We’re being asked to **determine the incorrect statement among the choices**

Recall that the ** quantum numbers** that define an electron are:

• *Principal Quantum Number* **(n)**: deals with the size and energy of the atomic orbital.

The possible values for n are **1 to ∞**.

• *Angular Momentum Quantum Number ***(l)**: deals with the shape of the atomic orbital.

The possible values for l are **0 to (n – 1)**.

• *Magnetic Quantum Number ***(m _{l})**: deals with the orientation of the atomic orbital in 3D space.

The possible values for m_{l} is the range of l: **–l to +l**.

Which statement about quantum numbers is __incorrect?__ Answer (e) if they are all correct or all incorrect.

a. The principal quantum number cannot equal zero.

b. When n = 3, the angular quantum number can be equal to 0, 1, or 2.

c. For an angular quantum number equal to 1, the magnetic quantum number can be +1, 0, o-1.

d. For any value of the angular quantum number (**l**), there are 2(2**l**+1) values of the magnetic quantum number.

e. All the above statements are correct or all are incorrect.

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