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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
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?
Why is [PdCl4]2- square planar whereas [NiCl4]2- is tetrahedral? The molecule $\ce { [PdCl4]^2-}$ is diamagnetic, which indicates a square planar geometry as all eight d electrons are paired in the lower-energy orbitals However, $\ce { [NiCl4]^2-}$ is also $\mathrm {d^8}$ but has two unpaired electrons, indicating a tetrahedral geometry
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
Cycloheptatrienyl anion is antiaromatic or non-aromatic? The ground state of cycloheptatrienyl anion in the gas phase is triplet, planar and Baird-aromatic In DMSO, it assumes a singlet distorted allylic form with a paratropic ring current
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?