Ch.7 - Quantum MechanicsWorksheetSee 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: How many orbitals are contained in the third principal level (n=3) of a given atom?A) 7B) 5C) 9D) 3E) 18

Solution: How many orbitals are contained in the third principal level (n=3) of a given atom?A) 7B) 5C) 9D) 3E) 18

Problem

How many orbitals are contained in the third principal level (n=3) of a given atom?

A) 7

B) 5

C) 9

D) 3

E) 18

Solution

We’re being asked to determine the number of orbitals contained in the third principal level (n = 3).


Recall that the quantum numbers that define an electron are:


• Principal Quantum Number (n): deals with the size and energy of the atomic orbital

The possible values for n are 1 to ∞.

• Angular Momentum Quantum Number (l): deals with the shape of the atomic orbital

The possible values for l are 0 to (n – 1).

• Magnetic Quantum Number (ml): deals with the orientation of the atomic orbital in 3D space. 

The possible values for ml are the range of l:  –l to +l.


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