Welcome to the **Quantum Numbers MDCAT** MCQs with Answers. In this post, we have shared **Quantum Numbers** Multiple Choice Questions and Answers for **PMC MDCAT 2024**. Each question in MDCAT Chemistry offers a chance to enhance your knowledge regarding **Quantum Numbers** MCQs in this MDCAT Online Test.

Which quantum number defines the shape of an orbital?

a) Principal quantum number (n)

b) Azimuthal quantum number (l)

c) Magnetic quantum number (m_l)

d) Spin quantum number (m_s)

What does the principal quantum number (n) represent?

a) Shape of the orbital

b) Size and energy level of the orbital

c) Orientation of the orbital

d) Spin of the electron

Which quantum number determines the orientation of an orbital?

a) Principal quantum number (n)

b) Azimuthal quantum number (l)

c) Magnetic quantum number (m_l)

d) Spin quantum number (m_s)

The spin quantum number (m_s) can have which values?

a) 0 and 1

b) -1/2 and +1/2

c) 0 and +1

d) +1 and -1

Which quantum number is represented by the symbol ‘l’?

a) Principal quantum number

b) Azimuthal quantum number

c) Magnetic quantum number

d) Spin quantum number

What is the range of possible values for the magnetic quantum number (m_l) when l = 2?

a) -1 to +1

b) -2 to +2

c) -3 to +3

d) 0 to 2

For an electron in a p orbital, the value of l is:

a) 0

b) 1

c) 2

d) 3

Which quantum number determines the number of orbitals in a subshell?

a) Principal quantum number (n)

b) Azimuthal quantum number (l)

c) Magnetic quantum number (m_l)

d) Spin quantum number (m_s)

If n = 3, how many different values can l take?

a) 1

b) 2

c) 3

d) 4

Which quantum number specifies the energy level of an electron in an atom?

a) Principal quantum number (n)

b) Azimuthal quantum number (l)

c) Magnetic quantum number (m_l)

d) Spin quantum number (m_s)

What is the maximum number of electrons that can be in a d subshell?

a) 2

b) 6

c) 10

d) 14

In which quantum number does the concept of orbitals with different shapes appear?

a) Principal quantum number (n)

b) Azimuthal quantum number (l)

c) Magnetic quantum number (m_l)

d) Spin quantum number (m_s)

Which quantum number can have integral values from -l to +l, including zero?

a) Principal quantum number (n)

b) Azimuthal quantum number (l)

c) Magnetic quantum number (m_l)

d) Spin quantum number (m_s)

What is the value of the spin quantum number (m_s) for an electron with spin-up orientation?

a) +1

b) -1

c) +1/2

d) -1/2

Which quantum number describes the angular momentum of an electron?

a) Principal quantum number (n)

b) Azimuthal quantum number (l)

c) Magnetic quantum number (m_l)

d) Spin quantum number (m_s)

For an electron in the 4f orbital, what is the value of l?

a) 0

b) 1

c) 2

d) 3

How many orbitals are present in an s subshell?

a) 1

b) 2

c) 3

d) 4

The maximum number of electrons in a p subshell is:

a) 2

b) 6

c) 10

d) 14

In which quantum number is the magnetic moment of an electron found?

a) Principal quantum number (n)

b) Azimuthal quantum number (l)

c) Magnetic quantum number (m_l)

d) Spin quantum number (m_s)

Which quantum number defines the specific orbital within a subshell?

a) Principal quantum number (n)

b) Azimuthal quantum number (l)

c) Magnetic quantum number (m_l)

d) Spin quantum number (m_s)

If l = 1, what type of orbitals are present?

a) s orbitals

b) p orbitals

c) d orbitals

d) f orbitals

Which quantum number has a maximum value of n-1?

a) Principal quantum number (n)

b) Azimuthal quantum number (l)

c) Magnetic quantum number (m_l)

d) Spin quantum number (m_s)

How many different orientations can the 3d orbitals have?

a) 1

b) 3

c) 5

d) 7

Which quantum number has integer values from -n to +n?

a) Principal quantum number (n)

b) Azimuthal quantum number (l)

c) Magnetic quantum number (m_l)

d) Spin quantum number (m_s)

The value of l for an s orbital is:

a) 0

b) 1

c) 2

d) 3

For which quantum number does the maximum value correspond to (n-1)?

a) Principal quantum number (n)

b) Azimuthal quantum number (l)

c) Magnetic quantum number (m_l)

d) Spin quantum number (m_s)

In an f subshell, how many orbitals are present?

a) 1

b) 3

c) 5

d) 7

Which quantum number has values ranging from -1 to +1?

a) Principal quantum number (n)

b) Azimuthal quantum number (l)

c) Magnetic quantum number (m_l)

d) Spin quantum number (m_s)

For which quantum number does the value of m_s indicate the direction of spin?

a) Principal quantum number (n)

b) Azimuthal quantum number (l)

c) Magnetic quantum number (m_l)

d) Spin quantum number (m_s)

Which quantum number specifies the shell of an electron?

a) Principal quantum number (n)

b) Azimuthal quantum number (l)

c) Magnetic quantum number (m_l)

d) Spin quantum number (m_s)

What is the maximum number of electrons in a 4p subshell?

a) 2

b) 6

c) 10

d) 14

Which quantum number is associated with the concept of orbitals having different shapes?

a) Principal quantum number (n)

b) Azimuthal quantum number (l)

c) Magnetic quantum number (m_l)

d) Spin quantum number (m_s)

What is the range of values for the principal quantum number (n)?

a) -1 to +1

b) 0 to ∞

c) 1 to ∞

d) 0 to n-1

How many different possible values are there for the magnetic quantum number (m_l) when l = 3?

a) 3

b) 4

c) 5

d) 7

In which quantum number is the concept of electron spin included?

a) Principal quantum number (n)

b) Azimuthal quantum number (l)

c) Magnetic quantum number (m_l)

d) Spin quantum number (m_s)

What is the maximum number of orbitals in a d subshell?

a) 1

b) 3

c) 5

d) 7

For which quantum number is the value of l always less than n?

a) Principal quantum number (n)

b) Azimuthal quantum number (l)

c) Magnetic quantum number (m_l)

d) Spin quantum number (m_s)

If n = 2, what are the possible values of l?

a) 0

b) 0 and 1

c) 1 and 2

d) 0, 1, and 2

Which quantum number defines the orientation of an electron’s spin?

a) Principal quantum number (n)

b) Azimuthal quantum number (l)

c) Magnetic quantum number (m_l)

d) Spin quantum number (m_s)

The number of different orbitals in an f subshell is:

a) 3

b) 4

c) 5

d) 7

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