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Physical Science Chemistry Revision

Total questions: 73

Worksheet time: 3hrs 34mins

Name
Class
Date
1.

What charge do electrons have?

a)

Positive

b)

Neutral

c)

Negative

2.

How many electrons can the third shell have?

a)

Two

b)

Eight

c)

Five

d)

Three

3.

Which two particles are contained in the nucleus of an atom?

a)

Protons and Neutrons

b)

Protons and Electrons

c)

Electrons and Neutrons

4.
How many electron shells/levels does this atom have?
a)
1
b)
2
c)
3
d)
4
5.
How many neutrons does a sodium atom have? (Use the image to help you)
a)
23
b)
11
c)
12
d)
34
6.
How many Electrons are in one atom of Lithium?
a)
3
b)
6
c)
7
d)
6.941
7.

The electronic configuration of Ca is?

a)

2,8,8,2

b)

2,8,8,8,8,6

c)

2,8,8

8.
Mg2+ and Cl- create...
a)
Mg2Cl
b)
MgCl2
c)
Mg2Cl2
d)
MgCl
9.

Na+ and Cl- create...

a)

Na2Cl

b)

NaCl2

c)

Na2Cl2

d)

NaCl

10.

Potassium and Sulfur create...

a)

KS

b)

KS2

c)

K2S

d)

K2S2

11.

The chemical formula of Iron (III) and bromine is

a)

FeBr

b)

Fe(III)Br

c)

FeBr₃

d)

Fe₂Br₃

12.
Be careful with this question.....
SO4 -2  and  Al +3
a)
(SO4)3Al2
b)
(SO4)2Al3
c)
Al3SO4
d)
Al2(SO4)3
13.

What is the formula for copper(I) and sulfate?

a)

CuSO3

b)

CuSO4

c)

Cu2SO3

d)

Cu2SO4

14.
Balance this equation:
 2Li + Cl2 -> LiCl
a)
2Li + Cl2 -> 4LiCl2
b)
2Li + Cl2 -> LiCl2
c)
2Li + Cl2 -> 2LiCl
15.
The substances listed on the left side of a chemical equation are the
a)
Products
b)
Coefficients
c)
Precipitates
d)
Reactants
16.
In chemical reactions, what does the principle of conservation of mass mean?
a)
Matter is not created or destroyed.
b)
The total mass of the reactants is greater than the total mass of the products.
c)
The total mass of the reactants is less than the total mass of the products.
d)
Matter is not changed.
17.
How many Hydrogen (H) atoms are in NH3O5
a)
3
b)
4
c)
5
d)
1
18.
Name the part in red:

H2 + O2 -> H2O
a)
Coefficient
b)
Product
c)
Yield
d)
Subscript
19.
Name the part in red:

_2_H2 + _1_O2 -> _2_H2O
a)
Coefficient
b)
Product
c)
Yield
d)
Subscript
20.
Name the part in red:

H2 + O2 -> H2O
a)
Coefficient
b)
Product
c)
Reactant
d)
Subscript
21.
Name the part in red:

H2 + O2 -> H2O
a)
Coefficient
b)
Product
c)
Reactant
d)
Subscript
22.
Which number should go in the blank?
_ H2 + O2 -> 2 H2O
a)
1
b)
2
c)
3
d)
0
23.
Is the following equation balanced or unbalanced ? 
Al + O2 --> Al2O3
a)
Balanced
b)
Unbalanced
24.
How many hydrogens are in 4H2O?
a)
6
b)
8
c)
2
d)
4
25.
 Balance this equation:

__ Al + __ HCl → __ H2 + __ AlCl3
a)
2, 6, 3, 2
b)
it is already balanced
c)
4, 12, 3, 4
d)
2, 1, 4, 5
26.
A sealed test tube containing 8 grams of iron filings and 5 grams of sulfur is heated until the material in the test tube glows bright red.  What is the mass of products? 
a)
Mass is less than 13 grams
b)
Mass is equal to 13 grams
c)
Mass is greater than 13 grams
d)
Mass cannot be measured
27.
Which problem is balanced?
a)
PbO2 + 2H2
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
28.

Iron filings are reacted with dilute hydrochloric acid to form iron(II) chloride and hydrogen gas. What is the missing state symbol in the equation below?


Fe(s) + 2HCl(l) → FeCl2(aq) + H2 (a)  

29.
How many atoms are there TOTAL in:
H2SO4
a)
6
b)
5
c)
7
d)
3
30.
Oxides ion
a)
O²⁻
b)
O³⁻
c)
O²⁺
d)
O⁻
31.
Hydroxide ion
a)
OH²⁻
b)
OH⁻
c)
OH⁺
d)
OH²⁺
32.
Sodium ion
a)
Na²⁺
b)
K²⁺
c)
Li⁺
d)
Na⁺
33.
Potassium ion
a)
Na⁺
b)
K⁺
c)
K²⁺
d)
K⁻
34.
Carbonate ion
a)
 CO₃²⁻
b)
CO₃³⁻
c)
CO₃⁻
d)
CO²⁻
35.
Sulphate ion
a)
SO⁴₂₋
b)
SO₄²⁻
c)
SO₃²⁻
36.
Ammonium ion
a)
NH₃⁺
b)
NH₄⁻
c)
NH₄⁺
d)
NH₃²⁻
37.
Chlorides ion
a)
Cl²⁻
b)
Cl⁻
c)
Cl₂⁻
38.
Zinc ion
a)
Zn²⁺
b)
Zn³⁺
c)
Zn⁺
d)
Zn²⁻
39.
Hydrogen ion
a)
H⁺
b)
H⁻
c)
H²⁺
d)
H²⁻
40.
Nitrates ion
a)
NO₃²⁻
b)
NO₄⁻
c)
NO₃⁻
d)
NO₃²⁻
41.
Bromide ion
a)
Br⁻
b)
Br²⁻
c)
Br⁺
42.

What is a mole ratio?

a)

An animal that burrows underground.

b)

How many moles of reactant are used up in a chemical reaction.

c)

The ratio of a reactant / product to a different one - compared by the number of particles.

d)

The process by which we multiply fractions by using numbers from a chemistry problem.

43.

2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

Ethane (C2H6) combusts in the above reaction. What is the mole ratio of ethane to oxygen gas?

a)
b)
c)
d)
44.

2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

Ethane (C2H6) combusts in the above reaction. What is the mole ratio of carbon dioxide to water?

a)
b)
c)
d)
45.

2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

New problem: How many moles of ethane (C2H6) are required to produce 13.5 moles of water from the above reaction?

a)

4.5 mol C2H6

b)

27 mol C2H6

c)

40.5 mol C2H6

d)

81 mol C2H6

e)

162 mol C2H6

46.

2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

New problem: If 3.5 moles of oxygen gas are used up as ethane combusts completely, how many moles of carbon dioxide are produced?

a)

0.5 mol CO2

b)

0.57 mol CO2

c)

2.0 mol CO2

d)

3.0 mol CO2

e)

3.5 mol CO2

47.

Which of the following statements regarding the mole is INCORRECT?

a)

A mole is a unit of quantity equal to 6.02 x 1023 particles.

b)

The number of particles in a mole is known as Avogadro’s number.

c)

A mole of particles of an element is numerically equal to the atomic mass of the element.

d)

none of the above

48.

What is the molar mass of PbSO4?

a)

303.27 g/mol

b)

255.27 g/mol

c)

163.87 g/mol

d)

372.27 g/mol

49.

What is the molar mass of PbSO4?

a)

303.27 g/mol

b)

255.27 g/mol

c)

163.87 g/mol

d)

372.27 g/mol

50.

How many formula units are in 2.5 moles of NaCl?

a)

1.5 x1024 formula units

b)

1.5 formula units

c)

4.2 formula units

d)

4.2 x10-24 molecules

51.
How many molecules are there in 31.8 moles of water?
a)
5.28 x 10-23 molecules
b)
1.91 x 1025 molecules
c)
5.28x 10-25
d)
1.91 x 1022
52.

What is the mass of 1.2 x 1024 atoms of C?

a)

2.0 grams

b)

24 grams

c)

0.17 grams

d)

1.4 x 1025 grams

53.

How many grams are in 1.2 moles of neon?

a)

0.059 grams

b)

7.2 x 1023 grams

c)

2.0 x 10-24 grams

d)

24 grams

54.

Calculate the number of atoms in 0.0340 g Zn.

a)

5.20 x 10-4 atoms Zn

b)

3.13 x 1023 atoms Zn

c)

3.13 x 1020 atoms Zn

d)

2.05 x 1022 atoms Zn

55.
How many formula units are there in 2.45 moles potassium chloride?
a)
4.07 x 10-24 
b)
1.47 x 1024 
c)
1.47
d)
4.07
56.

To melt the ice, Juan throws 455 g of calcium chloride, CaCl2 on his sidewalk. How many moles of CaCl2 did he throw?

a)

50,500 moles

b)

4.10 moles

c)

7.56 x 10-22 moles

d)

111 moles

57.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
58.

Select the correct molar ratio taken from this balanced equation:


1 N­2 + 3 H2 --> 2 NH3

a)

1 N­2 = 3 H2

b)

1 mol N­2 = 2 mol NH3

c)

2 mol N­2 = 1 mol NH3

d)

3 mol N­2 = 3 mol NH3

59.

1 N­2 + 3 H2 --> 2 NH3


How many moles of NH3 will be produced from 10.2 x 10^25 molecules of H2?


(6.02 x 10^23 molecules H2= 1 mol H2)

a)

113 mol NH3

b)

254 mol NH3

c)

169 mol NH3

d)

508 mol NH3

60.
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
61.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
62.

When you make a dilution, which of these values remains constant?

a)

The molarity (M)

b)

The total moles of solute

c)

The volume (V)

d)

The concentration

63.

As we dilute a solution.....

a)

The volume increases and the molarity (M) increases

b)

The volume increases and the molarity (M) decreases

c)

The volume decreases and the molarity (M) increases

d)

The volume decreases and the molarity (M) decreases

64.

Calculate the Molarity in a solution containing 40.0 g of NaCl dissolved in 500.0 ml of H2O.

a)

0.08 M

b)

12.5 M

c)

1.37 M

d)

0.74 M

65.

A solution is made by dissolving 0.50 mole of NaCl in enough water to give a final volume of 400.0 mL. What is the molarity of the solution?

a)

0.10 M

b)

0.40 M

c)

1.25 M

d)

2.33 M

66.
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
67.

How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?

a)

27.8 mL

b)

.278 mL

c)

2.8 mL

d)

278 mL

68.

How many moles of solute are present in 50.0 mL of 0.20M KNO3?

a)

10.0 moles solute

b)

0.05 moles solute

c)

1.00 moles solute

d)

0.01 moles solute

69.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
70.

Glycerol has a molar mass of 92.09g/mol. Its percent composition is: 39.12% C, 8.75% H, and 52.13% O. What is the molecular formula for glycerol?

a)

C2H3O2

b)

CH2O

c)

C2H4O2

d)

C3H8O3

71.

2.40 g of an explosive, J, contains 0.473 g of nitrogen. J also contains 33.8% carbon and 1.41% hydrogen by mass. The remainder of J is oxygen.


What is the empirical formula of J?

a)

C4HNO2

b)

CH2N2O

c)

C2HNO2

d)

CHNO

72.

Given the following, determine the empirical formula: 42.07% sodium, 18.89% phosphorus, and 39.04% oxygen.

a)

NaPO2

b)

Na2PO3

c)

Na3PO4

d)

Na3PO3

73.
Which of the following is considered an empirical formula?
a)
CH3COOH
b)
C6H12O6
c)
H2O

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