Ch.5 - Periodicity & Electronic Structure of Atoms

McMurry8th EditionChemistryISBN: 9781292336145Not the one you use?Change textbook

McMurry 8th Edition

Ch.5 - Periodicity & Electronic Structure of Atoms

Problem 10

Chapter 5, Problem 10

What are the possible values of n, l, and ml for an electron in a 5p orbital? (LO 5.12)

Name: Chemistry
Author: McMurry
ISBN: 9781292336145

Verified step by step guidance

insert step 1> Identify the principal quantum number (n) for a 5p orbital. The number before the letter (p) indicates the principal quantum number, so n = 5.

insert step 2> Determine the azimuthal quantum number (l) for a p orbital. The azimuthal quantum number (l) is associated with the shape of the orbital: s = 0, p = 1, d = 2, f = 3. For a p orbital, l = 1.

insert step 3> Identify the possible values of the magnetic quantum number (m_l). The magnetic quantum number (m_l) can range from -l to +l, including zero. For l = 1, m_l can be -1, 0, or +1.

insert step 4> Summarize the possible values of n, l, and m_l for an electron in a 5p orbital.

insert step 5> Conclude that for an electron in a 5p orbital, n = 5, l = 1, and m_l can be -1, 0, or +1.

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. There are four quantum numbers: the principal quantum number (n), the azimuthal quantum number (l), the magnetic quantum number (ml), and the spin quantum number (ms). Each of these numbers provides specific information about the electron's energy level, shape, orientation, and spin.

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. For a 5p orbital, n is equal to 5.

Azimuthal Quantum Number (l)

The azimuthal quantum number (l) defines the shape of the orbital and can take integer values from 0 to (n-1). For p orbitals, l is always equal to 1. Therefore, for a 5p orbital, l is 1, indicating that the electron is in a p-type orbital, which has a characteristic dumbbell shape.

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Magnetic Quantum Number

Related Practice

Textbook Question

Identify each of the following orbitals, and give n and l quantum numbers for each.(a)

Calculate the wavelength in nm of the light emitted when an electron makes a transition from an orbital in n = 5 to an orbital in n = 2 in the hydrogen atom. (LO 5.8)(a) 2.31 * 10-3 nm (b) 4.34 * 10-2 nm (c) 231 nm(d) 434 nm

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Textbook Question

What are the possible values of n, l, and ml for the orbital shown? (LO 5.13)

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Textbook Question

Two electromagnetic waves are represented below. (

(a) Which wave has the greater intensity?

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Textbook Question

Which arrow in the energy diagram for an atom represents the absorption of light with the shortest wavelength? (LO 5.7)

When a copper salt such as Cu(NO3)2 is burned in a flame, a blue-green color is emitted. Which figure represents the emission spectrum for the element copper? (LO 5.6)? (a)

(b)

(c)

(d)

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