Question

Which of the following quantum numbers determines the shape of an orbital?

• A. Principal quantum number (n)
• B. Azimuthal quantum number (l)
• C. Magnetic quantum number (m)
• D. Spin quantum number (s)

Hint:

Remember: - \( n \) = size, - \( l \) = shape, - \( m \) = orientation, - \( s \) = spin

Answer 1

The Correct Option is B

The azimuthal quantum number \( l \) defines the shape of the orbital: - \( l = 0 \) → s orbital (spherical) - \( l = 1 \) → p orbital (dumbbell) - \( l = 2 \) → d orbital (cloverleaf) - \( l = 3 \) → f orbital (complex) (a) Principal quantum number \( n \) determines energy level and size.
(c) Magnetic quantum number \( m \) determines orientation.
(d) Spin quantum number \( s \) represents the spin of electron (±½).