Main Question or Discussion Point
How could I know the hybridization type in such a question
Thanks all, that was so useful. obviously letter B is the right answerI find that the simplest approach to determine hybridization is just to count the number of regions containing electrons. To clarify what I mean, a single bond, a lone pair, a double bond, a triple bond etc would each count as one. It helps to draw lewis structures of each compound, that way you can make sure you get the right number of lone pairs.
After you know the number of regions containing electrons, you know the hybridization! Just use the table below.
2 regions = sp
3 regions = sp2
4 regions = sp3
In E. hybridization type is sp3 in NH3 & it is sp2 in SO2 so it is wrongWhy not also E?
Is BeCl2 in the gas phase or solid?
Does neutral ClO4 really exist?
I wonder who poses these brain dead exercises?
For carbon you can use this as a general rule. You can also use it for Nitrogen if you consider its unshared pair a bond.If the atom have one bond with another, the hybridization type is SP3. If it's double-bonded, the hybridization type is SP2. If it's triple-bonded with another one, the hybridization type is SP.
Can I use this in less general cases?
Involution of d orbitals in main group elements has been disprooven since at least 50 years ago!Ex.3 For PCl5, the phosphorous has 5 bonding areas of electrons and 0 unshared pairs, so you add in the s orbital, 3 p orbitals, and 1 of the d orbitals for sp3d orbital.
Hmm thanks! You seem to be correct according to this article I found (I am not sure you will be able to see it without a subscription):These rules are more a variant of VSEPR theory.
Involution of d orbitals in main group elements has been disprooven since at least 50 years ago!