Quantum Numbers MCQs

Quantum numbers are used to describe the position and energy of electrons in an atom. Atomic orbitals vary in size, energy, shape, and orientation, and each orbital is defined by three quantum numbers: the principal quantum number (n), the azimuthal quantum number (l), and the magnetic quantum number (m or m_l). The fourth quantum number, known as the spin quantum number (s or m_s), indicates the spin of the electron within the orbital.

The maximum number of electrons that can fit in an orbital with n = 3 and l = 1?

(a) 14
(b) 6
(c) 10
(d) 2

Which of the following quantum numbers tells the three-dimensional shape of an atomic orbital?

(a) Azimuthal quantum number
(b) Principal quantum number
(c) Spin quantum number
(d) Magnetic quantum number

The maximum number of electrons that can fit in all the orbitals with n = 2 and l = 1?

(a) 8
(b) 2
(c) 6
(d) 4

What is the maximum number of electrons, which can have following quantum numbers, n = 3, l = 1, m = -1?

(a) 2
(b) 6
(c) 10
(d) 4

The maximum number of electrons with l = 3 is

(a) 14
(b) 2
(c) 10
(d) 6

The maximum number of orbitals present in a subshell can be represented by

(a) 2l + 1
(b) 2n²
(c) 4l + 2
(d) 4l – 2

How many orbitals can have the following quantum numbers, n = 3, l = 1, ml = 0?

(a) 4
(b) 2
(c) 1
(d) 3

Which of the following quantum numbers governs the spatial orientation of an atomic orbital?

(a) Magnetic quantum number
(b) Spin quantum number
(c) Azimuthal quantum number
(d) Principal quantum number

Which of the following quantum numbers can distinguish between two electrons present in the same orbital?

(a) Azimuthal quantum number
(b) Principal quantum number
(c) Magnetic quantum number
(d) Spin quantum number

The maximum number of electrons which can be present in a subshell can be represented by

(a) 2l + 1
(b) 2n²
(c) 4l + 2
(d) 4l – 2