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What are the possible values of ml for each value of l? c. 2 d. 3
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Ch.8 - The Quantum-Mechanical Model of the Atom
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
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Capitolo 8, Problema 62a
What are the possible values of ml for each value of l? a. 0
Guida verificata passo dopo passo1
Identify the quantum number 'l' given in the problem. In this case, 'l' is 0.
Recall that the magnetic quantum number 'ml' can take on integer values from -l to +l, including zero.
Since 'l' is 0, calculate the range of 'ml' by substituting 0 into the range -l to +l.
Determine that the only value 'ml' can take when 'l' is 0 is 0.
Conclude that the possible value of 'ml' for 'l' = 0 is 0.
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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. They include the principal quantum number (n), azimuthal quantum number (l), magnetic quantum number (ml), and spin quantum number (ms). Each quantum number provides specific information about the electron's energy level, shape, orientation, and spin.
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02:55
Principal Quantum Number
Azimuthal Quantum Number (l)
The azimuthal quantum number (l) determines the shape of an electron's orbital and can take on integer values from 0 to n-1, where n is the principal quantum number. For example, if n=2, l can be 0 or 1, corresponding to s and p orbitals, respectively. The value of l is crucial for understanding the types of orbitals and their geometrical arrangements.
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03:06Magnetic Quantum Number
Magnetic Quantum Number (ml)
The magnetic quantum number (ml) specifies the orientation of an orbital in space and can take on integer values ranging from -l to +l, including zero. For each value of l, there are 2l + 1 possible values of ml. For instance, if l=1 (p orbital), ml can be -1, 0, or +1, indicating the three different orientations of p orbitals.
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