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
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Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: The ground-state electron configuration of a Mn2+ ion is 1s22s22p63s23p63d5. Therefore, Mn2+ isa. paramagnetic with two unpaired electrons.b. paramagnetic with one unpaired electron.c. paramagnetic wi

Problem

The ground-state electron configuration of a Mn2+ ion is 1s22s22p63s23p63d5. Therefore, Mn2+ is

a. paramagnetic with two unpaired electrons.

b. paramagnetic with one unpaired electron.

c. paramagnetic with five unpaired electrons.

d. diamagnetic.

e. paramagnetic with three unpaired electrons.

Solution

We have to determine if Mn2+ ion is paramagnetic or diamagnetic and how many unpaired electrons it has.

Manganese is a transition metal that belongs to group 7B.

The given electronic configuration of Mn2+ ion is:


1s2 2s2 2p6 3s2 3p6 3d5


An orbital which is completely filled cannot contain any unpaired electrons as all of the electrons in a full orbital have to be paired.


This means there will no unpaired electrons in orbitals from 1s to 3p since they are all filled and all of the electrons contained within will be paired.


An orbital, which is partially-filled, can have unpaired electrons.


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