Number of bond pairs and lone pairs respectively that the central atom in xenon difluoride has

Options

A. 2,6
B. 2, 3
C. 2,4
D. 2, 2

Answer

To determine the number of bond pairs and lone pairs around the central atom in xenon difluoride (XeF2), we can follow these steps:

### Step 1: Identify the Central Atom
The central atom in xenon difluoride is xenon (Xe).

### Step 2: Determine the Valence Electrons
Xenon is a noble gas and has a complete octet in its ground state, with the electron configuration of [Kr] 5s² 5p⁶. However, in the case of xenon difluoride, xenon can expand its octet.

- **Valence Electrons of Xenon**: 8 (from 5s and 5p orbitals)

### Step 3: Consider the Bonding with Fluorine
Each fluorine atom (F) contributes one electron to form a bond with xenon. Since there are two fluorine atoms in xenon difluoride, xenon will use two of its valence electrons to form bonds.

- **Electrons used for bonding**: 2 (1 from each F)

### Step 4: Calculate Remaining Electrons
After forming bonds with the two fluorine atoms, we can calculate the remaining valence electrons for xenon.

- **Remaining Electrons**: 8 (total) - 2 (bonding) = 6 electrons

### Step 5: Determine Lone Pairs
The remaining 6 electrons will be arranged as lone pairs around the xenon atom. Each lone pair consists of 2 electrons.

- **Lone Pairs**: 6 electrons / 2 = 3 lone pairs

### Step 6: Count Bond Pairs
From the previous steps, we have determined that there are 2 bond pairs (one from each fluorine).

### Final Answer
Thus, the central atom in xenon difluoride has:
- **Bond Pairs**: 2
- **Lone Pairs**: 3

### Summary
The number of bond pairs and lone pairs respectively that the central atom in xenon difluoride has is:
- **2 bond pairs and 3 lone pairs**.

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