The geometry of `ClO_(3)^(-)` according to valence shell electron pair repulsion theory will be

Options

A. Planar triangle
B. Pyramidal
C. Tetrahedral
D. Square planer.

Answer

To determine the geometry of the chlorate ion, \( \text{ClO}_3^{-} \), according to the Valence Shell Electron Pair Repulsion (VSEPR) theory, we can follow these steps:

### Step 1: Determine the central atom and its valence electrons
The central atom in \( \text{ClO}_3^{-} \) is chlorine (Cl). Chlorine is in group 17 of the periodic table and has 7 valence electrons.

### Step 2: Count the number of bonds and lone pairs
In \( \text{ClO}_3^{-} \):
- Chlorine forms three single bonds with three oxygen atoms.
- Additionally, there is one lone pair of electrons on the chlorine atom.

### Step 3: Calculate the total number of electron pairs
The total number of electron pairs around the chlorine atom can be calculated as follows:
- 3 bond pairs (from the Cl-O bonds)
- 1 lone pair

Thus, the total number of electron pairs = 3 (bond pairs) + 1 (lone pair) = 4 electron pairs.

### Step 4: Determine the geometry using VSEPR theory
According to VSEPR theory, the arrangement of electron pairs around a central atom determines the molecular geometry:
- With 4 electron pairs, the geometry is based on a tetrahedral arrangement.
- However, since one of these pairs is a lone pair, the molecular geometry is adjusted to account for this lone pair.

### Step 5: Identify the molecular geometry
The presence of one lone pair will distort the tetrahedral arrangement, leading to a trigonal pyramidal shape for the molecule.

### Conclusion
Therefore, the geometry of \( \text{ClO}_3^{-} \) according to VSEPR theory is **trigonal pyramidal**.

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