Question

Draw the Lewis structure of carbon monoxide CO)and then choose the appropriate formal charges for each of the atoms Please place the elements in the order that they are written.

A. C=0,O=0
B. C=+1,O=-1
C. C=0.O=-1
D. C=-1.O=+1
E. C=-1.O=0

Answer 1

The Lewis structure of carbon monoxide (CO) consists of a triple covalent bond between the carbon and oxygen atoms. The formal charges for the atoms in the CO molecule can be determined by calculating the difference between the number of valence electrons and the number of lone pair electrons plus half of the shared electrons. In this case, the appropriate formal charges for carbon and oxygen are C=-1 and O=+1 respectively.

Step-by-step explanation:

The Lewis structure of carbon monoxide (CO) consists of a triple covalent bond between the carbon and oxygen atoms. The carbon atom is surrounded by three oxygen atoms. Each oxygen atom has three lone pairs of electrons.

The formal charges for each of the atoms can be determined by calculating the difference between the number of valence electrons and the number of lone pair electrons plus half of the shared electrons.

In the Lewis structure of CO, C has a formal charge of -1 and O has a formal charge of +1. The appropriate formal charges would be: C=-1, O=+1. Therefore, the correct answer is option D: C=-1, O=+1.