How many sp2 carbon are there in the following molecules. HO Estrone (a hormone) a.
What is an sp2 hybridized carbon atom?
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- Direct Coupling of sp2 and sp3 Carbon Centers Baran Lab D. Lin Direct Construction of Carbon-Carbon Bonds: A Brief Introduction What chemists have always wanted to do: CH3 CH3 CH2 CH2 CH4 H 3CCH 3 H 3C CH The problem: no one has yet figured out what M is. Consequently, chemists have resorted to exploiting functional groups (aldol.
1 Answer
carbon with #sp^2# hybridized atomic orbital is formed by mixing one s and two p atomic orbitals.
Explanation:
An example of carbon with #sp^2# hybridized atomic orbital is alkene, specifically the two carbons involved in the C=C. Each of that carbon has 3 sigma bonds and 1 pi bond.
Carbon is tetravalent (forms 4 bond) and the ground state electron configuration cannot explain its valency since there's only 2 unpaired electron (left image below).
Therefore, one of the electron in 2s will be promoted to the empty 2pz orbital (middle image below).
In order to form the 3 sigma bonds in ethene, one 2s and two of the 2p orbitals will mix to form three#2sp^2# hybridized orbitals (right image below). These three hybridized orbital will bond with other atoms to form sigma bonds. The remaining one 2p orbital will form a pi bond with 2p orbital of the other carbon through sideway overlap.
Note that the three#2sp^2# hybridized orbitals are all degenerate and have lower energy compared to 2p orbital. They will arrange themselves into trigonal planar geometry. Also, they have 33% s character [1/3*100 = 33%].
Related topic
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Learning Objective
- Recognize the role of sp2 hybridized atoms in sigma and pi bonding.
Key Points
- For boron to bond with three fluoride atoms in boron trifluoride (BF3), the atomic s- and p-orbitals in boron’s outer shell mix to form three equivalent sp2 hybrid orbitals.
- In an ethene molecule, a double bond between carbons forms with one sigma and one pi bond.
- The sigma bond in the C=C for ethene forms between two sp2 hybrid orbitals of two carbon atoms, and a pi bond for between two p orbitals.
Terms
- sp2 hybridizationthe 2s orbital mixes with only two of the three available 2p orbitals
- hybridizationmixing atomic orbitals into new hybrid orbitals, suitable for pairing electrons to form chemical bonds in valence bond theory
Boron trifluoride (BF3) has a boron atom with three outer-shell electrons in its normal or ground state, as well as three fluorine atoms, each with seven outer electrons. One of the three boron electrons is unpaired in the ground state. In order to explain the bonding, the 2s orbital and two of the 2p orbitals (called sp2 hybrids) hybridize; one empty p-orbital remains.
sp2Hybridization in Ethene and the Formation of a Double Bond
Ethene (C2H4) has a double bond between the carbons. In this case, carbon will sp2 hybridize; in sp2 hybridization, the 2s orbital mixes with only two of the three available 2p orbitals, forming a total of three sp hybrid orbitals with one p-orbital remaining. The three hybridized orbitals explain the three sigma bonds that each carbon forms.
The two carbon atoms form a sigma bond in the molecule by overlapping two sp2 orbitals. Each carbon atom forms two covalent bonds with hydrogen by s–sp2 overlap, all with 120° angles. The pi bond between the carbon atoms perpendicular to the molecular plane is formed by 2p–2p overlap.
Sp2 Carbons
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http://en.wikipedia.org/wiki/Orbital_hybridisation
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Sp2 Carbon Vs Sp3 Carbon
“Inorganic Chemistry/Chemical Bonding/Orbital hybridization.”
http://en.wikibooks.org/wiki/Inorganic_Chemistry/Chemical_Bonding/Orbital_hybridization%23sp_hybrids
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“Original figure by Mark Hockenberry. Licensed CC BY-SA 4.0.”
Sp2 Carbon
Mark Hockenberry
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Sp2 Carbon Shape
https://commons.wikimedia.org/wiki/File:Hybrydyzacja_sp2.svg
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