Question

What will be the value of x in Fe⁺⁺, if the magnetic moment \(\mu = \sqrt{24}\) BM

• A. 0
• B. 2
• C. 1
• D. 3

Answer 1

The Correct Option is B

The value of x in Fe⁺⁺ can be determined by considering the magnetic moment (µ) and the number of unpaired electrons in the Fe⁺⁺ ion.
In an Fe⁺⁺ ion, the iron atom loses two electrons, resulting in a 2⁺ charge. 
To determine the number of unpaired electrons, we can use the fact that the magnetic moment (µ) is given by the formula: 
\(\mu = \sqrt{n(n+2)}\) BM Where n represents the number of unpaired electrons. 

Given that \(µ = \sqrt{24}\) BM, 
we can solve for n: \(\sqrt{n(n+2)} = \sqrt{24}\)
Squaring both sides: \(n(n+2) = 24\)
Expanding the equation: \(n^2 + 2n = 24\)
Rearranging and simplifying: \(n^2 + 2n - 24 = 0\)
Factorizing the quadratic equation: \((n - 4)(n + 6) = 0\)
Solving for n: n = 4 or n = -6 

Since the number of unpaired electrons cannot be negative, we discard the n = -6 solution.
 Therefore, the Fe⁺⁺ ion has 4 unpaired electrons. 
In Fe⁺⁺, x represents the oxidation state of iron. 
Since Fe⁺⁺ has a 2⁺ charge, the value of x is 2. 
Therefore, the correct value of x in Fe⁺⁺ is (2) 2.