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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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Quantum Numbers: Angular Momentum Quantum Number concept. You can view video lessons to learn Quantum Numbers: Angular Momentum Quantum Number. Or if you need more Quantum Numbers: Angular Momentum Quantum Number practice, you can also practice Quantum Numbers: Angular Momentum Quantum Number practice problems.

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Based on our data, we think this problem is relevant for Professor De La Cruz's class at VALENCIA.