The two electron have the following sets of quantum number
X `3,2 -2,+ 1//2`
Y `3,0,0, + 1//2`
What is true of the following

Options

A. X and Y have same energy
B. X and Y have unequal energy
C. X and Y have represent same orbital
D. None of the statement is correct

Explanation

To solve the question regarding the two electrons with given quantum numbers, we will analyze the quantum numbers step by step.

### Step 1: Identify the quantum numbers for each electron.
- For electron X, the quantum numbers are:
- Principal quantum number (n) = 3
- Azimuthal quantum number (l) = 2
- Magnetic quantum number (m) = -2
- Spin quantum number (s) = +1/2

- For electron Y, the quantum numbers are:
- Principal quantum number (n) = 3
- Azimuthal quantum number (l) = 0
- Magnetic quantum number (m) = 0
- Spin quantum number (s) = +1/2

### Step 2: Determine the type of orbitals for each electron.
- For electron X (n=3, l=2):
- The azimuthal quantum number (l=2) corresponds to d orbitals. Therefore, electron X is in the 3d orbital.

- For electron Y (n=3, l=0):
- The azimuthal quantum number (l=0) corresponds to s orbitals. Therefore, electron Y is in the 3s orbital.

### Step 3: Calculate the n + l values for both electrons.
- For electron X:
- n + l = 3 + 2 = 5

- For electron Y:
- n + l = 3 + 0 = 3

### Step 4: Compare the n + l values to determine energy levels.
- Since the n + l value for electron X (5) is greater than that for electron Y (3), this indicates that electron X is in a higher energy orbital compared to electron Y.

### Step 5: Conclusion based on the analysis.
- Electron X is in the 3d orbital, which is of higher energy than the 3s orbital where electron Y is located. Therefore, we conclude that:
- Electron X is in a more energetic orbital than electron Y.

### Final Answer:
- The correct statement is that electron X is in a higher energy orbital than electron Y.