Oxygen cannot exhibit higher oxidation states due to

Options

A. small size
B. more electronegativity
C. less density
D. absence of d' orbitals

Answer

To answer the question "Oxygen cannot exhibit higher oxidation states due to," we can analyze the factors affecting the oxidation states of oxygen step by step.

### Step-by-Step Solution:

1. **Understanding Oxidation States**:
- Oxidation states refer to the degree of oxidation of an atom in a compound. Higher oxidation states indicate the loss of more electrons.

2. **Oxygen's Position in the Periodic Table**:
- Oxygen is located in Group 16 of the periodic table and has an atomic number of 8. Its electronic configuration is \(1s^2 2s^2 2p^4\).

3. **Valence Electrons**:
- The valence shell of oxygen consists of 2s and 2p orbitals. Specifically, it has 6 valence electrons (2 from 2s and 4 from 2p).

4. **Limitations of Higher Oxidation States**:
- To exhibit higher oxidation states, an element typically needs to promote electrons to higher energy orbitals. This often involves moving electrons from the valence shell to available d orbitals.

5. **Absence of d Orbitals**:
- Oxygen is in the second period of the periodic table, where the principal quantum number is 2. This means it does not have d orbitals available in its valence shell (the 3d orbitals start from the third period).

6. **Conclusion**:
- Since oxygen lacks d orbitals, it cannot promote electrons to higher energy levels to form higher oxidation states. Therefore, the maximum oxidation state that oxygen can exhibit is -2 (when it gains two electrons).

### Final Answer:
Oxygen cannot exhibit higher oxidation states due to the absence of d orbitals in its valence shell.

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