WorksheetsAQA Giant Covalent and Metallic
Total questions: 21
Worksheet time: 16mins
Name
Class
Date
1.
What type structure is diamond, graphite and silicon dioxide?
a)
Giant ionic
b)
Giant covalent
c)
Simple molecule
d)
Giant metallic
e)
Monatomic
2.
How many bonds does each carbon have in diamond?
a)
4
b)
3
c)
0
d)
7
e)
1
3.
What property of diamond is an effect of LOTS of energy being required to break the many covalent bonds?
a)
Refractive index
b)
Brilliance
c)
Transparency
d)
Conductivity
e)
Melting point
4.
Explain why most giant covalent substances do not conduct electricity
a)
No free ions
b)
Delocalised electrons
c)
Ionic bonding
d)
No free electrons
e)
Too large
5.
Explain why graphite conducts electricity
a)
Has free electrons
b)
Has free ions
c)
Is a metal
d)
Is a solid
e)
Is a lubricant
6.
Explain why graphite can act as a lubricant
a)
High melting point
b)
Low melting point
c)
Is a metal
d)
Free electrons
e)
Layers slide
7.
Explain why graphite can act as a lubricant
a)
High melting point
b)
Low melting point
c)
Is a metal
d)
Free electrons
e)
Layers slide
8.
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
9.
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.
10.
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
11.
What structure is shown in the diagram?
a)
Diamond
b)
Graphite
c)
fullerene
12.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
13.
At room temperature, most metals are
a)
liquid
b)
solid
c)
gas
d)
an alloy
14.
What does malleable mean?
a)
able to be shaped
b)
will break easily
c)
can be used for wire
d)
is shiny
15.
What is the ability of a substance to allow heat, sound, or electricity to flow through it?
a)
Malleability
b)
Ductility
c)
Solubility
d)
Conductivity
16.
Which of these are considered properties of metals? (choose ALL that apply)
a)
brittleness
b)
low melting point
c)
luster (shininess)
d)
malleability
e)
ductility
17.
What type of bonding consists of positive ions surrounded by a sea of electrons?
a)
Metallic
b)
Ionic
c)
Covalent
d)
Coordinate
18.
Explain why metals can conduct electricity
a)
Free electrons
b)
Free moving ions
c)
Free electrons to carry charge
d)
They are conductive
19.
Explain why pure metals are soft
a)
Free electrons
b)
Soft ions
c)
Layers of ions cannot slide
d)
Layer of ions can slide easily
20.
What is an alloy?
a)
Mixture of elements
b)
Mixture of non-metals
c)
Mixture of metal & other element(s)
d)
Metallic compund
21.
Explain why alloys can be harder than pure metals
a)
Fewer electrons
b)
Layers of ions slide less easily
c)
More electrons
d)
more layers
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