Ch.7 - Quantum MechanicsWorksheetSee all chapters
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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
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Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
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Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: List all the orbitals in each principal level. Specify the three quantum numbers for each orbital.n = 4

Solution: List all the orbitals in each principal level. Specify the three quantum numbers for each orbital.n = 4

Problem

List all the orbitals in each principal level. Specify the three quantum numbers for each orbital.

n = 4

Solution

We have to list all orbitals in the given level (n=4) and write the three quantum numbers for each orbital.

To determine the possible values of ℓ, m and ms, when n = 4 , let’s first define the possible values of the quantum numbers:


principal quantum number (n) → energy level in orbitals and its value could be any positive integer starting from 1.

angular momentum quantum number (ℓ) → (l) has to be at least 1 less than n, range of values from 0 up to (n-1).

magnetic quantum number (m) → range of values from -ℓ to + ℓ.

spin quantum number (ms) → has two values: +½ and -½.

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