Grade 12 Chemistry: Metallic Bonding
A comprehensive worksheet for Grade 12 Chemistry students covering the principles and properties of metallic bonding.
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Grade 12 Chemistry: Metallic Bonding
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Read each question carefully and provide clear, concise answers. Show all your work for calculations.
1. Which of the following best describes the nature of metallic bonding?
Sharing of electrons between two non-metal atoms.
Electrostatic attraction between positive ions and a 'sea' of delocalized electrons.
Transfer of electrons from a metal atom to a non-metal atom.
Formation of a crystal lattice of alternating positive and negative ions.
2. The malleability and ductility of metals can be attributed to:
The strong directional bonds between metal atoms.
The ability of delocalized electrons to absorb and re-emit light.
The ability of metal ions to slide past each other without breaking the metallic bond.
The fixed positions of electrons in the metallic lattice.
3. In metallic bonding, the valence electrons are and are often referred to as a ' of electrons'.
4. Metals generally have high points and are good conductors of and .
5. Explain, in terms of metallic bonding, why metals are excellent conductors of electricity.
6. Describe the 'electron sea model' and how it accounts for the characteristic properties of metals.
7. All metals are equally strong due to the uniform nature of metallic bonding.
True
False
8. The lustrous appearance of metals is due to the interaction of light with their delocalized electrons.
True
False
Match each property of metals with the correct explanation based on metallic bonding.
9. Electrical Conductivity
a. Delocalized electrons can move freely and carry charge.
10. Malleability
b. Metal ions can slide past each other without repelling.
11. High Melting Point
c. Strong electrostatic forces between positive ions and delocalized electrons.
The diagram below illustrates a representation of metallic bonding.
