Textbook Question
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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Ch.6 - Electronic Structure of Atoms
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 6, Problem 58a
Give the values for n, l, and ππ for a. each orbital in the 2p subshell
Verified step by step guidance1
n is the principal quantum number, which indicates the energy level of the electron. For the 2p subshell, n = 2.
The azimuthal quantum number, l, defines the shape of the orbital. For p orbitals, l = 1.
The magnetic quantum number, ml, describes the orientation of the orbital in space. It can take values from -l to +l, including zero.
For the 2p subshell, where l = 1, the possible values for ml are -1, 0, and +1.
Thus, the 2p subshell has three orbitals, each with the following quantum numbers: (2, 1, -1), (2, 1, 0), and (2, 1, +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. They include the principal quantum number (n), azimuthal quantum number (l), and magnetic quantum number (ml), which together provide information about the energy level, shape, and orientation of an orbital.
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02:55
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 higher energy levels and greater distances from the nucleus. For the 2p subshell, n is 2.
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02:55Principal Quantum Number
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 equal to 1, indicating a specific shape (dumbbell) and the presence of three different orientations in space. Thus, for the 2p subshell, l is 1.
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03:06Magnetic Quantum Number
Related Practice
Textbook Question
How many unique combinations of the quantum numbers l and ππ are there when b. n = 4?
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Textbook Question
(a) For n = 4, what are the possible values of l?
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Textbook Question
Which of the following represent impossible combinations of n and l? (a) 1p (b) 4s (c) 5f (d) 2d
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Textbook Question
For the table that follows, write which orbital goes with the quantum numbers. Don't worry about x, y, z subscripts. If the quantum numbers are not allowed, write 'not allowed.' n l ml Orbital 2 1 -1 2p (example) 1 0 0 3 -3 2 3 2 -2 2 0 -1 0 0 0 4 2 1 5 3 0
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Textbook Question
Calculate the uncertainty in the position of (a) an electron moving at a speed of 13.00 Β± 0.012 Γ 105 m/s (b) a neutron moving at this same speed. (The masses of an electron and a neutron are given in the table of fundamental constants in the inside cover of the text.)
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