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9.3 Hybridization | General Chemistry

Chad provides a lesson on hybridization and hybrid orbitals. The lesson begins with an introduction to Valence Bond Theory which describes a bond as resulting from the overlap of atomic orbitals. It is then shown how it is not possible for carbon to be using its 's' and 'p' orbitals to form bonds with the hydrogen atoms in CH4 (methane) as it would not result in the proper bond angles (109.5 degrees). The combination of carbon's 's' and 'p' orbitals results in the creation of four sp3 hybrid orbitals that are oriented 109.5 degrees apart, and these are responsible for bond formation when overlapping with the 's' orbitals of the hydrogen atoms. The lesson is concluded by showing how to determine the hybridization of an atom based upon the number of electron domains around it: 2 electron domains = sp hybridization 3 electron domains = sp2 hybridization 4 electron domains = sp3 hybridization 5 electron domains = sp3d hybridization 6 electron domains = sp3d2 hybridization The last two, sp3d and sp3d2 hybridization only occur with expanded octets which are only possible for elements in the 3rd row of the periodic table or below which will have d orbitals in their valence shell. 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 https://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 at https://www.chadsprep.com/genchem-you... 00:00 Lesson Introduction 00:53 Hybrid Orbitals Explained - Valence Bond Theory 04:16 sp3 Hybridization in CH4 10:36 sp vs sp2 vs sp3 Hybridization https://www.chadsprep.com/