Give the correct order of initials T or F for following statements. Use T if statement is true and F if it is falese `:`
`(I)` The order of repulsion between different pair of electron is `I_(p)-I_(p)gtI_(p)-b_(p)gtb_(p)-b_(p)`
`(II)` In general, as the number o flone pair of electron on central atom increases, value of bond angle from normal bond angle also increases
`(III)` The number of lone pair on O in `H_(2)O` is 2 while on N in `NH_(3)` is 1
`(IV)` The structures of xenon fluorides and xenon oxyfluorides could not be explained on the basis of VSEPR theory

Options

A. T T TF
B. TFTF
C. TFT T
D. TF F F

Explanation

To solve the question, we will evaluate each statement one by one and determine whether they are true (T) or false (F).

### Step-by-Step Solution:

**Statement (I):** The order of repulsion between different pairs of electrons is \( I_p - I_p > I_p - b_p > b_p - b_p \).

- **Analysis:**
- Lone pair-lone pair (I_p - I_p) repulsions are indeed the strongest due to the high electron density associated with lone pairs.
- Lone pair-bond pair (I_p - b_p) repulsions are weaker than lone pair-lone pair but stronger than bond pair-bond pair (b_p - b_p) repulsions.
- Therefore, this statement is **True (T)**.

**Statement (II):** In general, as the number of lone pairs of electrons on the central atom increases, the value of bond angle from the normal bond angle also increases.

- **Analysis:**
- As the number of lone pairs increases, the bond angles actually decrease due to increased repulsion from lone pairs. For example, in methane (no lone pairs), the bond angle is 109.5°, in ammonia (one lone pair), it is about 107°, and in water (two lone pairs), it is about 104.5°.
- Therefore, this statement is **False (F)**.

**Statement (III):** The number of lone pairs on O in \( H_2O \) is 2 while on N in \( NH_3 \) is 1.

- **Analysis:**
- In water (\( H_2O \)), oxygen has two lone pairs. In ammonia (\( NH_3 \)), nitrogen has one lone pair. This statement is accurate.
- Therefore, this statement is **True (T)**.

**Statement (IV):** The structures of xenon fluorides and xenon oxyfluorides could not be explained on the basis of VSEPR theory.

- **Analysis:**
- The VSEPR theory can indeed explain the structures of xenon fluorides and xenon oxyfluorides. The shapes and angles can be predicted using VSEPR theory based on the number of bonding and lone pairs around the xenon atom.
- Therefore, this statement is **False (F)**.

### Final Order of Statements:
- (I) T
- (II) F
- (III) T
- (IV) F

Thus, the correct order of initials is **TFTF**.