Atomicity of phosphorus is :

Question

Accepted Answer

The atomicity of an element refers to the number of atoms present in a molecule of that element. For phosphorus, the correct atomicity is 4, which corresponds to Option 3. This is because phosphorus commonly exists as a tetraatomic molecule, denoted as P₄. In its most stable form, phosphorus forms a molecule consisting of four phosphorus atoms bonded together in a tetrahedral structure. This is the most common and stable form of phosphorus found in nature.

Now, let's explain why the other options are incorrect:

1. **Option 1: 2** - This option is incorrect because phosphorus does not naturally exist as a diatomic molecule (P₂) under normal conditions. Diatomic molecules are more characteristic of gases like oxygen (O₂) or nitrogen (N₂), but not phosphorus.

2. **Option 2: 0** - This option is incorrect because an atomicity of 0 would imply that phosphorus does not form molecules, which is not true. Phosphorus does form molecules, specifically P₄, as mentioned earlier.

3. **Option 4: 3** - This option is incorrect because phosphorus does not naturally exist as a triatomic molecule (P₃). There is no stable form of phosphorus that consists of three atoms bonded together.

In conclusion, the atomicity of phosphorus is 4, as it forms stable tetraatomic molecules (P₄), making Option 3 the correct answer.