In this problem, we are being asked to determine the **maximum number of electrons in an atom that has a quantum number of n = 4, ℓ = l, and ml = 0**.

**Next, let’s define and determine the possible values of the quantum numbers:**

• the **principal quantum number**** ****→**** **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

• **magnetic quantum number (m _{ℓ})**

▪ The **m _{ℓ} values **(for each ℓ) represent

**s subshell**→ 1 orbital**p subshell**→ 3 orbitals**d subshell** → 5 orbitals**f subshell** → 7 orbitals

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

n = 4, l = 1, ml = 0

Frequently Asked Questions

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 concept. If you need more Quantum Numbers practice, you can also practice Quantum Numbers practice problems.