Q. No.1. n=4,l=3, m1 =-3, -2, -1, 0, +1, +2, +3, ms=-1/2
2. n=5, l=2, m1 =-2, -1, +1, +2, ms=+1/2
3. n=4, l=2, m1 = -2, -1, 0, +1, +2, ms=-1/2
4. n=5,l=3, m1 =-3, -2, -1, 0, +1, +2, +3, ms=+1/2
| I: | The value of wave function, \(\Psi\) depends upon the coordinates of the electron in the atom |
| II: | The probability of finding an electron at a point within an atom is proportional to the orbital wave function |
In light of the above statements, choose the correct answer from the options given below:
1. Statement I is true but Statement II is false.
2. Statement I is false but Statement II is true.
3. Both Statement I and Statement II are true.
4. Both Statement I and Statement II are false.
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 |
n = 3, l = 1 and m = –1.
2. 4
3. 2
4. 10
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
The orientation of an atomic orbital is governed by:
1. azimuthal quantum number
2. spin quantum number
3. magnetic quantum number
4. principal quantum number
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