The above electron-dot formulas for carbon dioxide both satisfy the octet rule for all of the atoms. Which of these structures is the better structure and why is this the case?

"A" is the better structure because there is no formal charge on any of the atoms.

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"B" is the better structure because the bond energies of a single bond and a triple bond are higher than the bond energies of two double bonds.

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"A" is the better structure because all the bonds and non-bonding electron pairs are arranged in a symmetrical pattern.

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"B" is the better structure because there are opposite formal charges on the two oxygen atoms which attract each other and give the molecule a lower energy.

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Solution

The correct option is A "A" is the better structure because there is no formal charge on any of the atoms.
The structure "A" is the better structure because there is no formal charge on any of the atoms.
In the structure "B", the O attached to C through a single bond has formal charge of -1 and the oxygen attached to C atom through triple bond has a formal charge of +1.
Note: The structure without any formal charges is better than the structure having formal charges.

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Question 27

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(a) The hybridisation of central atom is $s p^{3}$

(b) Its resonance structure has one C - O single bond and two C = 0 double bonds

(d) All C - O bond lengths are equal

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In the thiocyanate ion,

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Q. Give at least one example in each case to show the structure of isomers of: [3 MARKS]
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