List I Quantum Number |
List II Information provided |
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A. | ml | I. | Shape of orbital |
B. | ms | II. | Size of orbital |
C. | l | III. | Orientation of orbital |
D. | n | IV. | Orientation of spin of electron |
I: | \(\Psi\) depends upon the coordinates of the electron in the atom. | The value of wave function,
II: | The probability of finding an electron at a point within an atom is proportional to the orbital wave function. |
Two electrons occupying the same orbital are distinguished by:
1. Magnetic quantum number
2. Azimuthal quantum number
3. Spin quantum number
4. Principal quantum number
What is the maximum number of orbitals that can be identified with the following quantum numbers?
n = 3, l = 1, m = 0
1. | 1 | 2. | 2 |
3. | 3 | 4. | 4 |
Maximum number of electrons in a subshell with l = 3 and n = 4 is:
1. 14
2. 16
3. 10
4. 12
The correct set of four quantum numbers for the valence electron of a rubidium atom (Z =37) is:
1. | \(5,1,1,+ {1 \over2}\) | 2. | \(6,0,0,+ {1 \over2}\) |
3. | \(5,0,0,+ {1 \over2}\) | 4. | \(5,1,0,+ {1 \over2}\) |
The incorrect set of quantum numbers among the following is:
1. n= 4, l= 0, m= 0, s= -1/2
2. n= 5, l= 3, m= 0, s= +1/2
3. n= 3, l= 2, m= -3, s= -1/2
4. n= 3, l= 2, m= 2, s= -1/2
Consider the following sets of quantum numbers:
Which of the following sets of quantum numbers is not possible?
1. ii, iii, and iv
2. i, ii, iii, and iv
3. ii, iv and v
4. i and iii