Paramagnetic vs Diamagnetic - Paired vs Unpaired Electrons - Electron Configuration

This chemistry video tutorial focuses on paramagnetism and diamagnetism. It shows you how to identify if an element is paramagnetic or diamagnetic by writing the ground state electron configuration using noble gas notation and determining if the element has unpaired electrons by drawing the orbital diagram. Elements with unpaired electrons are paramagnetic which are weakly attracted to an external magnetic field. Elements with paired electrons only are diamagnetic and are weakly repelled by an external magnetic field.
Speed of Light, Frequency, Wavelength:
• Speed of Light, Freque...
Photon Energy:
• How To Calculate The E...
The Photoelectric Effect:
• Photoelectric Effect, ...
De Broglie Wavelength:
• De Broglie Wavelength ...
The Bohr Model of Hydrogen:
• Bohr Model of the Hydr...
Heisenberg's Uncertainty Principle:
• Heisenberg's Uncertain...
________________________________
Intro to Quantum Numbers:
• Quantum Numbers
Orbitals & Atomic Energy Levels:
• Orbitals, Atomic Energ...
Maximum Number of Electrons:
• How To Determine The M...
Intro to Electron Configuration:
• Electron Configuration...
Electron Configuration Exceptions:
• Electron Configuration...
Noble Gas Notation:
• Electron Configuration...
Electron Configuration of Ions:
• Electron Configuration...
_______________________________
Orbital Diagrams:
• Orbital Diagrams and E...
Paired & Unpaired Electrons:
• How To Determine The N...
Aufbau's Principle & Hund's Rule:
• Aufbau's Principle, Hu...
Paramagnetic & Diamagnetic Elements:
• Paramagnetic & Diamagn...
Valence Electrons & Periodic Table:
• Valence Electrons and ...
Effective Nuclear Charge:
• How To Calculate The E...
_________________________________
Slater's Rule:
• How To Use Slater's Ru...
How To Identify The Element:
• Electron Configuration...
Quantum Numbers - Mega Review:
• Quantum Numbers - n, l...
Quantum Numbers - Practice Test:
• Orbitals, Quantum Numb...
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[@TheOrganicChemistryTutor]

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[@EdW4rdO1]

So do you always have to the electron configuration to figure out whether it’s diamagnetic or paramagnetic? Or is there a shortcut?

[@furiko9989]

Can you also use this method to prove dia/paramagnetism for molecules like magnetite? Asking for a school project 😅

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[@mrPottz]

I have a question why are some elements still considered diamagnetic even though they leave an unpaired electron. For example, copper. When filling up the 3d shell, in Cu, you're left with 1 unpaired, So shouldn't that be considered paramagnetic?

[@hil1249]

how do you solve them when they are ions? do you just subtract the superscript number if its a cation and add if its an anion? and do it the same way after you've done that?

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[@mykulpierce]

Does the strength of a diamagnetic substance have any correlation to the number of paired electrons? Bismuth for example is one of the most dynamic substances and further along in periodic table. Does this rule holds true for molecules of various substances? For example hemoglobin is diamagnetic despite it containing iron.

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[@tuannguyen6932]

I believe that this rule do not apply to Fe, Ni and Co because they are ferromagnetic. Am I right?

[@binodpandey4407]

I have heard that nickel is ferro magnetic substances am I wrong?

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[@SalmanZafar-no9ov]

Manganese has more unpaired electrons than Iron so why is Iron ferromagnetic Manganese paramagnetic?
Please sir tell me please

[@reardelt]

Also, well magnesium is paramagnetic, not diamagnetic. Number of unpaired electrons isn't the only factor determining the magnetic properties of a metal

[@sirilandsariah]

Why is it not 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 3d^7 for the Mn25?

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but isnt nickel ferromagnetic?

[@EsotericGold_net]

I thought it was ferromagnetic to

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[@Mnzmanzmz]

Sulfur is lower or higher affinity than Na, and mg??

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Could you explain for water as diamagnetic

[@lookstheory2.0]

Some source say Nickel is Ferromagnetic?

[@katiegehrmann5840]

Why isn't Carbon paramagnetic if it has two unpaired electrons in 2p?

[@reardelt]

Why isn't Nitrogen paramagnetic? Doesn't it have 3 unpaired electrons in its 2p shell?

[@mdbakibillah6491]

Can please explain why palladium is diamagnetic?

[@rosslindtirado8916]

what if the question is 8 Oxygen and at the upper right side of it is 2-

[@inayatali1021]

Can you solve me plz what's O2 para or dimagnetic?

[@miinas3617]

Cu should be diamagnetic but it has unpaired elecron (3d9)

[@_PsyChoPaThiCX.___.]

5:07 it should be ferromagnetic?

[@shesunaga9788]

which chemicals are used in Diamagnetism ?

[@atila8623]

What about ferromagnetic materials

[@mohammudvai8004]

Isn't Ni ferromagnetic?

[@abhishekmaurya6862]

magnesium is paramagnetic element, not diamagnetic

[@corrayatom]

can we prove Fe is ferromagnetic this way?

[@bofengwu7108]

how about ferromagnetic

[@giselleformon]

Is carbon paramagnetic? It has unpaired electrons

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[@dr.bharatipatil3074]

But Nickel is ferromagnetic

[@alessiamaterazzetti5975]

What about Bi?! If I am not wrong according to the electronic configuration I have 3 unpaired electrons and so it should be paramagnetic... However Bismuth is Diamagnetic... How come?! Are there any other exceptions?

[@anjaniyadav5432]

Paramegnative & dimagnetive difference

[@bushbob5074]

I am no expert... but I think he misused the terms...
Ferromagnetic means it like to be a magnet... like steal
Paramagnetic means it is mildly magnetic, hardly sticks... like glass.
Diamagnetic means it hates the magnetic field and will try get away from it... like graphite.

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@@bushbob5074 exactly

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Bro mg is paramagnetic it's exception

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Ni -- is never, what? magnetic! No power! AKA plastic CDs-- you still buy?

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8=4 is, Oriental linear -- grammar! How did he, calculate that, for any calculus rule? Did not! And 4s = 4f! Where magnesium -- isn't magnetic, it burns, itself out-- inverse! In many-- burn rates! Nes = racist!

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Show molecules 😡

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