The electronic configuration of an element is 1S\(^2\) 2S\(^2\) 2P\(^6\) 3S\(^2\) 3P\(^3\). How many unpaired electrons are there in the element?
5
4
3
2
Explanation
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Let's analyze the given electronic configuration step by step:
1S^2\ 2S^2\ 2P^6\ 3S^2\ 3P^3
1. Identify the element:
The total number of electrons = 2 + 2 + 6 + 2 + 3 = 15
Atomic number 15 corresponds to phosphorus (P).
2. Determine the unpaired electrons:
The 3p orbital has 3 electrons:
The p subshell has three orbitals (px, py, pz).
According to Hund’s rule, electrons fill these orbitals singly first before pairing.
So, the three 3p electrons remain unpaired, one in each orbital.
Answer:
The number of unpaired electrons = 3
Correct option: C. 3
Seriously..this 1s^2 poo's still confusing...no wonder no body knows squat about it
Easy way for me is, jst draw the structure and count the remaining ones to make it 8 at the outer shell.
