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
Electron Configuration
Paramagnetic and Diamagnetic
Effective Nuclear Charge
The Spin Quantum Number
Orbital Shapes
Periodic Trends: Atomic Radius
Periodic Trends: Ionic Radius
Periodic Trends: Ionization Energy
Periodic Trends: Electron Affinity
Additional Practice
Orbital Diagrams
Coulomb's Law
Quantum Numbers
Periodic Trends
Periodic Trends: Metallic Character
Additional Guides
Atomic Radius
Ionization Energy

Paramagnetism refers to elements or ions that contain at least one unpaired electron, while diamagnetism refers to elements or ions with no unpaired electrons. 

Understanding Paramagnetism & Diamagnetism

Concept #1: Paramagnetism vs. Diamagnetism 


In this new video, we're going to take a look at paramagnetic and diamagnetic ions.
What do we mean by paramagnetism or diamagnetism? Well, paramagnetism means that our element, or sometimes our ion, has unpaired electrons. Remember, we talked about having electron orbitals. We'll say that this is an s and this is a p. If this is one up and one down, we'd say that those two electrons are paired up with each other. They're next to each other in the same orbital.
Let's say we had another electron over here. There's only one electron within that electron orbital by itself. We'd say that that electron, which is pointing up, is unpaired. As a result, whichever element or ion this is that element would have an unpaired electron and as long as you have one unpaired electron, you would be paramagnetic.
Elements or ions with unpaired electrons are actually – they can be influenced like magnets. That's where the name comes from, paramagnetism. If you're diamagnetic, diamagnetic means you have no unpaired electrons at all. Therefore you won't be influenced by any type of magnet. Just remember that paramagnetism means you have at least one unpaired electron. Diamagnetism means you have no unpaired electrons. 

An element or ion is diamagnetic when it has no unpaired electrons. 

An element or ion is paramagnetic when it has at least one unpaired electron. 

Example #1: Write the condensed electron configuration of each ion and state if the ion is   paramagnetic   or   diamagnetic.

a. Ni3+                       b. S2-

Practice: Write the condensed electron configuration and state if the ion is paramagnetic or diamagnetic.