The shape of `[CH_(3)]^(o+)` is_____ .

Explanation

To determine the shape of the methyl cation \([CH_3]^+\), we can follow these steps:

### Step 1: Identify the central atom and its valence electrons
The central atom in the methyl cation is carbon (C). Carbon has an atomic number of 6, which means it has 4 valence electrons in its outer shell (2s² 2p²).

### Step 2: Determine the electron configuration of the cation
When carbon forms a methyl cation \([CH_3]^+\), it loses one electron. Therefore, the electron configuration of the outer shell becomes 2s² 2p¹, resulting in a total of 3 valence electrons.

### Step 3: Count the number of bonds and lone pairs
In the methyl cation, carbon forms three bonds with three hydrogen atoms. Since there are no lone pairs on the carbon atom, we have:
- Bond pairs: 3 (from the three C-H bonds)
- Lone pairs: 0

### Step 4: Calculate the steric number
The steric number is the sum of the number of bond pairs and lone pairs. Here, the steric number is:
\[ \text{Steric number} = \text{Number of bond pairs} + \text{Number of lone pairs} = 3 + 0 = 3 \]

### Step 5: Determine the molecular geometry
With a steric number of 3, the molecular geometry of the methyl cation is trigonal planar. This means that the three hydrogen atoms are arranged in a plane around the carbon atom.

### Step 6: Identify the hybridization
The hybridization corresponding to a steric number of 3 is \(sp^2\). This indicates that one s orbital and two p orbitals from carbon hybridize to form three equivalent \(sp^2\) hybrid orbitals.

### Final Answer
The shape of \([CH_3]^+\) is **trigonal planar**.

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