Astatine is the element below iodine in the group `VIIA` of the periodic table. Which of the following statements is not true for astatine?

Options

A. It is less electronegative than iodine
B. It will exhibit only - 1 oxidation state.
C. Intermoleculer forces between the astaine molecules will be larger than that between iodine molecules.
D. None of these.

Answer

To determine which statement about astatine (At) is not true, we can analyze the properties of astatine in comparison to iodine (I), as well as the general trends in the periodic table for group VIIA (halogens).

### Step-by-Step Solution:

1. **Identify the Position of Astatine**:
Astatine is located below iodine in group VIIA of the periodic table.

**Hint**: Remember that elements in the same group share similar chemical properties.

2. **Understand Trends in the Group**:
As we move down a group in the periodic table, the atomic size increases, and electronegativity generally decreases.

**Hint**: Consider how atomic size and electronegativity are related in the periodic table.

3. **Analyze the Statements**:
- **Statement 1**: Astatine is less electronegative than iodine.
- This statement is true because, as mentioned, electronegativity decreases down the group.

- **Statement 2**: Astatine will exhibit only negative oxidation states.
- This statement is false. Astatine can exhibit positive oxidation states due to the presence of d and f orbitals, which allow for electron promotion.

- **Statement 3**: The intermolecular forces between astatine molecules will be larger than those between iodine molecules.
- This statement is true. Astatine, being larger than iodine, has greater van der Waals forces due to its larger electron cloud, but the intermolecular forces are generally weaker due to increased distance.

4. **Conclusion**:
The only statement that is not true for astatine is that it will exhibit only negative oxidation states. Therefore, the answer is Statement 2.

### Final Answer:
The statement that is not true for astatine is: "Astatine will exhibit only negative oxidation states."