Question

1. define the term allotrope.
2. why do allotropes of the same element have different physical and chemical properties? explain using examples from carbon.
3. how many covalent bonds does each carbon atom form in diamond?
4. explain why diamond is very hard and has a high melting point.
5. why does diamond not conduct electricity?
6. how is the structure of graphite different from diamond?
7. why can graphite conduct electricity?
8. what are fullerenes, and how is their structure different from diamond and graphite?
9. what makes carbon nanotubes strong and useful in materials and electronics?
10. other elements, like oxygen and sulfur, also have allotropes. how does the arrangement of atoms in these allotropes affect their properties?

Explanation:

• Allotrope: Different forms of the same element.
• Diamond - Type of Structure: Giant covalent lattice.
• Diamond - Number of Covalent Bonds per Atom: 4.
• Diamond - Conducts Electricity?: No (no free electrons).
• Diamond - Hardness: Very hard (strong covalent bonds in 3D).
• Diamond - Uses: Jewellery, cutting tools.

Answer:

Allotrope	Diamond
Number of Covalent Bonds per Atom	4
Conducts Electricity?	No
Hardness	Very hard
Uses	Jewellery, cutting tools