Textbook Question
What is the maximum number of electrons that can occupy each of the following subshells? a. 3p, b. 5d, c. 2s, d. 4f.
Table of contents
- 1. Intro to General Chemistry3h 48m
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- 23. Chemistry of the Nonmetals2h 39m
- Main Group Elements: Bonding Types4m
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- 24. Transition Metals and Coordination Compounds3h 19m
- Atomic Radius & Density of Transition Metals11m
- Electron Configurations of Transition Metals7m
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- Paramagnetism and Diamagnetism10m
- Ligands10m
- Complex Ions5m
- Coordination Complexes7m
- Classification of Ligands11m
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- Isomerism in Coordination Complexes17m
- Orientations of D Orbitals4m
- Intro to Crystal Field Theory10m
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- Crystal Field Theory Summary8m
- Magnetic Properties of Complex Ions9m
- Strong-Field vs Weak-Field Ligands6m
- Magnetic Properties of Complex Ions: Octahedral Complexes11m
- 1. The Chemical World10m
9. Quantum Mechanics
Quantum Numbers: Number of Electrons
Multiple Choice
How many electrons can occupy the third energy level (n = 3) of an atom?
A
6
B
8
C
18
D
32
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Verified step by step guidance1
Recall that the maximum number of electrons that can occupy a given energy level (n) is given by the formula \$2n^2$.
Identify the principal quantum number for the third energy level: \(n = 3\).
Substitute \(n = 3\) into the formula: \(2 \times (3)^2\).
Calculate the value inside the parentheses first: \((3)^2 = 9\).
Multiply by 2 to find the maximum number of electrons: \(2 \times 9 = 18\).
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