The shape of chlorate ions is

Options

A. Angular
B. Pyramidal
C. Tetrahedral
D. Trigonal planar

Answer

To determine the shape of the chlorate ion (ClO3^-), we can follow these steps:

### Step 1: Identify the central atom and its valence electrons
The central atom in the chlorate ion is chlorine (Cl). Chlorine has an atomic number of 17, which means it has 7 valence electrons.

### Step 2: Determine the number of bonds and lone pairs
In the chlorate ion (ClO3^-), chlorine is bonded to three oxygen atoms. To visualize this, we can represent the bonds:
- Each Cl-O bond is a sigma bond.
- The chlorate ion has a negative charge, which means there is an additional electron.

### Step 3: Count the total number of valence electrons
- From chlorine: 7 electrons
- From three oxygen atoms: 3 × 6 = 18 electrons
- Plus one extra electron due to the negative charge: 1 electron
- Total = 7 + 18 + 1 = 26 valence electrons

### Step 4: Draw the Lewis structure
- Chlorine forms three single bonds with three oxygen atoms.
- One of the oxygen atoms can form a double bond with chlorine, while the other two will have single bonds.
- This results in one lone pair remaining on the chlorine atom.

### Step 5: Determine the steric number
The steric number is calculated as:
- Number of sigma bonds + Number of lone pairs
- Here, we have 3 sigma bonds (from Cl-O) and 1 lone pair on chlorine.
- Steric number = 3 + 1 = 4

### Step 6: Determine the hybridization
With a steric number of 4, the hybridization of the central atom (Cl) is sp³.

### Step 7: Determine the molecular shape
- The geometry corresponding to a steric number of 4 is tetrahedral.
- However, due to the presence of one lone pair, the shape of the chlorate ion is trigonal pyramidal.

### Final Answer
The shape of the chlorate ion (ClO3^-) is **trigonal pyramidal**.

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