Which one of the following is wrong ?

Options

A. Oxygen and sulphur belong to the same group of periodic table
B. Oxygen is a gas while sulphur is solid
C. Both oxygen and sunphur show `+2, +4` and `+6` oxidation states.
D. `H_2 S` has no hydrogen bonding

Explanation

To solve the question "Which one of the following is wrong?" regarding the properties of oxygen and sulfur, we will analyze each statement provided.

### Step-by-Step Solution:

1. **Identify the Group**:
- Oxygen and sulfur are both in Group 16 of the periodic table. This statement is correct.

**Hint**: Check the periodic table to confirm the group placement of elements.

2. **Physical State**:
- Oxygen exists as a gas (O₂) at room temperature, while sulfur exists as a solid. This statement is also correct.

**Hint**: Recall the physical states of elements at room temperature.

3. **Oxidation States**:
- The statement claims that both oxygen and sulfur can show +2, +4, and +6 oxidation states. This is where we need to analyze further.
- Sulfur can exhibit +2, +4, and +6 oxidation states due to the availability of empty d-orbitals in its electronic configuration (3s² 3p⁴).
- However, oxygen can only exhibit +2 oxidation state (as in OF₂) and does not have the capacity to show +4 and +6 oxidation states due to the absence of empty d-orbitals in its electronic configuration (1s² 2s² 2p⁴). Therefore, this statement is incorrect.

**Hint**: Consider the electronic configurations and the concept of oxidation states in relation to available orbitals.

4. **Hydrogen Bonding**:
- The statement regarding hydrogen sulfide (H₂S) not having hydrogen bonding is correct. Hydrogen bonds typically form between hydrogen and highly electronegative elements with small atomic sizes, such as fluorine, nitrogen, and oxygen. Sulfur, being larger and less electronegative, does not form hydrogen bonds with hydrogen.

**Hint**: Review the criteria for hydrogen bond formation.

### Conclusion:
The wrong statement among the options is the one that claims both oxygen and sulfur can show +2, +4, and +6 oxidation states. Oxygen can only show a +2 oxidation state due to its electronic configuration.

### Final Answer:
The wrong statement is: "Oxygen and sulfur show +2, +4, +6 oxidation states."

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