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WorksheetsGiant covalent structures
Total questions: 15
Worksheet time: 11mins
Name
Class
Date
1.
Elements such as Silicon, diamond and graphite. Compounds include SiO2
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent
2.
Low melting and boiling points which increase with increasing molecule size due to increased intermolecular forces.
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent
3.
Melting points are very high – a large amount of energy is needed to break all the covalent bonds
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent
4.
Formulae of these might include H2O
each molecule contains 1 O and 2H atoms
each molecule contains 1 O and 2H atoms
a)
simple covalent molecules
b)
metallic
c)
ionic
d)
giant covalent
5.
What structure is shown in the diagram?
a)
Diamond
b)
Graphite
c)
Carbon fiber
d)
Carbon nanotubes
6.
Why is diamond strong?
a)
It's made of carbon
b)
It doesn't conduct electricity
c)
It forms 4 strong covalent bonds
d)
So it can cut glass
7.
Why is graphite so soft?
a)
A. The atoms are arranged in hexagons in layers that are held together strongly
b)
B. The atoms are arranged in hexagons in layers that are held together weakly
c)
C. Carbon is strongly bonded to 3 other carbon atoms.
d)
D. Carbon is weakly bonded to 3 other carbon atoms.
8.
What element are diamond and graphite made up of?
a)
A. Sodium
b)
B. Carbon
c)
C. Carbon dioxide
d)
D. Silicon
9.
Why does graphite conduct electricity?
a)
Ions are free to move to carry the charge
b)
Atoms can move
c)
Free electrons that can carry the charge
10.
Graphite is a good conductor because
a)
all electrons are free moving electrons
b)
free delocalization of electrons in its 3D lattice structure
c)
free delocalized electrons in a 2D layered structure
d)
covalently bonded layers allow electricity to flow
11.
Diamond has a very high melting point due to
a)
Strong covalent bonds between carbon atoms in a layered structure
b)
All carbon atoms are covalently bonded to 3 other carbons
c)
Strong ionic bonds in a lattice structure
d)
Carbon atom covalently bonded to 4 other Carbons in a giant structure
12.
What structure is shown in the diagram?
a)
Diamond
b)
Graphite
c)
fullerene
13.
Each carbon is graphite forms _____ bonds
a)
1
b)
2
c)
3
d)
4
14.
Why is graphite so soft and slippery?
a)
It is made of layers of atoms with weak forces between them
b)
It is made of small molecules
c)
It is an ionic compound
d)
The covalent bonds are weak
15.
How are covalent bonds explained?
a)
When one atom takes the other atom's electron
b)
When the atom shares an electron with an another atom
c)
When the two nucleus merge
d)
When the neutrons leave the nucleus
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