Write the electronic configuration and find the no. of unpaired electrons as well as total spin for the following atoms:
`(i) `_(6)C` (ii) `_(8)O` (iii) `_(15)P`
`(iv) `_(21)Sc` (v) `_(26)Fe` (vi) `_(10)Ne`

Explanation

To solve the problem, we will write the electronic configurations for each atom, determine the number of unpaired electrons, and calculate the total spin for each atom.

### Step-by-Step Solution:

**(i) Carbon (C, Atomic Number 6)**
1. **Electronic Configuration**: The electronic configuration of carbon is \(1s^2 2s^2 2p^2\).
2. **Unpaired Electrons**: In the \(2p\) subshell, there are 2 electrons. Since they can occupy separate orbitals, both are unpaired.
3. **Total Spin**: Each unpaired electron has a spin of \(+\frac{1}{2}\). Therefore, total spin = \(2 \times \frac{1}{2} = 1\).
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