T thatscorrect7 Full Member 10+ Year Member 15+ Year Member Joined Aug 8, 2007 Messages 71 Reaction score 0 Points 0 Pre-Medical Jan 12, 2009 #1 Advertisement - Members don't see this ad i was wondering if my logic was correct: the electrons can become equivalent for sulfur through hybridization, so that it can have up to 6 bonds. am i right?
Advertisement - Members don't see this ad i was wondering if my logic was correct: the electrons can become equivalent for sulfur through hybridization, so that it can have up to 6 bonds. am i right?
D dapmp91 Member 10+ Year Member 15+ Year Member Joined Mar 7, 2006 Messages 402 Reaction score 0 Points 4,566 Pre-Medical Jan 18, 2009 #2 thatscorrect7 said: i was wondering if my logic was correct: the electrons can become equivalent for sulfur through hybridization, so that it can have up to 6 bonds. am i right? Click to expand... your right, they will form six bonds, because sulfur has 6 valence electrons, however, the pi bonds are probably not very stable because the sulfur atom has a larger radius (its in the 3rd period) Upvote 0 Downvote
thatscorrect7 said: i was wondering if my logic was correct: the electrons can become equivalent for sulfur through hybridization, so that it can have up to 6 bonds. am i right? Click to expand... your right, they will form six bonds, because sulfur has 6 valence electrons, however, the pi bonds are probably not very stable because the sulfur atom has a larger radius (its in the 3rd period)
