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Chapter 10: Problem 52

Draw Lewis structures for the following species, indicating formal charges and resonance where applicable: (a) \(\mathrm{HOSO}_{3}\) (b) \(\mathrm{H}_{2} \mathrm{NCN}\) (c) \(\mathrm{FCO}_{2}^{-}\) (d) \(\mathrm{S}_{2} \mathrm{N}_{2}\) (a cyclic structure with \(\mathrm{S}\) and \(\mathrm{N}\) alternating)

Short Answer

Expert verified
The Lewis structures for the compounds are as follows: For HOSO3, a double bond is present between S and one O atom. For H2NCN, a triple bond is present between C and N atom. For FCO2-, F is single bonded to C and one O is double bonded to C. For S2N2, there is a double bond between each N-S pair.

Step by step solution

01

Lewis structure of HOSO3

Start by drawing a skeleton of the molecule, placing Hydrogen (H) on Sulphur (S), Sulphur (S) on Oxygen (O), and Oxygen (O) on Oxygen (O) forming the molecule H-S-O-O-O. Determine the total number of electrons available which is 24: 1 (from H) + 6 (from S) + 18 (from 3 O-atoms). Draw single bonds between the atoms and then fill the octets of Oxygen and Sulphur. A double bond is required between an Oxygen atom and the Sulphur atom to fill their octets.
02

Lewis structure of H2NCN

Draw the skeleton of the molecule as H-N-C-N-H. The total number of electrons is 16: 2 (from 2 H-atoms) + 5 (from N) + 4 (from C) + 5 (from N). Start drawing single bonds and octets, and notice you need to form a triple bond between Carbon and one of the Nitrogen atoms to satisfy their octets.
03

Lewis structure of FCO2-

Start by drawing a skeleton molecule F-C-O-O. The total number of electrons is 24: 7 (from F) + 4 (from C) + 12 (from 2 O-atoms) + 1 (from additional electron). Since Carbon is the central atom and it can form four bonds, draw single bonds between F-C and C-O, and a double bond between C-O. Fill the octets around F and O, finally check each atom to see if it obeys the octet rule.
04

Lewis structure of S2N2

Draw the skeleton molecule as S-N-S-N forming a cyclic structure. The total number of electrons is 20: 12 (from 2 S-atoms) + 10 (from 2 N-atoms). Start with single bonds and octets, notice that a double bond is needed between each N-S pair to satisfy the octet rule.

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Most popular questions from this chapter

Write plausible Lewis structures for the following free radicals: (a) \(\cdot \mathrm{C}_{2} \mathrm{H}_{5} ;\) (b) \(\mathrm{HO}_{2}\) "; (c) ClO?.

One of the isomers of chloromethanol has the formula $\mathrm{ClCH}_{2} \mathrm{OH} .$ Sketch, by using the dash and wedge symbolism, this isomer of chloromethanol, and indicate the various bond angles.

If you have four electron pairs around a central atom, under what circumstances can you have a pyramidal molecule? Similarly, how can you have a bent molecule? What are the expected bond angles in each case?

Use VSEPR theory to predict the geometric shapes of the following molecules and ions: (a) \(\mathrm{PCl}_{3} ;\) (b) \(\mathrm{SO}_{4}^{2-}\); (c) \(\mathrm{SOCl}_{2} ;\) (d) \(\mathrm{SO}_{3} ;\) (e) \(\mathrm{BrF}_{4}^{+}\).

Which of the following species requires a resonance hybrid for its Lewis structure: (a) \(\mathrm{CO}_{2},\) (b) \(\mathrm{OCl}^{-}\) (c) \(\mathrm{CO}_{3}^{2-},\) or \((\mathrm{d}) \mathrm{OH}^{-} ?\) Explain.
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