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
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: What is the maximum number of electrons that can occupy individual 2s and 2p orbitals?a. 2 and 2, respectivelyb. 2 and 6, respectivelyc. 2 and 2, respectivelyd. 1 and 2, respectivelye. 1 and 3, respectively

Problem

What is the maximum number of electrons that can occupy individual 2s and 2p orbitals?

a. 2 and 2, respectively

b. 2 and 6, respectively

c. 2 and 2, respectively

d. 1 and 2, respectively

e. 1 and 3, respectively

Solution

Establish the quantum numbers and determine the maximum number of electrons that can occupy 2s and 2p orbitals 

The first three quantum numbers are:

  • principal quantum number (n) →energy level in orbitals and its value could be any positive integer starting from 1 to infinity.
  • angular momentum quantum number (ℓ)→ (l) has to be at least 1 less than n, range of values from 0 up to (n-1)

Each ℓ value corresponds to a subshell:

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