Ch.8 - Periodic Properties of the ElementsWorksheetSee all chapters
All Chapters
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: Based on the following atomic orbital shape, which of the following set of quantum numbers is correct:a) n = 2,  ℓ = 1, m ℓ  = 0b) n = 3, ℓ = 2, m ℓ  =  –1c) n = 4, ℓ = 0, m ℓ  = +1d) n = 1, ℓ = 1, m 

Solution: Based on the following atomic orbital shape, which of the following set of quantum numbers is correct:a) n = 2,  ℓ = 1, m ℓ  = 0b) n = 3, ℓ = 2, m ℓ  =  –1c) n = 4, ℓ = 0, m ℓ  = +1d) n = 1, ℓ = 1, m 

Problem

Based on the following atomic orbital shape, which of the following set of quantum numbers is correct:

a) n = 2,  ℓ = 1, m   = 0

b) n = 3, ℓ = 2, m   =  –1

c) n = 4, ℓ = 0, m   = +1

d) n = 1, ℓ = 1, m  = 0

Solution

We’re being asked to determine the correct set of quantum numbers for the given atomic orbital shape. Let’s first define the quantum numbers.

• the 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)

▪ Each ℓ value corresponds to a subshell/sublevel:

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