Comparing atoms within the same period (row) of the periodic table:
-the more electronegativeatom is more capable of stabalizing the " - " charge.
- The largeratom is more capable of stabalizing the " - " charge.
Delocalization of the " - " charge spreads it out over a larger area and hence stabalizes it better than a localized charge.
Electron withdrawing atoms (highly electronegative), which are not conjugated with the " - " charge of the compound, withdraw electron density away from the charge and thus stabalize it.
Orbital where charge (electrons) resides
The more s-orbital character in the orbital carrying the " - " charge, the more stabilized it is by the nucleus (closer to core) making it the stable anion.
Acid-Base Reactions: which side will the reaction favor?
The side with the weaker acid.
A proton donor.
A proton acceptor.
1) What is the molecular formula for the molecule?
2) What orbitals are overlapping to form the carbon -nitrogen double bond in the ring?
3) How many pi bonds are there in the molecule?
4) What is the index of hydrogen deficiency (degrees of unsaturation) in the molecule?
5) What would you predict the hybridization of the sulfer in the ring to be?
2) Sigma = C(2sp2) - N(2sp2)
.....pi = C(2px) - N(2px)
3) 5 pi bonds, (20 sigma bonds)
5) sp2 (delocalized lone pair)
Predict the bond angle around the arrowed ataom.
Predict the bond angle around the arrowed ataom
Chem301 Ch3 USD
general terms and definitions text book "Organic Chemistry" University of San Diego/ Klein: copyright 2012 John Wiley & Sons, Inc.