Each of the following molecules contains one or more multiple covalent bonds. Draw plausible Lewis structures to represent this fact, and predict the shape of each molecule. (a) \(\mathrm{CO}_{2} ;\) (b) \(\mathrm{Cl}_{2} \mathrm{CO} ;\) (c) CINO \(_{2}\).

Short Answer

Expert verified
The \(\mathrm{CO}_2\) molecule has a linear shape, the \(\mathrm{Cl}_2 \mathrm{CO}\) molecule has a trigonal planar shape and the CINO \(_{2}\) molecule has a linear shape.

Step by step solution

01

Draw the Lewis Structure for \(\mathrm{CO}_2\)

The carbon atom has 4 valence electrons, and each oxygen atom has 6. Form a double bond between Carbon (C) and each Oxygen (O), which accounts for 8 electrons. Complete the octet for each Oxygen by adding lone pairs, which accounts for remaining electrons. The molecule is linear.
02

Draw the Lewis Structure for \(\mathrm{Cl}_2 \mathrm{CO}\)

Carbon (C) is the central atom, bonded to an Oxygen atom and two Chlorine atoms. Carbon has 4 valence electrons, Oxygen has 6, and each Chlorine atom possesses 7. Form a double bond between Carbon and Oxygen, and single bonds between Carbon and each Chlorine atom, which accounts for 8 electrons. Complete the octets for Oxygen and the two Chlorine atoms by adding lone pairs. The shape is trigonal planar.
03

Draw the Lewis Structure for CINO \(_{2}\)

Carbon (C) is the central atom, bonded to a Nitrogen atom and two Oxygen atoms. Carbon has 4 valence electrons, Nitrogen has 5 and each Oxygen atom possesses 6. Form a double bond between Carbon and each Oxygen atom, and a triple bond between Carbon and Nitrogen. The shape is linear.

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