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Y9 Chapter 2

Total questions: 50

Worksheet time: 30mins

Name
Class
Date
1.

Why is diamond hard and strong? It has

a)

weak intermolecular forces

b)

weak covalent bonds

c)

strong covalent bonds

d)

van der Waals forces of attraction

2.
Which statement is a true comparison of diamonds and graphite?
a)
diamonds are extremely hard and colorless where as graphite is a very soft gray substance. 
b)
diamonds are extremely soft and colorless where as graphite is a very hard gray substance.
c)
Diamonds are made only from carbon where as graphite is a carbon compound containing metal electrons
3.
Which is used in pencils ?
a)
graphite
b)
diamond
c)
fullerene
d)
none of these
4.
What structure is shown in the diagram?
a)
Diamond
b)
Graphite
5.

Which of the following statements about graphite and diamond is true?

a)

They have the same crystal structure

b)

They have the same degree of hardness

c)

They have the same electrical conductivity

d)

They can undergo the same chemical reactions

6.

Covalent structures have low melting and boiling points because it does not take much energy to break the _____ intermolecular forces.

a)

weak

b)

strong

7.

Why do simple covalent substances not conduct electricity?

a)

They have low melting points.

b)

They have low boiling points.

c)

There are no delocalised electrons or free ions to carry the charge.

d)

The molecules are too large.

8.

Select the properties of simple covalent substances.

a)

Low melting and boiling points.

b)

High melting and boiling points.

c)

Do not conduct electricity.

d)

Good conductors of electricity.

9.

The structure of ammonia is shown in the diagram. What is the formula for ammonia?

a)

NH3

b)

HN3

c)

N3H

d)

HN3

10.

Fluorine is a diatomic molecule. Fluorine is in Group 7. How many electrons are shared in this covalent bond?

(a)  

11.

Oxygen is a diatomic molecule. Oxygen is in Group 6. How many electrons are shared in this covalent bond?

(a)  

12.

Atoms can only share electrons in the (a)   shell.

13.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)

pairs of electrons are shared between two non-metal atoms.

d)

two non-metal atoms are attracted to each other by opposite charges.

14.

What type of bond involves the sharing of electrons between atoms?

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

15.

What two types of atoms make a covalent bond?

a)

2 non-metals

b)

1 metal and 1 non-metal

c)

2 metals

16.

An atom with 2 protons, 3 neutrons, and 4 electrons has a charge of ____.

a)

+2

b)

-2

c)

+3

d)

0

17.

How many electrons would a Nitrogen ion gain/lose? If it has 5 valence electrons.

a)

lose 5

b)

gain 5

c)

lose 3

d)

gain 3

18.

If an ion gains an electron, it becomes

a)

Positive

b)

Stable

c)

Atomic

d)

Negative

19.

If an electron is removed, an ion becomes

a)

An atom

b)

Positive

c)

Negative

d)

Neutral

20.

An example of an ionic compound is Sodium Chloride, which is made from Na+ and Cl- ions. Why do these ions form an ionic bond?

a)

They have like charges

b)

They are from the same group

c)

They are from the same period

d)

They have opposite charges

21.

Oxygen is in group 6 of the periodic table, which ion would it form?

a)

O-

b)

O+

c)

O2-

d)

O2+

22.

Lithium is in group 1 of the periodic table, which ion would it form?

a)

Li-

b)

Li2-

c)

Li+

d)

Li2+

23.

Ionic bonds are formed from a combination of metal elements and __________________ elements.

a)

non-metal

b)

receive

c)

metal

d)

donate

24.

In the formation of ionic bonds, the electrons will be ____________ from metal elements to non-metal elements.

a)

oppositely

b)

receive

c)

transferred

d)

donate

25.

Which of the below is an ionic compounds?

a)

Ni

b)

MgCl2

c)

H2O

d)

CH4

26.

Atoms form ions because they want to have a (a)   outer shell.

27.
How many electrons are in a Li+ ion?
a)
1
b)
2
c)
3
d)
4
28.

Non-metals ________ electrons when they become ions.

a)

lose

b)

gain

c)

neither

29.
Metals __________ electrons when they become ions
a)
lose
b)
gain
c)
neither
30.

What is a charged atom known as?

a)

Electron

b)

Proton

c)

Ion

d)

Neutron

31.
Anions are...
a)
Positive
b)
Negative
c)
Neutral
d)
Crying
32.
Cations are...
a)
Positive
b)
Negative
c)
Neutral
d)
Purring
33.
What is an ion?
a)
A Charged Atom
b)
A Large Atom
c)
A Small Atom
d)
A Cute Atom
34.

How many protons, neutrons, and electrons are in Oxygen?

a)

Protons = 8; Neutrons = 16; Electrons = 8

b)

Protons = 8; Neutrons = 8; Electrons = 8

c)

Protons = 16; Neutrons = 8; Electrons = 16

d)

Protons = 16; Neutrons = 24; Electrons = 16

35.

How many electrons are in Potassium?

a)

19

b)

20

c)

58

d)

39

36.

How many neutrons are in Argon?

a)

18

b)

40

c)

58

d)

22

37.

How many electrons are in Sulfur?

a)

32

b)

16

c)

48

d)

8

38.

How many neutrons are in Phosphorus?

a)

16

b)

15

c)

31

d)

46

39.

How many protons are in Silicon?

a)

7

b)

42

c)

28

d)

14

40.

How many electrons are in Aluminium?

a)

40

b)

27

c)

13

d)

14

41.

X atom has 10 proton and 11 neutron. How many electron does it have?

a)

10

b)

11

c)

12

d)

13

42.

Neutrons + Protons = _________

a)

Atomic Number

b)

Atomic Mass

c)

Electrons

d)

Element

43.

What is the number of protons in an atom in this diagram?

a)

10

b)

7

c)

3

d)

4

44.

How many neutrons are there in one atom of magnesium?

a)

12

b)

6

c)

24

45.

The fluorine atom has an atomic number (proton number) of

a)

19

b)

9

c)

10

46.

Non-charged subatomic particle is

a)

Proton

b)

Electron

c)

Neutron

47.

Subatomic particle with negative charge is

a)

Proton

b)

Electron

c)

Neutron

48.

Subatomic particles with positive charge is

a)

Proton

b)

Neutron

c)

Electron

49.

The diagram shows you a Helium symbol in periodic table. What is electron number of Helium?

a)

6

b)

4

c)

2

50.
The nucleus of an atom is made of
a)
electrons and protons
b)
electrons and neutrons
c)
protons and neutrons
d)
empty space

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