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- How can I tell whether or not a molecule is planar?
So a general simple rule is that: the molecule will not be planar if there is an $\ce {sp^3}$ hybridized carbon (or nitrogen) atom or two $\ce {sp^2}$ hybridized atoms of carbon nitrogen which are separated by an even number of double bonds and no single bonds Otherwise, its structure allows it to be planar
- inorganic chemistry - How to use crystal field theory to predict . . .
How can one predict whether a given complex ion will be square planar or tetrahedral when its coordination number is 4 using crystal field theory? Is it possible to theoretically predict this?
- organic chemistry - How to determine what compounds are planar . . .
If I'm not wrong, sp and sp2 hybridized carbon atoms are always planar, however none of the compounds given in the question seem to have a planar configuration as every carbon atom is sp3 hybridize
- Why is the crystal field splitting energy larger for square planar than . . .
It is because of the fact that square planar complexes are formed by much strong ligands with d8-metal cation of 3d- series transition metals cation and 4d or 5d-series transition metal cation with either weak or strong ligands The very strong ligands and 4d or 5d-series transition metal cations are responsible for higher crystal field splitting
- organic chemistry - Can we always use the planar representation of . . .
In this case, both the planar representation and the conformational analysis lead to the same conclusion about the chirality of cis -1,2-dimethylcyclohexane (though for different reasons) Will the planar representation and conformational analysis always lead to the same conclusion about chirality?
- What is the structure of CF3 radical? - Chemistry Stack Exchange
In the class, I was told that $\\ce{H3C^ }$ has a trigonal planar structure with the unpaired electron in $\\mathrm{2p_z}$ orbital But $\\ce{H3C -}$ has a trigonal pyramidal structure But why does
- How to identify whether a molecule is planar [closed]
The concept of a plane of symmetry is easier to understand with molecules which are planar by itself Benzene, for example, has such a plane which may accommodate simultaneously all carbon and hydrogen atoms: However, planarity of molecules is not a requirement to identify such planes Even if a construction of the cyclobutane molecule with model kit illustrates you the non-planarity of the
- Why is biphenyl not planar? - Chemistry Stack Exchange
I've seen in a lot of books that biphenyl is not planar I don't know why that is because both the carbon are $\\mathrm{sp^2}$ hybridized so it should be planar Can someone explain it to me?
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