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: Write out the four possible quantum numbers for each of the electrons in the diagram below. Give them in the order of: n, l, ml, and ms.HINT: There are 6 electrons therefore you should give 6 answers.

Solution: Write out the four possible quantum numbers for each of the electrons in the diagram below. Give them in the order of: n, l, ml, and ms.HINT: There are 6 electrons therefore you should give 6 answers.

Problem

Write out the four possible quantum numbers for each of the electrons in the diagram below. Give them in the order of: n, l, ml, and ms.

HINT: There are 6 electrons therefore you should give 6 answers.

Solution

We’re being asked to write the four possible quantum numbers for each of the electrons in the given diagram below:


Let’s first define and determine the possible values of the four quantum numbers:

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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