9.1 VSEPR Theory and Molecular Shapes | General Chemistry
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- Опубліковано 28 лип 2024
- Chad provides a comprehensive lesson on VSEPR Theory and Molecular Geometry. The five fundamental Electron Domain Geometries (EDGs) including the bond angles are first covered: Linear, Trigonal Planar, Tetrahedral, Trigonal Bipyramidal, and Octahedral. Then the corresponding Molecular Geometries are covered being grouped by the number of electron domains with examples of each being presented. This includes the following:
2 Electron Domains: Linear
3 Electron Domains: Trigonal Planar & Bent
4 Electron Domains: Tetrahedral, Trigonal Pyramidal, & Bent
5 Electron Domains: Trigonal Bipyramidal, See-saw (aka Sawhorse), T-shaped, & Linear
6 Electron Domains: Octahedral, Square Pyramidal, & Square Planar
The effect of lone pairs and pi bonds reducing bond angles is also covered.
I've embedded this playlist as a course on my website with all the lessons organized by chapter in a collapsible menu and much of the content from the study guide included on the page. Check this lesson out at www.chadsprep.com/chads-gener...
If you want all my study guides, quizzes, final exam reviews, and practice exams, check out my General Chemistry Master Course (free trial available) at www.chadsprep.com/genchem-you...
00:00 Lesson Introduction
00:44 VSEPR Theory, Electron Domain Geometry, and Molecular Geometry
12:09 Linear Molecular Geometry
13:55 3 Trigonal Planar Molecular Geometry (& Bent)
18:51 Tetrahedral Molecular Geometry (& Trigonal Pyramidal & Bent)
24:24 Trigonal Bipyramidal Molecular Geometry (& See-saw, T-shaped, & Linear)
29:54 Octahedral Molecular Geometry (& Square Pyramidal & Square Planar)
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Great explanatory video - best video series on YT by far! Still though, I don't know why the Trigonal Bipyramidal structure with 2 LP can't be 180 degrees apart like it would be for octahedral with 2 LPs (Square pyramidal)? Is it possible that it would not be stable since all bonds are not 90 degrees? Still scratching my head a bit...
Is this for ICl3? Assuming you mean why don't the lone pairs go axial 180 degrees apart? I know it 'looks' as if the axial positions are less crowded but it is acually the opposite if we look at bond angles - you can see this on the thumbnail actually. Lone pairs experience greater repulsion from bonding atoms as well as each other. Axial positions are 90 degrees apart from equatorial positions. So a lone pair in axial position will have 3x90 degree interactions with the equatorial bonding atoms. If we put the lone pair in equatorial position it has only 2x90 degree interactions and everything else is 120 degrees. As far as the electrons are concerned, they are less crowded in equatorial positions. Hope that helps!
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Can u make a video on Torque? please
Hello! I have a physics playlist as well which includes an entire chapter on Torque. You can watch the first torque lesson on youtube here: ua-cam.com/video/7Okt5ELRJEk/v-deo.html
Or as part of a navigable embedded playlist on my website here: www.chadsprep.com/chads-general-physics-videos/torque-physics/
Hope this helps!
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Seriously, This video worth more than 600 Likes and 19K views. I just learnt everything in 30 mins that my teacher explained in 2 weeks lecture and I still confused after all the lectures.
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Please slow down when talking
I get that a lot - you can adjust the playback speed to your liking under the settings. Hope that helps!
@@ChadsPrepThat’s what I do; .75x works really well without distorting your content. Thanks for all your help!😊
@@Zen-ig7do Excellent - Happy Studying!