Question:
Consider the following ionization energy order
(A) IE₁: Cr > Mn
(B) IE₂: Cr < Mn
(C) IE₁: Cr < Mn
(D) IE₂: Cr > Mn
Correct order among the following:
Consider the following ionization energy order
(A) IE₁: Cr > Mn
(B) IE₂: Cr < Mn
(C) IE₁: Cr < Mn
(D) IE₂: Cr > Mn
Correct order among the following:
(A) IE₁: Cr > Mn
(B) IE₂: Cr < Mn
(C) IE₁: Cr < Mn
(D) IE₂: Cr > Mn
Correct order among the following:
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When comparing ionization energies, remember that half-filled and fully filled orbitals provide extra stability, which affects the ease of ionization.
Updated On: Apr 7, 2026
- A and B
- B and C
- C and D
- A and D
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The Correct Option is C
Solution and Explanation
In order to answer this question, let's first analyze the ionization energies of Cr and Mn.
Step 1: Ionization Energy for Cr and Mn.
- Chromium (Cr) has an electron configuration of \([Ar]\,3d^5\,4s^1\). This configuration is relatively stable because of the half-filled \(3d\)-orbitals.
- Manganese (Mn) has an electron configuration of \([Ar]\,3d^5\,4s^2\), which is also stable due to the half-filled \(3d\)-orbitals but with an additional \(4s\)-electron.
This stability impacts their ionization energies: - \( \mathrm{IE}_1 \) for Cr is slightly higher than for Mn because the ionization of Cr results in a stable half-filled \(3d^5\) configuration.
- \( \mathrm{IE}_2 \) for Cr is lower than for Mn because removing a second electron from Cr is easier than removing the second from Mn.
Step 2: Analyzing the Statements.
- (A) IE₁: Cr > Mn : This is correct.
- (B) IE₂: Cr < Mn : This is correct.
- (C) IE₁: Cr < Mn : This is incorrect.
- (D) IE₂: Cr > Mn : This is incorrect.
Step 3: Conclusion.
The correct statements are (A) and (B). Final Answer: Option (A) and (B).
- Chromium (Cr) has an electron configuration of \([Ar]\,3d^5\,4s^1\). This configuration is relatively stable because of the half-filled \(3d\)-orbitals.
- Manganese (Mn) has an electron configuration of \([Ar]\,3d^5\,4s^2\), which is also stable due to the half-filled \(3d\)-orbitals but with an additional \(4s\)-electron.
This stability impacts their ionization energies: - \( \mathrm{IE}_1 \) for Cr is slightly higher than for Mn because the ionization of Cr results in a stable half-filled \(3d^5\) configuration.
- \( \mathrm{IE}_2 \) for Cr is lower than for Mn because removing a second electron from Cr is easier than removing the second from Mn.
Step 2: Analyzing the Statements.
- (A) IE₁: Cr > Mn : This is correct.
- (B) IE₂: Cr < Mn : This is correct.
- (C) IE₁: Cr < Mn : This is incorrect.
- (D) IE₂: Cr > Mn : This is incorrect.
Step 3: Conclusion.
The correct statements are (A) and (B). Final Answer: Option (A) and (B).
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