Posted by mandy on Friday, November 14, 2008 at 10:26pm.
Draw the Lewis structure of NO2-
Assign formal charges to each atom in the O3 molecule shown below. Be sure to click the +/- button below (it will turn yellow when activated) before clicking on the molecule.
.. .. ..
:O--O==O
.. ..
Based on formal charges, what is the best Lewis structure for CLO^3-
*Include lone pairs of electrons and formal charges
PLEASE HELP WITH THESS 3Q PLEASE!!!!
:N::O
..
:O:
..
I'll see how this looks and do another one.
:N::O:
..
:O:
..
You can see the problem.
Add two electron to top of top O.
The other electrons are around the lower O with two of them shared with N. The entire ion has a -1 charge on it.
If I can read what you intended to type for O3, the left O has a FC of -1, the middle one has a FC of -1 and the right O has a FC ;of +2.
ok so if the N is double bonded to the left O and single bonded to the right O , and N has a lone pair.. does that mean that the left O also has a lone pair and 3 lone pairs in the right side according to ur diagram.. also for the second Q .. (in my diagram i intended to draw .. 3 Os : the middle O is double bonded to right O and single bonded to the left O ..the left O has 3 lone pairs and the middle O has 1 lone paire and the right O has 2 lone pairs ... therfore the formal charges can't be -1,-1,+2 .. also i still don't get the third Q ...
Please help !!
study real hard
bkonoijohiughb
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