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Chemistry - Calculations, periodic table, bonding revision

Total questions: 80

Worksheet time: 1hrs 25mins

Name
Class
Date
1.

Calculate the Mr of Na2SO4.10H2O

a)

142

b)

178

c)

322

d)

161

2.

Calculate the number of moles in 25.25g of KNO3

a)

2

b)

0.25

c)

0.75

d)

4

3.

Calculate the mass of 0.5 mol of NaOH

a)

15g

b)

10g

c)

20g

d)

40g

4.

How many moles are in 225 g of CO?

a)

28.01 mole

b)

4.82 x 1024 mole

c)

6,302,25 mole

d)

8.0357 mole

5.
What is the total number of atoms in 1.0 mole of CO2?
a)
1.5 x 1023
b)
12 x 1023
c)
3 x 1023
d)
18 x 1023
6.
The total number of sodium atoms in 46.0 grams is
a)
3.01 x 1023
b)
6.02 x 1023
c)
12 x 1023
d)
24 x 1023
7.
Which sample of O2 contains a total of 3 x 1023 molecules?
a)
1.0 moles
b)
2.0 moles
c)
16.0 grams
d)
32.0 grams
8.
The total number of molecules in 34.0 grams of NH3 is equal to 
a)
1.00 x 22.4
b)
2.00 x 22.4
c)
1.00 (6.02 x 1023)
d)
2.00 (6.02 x 1023)
9.

What is the mass of 3.0 x 1023 atoms of neon?

a)

1.0 g

b)

0.5 g

c)

9.97g

d)

20.0 g

10.
What is the number of moles of N2 that contains 9.03 x 1023 molecules?
a)
0.667
b)
1.50
c)
33.6
d)
42.0
11.
Which represents the greatest mass of chlorine?
a)
1 mole of chlorine
b)
1 atom of chlorine
c)
1 grams of chlorine
d)
1 molecule of chlorine
12.

Which mass contains 6.0 x 1023 particles ?

a)

6.0 g of carbon

b)

16 g of sulfur

c)

3.0 g of helium

d)

28 g of silicon

13.

Which amount contains the largest mass?

a)

1 mole of water molecules

b)

0.25 mole of magnesium oxide

c)

10 moles of hydrogen atoms

d)

6 dm3 of sulfur dioxide gas at r.r.p.

14.

One mole of hydrogen and one mole of ammonia have the same

a)

mass in grams

b)

number of molecules

c)

number of atoms

d)

relative molecular mass

15.

The relative molecular mass of calcium hydroxide is

a)

40.1

b)

57.1

c)

74.1

d)

91.1

16.

What is the mass of 1 mole of nitrogen gas?

a)

56.0 g

b)

28.0 g

c)

14.0 g

d)

12.0 g

17.

When does a chemical reaction stop?

a)

when the laboratory closes

b)

when the excess reactant is used up

c)

when the limiting reactant is used up

d)

chemical reactions never stop

18.

Fe + S → FeS


0.8 moles of Fe are allowed to react an excess of S. What is the mass of FeS produced?


(Ar of Fe = 56, Ar of S = 32)

a)

25.6 g

b)

44.8 g

c)

70.4 g

d)

88 g

19.

2CO + O2 → 2CO2


What is the mass of CO2 produced by reacting 2 moles of O2 with an excess of CO?


(Ar of C = 12, Ar of O = 16)

a)

22 g

b)

44 g

c)

88 g

d)

176 g

20.

2H2 + O2 → 2H2O


How many moles of water can be made from 100 g of hydrogen?


(Ar of H = 1, Ar of O = 16)

a)

25 mol

b)

50 mol

c)

100 mol

d)

200 mol

21.

2C2H6 + 7O2 → 4CO2 + 6H2O


What is the mass of C2H6 used to produce 2 moles of CO2?


(Ar of C = 12, Ar of H = 1, Ar of O = 16)

a)

2 g

b)

30 g

c)

60 g

d)

120 g

22.

CH4 + 2O2 → CO2 + 2H2O


24 g of CH4 will produce how many grams of CO2?


(Ar of C = 12, Ar of H = 1, Ar of O = 16)

a)

15 g

b)

24 g

c)

44 g

d)

66 g

23.

Zn + 2HCl → ZnCl​2 ​​+ H​2​​


When 14.6 g of HCl is used, what is the mass of H2 produced?


(Ar of H = 1, Ar of Cl = 35.5)

a)

0.2 g

b)

0.4 g

c)

0.8 g

d)

7.3 g

24.

2NaClO3 → 2NaCl + 3O2


What is the mass of O2 produced from 213 g of NaClO3?


(Ar of Na = 23, Ar of Cl = 35.5, Ar of O = 16)

a)

48 g

b)

96 g

c)

213 g

d)

319.5 g

25.

2Al + 3H2SO4 → Al2(SO4)3 + 3H2


What is the mass of aluminum sulfate formed if 147 g of sulfuric acid completely reacted with aluminum?


(Ar of Al = 27, Ar of H = 1, Ar of S =32, Ar of O = 16)

a)

49 g

b)

98 g

c)

342 g

d)

513 g

26.
Ionic bonds form between metals and ____.
a)
metalloids
b)
metals
c)
nonmetals
27.
What is the chemical formula for the molecule in the image, carbon dioxide? 
a)
H2O
b)
CO2
c)
CO
d)
CH4
28.
What type of bonding is present in carbon dioxide?
a)
covalent
b)
single
c)
ionic
d)
metallic
29.
Which particles are represented by dots and crosses in the image?
a)
neutrons
b)
ions
c)
electrons
d)
protons
30.
Carbon dioxide is a small molecule. Which of the following is a property of small molecules?
a)
conduct electricity
b)
form lattices
c)
high boiling point
d)
low melting point
31.
Which type of bond has one pair of electrons shared between atoms?
a)
ionic
b)
single covalent
c)
metallic
d)
double covalent
32.
Which is described as the force holding atoms together?
a)
formula unit
b)
cation
c)
lattice
d)
chemical bond
33.
What type of bond is this?
a)
ionic
b)
covalent
c)
metallic
d)
peptide
34.
Nitrogen will form which of the following ions?
a)
N
b)
N-3
c)
N-5
d)
N+5
35.
If a compound has a high melting point, and conducts electricity as a solid and as a liquid, what type of structure is it?
a)
metallic
b)
ionic lattice
c)
giant covalent
36.
If a compound has a high melting point, doesn't conduct electricity as a solid but DOES as a liquid, what type of structure is it?
a)
metallic
b)
ionic lattice
c)
giant covalent
37.
If a compound has a high melting point, doesn't conduct electricity as a solid OR as a liquid, what type of structure is it?
a)
metallic
b)
ionic lattice
c)
giant covalent
38.
Magnesium is in group 2. What is the symbol for a magnesium ion?
a)
Mg2-
b)
Mg-
c)
Mg2+
d)
Mg+
39.
Potassium is in group 1. What is the symbol for a magnesium ion?
a)
K2+
b)
K+
c)
K2-
d)
K-
40.
Chlorine is in group 7. What is the symbol for a chlorine ion?
a)
Cl7-
b)
Cl6-
c)
Cl2-
d)
Cl-
41.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
42.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
43.
What element is this?  What is the mass number of this atom?
a)
sodium, 23
b)
magnesium, 23
c)
magnesium, 12
d)
sodium, 11
44.
What quantities vary between isotopes of an element?
a)
protons, electrons, and atomic mass
b)
protons, electrons, and atomic number
c)
neutrons and electrons
d)
neutrons and atomic mass
45.
What is the mass number?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
46.
What is the atomic number of this nucleus?
a)
1
b)
3
c)
4
d)
7
47.
What is the mass number of this nucleus?
a)
1
b)
3
c)
4
d)
7
48.
What is the atomic number of this atom?
a)
8
b)
16
c)
24
d)
none of the above
49.
Complete the missing label on the diagram.
a)
Neutron
b)
Centre
c)
Nucleus
d)
Sub atomic particle
50.
Which one is the property of ionic compounds?
a)
high melting point
b)
not a crystal structure
c)
will not dissolve into water
d)
can't conduct electricity when melted
51.
What is the formula for the compound formed by magnesium ions and oxygen ions?
a)
MgO
b)
Mg2O3
c)
Mg2O2
d)
MgO3
52.
Graphene is a single layer of graphite. The bonds between the atoms in graphene are: 
a)
ionic
b)
covalent
c)
metallic
53.
Graphene is made of ________ atoms.
a)
chlorine
b)
chromium
c)
carbon
d)
silicon
54.
In graphene each atom bonds to ______ other atoms.
a)
1
b)
2
c)
3
d)
4
55.
What does the symbol Ca stand for?
a)
Carbon
b)
Calcium
c)
Chromium
d)
Copper
56.
What does the symbol C stand for?
a)
Carbon
b)
Calcium
c)
Chromium
d)
Copper
57.
What does the symbol O stand for?
a)
Carbon
b)
Calcium
c)
Chromium
d)
Oxygen
58.
How many atoms of calcium are in the molecule CaCO3?
a)
1
b)
2
c)
3
d)
4
59.

Why do the elements in the same group behave similarly?

a)

They have the same number of protons

b)

They have the same number of outer electrons (valence electrons)

c)

They have the same number of neutrons

d)

They have the same number of shells

60.

As you go down group 2, how many electrons will the elements have in the outer shell?

a)

1

b)

2

c)

3

d)

4

61.

Is it easier to remove an electron that is ...

a)

Closer to the nucleus

b)

Further away from the nucleus

c)

On it's own and unpaired

62.
How many electrons does potassium K contain? (click to see image)
a)
19
b)
39
c)
20
d)
40
63.
How many protons are in this element?
a)
79
b)
196
c)
117
d)
Cannot be determined
64.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
65.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
66.
Elements which are shiny, conduct electricity and heat are called
a)
metal
b)
nonmetal
c)
metalloid
d)
nonexistent
67.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
68.
The atomic number tells you what?
a)
number of electrons
b)
number of protons
c)
number of neutrons
d)
both electrons and protons in an atom.
69.
An atom is made up of protons, neutrons, and electrons.  Which is the smallest subatomic particle?
a)
Proton
b)
Neutron
c)
Electron
d)
Idontknowatron
70.

Which element is similar to F?

a)

Ne

b)

Cl

c)

O

d)

Ca

71.

Which element is similar to B?

a)

C

b)

Al

c)

Cl

d)

Na

72.

Which element is similar to He?

a)

H

b)

Ar

c)

Au

d)

Hg

73.

Which element is similar to Mg?

a)

Ca

b)

B

c)

O

d)

Cl

74.

Which element is similar to Li?

a)

Be

b)

K

c)

Fe

d)

I

75.

A student drew a dot cross diagram with 7 valence electrons. Which of the following elements might have the student drawn?

a)

Cl (Chlorine)

b)

Ne (Neon)

c)

N (Nitrogen)

d)

Li (Lithium)

76.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
77.
Rows on the period table are called _____ while columns are called _____.
a)
groups, families
b)
groups, periods
c)
periods, groups
d)
families, groups
78.
 Why does group number 18 have the least reactive elements?
a)
They all have an odd number of protons.
b)
They all have an even number of protons. 
c)
They have the largest masses.
d)
Their electron shells are the most filled and do not need to be very reactive.
79.
The period for Bromine is ___________.
a)
3
b)
2
c)
4
80.

Which of the following is a conclusion of Rutherford's gold foil experiment?

a)

The nucleus is negatively charged

b)

The atom is dense solid and is indivisible

c)

The mass is conserved when atoms react chemically

d)

The nucleus is very small and the atom is mostly empty space

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