Fluorine does not show positive oxidation state due to the -

Options

A. Absence of s-orbitals
B. Absence of p-orbitals
C. Absence of d-orbitals
D. Highest electronegativity

Answer

### Step-by-Step Solution:

1. **Understanding the Question**: The question asks why fluorine does not exhibit a positive oxidation state.

2. **Atomic Number and Electron Configuration**: Fluorine has an atomic number of 9. Its electron configuration is 1s² 2s² 2p⁵. This means it has a total of 7 valence electrons (2 in the 2s orbital and 5 in the 2p orbital).

3. **Valence Electrons and Oxidation States**: The oxidation state of an element is determined by the number of electrons it can lose, gain, or share. Elements with fewer valence electrons tend to lose them and show positive oxidation states, while those with more valence electrons tend to gain electrons and show negative oxidation states.

4. **Electronegativity**: Fluorine is the most electronegative element in the periodic table. Electronegativity is a measure of an atom's ability to attract and hold onto electrons. Because fluorine has a high electronegativity, it strongly attracts electrons rather than losing them.

5. **Position in the Periodic Table**: Fluorine is located in Group 17 (the halogens) and Period 2 of the periodic table. As you move from left to right across a period, electronegativity increases. Being in the second period and having a high effective nuclear charge, fluorine's outer electrons are held tightly, making it unlikely to lose them.

6. **Conclusion**: Due to its high electronegativity and the stability of its electron configuration, fluorine does not show a positive oxidation state. Instead, it tends to gain one electron to achieve a stable noble gas configuration, resulting in a -1 oxidation state.

### Final Answer:
Fluorine does not show a positive oxidation state due to its **high electronegativity**.

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