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: In the ground-state electron configuration of Fe 3+ , how many unpaired electrons are present?

Solution: In the ground-state electron configuration of Fe 3+ , how many unpaired electrons are present?

Problem

In the ground-state electron configuration of Fe 3+ , how many unpaired electrons are present?

Solution

We are being asked how many electrons are unpaired in the ground-state electron configuration of Fe3+ ion. To figure that out, let’s first write the electron configuration of a neutral (uncharged) Fe atom.

Ground-state means that Iron is in its lowest energy form (not in an excited state). 

Neutral element:       Atomic number = # protons = # of electrons


Neutral Iron (Fe):

Atomic number = 26
# of electrons = 26 e-

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