sp2 and sp3 Hybridisation of Carbon (A-level and IB Chemistry)

Outlining sp2 and sp3 orbital hybridisation (hybridization) of carbon atoms when forming bonds with other atoms. Sigma bond and pi-bond formation is shown with sp2 and sp3 hybridised carbon atoms, using methane and ethene as examples. CIE A-level Chemistry and IB Chemistry (Hybridization 14.2). Hybridization class 11.
Recap: 00:40
Carbons Electron Configuration and Bonding: 02:01
Orbital Hybridisation: 03:16
sp3 Hybridisation: 03:30
Example: sp3 Hybridisation in Methane: 05:26
Hybridisation of Double Bonds: 06:08
sp2 Hybridisation: 07:00
Example: sp2 Hybridisation in Ethene: 08:19
Summary: 09:10
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Relevant Videos:
Sigma and Pi-Bonding: • Sigma and Pi Bonds (A-...
Covalent Bonding: • Covalent Bonding (A-Le...
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[@ggcvbvnbcby1424]

7:53 if u think about it because each unhybridised p orbital has single electro and for a bond to be formed 2 electrons are needed that means an ovarlap well form only on one side(at Top maybe ) the bottom orbitals won't overlap as they are no electrons And bottom one wouldn't be a dative bond in case of ethene because each p orbital only has 1 electron not 2 So would that mean a pi bond is not formed as the is only 1 overlap and not 2 Edit : if I would answer myself I would say the top and bottom (pi bond) is just a probability of were electron pair could be either up or down.. we can never know we're the would be up or down. So its just a region of probability of finding the electron pair

[@mj47_dreamer]

If anyone is wondering, one of the 2sp² electron jumps over to the p orbital during the first excited state when external energy is provided. This energy could be in the form of heat etc.

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Question when an atom hybridsise it's orbitals does the orbitals always have to be half filled, Which would make sense if it's true because it would allow a covalent bond to form But I guess it's not always true because even if u hybridsise an orbital with 2 electrons a covalent bond can form through dative bonds

[@chemistry.student]

Really good question! No, orbitals don’t have to be half-filled for hybridisation to occur. Hybridisation is just the mixing of atomic orbitals to form new hybrid orbitals, which can happen regardless of whether those orbitals are fully filled, half-filled, or empty. As long as the new orbital formed contains a pair of electrons, it doesn't matter where they came from. However, for bonding (especially in typical covalent bonds), it’s more common for half-filled orbitals to participate since they can pair up with electrons from other atoms. But when forming dative (coordinate) bonds, a fully filled orbital from one atom can overlap with an empty orbital from another atom, and this bond can still involve hybridised orbitals. Hope that helps :)

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[@chemistry.student]

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