We’re being asked to determine the correct set of quantum numbers for the given atomic orbital shape. Let’s first define the quantum numbers.

• the **principal quantum number (n) → **energy level in orbitals and its value could be **any positive integer** starting from 1

• **angular momentum quantum number (ℓ)**** ****→ ****(l) has to be at least 1 less than n, **range of values from** 0 up to (n-1)**

▪ Each **ℓ value **corresponds to a **subshell/sublevel**:

Based on the following atomic orbital shape, which of the following set of quantum numbers is correct:

a) n = 2, ℓ = 1, m _{ℓ} = 0

b) n = 3, ℓ = 2, m _{ℓ} = –1

c) n = 4, ℓ = 0, m _{ℓ} = +1

d) n = 1, ℓ = 1, m _{ℓ} = 0