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 determine the correct order of initials T (True) or F (False) for the given statements, we will analyze each statement one by one.

### Step-by-Step Solution:

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

1. **Analysis:** According to VSEPR (Valence Shell Electron Pair Repulsion) theory, the repulsion between lone pairs (I_p) is greater than the repulsion between lone pair and bond pair (I_p - b_p), which in turn is greater than the repulsion between bond pairs (b_p - b_p).
2. **Conclusion:** This statement is **True (T)**.

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

1. **Analysis:** Increasing the number of lone pairs on the central atom actually decreases the bond angle. For example, in water (H₂O), which has two lone pairs, the bond angle is 104.5°, while in ammonia (NH₃), which has one lone pair, the bond angle is 107.5°.
2. **Conclusion:** This statement is **False (F)**.

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**Statement III:** The number of lone pairs on O in H₂O is 2 while on N in NH₃ is 1.

1. **Analysis:** In H₂O, oxygen has 6 valence electrons, 2 of which are used to form bonds with hydrogen, leaving 2 lone pairs. In NH₃, nitrogen has 5 valence electrons, 3 of which are used to form bonds with hydrogen, leaving 1 lone pair.
2. **Conclusion:** This statement is **True (T)**.

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

1. **Analysis:** The structures of xenon fluorides (like XeF₂) and xenon oxyfluorides (like XeOF₂) can indeed be explained using VSEPR theory. For example, XeF₂ has a linear shape due to its steric number of 5, and XeOF₂ has a T-shaped geometry.
2. **Conclusion:** This statement is **False (F)**.

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### Final Order of Initials:
- **I:** T
- **II:** F
- **III:** T
- **IV:** F

Thus, the correct order is **T, F, T, F**.

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