Quantum Mechanical Model of Atom

Among the following, the INCORRECT statement is

The electronic configuration which obeys Hund's rule for the ground state of carbon atom is:

Maximum number of electrons that can be accommodated in the subshell with azimuthal quantum number $\mathrm{l}=4$, is:

For a one-electron atom, the set of allowed quantum numbers is:

Which of the following is not correct for electronic distribution in the ground state?

If an electron has spin quantum number $+1/2$ and the magnetic quantum number $-1$, it cannot be present in

Which of the following explains the sequence of filling electrons in different shells?

The correct order of increasing energy of atomic orbitals is

A $5\mathrm{f}-$orbital has

For a $\mathrm{f}-$orbital, the values of $\mathrm{m}$ are

For how many orbitals, the quantum numbers $\mathrm{n}=3, \mathrm{l}=2, \mathrm{m}=+2$ are possible?

The maximum number of electrons in a subshell with $\mathrm{l}=2$ and $\mathrm{n}=3$ is

The maximum number of electrons in a subshell of an atom is determined by

Which of the following sets of quantum numbers is correct for an electron in $4\mathrm{f}-$orbital?

The electrons identified by the quantum numbers $\mathrm{n}$ and $\mathrm{l}$.

(A) $\mathrm{n}=4, \mathrm{l}=1$

(B) $\mathrm{n}=4, \mathrm{l}=0$

(C) $\mathrm{n}=3, \mathrm{l}=2$

(D) $\mathrm{n}=3, \mathrm{l}=1$

These can be placed in the order of increasing energy as

Which of the following should be the possible subshells for $\mathrm{n}+\mathrm{l}=7$?

What should be the maximum number of electrons in the possible subshells for $\mathrm{n}+l=4$?

For azimuthal quantum number $\mathrm{l}=3$, the maximum number of electrons will be

In a given atom, no two electrons can have the same values for all the four quantum numbers. This is called

The total number of electrons that can be accommodated in all orbitals having principal quantum number $2$ and azimuthal quantum number $1$ is