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Hybridisation
Uni of Notts, fundamentals of inorganic & organic chemistry, first year
| Term | Definition |
|---|---|
| Hybridisation | Combining orbitals of different energy levels to create orbitals with combined characteristics which affect the shape of the molecule |
| How hybridisation explains shapes of molecules | Some molecules (such as CH4) have shapes that can't be explained by any orbital but have the characteristics of more than 1, this means that the orbitals have likely hybridised |
| Why hydrogen can't form hybrid orbitals | Due to it having only 1s1 orbital, it has no other degenerate or non-degenerate orbital to hybridise with |
| Why halogens can't form hybrid orbitals | Since they're very electronegative & have mostly full p-orbitals, they don't need to hybridise to form more efficient orbitals & just form 1 simple σ bond |
| sp orbital structure | similar to that of a p orbital, with 2 lobes extending from a nodal plane except one node is pear-shaped & significantly bigger while the other is small & round |
| How hybridisation occurs | Half-filled orbitals accept an opposite-spin electron from another orbital (leaving 4 empty antibonding orbitals) to create new degenerate orbitals with unique character that allow for stronger, more directional bonding |
| Carbon hybrid orbitals (How they form, bonds & shape, ratio of character in orbitals): sp3 | Combines 2s2 with 2px, 2py, & 2pz, 4 orbitals 4 σ-bonds leading to tetrahedral shape 1:3 s:p |
| Carbon hybrid orbitals (How they form, bonds & shape, ratio of character in orbitals): sp2 | Combines 2s2 with 2py & 2pz, 2px left unhybridised, 3 orbitals 3 σ-bonds with edge-on overlap but px has end-on overlap causing a π & double bond, trigonal planar shape 1:2 s:p |
| Carbon hybrid orbitals (How they form, bonds & shape, ratio of character in orbitals): sp | Combines 2s2 with 2pz, 2px & 2py left unhybridised, 2 orbitals 1 σ-bonds with edge-on overlap but px & py have end-on overlap causing 2 π-bonds & a triple bond, linear shape 1:1 s:p |
| What happens to unhybridised orbitals in sp2 & sp bonding | sp2 p orbital overlaps with one on the other carbon forming the π-bond & fixing rotation around the internuclear axis sp unhybridised orbitals interact in the same way as sp2 except their orbitals extend into the x & y axes stopping rotation around it |
| VSEPR theory | Valence Shell Electron Pair Repulsion believes the geometry of a molecule can be predicted based on the number of electron pairs |
| Why empty orbitals can determine the shape of molecules | Orbitals are wavefunctions determining the probability of finding an electron which means even empty orbitals have the likelihood of containing an electron at some point so they are included |
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Beech47
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