Pauli's Exclusion Principle

Q. If the nitrogen atom had an electronic configuration of $1s^7$ it would have lower energy than that of the normal ground state configuration $1s^2,2s^2,2p^3$ because the electrons would be closer to the nucleus. $1s^7$ is not observed because it violates:

1. Heisenberg’s uncertainty principle
2. Hund’s rule
3. Pauli's exclusion principle
4. Aufbau Principle

Q.

Any p-orbital can accommodate up to:

1. 2 electrons with opposite spins

2. 4 electrons

3. 6 electrons

4. 2 electrons with parallel spins

Q. If carbon has electronic configuration $1s^6$, it would have lower energy than that of the normal ground state configuration $1s^{2}2s^{2}2p^2$, because the electrons would be closer to the nucleus. Yet $1s^6$ is not observed, since it violates

1. Heisenberg uncertainty principle
2. Hund's rule of maximum multiplicity
3. Pauli's exclusion principle
4. Bohr's postulate of stationary orbits

Q. Any '$p$' orbital can accommodate upto:

1. Four electrons
2. Six electrons
3. Two electrons with parallel spins
4. Two electrons with opposite spins

Q. The ground state electronic configuration of nitrogen atom can be represented by

1. 
2. 
3. 
4. 

Q. The possible number of electrons for which n = 4, $l$ = 3 and s = +$\frac{1}{2}$ is:

1. 7
2. 5
3. 10
4. 14

Q. An orbital can have 10 electrons

1. True
2. False