Carbon: Introduction

Carbon is a versatile element, crucial in organic chemistry, forming various molecules due to its ability to create up to four covalent bonds. It exists in different forms called allotropes, including graphite, diamond, and amorphous carbon. Graphite is soft and conducts electricity due to delocalised electrons, while diamond is hard and non-conductive due to its lattice structure. Amorphous carbon lacks a consistent structure, found in materials like coal and charcoal. The structure of carbon's covalent bonds significantly influences the properties of these materials.

What makes carbon a unique element in forming different molecules?

• It is only found in living organisms.

• It can form up to two covalent bonds.

• It is the heaviest element in the universe.

• It can form up to four covalent bonds.

Why is graphite able to conduct electricity?

• Because it is the hardest material known.

• Because it is composed of amorphous carbon.

• Because it has delocalized electrons that can move between layers.

• Because it has a three-dimensional lattice structure.

What is the primary structural difference between graphite and diamond?

• Graphite is a liquid at room temperature, while diamond is solid.

• Graphite has a two-dimensional layer structure, while diamond has a three-dimensional lattice structure.

• Graphite is composed of amorphous carbon, while diamond is not.

• Graphite has a three-dimensional structure, while diamond has a two-dimensional structure.

Which of the following is considered an amorphous form of carbon?

• Diamond

• Graphite

• Silicon

• Charcoal

How does the lack of a uniform pattern in amorphous carbon affect its properties?

• It makes the material extremely hard.

• It allows the material to conduct electricity.

• It prevents the material from forming covalent bonds.

• It makes the material transparent.