Ch.5 - Periodicity & Electronic Structure of Atoms

McMurry8th EditionChemistryISBN: 9781292336145Non è quello che usi tu?Cambia libro di testo

McMurry 8th Edition

Ch.5 - Periodicity & Electronic Structure of Atoms

Problema 111b

Capitolo 5, Problema 111b

Given the subshells 1s, 2s, 2p, 3s, 3p and 3d, identify those that meet the following descriptions. (b) Can have m_l = -1

Guida verificata passo dopo passo

Step 1: Understand that the magnetic quantum number (ml) describes the specific orbital within a subshell where an electron is likely to be found. It can have values ranging from -l to +l, where l is the azimuthal quantum number (also known as the orbital quantum number or angular momentum quantum number).

Step 2: Recall that the azimuthal quantum number (l) for a subshell is determined by the type of the subshell: s subshells have l=0, p subshells have l=1, d subshells have l=2, and so on.

Step 3: Since ml can range from -l to +l, a subshell can have ml = -1 if its azimuthal quantum number l is 1 or greater.

Step 4: From the given subshells, identify those with l=1 or greater. These are the 2p, 3p, and 3d subshells.

Step 5: Therefore, the subshells that can have ml = -1 are the 2p, 3p, and 3d subshells.

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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 include the principal quantum number (n), azimuthal quantum number (l), magnetic quantum number (ml), and spin quantum number (ms). Each number provides specific information about the electron's energy level, shape, orientation, and spin.

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02:55

Principal Quantum Number

Magnetic Quantum Number (ml)

The magnetic quantum number (ml) determines 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 example, if l = 1 (p subshell), ml can be -1, 0, or +1. This concept is crucial for understanding how orbitals are arranged in a magnetic field and how they interact with other orbitals.

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03:06

Magnetic Quantum Number

Subshells and Their Designations

Subshells are divisions of electron shells that contain orbitals of the same type. They are designated by the letters s, p, d, and f, corresponding to different values of l (0, 1, 2, and 3, respectively). In this context, the 2p subshell has l = 1, allowing for ml values of -1, 0, and +1, while the 3p subshell also allows ml = -1, making them relevant to the question.

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01:02

Angular Momentum Quantum Number and Subshell

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