Phosphorous does not show oxidation state of `+ 4`.

Answer

To determine whether phosphorus can exhibit an oxidation state of +4, let's analyze the electronic configuration and bonding characteristics of phosphorus.

### Step 1: Understand the Electronic Configuration of Phosphorus
Phosphorus (P) has an atomic number of 15. Its electronic configuration is:
\[ \text{1s}^2 \text{2s}^2 \text{2p}^6 \text{3s}^2 \text{3p}^3 \]
This shows that phosphorus has 5 valence electrons (2 from 3s and 3 from 3p).

**Hint:** Remember that the oxidation state is related to the number of valence electrons and how they can bond with other elements.

### Step 2: Determine Possible Oxidation States
Phosphorus can exhibit various oxidation states, including -3, 0, +3, and +5. The +5 oxidation state is achieved when phosphorus forms five bonds, utilizing all five valence electrons.

**Hint:** Consider how many bonds phosphorus can form based on its valence electrons.

### Step 3: Analyze the +4 Oxidation State
To achieve an oxidation state of +4, phosphorus would need to form four bonds. This would leave one unpaired electron. However, for phosphorus to maintain a +4 oxidation state, it would need to bond with four electronegative atoms (let's denote them as X).

**Hint:** Think about the stability of having an unpaired electron in the valence shell.

### Step 4: Stability of the +4 Oxidation State
When phosphorus forms four bonds, it would theoretically have one unpaired electron. This configuration is unstable because the presence of an unpaired electron makes the molecule reactive and less stable.

**Hint:** Reflect on the stability of compounds and how unpaired electrons affect reactivity.

### Step 5: Conclusion
Due to the instability associated with the +4 oxidation state and the lack of known stable compounds exhibiting this state, it can be concluded that phosphorus does not show an oxidation state of +4.

**Final Answer:** True, phosphorus does not show an oxidation state of +4.