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Ch.6 - Electronic Structure of Atoms
Brown - Chemistry: The Central Science 15th Edition
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Tutti i libri di testoBrown 15th EditionCh.6 - Electronic Structure of AtomsProblema 59a
Capitolo 6, Problema 59a

A certain orbital of the hydrogen atom has n = 4 and l = 2. a. What are the possible values of ml for this orbital?

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Identify the given quantum numbers: n = 4 and l = 2.
Understand that the magnetic quantum number, m_l, depends on the azimuthal quantum number, l.
Recall that the possible values of m_l range from -l to +l, including zero.
For l = 2, list the possible values of m_l: -2, -1, 0, 1, 2.
Conclude that the possible values of m_l for this orbital are -2, -1, 0, 1, and 2.

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Quantum Numbers

Quantum numbers are a set of numerical values that describe the unique quantum state of an electron in an atom. The four quantum numbers are principal (n), azimuthal (l), magnetic (ml), and spin (ms). Each number provides specific information about the electron's energy level, shape, orientation, and spin, which are essential for understanding electron configurations.
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Principal Quantum Number

Principal Quantum Number (n)

The principal quantum number (n) indicates the main energy level or shell of an electron in an atom. It can take positive integer values (1, 2, 3, ...), with higher values corresponding to electrons that are further from the nucleus and have higher energy. In this case, n = 4 signifies that the electron is in the fourth energy level.
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Principal Quantum Number

Magnetic Quantum Number (ml)

The magnetic quantum number (ml) describes the orientation of an orbital in space and can take on integer values ranging from -l to +l, where l is the azimuthal quantum number. For l = 2, which corresponds to a d-orbital, ml can have values of -2, -1, 0, +1, and +2, indicating the different orientations of the d-orbitals.
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Magnetic Quantum Number
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