Graphite is often described as a good conductor of electricity even though it is a non metallic form of carbon. Decide whether this statement about the electrical conductivity of graphite is correct or incorrect.

Introduction / Context:

Carbon exists in different forms called allotropes, such as diamond and graphite. These forms have very different physical properties. This question focuses on the electrical property of graphite and asks you to decide whether the statement that graphite is a good conductor of electricity is correct or not.

Given Data / Assumptions:

• Graphite is a crystalline form of carbon.
• The statement claims that graphite is a good conductor of electricity.
• No special conditions such as very high temperature or solution state are mentioned.

Concept / Approach:

In graphite, each carbon atom is covalently bonded to three other carbon atoms in a planar hexagonal arrangement, forming layers. Each carbon atom has one electron that is delocalised and free to move within the layer. These mobile electrons enable electrical conduction along the layers. In contrast, diamond has each carbon bonded to four neighbours in a rigid three dimensional network with no free electrons, so diamond acts as an insulator. By comparing these structures, we can decide whether the given statement about graphite is correct.

Step-by-Step Solution:

Verification / Alternative check:

Everyday examples include the use of graphite rods as electrodes in batteries and in electrolysis experiments in school laboratories. A material selected for electrodes must conduct electricity. This practical use confirms that graphite conducts electric current well enough for many applications.

Why Other Options Are Wrong:

Option B: The statement is incorrect contradicts the known fact that graphite is conductive, so it is wrong.

Option C: Graphite conducts only when it is red hot is incorrect because graphite electrodes conduct at room temperature.

Option D: Graphite conducts only when dissolved in water is also wrong because graphite is not used as an ionic solution but as a solid electrode.

Common Pitfalls:

Students sometimes generalise that all non metals are poor conductors and therefore assume graphite must also be an insulator. Graphite is an important exception. Another confusion arises from mixing properties of diamond and graphite. Remember that structure determines properties, and the layered structure of graphite with delocalised electrons explains its conductivity.

Final Answer:

The correct evaluation is that The statement is correct.