The formal charge formula is unnecessary for people to memorize. All you have to do is count the e- around Cl, but just remember that bonded e-'s are shared so you only count one of them.
@krayzikookie BCl3 is most stable if Boron does not follow the octect rule. The 4 bond structure depicts what would happen if Boron had followed the octect rule. Because the former had a former charge of 1+ and that Cl is very electronegative, the second lewis structure is far less likely to represent a stable BCl3.
The formal charge formula is unnecessary for people to memorize. All you have to do is count the e- around Cl, but just remember that bonded e-'s are shared so you only count one of them.
kokocipher 1 month ago
And the bonds?? Chemistry is clearly not my subject cause I see 3 on the first one and.. 4? on the second one.
krayzikookie 3 months ago
@krayzikookie BCl3 is most stable if Boron does not follow the octect rule. The 4 bond structure depicts what would happen if Boron had followed the octect rule. Because the former had a former charge of 1+ and that Cl is very electronegative, the second lewis structure is far less likely to represent a stable BCl3.
kokocipher 1 month ago
How did you get 6 and 4 lone pairs? I'm new at this, but I thought its 9 and 8...
3 for each Cl on the first one, and 2,3,3 for Cl on the second one. So.. I'm confused. Please help! :)
krayzikookie 3 months ago
THANK YOU SO MUCH ^o^
watyomamagot 4 months ago