The hybrid state of C in `CS_(2)` should be

Options

A. `sp^2`
B. `sp`
C. `sp^3`
D. `sp^3d`

Explanation

To determine the hybrid state of carbon in carbon disulfide (CS₂), we can follow these steps:

### Step 1: Identify the molecular structure
Carbon disulfide (CS₂) consists of one carbon atom bonded to two sulfur atoms. The molecular geometry can be predicted based on the number of bonds and lone pairs around the carbon atom.

**Hint:** Look at the number of atoms bonded to carbon and any lone pairs on carbon.

### Step 2: Count the valence electrons
Carbon has 4 valence electrons, while each sulfur atom has 6 valence electrons. In CS₂, carbon forms two double bonds with the sulfur atoms. This means that carbon uses its 4 valence electrons to form these bonds.

**Hint:** Remember that carbon typically forms four bonds to achieve a stable electron configuration.

### Step 3: Determine the hybridization
In CS₂, carbon is forming two sigma bonds with the sulfur atoms. Since carbon is forming two bonds and has no lone pairs, we can determine its hybridization. The hybridization can be determined using the formula:

- Number of sigma bonds + Number of lone pairs on the central atom = Hybridization state.

Here, we have:
- 2 sigma bonds (one with each sulfur)
- 0 lone pairs on carbon

So, 2 + 0 = 2, which corresponds to sp hybridization.

**Hint:** Use the formula for hybridization to find the hybrid state based on the number of bonds and lone pairs.

### Step 4: Confirm the molecular geometry
The sp hybridization indicates that the geometry around the carbon atom is linear, as the bond angles will be 180 degrees. This is consistent with the structure of CS₂.

**Hint:** Visualize the molecular geometry to confirm that it matches the predicted hybridization.

### Conclusion
The hybrid state of carbon in CS₂ is **sp**.

**Final Answer:** The hybrid state of C in CS₂ is sp.

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