Free Printable Revision Quiz

1.

Which of the following statement best describes an ionic bond?

a)

The sharing of electrons between two ions

b)

The strong electrostatic forces of attraction between cations and electrons

c)

The transfer of electrons between two atoms

d)

The strong electrostatic forces of attraction between oppositely charged ions

2.

What type of bond is illustrated above?

a)

Metallic

b)

Ionic

c)

Covalent

d)

Wiggly

3.

Which of the following compounds is formed by ionic bonding?

a)

HF

b)

PCl₅

c)

MgCl₂

d)

CH₄

4.

Which of the following properties of metal indicates that it can be drawn into wires?

a)

malleability

b)

ductility

c)

electrical conductivity

d)

flexibility

5.

Which of the following are some general physical properties of giant covalent compounds

a)

High melting and boiling points

b)

Insoluble in water

c)

Able to conduct electricity

d)

Brittle

6.

Which of the following compounds does not contain covalent bonds?

a)

$HCl$

b)

$NaNO_3$

c)

$\left(NH_4\right)_2CO_3$

d)

$CuCl_2$

7.

Elements on the LEFT side of the periodic table will most likely form:

a)

Positive ions

b)

Negative ions

c)

Neutral Ions

d)

None of these

8.

Which of the following gives the correct chemical formula for the compound Magnesium Phosphide?

a)

Mg₂P₃

b)

MgP

c)

Mg₃P₂

d)

MgP₂

9.

What is the little number after an element in a chemical formula mean?

Example: H₂

a)

It's just a number there is no meaning

b)

It means that there is a certain number of molecules in the substance

c)

It means that there is a certain number of atoms/ions of the element in the molecule

10.

Which of the following gives the correct chemical formula for the compound dinitrogen monoxide?

a)

NO

b)

N₂O

c)

N₂O₂

d)

O₂N₂

11.

At the end of chemical reactions, what is the total mass of the reactants compared to the total mass of the products?

a)

the product is doubled

b)

the product is half the mass of the reactants

c)

the mass is the same

d)

the mass changes depending on the reaction

12.

Is the equation balanced?:

$2H_2O\ +\ O_2\ \rightarrow\ 4MgO+Fe$

a)

Yes

b)

No

13.

Balance the following equation

......\ Fe\ \left(s\right)\ +\ ......\ O_2\ \left(g\right)\ \rightarrow\ ......\ Fe_2O_3\ \left(s\right)

a)

2 , 2 , 1

b)

2 , 3 , 2

c)

4 , 2 , 1

d)

4 , 3 , 2

14.

What is the right ratio of chemicals for the balanced chemical equation?

$.....\ AgNO_3+.....\ MgI_2\ \ \rightarrow\ \ .....\ AgI+.....\ Mg\left(NO_3\right)_2$

a)

1 , 2 , 1 , 2

b)

1 , 2 , 2 , 1

c)

2 , 1 , 1 , 2

d)

2 , 1 , 2 , 1

15.

Which of the following statements is INCORRECT?

a)

0.5 mol of potassium manganate(VII), $KMnO_4$ contains 1.0 mol of ions.

b)

1 mol of water contains $6.02\times10^{23}$ water molecules

c)

The mass of 1 mol of CaO is 56 g.

d)

In 152 g of carbon disulfide, there are 2.5 mol of carbon disulfide molecules.

16.

Determine the number of moles of calcium oxide formed when 10.0 g of calcium is burnt in a plentiful supply of oxygen?

a)

0.125 mol

b)

0.250 mol

c)

4.00 mol

d)

6.00 mol

17.

Find the empirical formula of a compound which contains 49.5% carbon, 5.2% hydrogen, 28.8% nitrogen and 16.5% oxygen by mass.

a)

$C_2HN_2O_2$

b)

$C_4H_5N_2O$

c)

$C_8H_5N_4O_2$

d)

$C_{19}H_2N_{11}O_6$

18.

Given that the empirical formula of a substance is $CHO_2$ , what is molecular formula of a substance with a molar mass of 90.0 g/mol?

a)

$CHO_2$

b)

$C_2HO_2$

c)

$C_2H_2O_2$

d)

$C_2H_2O_4$

19.

Phosphorus(III) chloride, $PCl_3$ , is made by the direct combination of phosphorus and chlorine.

$P_4\ \left(s\right)+6Cl_2\ \left(g\right)\ \rightarrow\ 4PCl_3\ \left(l\right)$

125 g of $P_4$ was reacted with 323 g of $Cl_2$ gas to produce phosphorus(III) chloride. Determine the limiting reactant in the reaction.

a)

Phosphorus

b)

Chlorine

c)

Phosphorus(III) chloride

20.

Phosphorus(III) chloride, $PCl_3$ , is made by the direct combination of phosphorus and chlorine.

$P_4\ \left(s\right)+6Cl_2\ \left(g\right)\ \rightarrow\ 4PCl_3\ \left(l\right)$

125 g of $P_4$ was reacted with 323 g of $Cl_2$ gas to produce phosphorus(III) chloride. Determine the mass of $PCl_3$ produced in the reaction.

a)

104 g

b)

417 g

c)

554 g

d)

626 g

21.

2.13 g of sodium chlorate(V) was heated to produce sodium chloride and oxygen.

$2NaClO_3\ \left(s\right)\ \rightarrow\ 2NaCl\ \left(s\right)+3O_2\ \left(g\right)$

What is the theoretical yield of the oxygen liberated from the reaction?

a)

0.160 g

b)

0.32 g

c)

0.480 g

d)

0.960 g

22.

2.13 g of sodium chlorate(V) was heated to produce sodium chloride and oxygen.

$2NaClO_3\ \left(s\right)\ \rightarrow\ 2NaCl\ \left(s\right)+3O_2\ \left(g\right)$

The theoretical yield of oxygen liberated is 0.960 g. However, only 0.775 g of oxygen was liberated. What is the percentage yield of the reaction?

a)

53.8 %

b)

80.7 %

c)

124 %

d)

I don't know

23.

Iron(III) oxide reacts with carbon monoxide to produce iron and carbon dioxide.

$Fe_2O_3\ \left(s\right)+3CO\ \left(g\right)\ \rightarrow\ 2Fe\ \left(s\right)+3CO_2\ \left(g\right)$

10.0 g of a sample of $Fe_2O_3\$ was reacted in excess CO and the iron produced was collected and measured. The mass of iron obtained was 5.60 g. Determine the percentage purity of the iron(III) oxide sample.

a)

62.5 %

b)

80.0 %

c)

125 %

d)

160 %

Revision Quiz

Total questions: 23

Worksheet time: 29mins

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