Which of the following sets of quantum numbers represent an impossible arrangement?
 

The quantum numbers of four electrons are given below.

                                  n            $\mathcal{l}$           m          s 

(1) Electron 1             3            0             0           -1/2

(2) Electron 2             4            0             0           1/2

(3) Electron 3            3             2             0           1/2

(4) Electron 4            3             1             0           -1/2

The correct order of decreasing energy of these electrons is - 

1. Electron 3 > Electron 1 > Electron 4> Electron 2

2. Electron 4> Electron 2 > Electron 3 > Electron 1

3. Electron 3 > Electron 2 > Electron 4 > Electron 1

4. Electron 2 > Electron 4 > Electron 3 > Electron 1

The maximum number of atomic orbitals associated with a principal quantum number 5 is-

1. 9

2. 12

3. 16

4. 25

The quantum number of the most energetic electron in an Ne atom in the first excited state is

The total number of orbitals having l = 3  is - 

1. 3

2. 7

3. 5

4. 9

To give designation to an orbital, we need

1. Principal and azimuthal quantum number

2. Principal and magnetic quantum number

3. Azimuthal and magnetic quantum number

4. Principal, azimuthal and magnetic quantum numbers.

Which one of the following statement is not true about the quantum numbers n, l, m and s

1. m gives the information on the energy of the electron in a given orbital.

2. l gives an idea of the shape of the orbital.

3. n gives information on the size of the orbit.

4. s gives the direction of spin of the electron in the orbital.

The total spin resulting for a 3d⁷ configuration is 

1. 3/2

2. 1/2

3. 2

4. 1

Which of the following set of quantum number is not valid

1. n = 1 , $\mathcal{l}$ = 2

2. n=2, m = 1

3. n =3, $\mathcal{l}$ = 0

4. n = 4, $\mathcal{l}$ = 2

The azimuthal quantum number characterizes:

1. e/m ratio of electron
2. Spin of electron
3. Angular momentum of the electron
4. Magnetic momentum of the electron