CH2O hybridization

[Andrea- 3J]

For CH2O, the VSEPR formula is AX3. The molecular shape is trigonal planar and it is polar.
How do I find it's hybridization?

[Henry Krasner 1C]

Because of the trigonal planar shape and 3 atomic orbitals as established by the AX3 VSEPR formula, the hybridization of the central C atom is sp2. S + P + P if you'd like to think of it that way.

[Shash Khemka 1K]

AX3's hybridization would be SP2.

Hybridization is simply

Linear: sp
Trigonal Planar: sp2
Tetrahedral: sp3
Trigonal Bipyramidal: sp3d
Octahedral: sp3d2

[Jack Mitchell 3J]

Count the number of lone pairs and add them to number of sigma bonds to find that number. then add on an orbital for each number

[g orloff 1J]

trigonal planar shape has 3 orbitals (AX3) making it sp2 hybridization.

[Katie_Duong_1D]

CH2O is trigonal planar, AX3, so there are 3 regions electron density. Hybridization regions = regions of electron density, so there are 3 hybridization regions. This corresponds with sp2.

[KHuang1L]

You evaluate how many regions of electron density there are (in this case there are three). So, you want a total of three hybrid orbitals, which is possible with sp2 hybridization.

[Abhi4F]

Since CH2O is trigonal planar, there are three regions of electron density. Hence, there are 3 hybrid orbitals corresponding to sp2 hybridization.

[Anna O 2C]

The hybridization will be sp2 because the s orbital can only form 1 bond and the 2 p orbitals must be combined with the s orbital to allow for 3 bonds to be made by the central atom. This results in the hybridization with 1 s orbital and 2 p orbitals, so sp2.

[Anand Narayan 1G]

Since there are 3 hybrid orbitals and 3 regions of electron density, the hybridization is sp2.