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Worksheets4.4 Metallic bonding and Allotropes
Total questions: 10
Worksheet time: 15mins
Name
Class
Date
1.
Define the term allotropes
a)
Atoms with same proton number but different number of neutrons
b)
Atoms with same proton number but different mass number
c)
Atoms in different arrangement in structure
d)
Atoms in different arrangement and different physical form
2.
Graphene is a good conductor because
a)
free moving electrons
b)
free delocalization of electrons in its structure
c)
free delocalized electrons in 2D structure
d)
free delocalized electrons in 3D
3.
What kind of bonding does atoms in graphene has?
a)
Covalent bonding
b)
Each carbon, bonded covalently to 3 other carbon atoms.
c)
Each carbon, bonded covalently to 4 other carbon atoms.
d)
Each carbon, bonded covalently to 3 other carbon atom in 2D
4.
Why graphene is a better conductor compared to C60?
a)
More delocalized electrons in graphene
b)
Electron move easily in graphene
c)
Electron move easily due to its planar flat structure
d)
Electron movement easier due to weak attraction with nuclei
5.
Which of the following is true about C60 ?
a)
Each carbon bonded covelently to 3 other carbon atoms
b)
Each carbon bonded covelently to 4 other carbon atoms
c)
2 single and 2 double bonds in its structure
d)
Hexagonal and pentagonal in shape
6.
C60 is a good conductor because
a)
It has one delocalized electron moving freely
b)
It has 60 delocalized electrons moving freely
c)
Free moving electrons
d)
Free moving delocalized electrons
7.
Define the term metallic bonding
a)
Attraction between positive nuclei and electrons
b)
Forces attraction between nuclei and electron
c)
Forces attraction between nuclei and sea of electrons
d)
Electrostatic attraction between nuclei and sea of electrons
8.
Why melting point increase across period 3, from Sodium (Na) to Aluminium (AI)?
a)
Size of atoms get smaller
b)
Attraction force between nuclei and free electron increase
c)
More free moving electrons
d)
Due to increase of sea of electron and size of atomic nuclei
9.
Why melting point decrease down group 1?
a)
Increase in size of atom down the group
b)
Increase in number of sea of electrons
c)
Increase in number of protons in nucleus
d)
Decrease in attractive force due to rise in proton number
10.
Gp 4, Diamond (C) and Silicon (S) has highest melting point due to
a)
Strong covalent bonds between carbon atoms
b)
All carbon atoms are covalently bonded
c)
Strong covalent bonds in a macromolecular structure
d)
Carbon atom covalently bonded in a macromolecular structure
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