In which of the following species, each atom carries same number of lone pair of electron on it?

Options

A. `XeO_(4)^(2-)`
B. `XeF_(2)`
C. `XeO_(6)^(4-)`
D. `O_(3)`

Answer

To solve the question "In which of the following species does each atom carry the same number of lone pairs of electrons?" we will analyze the given options one by one.

### Step-by-Step Solution:

1. **Analyze the first option: XeO4^2-**
- **Structure:** In XeO4^2-, xenon (Xe) is the central atom bonded to four oxygen atoms. Two of these oxygen atoms are negatively charged (O^-) and are single-bonded to xenon, while the other two oxygen atoms are double-bonded.
- **Lone Pairs Calculation:**
- **Xenon (Xe):** It has 8 valence electrons. It forms 6 bonds (4 with O and 2 with O^-). Therefore, it has 1 lone pair left (8 - 6 = 2 electrons, which form 1 lone pair).
- **Oxygen (O):** Each of the double-bonded oxygens has 2 lone pairs, and each of the single-bonded oxygens (O^-) has 3 lone pairs.
- **Conclusion:** The number of lone pairs is different for xenon and oxygen atoms. Thus, this option is not valid.

2. **Analyze the second option: XeF2**
- **Structure:** In XeF2, xenon is the central atom bonded to two fluorine atoms.
- **Lone Pairs Calculation:**
- **Xenon (Xe):** It has 8 valence electrons. It forms 2 bonds with fluorine, leaving 3 lone pairs (8 - 2 = 6 electrons, which form 3 lone pairs).
- **Fluorine (F):** Each fluorine atom has 3 lone pairs (since they have 7 valence electrons and form 1 bond).
- **Conclusion:** All atoms (Xe and F) have the same number of lone pairs (3 for Xe and 3 for each F). Thus, this option is valid.

3. **Analyze the third option: XeO6^4-**
- **Structure:** In XeO6^4-, xenon is bonded to six oxygen atoms.
- **Lone Pairs Calculation:**
- **Xenon (Xe):** It forms 6 bonds with oxygen, using all 8 valence electrons. Therefore, it has 0 lone pairs (8 - 6 = 2 electrons, which do not form a lone pair).
- **Oxygen (O):** Each oxygen atom will have 2 lone pairs.
- **Conclusion:** The number of lone pairs is different for xenon and oxygen atoms. Thus, this option is not valid.

4. **Analyze the fourth option: O3 (Ozone)**
- **Structure:** Ozone consists of three oxygen atoms.
- **Lone Pairs Calculation:**
- **Central Oxygen:** The central oxygen is bonded to two other oxygens, leaving it with 1 lone pair.
- **Terminal Oxygens:** Each terminal oxygen has 2 lone pairs.
- **Conclusion:** The number of lone pairs is different for the central and terminal oxygen atoms. Thus, this option is not valid.

### Final Answer:
The only species where each atom carries the same number of lone pairs of electrons is **XeF2**.

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