$4d, 5p, 5f$ and $6p$ orbitals are arranged in the order of decreasing energy. The correct option is

Consider the following pairs of electrons:
$(A)$ $(a)$ $n=3, l=1, m_{l}=1, m_{s}=+\frac{1}{2}$
$(b)$ $n=3, l=2, m_{l}=1, m_{s}=+\frac{1}{2}$
$(B)$ $(a)$ $n=3, l=2, m_{l}=-2, m_{s}=-\frac{1}{2}$
$(b)$ $n=3, l=2, m_{l}=-1, m_{s}=-\frac{1}{2}$
$(C)$ $(a)$ $n=4, l=2, m_{l}=2, m_{s}=+\frac{1}{2}$
$(b)$ $n=3, l=2, m_{l}=2, m_{s}=+\frac{1}{2}$
The pair$(s)$ of electrons present in degenerate orbitals is/are...... .

An electron having the quantum numbers $n = 4, l = 3, m = 0, s = -\frac{1}{2}$ would be in the orbital

For electrons having principal quantum number $n = 3$,the number of $(i)$ subshells and $(ii)$ orbitals would be respectively:

The atomic orbitals are progressively filled in order of increasing energy. This principle is called as

Which quantum number determines the shape of the subshell?