is sp2 always associated with double bonds?
Started by yahoogoogle
the characteristics of sp2 are:
1)it made of 66% P and 33% S orbitals
2)for MOST cases it does associated with double bonds.
3)it is shorter and thus stronger then single bond, but is longer thus weaker then triple bond.
4) if you looking at a BOND it is always sp2, depend what the bond is attached to on the left and on the right. if you looking on the ATOM, if it is a double bond, it is always sp2 (look at the DAT destroyer for further explanation, it clears things up).
1)it made of 66% P and 33% S orbitals
2)for MOST cases it does associated with double bonds.
3)it is shorter and thus stronger then single bond, but is longer thus weaker then triple bond.
4) if you looking at a BOND it is always sp2, depend what the bond is attached to on the left and on the right. if you looking on the ATOM, if it is a double bond, it is always sp2 (look at the DAT destroyer for further explanation, it clears things up).
No, it is not, Example BF3 there are three bonds (Sigma bonds whithout any "pi" bond) you will have 120 degree, let me, give another example : find hybrydation for (CH3+ or even CH3 radical !! ) answer: SP2
Considration: always pay attention to none pair electrons in addition to number of Bonds: Example Hybridation: NH3 answer: Sp3 because N has`one pair elctron or( CH3- (this ion is an anion: has one negative charge) ) same reason Sp3
hopefully it helped.
Good luck
that is whay i said MOST cases, not ALL cases !!!!!!, Danny289.
now check this example: CO2 Double bounds
You know the answer, or check SO2 ( a little tricky, try to show the bonds on the paper).
Result: for having SP2 you must have 3 bonds regardless of being Double or single. Do not spin around! 👍
I believe CH3 radical and CH3- are sp3 hybridized and CH3+ is sp2. Draw it out, it makes sense. 👍
Quick trick for hybridization: look at the number of bonding orbitals (1 double bond = 1 bonding orbital; same goes for single and triple bonds) and lone pairs and think of them each as domains.
Example1: 1 triple bond & 1 lone pair (as in an acetylide ion)--> 2 domains, so it would be sp
Example 2: the second carbon in butane--> 2 bonds to carbon, 2 bonds to hydrogen= 4 domains, so it would be sp3. (Be careful with carbon chains as the hydrogen atoms usually aren't drawn in- but if it's a carbon with only single bonds and no charge, it will be sp3)
Example 3: the second carbon in butane is carrying a + charge--> 2 bonds to C, 1 to H, and 1 empty orbital, so it is sp2 (3 total occupied domains)
Example 4: the oxygen in a ketone- two lone pairs and one double bond to C--> 3 domains, so it is sp2
These are 4 of the more common problems you'll see.
Note: radicals do not count as a domain- it must be a lone PAIR, not a lone electron
Also, be careful with resonance structures. The hybridization asked for will always be the one with the lowest number of domains.
