Structure of Diamond and Graphite, Properties - Basic Introduction

This chemistry video tutorial provides a basic introduction into the structure of diamond and graphite. Diamond has a tetrahedral geometry around each carbon atom with an sp3 hybridization. Graphite has a trigonal planar geometry around each carbon atom with an sp2 hybridization. Graphite conducts electricity due to the electron delocalization of its pi electrons where as diamond as an electrical insulator due to its localized valence electrons; however, diamond is excellent conductor of heat. Diamond is colorless and graphite is black. Diamond is hard due to its strong network covalent bonds where as graphite is slippery due to the weak interactions between the 2D layers within the structure of graphite.

Sigma and Pi Bonding:

Hybridization of Atomic Orbitals:

Molecular Orbital Theory:

Dipole Dipole Forces of Attraction:

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Hydrogen Bonding:

London Dispersion Forces:

Ion Dipole Forces:

Bragg's Equation For X-Ray Diffraction:

Molecular & Network Covalent Solids:

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Metallic Bonding:

Metal Alloys:

Diamond Vs Graphite:

Semiconductors:

Unit Cell Chemistry:

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Final Exams and Video Playlists:

Full-Length Videos and Worksheets:

Chemistry PDF Worksheets:

[SaebaRyo]

Thank you, I am right now studying the allotropes of C, and wanna write descriptive infos about both diamond & graphite. This is very useful

[papanoel]

You are my savior my guy. I been struggling on this final paper for carbon

[georgesadler]

Professor Organic Chemistry Tutor, thank you for explaining the difference between Graphite and Diamond in AP/General Chemistry. In diamond, each carbon atom is at the center of a tetrahedron, on each corner of which is another carbon atom. In graphite, the carbon atoms are linked together in planes of hexagons. Within a layer, a carbon atom is bonded to three other carbon atoms; one third of the bonds are double bonds. The layers are held to one another by weak dispersion forces.This is an error free video/lecture on YouTube TV with the Organic Chemistry Tutor.

[ThokozaniYohane-ln]

If our lectures teaches the same as you do, nothing will never become difficult!, keep it up

[demonkgeneration]

Really helpfull for the theory of my project and viva

[matthewwang-qr]

Bro I am doing a chemistry project about Diamond and graphite, yhis video helps me a lot

[geetugupta]

5:20, are those interactions known as Vanderwals forces by any chance?...I remember I've heard that term before.

[myatmyat]

Thanks a lot for excellent presentation.

[gstudios]

why is graphite used in making handles for tennis racquets

[shaneyawlover]

Wait why particularly the pi bonds are hard to break? Aren't sigma bonds stronger? (but double and triple bonds are stronger than single since they have both pi and sigma)

[demonetization]

Thank you so much I was struggling when I saw my homework and saw the structure of graphite. The question says graphite has a free electron but I didn’t see it as I thought all of them were connected in the structure. It turns out to be in the dot and cross diagram when the carbon are bonded, forming its 2 1 1 bonding

[SantiagoRuhozu]

I want to explain to the students that what is structure of diamond

[WhiteChomos]

It would be easier just to say 825k lbs per square in…instead of n

[shubhamborganve]

Sir please make kannada video I am not perfect in English

[muntee]

Well i guess ‘graphite’ does not naturally exist then.