Write True/False:
Fluorine cannot have +1 oxidation state.

Answer

To determine whether the statement "Fluorine cannot have +1 oxidation state" is true or false, we can follow these steps:

### Step 1: Understand the Atomic Structure of Fluorine
Fluorine has an atomic number of 9. This means it has 9 electrons. The electronic configuration of fluorine is:
- 1s² 2s² 2p⁵

### Step 2: Analyze the Valence Electrons
In the outermost shell (2nd shell), fluorine has:
- 2 electrons in the 2s subshell
- 5 electrons in the 2p subshell

This gives a total of 7 valence electrons (2 from 2s and 5 from 2p).

### Step 3: Determine the Tendency of Fluorine
Fluorine has a strong tendency to gain electrons to achieve a stable octet configuration. It is highly electronegative and typically gains one electron to form a -1 oxidation state (F⁻).

### Step 4: Consider the Possibility of Losing Electrons
For fluorine to have a +1 oxidation state, it would need to lose one electron. However, since it has only one electron deficiency in its p subshell, it is more favorable for fluorine to gain an electron rather than lose one.

### Step 5: Check for d-Orbitals
Fluorine does not have d-orbitals available to promote electrons. The absence of d-orbitals means that fluorine cannot excite its electrons to higher energy levels, which would be necessary for it to lose an electron and exhibit a +1 oxidation state.

### Conclusion
Given the above analysis, we conclude that fluorine cannot have a +1 oxidation state. Therefore, the statement "Fluorine cannot have +1 oxidation state" is **False**.

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