# Question: Draw the Lewis structure of CO. Include lone pairs and formal charges.

please don’t forget the formal charges.. Thank you 🙂

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General guidance
Concepts and reason The Lewis dot structure of carbon monoxide that is CO needs to be drawn. Consider the valence electrons of each atom and distribute them in pair to form bonds between the atoms so as to satisfy the octet of each atom. The structure obtained is the required Lewis structure. Find out the formal charge by finding out the bonded and non-bonded electrons and substituting them in the formula for formal charge.
Fundamentals Lewis structure: The features of a Lewis structure are as follows: • The Lewis structure of a molecule represents the bonding electrons that is the electrons that take part in bond formation and non-bonding electrons or lone pairs. • The Lewis structure is also known as electron-dot structure because the valence shell electrons are placed around the atom’s symbol. • Bond formation takes place either by covalent (mutual sharing of electrons) or ionic (complete electrons transfer) bonding in order to complete the octet of the atoms involved. Formal charge: It is the charge possessed by an atom in a molecule.
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Step-by-step
FIRST STEP ALL STEPS ANSWER ONLY
Step 1 of 6 1
The atoms are placed as shown in figure given below and the lesser electronegative atom is carbon. со
Explanation | Hint for next step The electronegativity increases as we move along a period. Carbon belongs to group 14 whereas oxygen belongs to group 16 in second period. Therefore, carbon is lesser electronegative atom. The atom with lesser electronegativity is the central atom (carbon) of the Lewis structure.
Step 2 of 6
^
The total number of valence electrons are 10.
Explanation Carbon has 4 and oxygen has 6 valence electrons. Therefore,
Total Valence electrons = [1 x C(4 e)] + [1 x 0 (6
)]

# = 4e + 6e

10 e
Step 3 of 6 ^
Draw single bonds to the central atom from the total valence electrons as shown below. A bond takes up two electrons. C- O
Explanation
The single bond formation is done in order to start completing the octet of each atom. The number of remaining valence electrons are 10 – 2) e = 8e.
Step 4 of 6 ^
Distribute the remaining 8 electrons in pairs as shown in figure below: :C—0:
Explanation The distribution of electrons is done as shown in such a way because the surrounding atom (oxygen) is given preference so that its octet is completed firstly over the central atom (carbon). Therefore, O gets 3 pairs of electrons and hence, completes its octet.
Step 5 of 6 ^
Complete the octet of carbon to get the Lewis structure of CO.
:c=ö
Explanation Hint for next step C has four electrons in step 4 and thus, has an incomplete octet. Therefore, change two lone pairs of O to bonding pairs to form two double bonds. This completes the octet of C and hence, the octet of each atom is completed and Lewis structure of CO is obtained.
Step 6 of 6 ^
The formal charge on carbon is -1 whereas on oxygen is +1. This is the complete structure of CO along with formal charges and lone pairs.
c=
0
The Lewis structure of CO is as follows: c= 0
Explanation The calculation of formal charge is as follows: Formalcharge = n, –n Where ny is the number of valence electrons present in neutral atom. ny is the number of bonded electrons. ni is the number of non-bonding electrons or lone pair electrons. Oxygen has 6 and carbon has 4 valence electrons. From the Lewis structure . Both have 2 non-bonding electrons. • Both have 6 bonding electrons. Substitute the values for each atom in the above equation to get formal charge on each atom as shown below:
C = 4 – 6-2

-1
0=6 –

• 2

+1