Identify the correct statements from the following :}
A. Heisenberg uncertainty principle is applicable to electrons.
B. The size of \(2p_x\) orbital is less than the size of \(3p_x\) orbital.
C. The energy of \(2s\) orbital of H atom is equal to the energy of \(2s\) orbital of Li.
D. The electronic configuration of Cr is \([Ar] 3d^5 4s^1\)
A. Heisenberg uncertainty principle is applicable to electrons.
B. The size of \(2p_x\) orbital is less than the size of \(3p_x\) orbital.
C. The energy of \(2s\) orbital of H atom is equal to the energy of \(2s\) orbital of Li.
D. The electronic configuration of Cr is \([Ar] 3d^5 4s^1\)
- A, B and C Only
- A, B and D Only
- B, C and D Only
- A, C and D Only
The Correct Option is B
Solution and Explanation
We need to evaluate each statement based on principles of quantum mechanics and atomic theory.
Step 2: Detailed Explanation:
Statement A: The Heisenberg uncertainty principle (\(\Delta x \Delta p \geq \frac{h}{4\pi}\)) applies to all microscopic particles, and the electron is the primary example used in atomic physics. This statement is correct.
Statement B: As the principal quantum number (\(n\)) increases, the distance of the orbital from the nucleus increases, thus increasing its size. A \(3p_x\) orbital is larger than a \(2p_x\) orbital. This statement is correct.
Statement C: The energy of an orbital in a hydrogen-like species depends on \(Z\) (\(E \propto -Z^2/n^2\)). For \(n=2\), the energy of the \(2s\) orbital in H (\(Z=1\)) will be different from that in Li (\(Z=3\)). Specifically, the higher nuclear charge of Li pulls the electrons closer, lowering the energy significantly compared to H. This statement is incorrect.
Statement D: Chromium (\(Z=24\)) has an exceptional configuration due to the extra stability of half-filled \(d\)-subshells. Instead of \([Ar] 3d^4 4s^2\), it is \([Ar] 3d^5 4s^1\). This statement is correct.
Since A, B, and D are correct, option (B) is the right choice.
Step 3: Final Answer:
The correct statements are A, B and D Only.
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