Which of the following molecule is hypovalent ?

Options

A. `AlF_(3)`
B. `Icl_(2)^(-)`
C. `BCl_(3)`
D. `ICl_(2)^(-)`

Answer

To determine which molecule is hypovalent, we need to understand the definition of hypovalent molecules. A hypovalent molecule is one where the central atom has fewer than 8 electrons in its valence shell.

Here’s how we can approach the problem step by step:

### Step 1: Identify the Central Atom
First, we need to identify the central atom in each of the given molecules. The central atom is typically the atom that can form the most bonds or is the least electronegative.

### Step 2: Count the Valence Electrons
Next, we need to count the total number of valence electrons for the central atom in each molecule. This includes the electrons that the atom contributes and any electrons it shares when forming bonds with surrounding atoms.

### Step 3: Determine the Electron Count
After counting the valence electrons, we will determine if the central atom has fewer than 8 electrons in its valence shell. If it does, then the molecule is hypovalent.

### Step 4: Compare with Other Molecules
If there are multiple molecules provided in the question, we will repeat the above steps for each molecule and compare the results.

### Conclusion
Finally, we will conclude which molecule is hypovalent based on the analysis.

### Example
If we consider a molecule like BF3 (Boron Trifluoride):
1. Central Atom: Boron (B)
2. Valence Electrons: Boron has 3 valence electrons.
3. Bonds: Boron forms 3 bonds with 3 fluorine atoms.
4. Total Electrons: Boron ends up with only 6 electrons in its valence shell.
5. Conclusion: Since Boron has fewer than 8 electrons, BF3 is a hypovalent molecule.