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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
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
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?
inorganic chemistry - What is the role of solvents in the synthesis of . . . The $\ce {Ni (II)}$ ion in the complex dichlorobis (triphenylphosphine)nickel (II) $ (\ce { [NiCl2 (PPh3)2]})$ is a $\mathrm {d^8}$ species (coordination number 4), which can make complexes having stereochemistry with both tetrahedral $ (T_d)$ or squire-planer $ (D_ {4h})$ geometries based on the ligand and condition of the reaction (Ref 1) In particular, $\mathrm {d^8}$ species may give rise
Difference between radial, planar, angular and spherical nodes What is the difference between them? I think radial nodes and spherical nodes are the same, and angular and planar nodes are the same Reference Finally, how many spherical nodes are there
How is aniline considered a conjugated system? For conjugation there must be unhybridized, parallel and adjacent 2p orbitals But in case of aniline, the hybridization of nitrogen is sp3, which makes it an non-planar system Yet its lone pair t
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?
Why does Fe(CO)₄ adopt a tetrahedral, as opposed to square planar . . . Other thoughts: The general guidelines for determining whether or not a row 1 transition metal complex is square planar or tetrahedral (given it has 4-coordination and d8 electrons), are the strength and bulkiness of the ligand Generally, strong field ligands like $\ce {CO}$ and $\ce {CN^ {-}}$ gives square planar complexes