In graphite, electrons are

Options

A. localised on each C-atom
B. localised on every third C-atom
C. spread out between the structure
D. Both (b) and (c )

Explanation

To solve the question "In graphite, electrons are...", we need to analyze the structure of graphite and the behavior of electrons within it. Here’s a step-by-step breakdown:

### Step 1: Understand the Structure of Graphite
Graphite is an allotrope of carbon where each carbon atom is bonded to three other carbon atoms. This bonding occurs through sp² hybridization.

**Hint:** Remember that sp² hybridization involves the mixing of one s orbital and two p orbitals, resulting in three sigma bonds and one unhybridized p orbital.

### Step 2: Identify the Bonding in Graphite
In graphite, each carbon atom forms three sigma bonds with neighboring carbon atoms, creating a planar hexagonal lattice. The fourth outer electron from each carbon atom is not involved in sigma bonding.

**Hint:** Visualize the hexagonal arrangement of carbon atoms to understand how the bonds are formed.

### Step 3: Analyze the Fourth Electron
The fourth electron from each carbon atom is in an unhybridized p orbital. These p orbitals overlap sideways with p orbitals from adjacent carbon atoms, forming a delocalized π bond system across the layers of graphite.

**Hint:** Think of the delocalized electrons as being spread out over the entire structure, rather than being localized on individual atoms.

### Step 4: Conclude the Behavior of Electrons
Due to the delocalization of these electrons, they are considered "free electrons." This delocalization allows them to move easily throughout the structure, which is why graphite can conduct electricity.

**Hint:** Recall that free-moving electrons are essential for electrical conductivity in materials.

### Final Answer
In graphite, electrons are spread out between the structure (the correct option is C).

### Summary of Steps:
1. Understand the sp² hybridization in graphite.
2. Identify the bonding and structure of carbon atoms in graphite.
3. Analyze the behavior of the fourth electron in the p orbital.
4. Conclude that these electrons are delocalized and contribute to electrical conductivity.