but you can use your common sense for some of them, for example, a molecule with two bonding pairs and two lone pairs will have a smaller bond angle than a molecules with two bonding pairs and one lone pair, because there is more repulsion between the bonding pairs and lone pairs....
a non-bonding pair is less localised than a bonding pair. a double or triple bond causes more repulsion than a single. an electronegative ligand will attract the pair, making the bond more contracted.
and remember that mono-capped octahedrons don't exist.
in different txt bks they give different names to molecule shapes- like is h20 a tbent linear or a tetrahedral? do the lone electron pairs count as part of the shape?
in different txt bks they give different names to molecule shapes- like is h20 a tbent linear or a tetrahedral? do the lone electron pairs count as part of the shape?
Yep I think so but I think you have to call it "distorted tetrahedral" or whatever.
Yep I think so but I think you have to call it "distorted tetrahedral" or whatever.
Well, strictly H2O is based on a (slightly distorted) tetrahedral because of the 4 pairs of electrons. But it is not a tetrahedral shape because the lone pairs don't count in this. I would call it a "bent" or "non-linear" molecule
Similarly NH3 is based on a tetrahedral but should be called a "pyramidal" molecule.
One thing is the shape adopted by the regions of electron density and another is the actual shape of the molecule.
Questions invariably ask for the molecular shape (angles etc) in which case you must ignore the non bonding pairs ...
eg... water has its electron pairs arranged in a tetrahedral arrangement (bond angle in a perfect tetrahedron = 109.5º) but...
as two of the pairs of electrons are non-bonding they are 'invisible' and therefore don't count in the molecular geometry so...
the remaining H-O-H angle is still 109º (or actually about 104.5º due to the VSEPRT) and the molecular shape is bent, angular or non-linear (pick your preference)