Which of the following represent valid sets of quantum...

Which of the following represent valid sets of quantum numbers? For a set that is invalid, explain briefly why it is not correct.
(a) $n=3, \ell=3, m_{\ell}=0$
(c) $n=6, \ell=5, m_{\ell}=-1$
(b) $n=2, \ell=1, m_{\ell}=0$
(d) $n=4, \ell=3, m_{\ell}=-4$

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Principal Quantum Number (n)

This number indicates the main energy level or shell of an electron in an atom and is a positive integer. It plays a crucial role in determining the size of the electron’s orbital and indirectly influences the energy of the electron.

Orbital Angular Momentum Quantum Number (?)

This quantum number defines the shape of the electron's orbital and is restricted to integer values ranging from 0 up to n-1. It is directly related to the magnitude of the orbital angular momentum and determines the orbital's angular characteristics.

Magnetic Quantum Number (m?)

This number specifies the orientation of the orbital angular momentum in space, and it can take any integer value between -? and ?, inclusive. It defines how the electron orbital is oriented relative to an external magnetic field.

Quantum Number Constraints

These are the rules that determine the allowed combinations of quantum numbers. They ensure that ? is less than n and that m? is within the range of -? to ?. Violating any of these constraints results in an invalid set of quantum numbers.

Transcript

Please give Ace some feedback