🤓 Based on our data, we think this question is relevant for Professor Randles' class at UCF.

What is the maximum number of electrons in an atom that can have the following quantum numbers?

A) n=2 m_{s }= -1/2

B) n=5, l= 3

C) n=4, l=3, m_{l}= -3

D) n=4, l=1, m_{l}=1

We are being asked to determine the **maximum number of electrons** in an atom for each set of quantum numbers given. To solve this problem, let’s first **define and determine the possible values of the four 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**:

Quantum Numbers

Quantum Numbers