In the molecule `ICI_(3)`, how many lone pairs of electrond are associated with idione ?

Explanation

To determine the number of lone pairs of electrons associated with iodine in the molecule ICl₃, we can follow these steps:

### Step 1: Identify the central atom
In the molecule ICl₃, iodine (I) is the central atom, and it is surrounded by three chlorine (Cl) atoms.

**Hint:** Look for the atom that is bonded to multiple other atoms; this is usually the central atom in a molecule.

### Step 2: Determine the valence electrons of iodine
Iodine is in group 17 of the periodic table, which means it has 7 valence electrons. The electronic configuration of iodine is [Xe] 5s² 5p⁵.

**Hint:** Remember that the group number can help you find the number of valence electrons for main group elements.

### Step 3: Consider the bonding in ICl₃
In ICl₃, iodine forms three single bonds with three chlorine atoms. Each bond uses one of iodine's valence electrons. Therefore, 3 of the 7 valence electrons are used for bonding.

**Hint:** Count how many electrons are used in bonding to find out how many are left for lone pairs.

### Step 4: Calculate the remaining electrons
After forming three bonds, iodine has 7 - 3 = 4 valence electrons remaining. These remaining electrons will form lone pairs.

**Hint:** Subtract the number of bonding electrons from the total valence electrons to find the lone pairs.

### Step 5: Determine the number of lone pairs
Since each lone pair consists of 2 electrons, the 4 remaining electrons can be grouped into 2 lone pairs.

**Hint:** Remember that lone pairs are pairs of electrons that are not involved in bonding.

### Conclusion
In the molecule ICl₃, iodine has **2 lone pairs of electrons**.

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