Textbook Question
What are the possible values of ml for each value of l? a. 0
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Ch.8 - The Quantum-Mechanical Model of the Atom
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving90
- Ch.2 - Atoms & Elements94
- Ch.3 - Molecules and Compounds103
- Ch.4 - Chemical Reactions and Chemical Quantities46
- Ch.5 - Introduction to Solutions and Aqueous Solutions65
- Ch.6 - Gases100
- Ch.7 - Thermochemistry85
- Ch.8 - The Quantum-Mechanical Model of the Atom51
- Ch.9 - Periodic Properties of the Elements79
- Ch.10 - Chemical Bonding I: The Lewis Model70
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory68
- Ch.12 - Liquids, Solids & Intermolecular Forces44
- Ch.13 - Solids & Modern Materials42
- Ch.14 - Solutions77
- Ch.15 - Chemical Kinetics88
- Ch.16 - Chemical Equilibrium57
- Ch.17 - Acids and Bases121
- Ch.18 - Aqueous Ionic Equilibrium126
- Ch.19 - Free Energy & Thermodynamics80
- Ch.20 - Electrochemistry87
- Ch.21 - Radioactivity & Nuclear Chemistry61
- Ch.22 - Organic Chemistry114
Chapter 8, Problem 61
What are the possible values of l for each given value of n? a. 1 b. 2 c. 3 d. 4
Verified step by step guidance1
Identify the principal quantum number (n) for each part of the question. The principal quantum number, n, determines the size and energy level of the orbital.
Recall that the azimuthal quantum number (l) can take on any integer value from 0 to n-1. This quantum number determines the shape of the orbital.
For n=1, calculate the possible values of l by substituting n into the formula l = 0 to n-1. Since n-1 equals 0, l can only be 0.
For n=2, calculate the possible values of l. Substitute n into the formula l = 0 to n-1. Since n-1 equals 1, l can be 0 or 1.
For n=3 and n=4, repeat the same process as above. For n=3, l can be 0, 1, or 2. For n=4, l can be 0, 1, 2, or 3.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Principal Quantum Number (n)
The principal quantum number, denoted as 'n', indicates the energy level of an electron in an atom and can take positive integer values (1, 2, 3, ...). It determines the size and energy of the orbital, with higher values corresponding to higher energy levels and larger orbitals.
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Principal Quantum Number
Azimuthal Quantum Number (l)
The azimuthal quantum number, represented as 'l', defines the shape of the electron's orbital and can take integer values from 0 to (n-1) for each principal quantum number 'n'. For example, if n=2, l can be 0 or 1, corresponding to s and p orbitals, respectively.
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Orbital Types
Different values of the azimuthal quantum number 'l' correspond to different types of orbitals: 'l=0' (s), 'l=1' (p), 'l=2' (d), and 'l=3' (f). Understanding these orbital types is essential for predicting the electron configuration and chemical properties of elements.
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