We’re being asked to which of the following represents an impossible combination of the quantum numbers n and l

Let’s first **define and determine the possible values of the first 2 quantum numbers**:

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

• **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**:

**ℓ**** = 0** → s subshell**ℓ**** = 1** → p subshell **ℓ**** = 2** → d subshell**ℓ**** = 3** → f subshell

Which of the following represents an impossible combination of the quantum numbers n and l?

A) 1s

B) 2d

C) 3p

D) 4d

E) 5f

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