Question:
What is the number of unpaired electrons in \(\mathrm{C}_0\) in +2 state?
What is the number of unpaired electrons in \(\mathrm{C}_0\) in +2 state?
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Write the electronic configuration of Co(II).
Updated On: Nov 13, 2026
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The Correct Option is B
Solution and Explanation
Step 1: Understanding the Concept
Cobalt \((Z=27)\) is \([\text{Ar}]3d^{7}4s^{2}\). In the \(+2\) state the two \(4s\) electrons are lost.
Step 2: Configuration
\(\text{Co}^{2+}:[\text{Ar}]3d^{7}\).
Step 3: Unpaired Electrons
In \(3d^{7}\) two orbitals are fully filled and three hold one electron each, so there are 3 unpaired electrons. Option (B).
Final Answer:
\(\text{Co}^{2+}\) has 3 unpaired electrons. \[ \boxed{\text{(B) }3} \]
Cobalt \((Z=27)\) is \([\text{Ar}]3d^{7}4s^{2}\). In the \(+2\) state the two \(4s\) electrons are lost.
Step 2: Configuration
\(\text{Co}^{2+}:[\text{Ar}]3d^{7}\).
Step 3: Unpaired Electrons
In \(3d^{7}\) two orbitals are fully filled and three hold one electron each, so there are 3 unpaired electrons. Option (B).
Final Answer:
\(\text{Co}^{2+}\) has 3 unpaired electrons. \[ \boxed{\text{(B) }3} \]
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