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Ch.5 - Periodicity & Electronic Structure of Atoms
All textbooksMcMurry 8th EditionCh.5 - Periodicity & Electronic Structure of AtomsProblem 111b
Chapter 5, Problem 111b

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

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1
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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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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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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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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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Related Practice
Textbook Question

Write the symbol, give the ground-state electron configuration, and draw an orbital-filling diagram for each of the following atoms. Use the abbreviation of the preceding noble gas to represent the inner-shell electrons. 

(c) The heaviest actinide metal

Textbook Question

Given the subshells 1s, 2s, 2p, 3s, 3p and 3d, identify those that meet the following descriptions. (a) Has l = 2

Textbook Question

Given the subshells 1s, 2s, 2p, 3s, 3p and 3d, identify those that meet the following descriptions. (e) Contains the outermost electrons in a beryllium atom

Textbook Question

Given the subshells 1s, 2s, 2p, 3s, 3p and 3d, identify those that meet the following descriptions. (f) Can contain two electrons, both with spin ms = +1/2

Textbook Question
At what atomic number is the filling of a g orbital likely to begin?