Ch.8 - Periodic Properties of the ElementsWorksheetSee 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

How many different orbitals can have the principal quantum number n = 3?

(a) 9 

(b) 4 

(c) 6 

(d) 5 

(e) 18


We’re being asked which of the following combinations could give the quantum numbers for the single valence electron of the copper in its ground state.

Recall that the 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:

 = 0 → s subshell
 = 1 → p subshell 
 = 2 → d subshell
 = 3 → f subshell

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

▪ The m values (for each ℓ) represent an orbital for the subshell:

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