net ionic equation for the reaction between HBr(aq) and LiOH(aq)?

a)

2 H+(aq) + O2-(aq) → H2O(l)

b)

2 H2 (aq) + O2(aq) → 2 H2O(l)

c)

2 H2 (g) + O2(g) → 2 H2O(l)

d)

H+(aq) + OH-(aq) → H2O(l)

89.

Hydrobromic acid              +             Lead (II) perchlorate

What is the net ionic equation?

a)

Br- +  Pb2+  --> PbBr2

b)

H+  +   Br- +  Pb2++ ClO4- --> H++  ClO4-+  PbBr2

c)

H+  +   Br- +  Pb2++ ClO4- --> HClO4 +  PbBr2

d)

HBr +  Pb2++ ClO4- --> HClO4 +  PbBr2

90.

Net ionic equation for

Nitrous acid and potassium hydroxide

a)

HNO3 + OH−→NO3−+H2O

b)

HNO2 + OH−→NO−2+H2O

c)

H+ + OH−→H2O

d)

HNO2 + OH−→NO2−+H2O

91.

Net Ionic equation for

Hydrochloric acid and ammonia

a)

HCl + NH4→NH4+ + Cl-

b)

HCl + NH3→NH4Cl

c)

HCl + NH3→NH4+ + Cl-

d)

H+ + NH3→NH4+

92.

Hydrochloric and Sodium sulfide

a)

H+ + S2- → H2S

b)

no reaction

c)

H+ + S2- → H2S + Cl2

93.

Net ionic for the decompositon of sulfurous acid

a)

H+ + SO3 2- → H2O + SO3

b)

H2SO4 → H2O + SO3

c)

H2SO3 → H2O + SO2

94.

Hydrochloric acid and sodium bicarbonate

net ionic reaction

a)

H+ + HCO3- → H2O + CO2

b)

no reaction

c)

H+ + HCO3- → H2O + CO2 + Cl-

d)

H+ + Na + + HCO3- → H2O + CO2 + Cl-

95.
Which is the name of the kind of solid substance formed in this figure?  
a)
aqueous 
b)
precipitate
c)
acid
d)
synthesis 
96.

When you mix magnesium nitrate and sodium hydroxide

a)

No precipitate

b)

NaOH

c)

NaNO3

d)

Mg(OH)2

97.

potassium chloride and sodium nitrate

a)

KNO3

b)

No precipitate

c)

NaCl

d)

KCl

98.
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) →
99.
In this equation,
CuCl2 + NaOH  → Cu(OH)2 + NaCl
Which product is insoluble?
a)
copper(II) hydroxide
b)
sodium chloride
c)
sodium hydroxide
d)
copper(II) chloride
100.

Which of the following pairs of solutions produces a precipitate when combined?

a)

Cu(NO3)2 and NaCl

b)

Fe(NO3)3 and MgCl2

c)

Cu(NO3)2 and K2CO3

d)

CaCl2 and NaNO3

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