Which species has the maximum number of lone pair of electrons
on the central atom ? .

Options

A. `[ClO_(3)]^(Θ)`
B. `XeF_(4)`
C. `N_(2)O`
D. `[I_(3)]^(Θ)`

Explanation

To determine which species has the maximum number of lone pairs of electrons on the central atom, we will analyze the Lewis structures of the given species: ClO3^-, XeF4, N2O, and I3^-.

### Step 1: Analyze ClO3^-
1. **Count the valence electrons for ClO3^-**:
- Chlorine (Cl) has 7 valence electrons.
- Each oxygen (O) has 6 valence electrons, and there are 3 oxygens, contributing 18 electrons.
- The negative charge adds 1 electron.
- Total: 7 + 18 + 1 = 26 valence electrons.

2. **Draw the Lewis structure**:
- Chlorine is the central atom bonded to three oxygen atoms.
- Two of the oxygen atoms are double bonded, and one is single bonded with a negative charge.
- After forming bonds, chlorine has 2 electrons left, which means it has 1 lone pair.

### Step 2: Analyze XeF4
1. **Count the valence electrons for XeF4**:
- Xenon (Xe) has 8 valence electrons.
- Each fluorine (F) has 7 valence electrons, and there are 4 fluorines, contributing 28 electrons.
- Total: 8 + 28 = 36 valence electrons.

2. **Draw the Lewis structure**:
- Xenon is the central atom bonded to four fluorine atoms.
- After forming bonds, xenon has 4 electrons left, which means it has 2 lone pairs.

### Step 3: Analyze N2O
1. **Count the valence electrons for N2O**:
- Each nitrogen (N) has 5 valence electrons, contributing 10 electrons for 2 nitrogens.
- Oxygen (O) has 6 valence electrons.
- Total: 10 + 6 = 16 valence electrons.

2. **Draw the Lewis structure**:
- One nitrogen is the central atom, forming a triple bond with the other nitrogen and a dative bond with oxygen.
- The central nitrogen has no lone pairs due to the formation of the dative bond.

### Step 4: Analyze I3^-
1. **Count the valence electrons for I3^-**:
- Each iodine (I) has 7 valence electrons, contributing 21 electrons for 3 iodines.
- The negative charge adds 1 electron.
- Total: 21 + 1 = 22 valence electrons.

2. **Draw the Lewis structure**:
- One iodine is the central atom bonded to two other iodines.
- After forming bonds, the central iodine has 6 electrons left, which means it has 3 lone pairs.

### Conclusion:
After analyzing all species:
- ClO3^- has 1 lone pair.
- XeF4 has 2 lone pairs.
- N2O has 0 lone pairs.
- I3^- has 3 lone pairs.

Thus, the species with the maximum number of lone pairs of electrons on the central atom is **I3^-**.