Ionic radii of
(1) `Ti^(4+) lt Mn^(7+)`
(2) `""^(35)Cl^(-) lt ""^(37)Cl^(-)`
(3) `K^(+) gt Cl^(-)`
(4)`P^(5+) gt P^(3+)` Correct the statements

Explanation

To correct the statements regarding the ionic radii, let's analyze each statement step by step.

### Step 1: Analyze the first statement
**Statement:** `Ti^(4+) < Mn^(7+)`

- **Explanation:** Titanium (Ti) has an atomic number of 22, and manganese (Mn) has an atomic number of 25. When titanium loses 4 electrons to form Ti^(4+), it has 18 electrons left. Manganese loses 7 electrons to form Mn^(7+), also resulting in 18 electrons. Both ions are isoelectronic (same number of electrons). However, Mn^(7+) has more protons (25) compared to Ti^(4+) (22). The greater positive charge from Mn's protons pulls the electron cloud closer, resulting in a smaller ionic radius.

- **Correction:** The correct statement should be `Ti^(4+) > Mn^(7+)`.

### Step 2: Analyze the second statement
**Statement:** `Cl^(35-) < Cl^(37-)`

- **Explanation:** Chlorine-35 and Chlorine-37 are isotopes of chlorine, meaning they have the same number of protons (17) but different numbers of neutrons. The ionic charge is the same for both (−1), and since isotopes have nearly the same size, their ionic radii will also be approximately equal.

- **Correction:** The correct statement should be `Cl^(35-) ≈ Cl^(37-)`.

### Step 3: Analyze the third statement
**Statement:** `K^(+) > Cl^(-)`

- **Explanation:** Potassium (K) has an atomic number of 19 and loses one electron to form K^(+), resulting in 18 electrons. Chlorine (Cl) has an atomic number of 17 and gains one electron to form Cl^(-), also resulting in 18 electrons. Both ions are isoelectronic. However, K has more protons (19) than Cl (17), which means K^(+) will have a smaller ionic radius compared to Cl^(-).

- **Correction:** The correct statement should be `K^(+) < Cl^(-)`.

### Step 4: Analyze the fourth statement
**Statement:** `P^(5+) > P^(3+)`

- **Explanation:** Phosphorus (P) has an atomic number of 15. When it loses 5 electrons to form P^(5+), it has 10 electrons left. When it loses 3 electrons to form P^(3+), it has 12 electrons left. Both ions have the same number of protons (15). However, P^(5+) has fewer electrons and thus a smaller ionic radius compared to P^(3+).

- **Correction:** The correct statement should be `P^(5+) < P^(3+)`.

### Summary of Corrections
1. `Ti^(4+) > Mn^(7+)`
2. `Cl^(35-) ≈ Cl^(37-)`
3. `K^(+) < Cl^(-)`
4. `P^(5+) < P^(3+)`