What are the possible values of mℓmℓ for an electron in a *d* orbital?

Express your answer numerically with sequential values separated by commas.

For an electron in a \(d\) orbital, the possible values of the magnetic quantum number \(m_\ell\) range from \(-\ell\) to \(+\ell\), where \(\ell\) is the azimuthal quantum number. For a \(d\) orbital, \(\ell = 2\).

Thus, the possible values of \(m_\ell\) are:

\[
m_\ell = -2, -1, 0, +1, +2
\]

Expressed numerically, the possible values of \(m_\ell\) for an electron in a \(d\) orbital are:

\(-2, -1, 0, 1, 2\).

Would you like further details or explanations? Here are some related questions you might consider:

1. What do the quantum numbers \(n\), \(\ell\), and \(m_\ell\) represent?
2. How does the shape of the \(d\) orbital compare to other orbitals?
3. What is the significance of the quantum number \(\ell\)?
4. Can you explain the distribution of electrons in orbitals?
5. How does the electron configuration change as you move across a period in the periodic table?

**Tip:** Remember that each orbital can hold a maximum of two electrons with opposite spins.

What are the possible values of mℓ for an electron in a d orbital? Express your answer numerically with sequential values separated by commas.

Understand the possible values of the magnetic quantum number (mℓ) for an electron in a d orbital. This problem covers core quantum mechanics concepts, including quantum numbers and their ranges, suitable for students in Grades 11-12.

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