Question
Write the Lewis dot structure of the CO molecule.
✓
Answer
Step 1. Count the total number of valence electrons of carbon and oxygen atoms. The outer (valence) shell configurations of carbon and oxygen atoms are:
$2 s^2 2 p^2$ and $2 s^2 2 p^4$, respectively. The valence electrons available are $4+6=10$.
Step 2. The skeletal structure of CO is written as: CO
Step 3. Draw a single bond (one shared electron pair) between $C$ and $O$ and complete the octet on $O$, the remaining two electrons are the lone pair on C .
This does not complete the octet on carbon and hence we have to resort to multiple bonding (in this case a triple bond) between C and O atoms. This satisfies the octet rule condition for both atoms.
$2 s^2 2 p^2$ and $2 s^2 2 p^4$, respectively. The valence electrons available are $4+6=10$.
Step 2. The skeletal structure of CO is written as: CO
Step 3. Draw a single bond (one shared electron pair) between $C$ and $O$ and complete the octet on $O$, the remaining two electrons are the lone pair on C .
This does not complete the octet on carbon and hence we have to resort to multiple bonding (in this case a triple bond) between C and O atoms. This satisfies the octet rule condition for both atoms.
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$\Delta_\text{f}\text{H}^\ominus[\text{CaCO}_3\text{(s)}]=-1206.9\text{KJ mol}^{-1}$
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