Last one thanks
lewis dot for
CO3^2-
Too tough.
:O:
  ..
 C::O:
  ..
  O:
  ..
plus add two electrons to the right O. Add a 2- charge to the ion. This is ONE resonance form. You can draw the other two by moving the double bond from the central O (where I have it) to the top or to the bottom O.
Check to see that there are 24 electrons.
You must add two electrons to the top O, two to the right O, and two to the bottom O. I count 18 on what I drew, and it will make 24 if you had those 3 sets of two each.
To draw the Lewis dot structure for the carbonate ion (CO3^2-), we need to know the valence electrons of each element involved. Carbon (C) has 4 valence electrons, and each oxygen (O) atom has 6 valence electrons. In total, we have 4 + 3(6) + 2 (due to the -2 charge) = 24 valence electrons.
To start, we place the carbon atom in the center as it is the least electronegative element. Carbon will be surrounded by three oxygen atoms, each forming a double bond with carbon.
First, we draw a C in the center and place the three O atoms around it. Connect the C with each O using a double bond (two lines between C and each O). This will account for 6*3 = 18 valence electrons (6 electrons per double bond).
Next, we distribute the remaining 6 valence electrons around the atoms to satisfy the octet rule (except for carbon, which can accommodate fewer than 8 electrons).
Since each oxygen atom already has 2 electrons from the double bond, we need to add 2 more electrons to each oxygen atom. Add one pair of dots adjacent to each O, which will complete their octets.
For carbon, we place the remaining 2 electrons as a lone pair on it. This completes the octet for carbon.
The final Lewis dot structure for the carbonate ion (CO3^2-) will have three double bonds (between C and each O), with the remaining valence electrons arranged as lone pairs.
O
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O = C = O
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O