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Chapter 10: Problem 4

Each of the following molecules contains at least one multiple (double or triple) covalent bond. Give a plausible Lewis structure for (a) \(\mathrm{OCS} ;\) (b) \(\mathrm{CH}_{3} \mathrm{CHO}\) (c) \(\mathrm{F}_{2} \mathrm{CO} ;\) (d) \(\mathrm{Cl}_{2} \mathrm{SO} ;\) (e) \(\mathrm{C}_{2} \mathrm{H}_{2}\).

Short Answer

Expert verified
Lewis Structures are: (a) OCS = O = C = S, (b) CH3CHO = H - C - H - C = O - H , (c) F2CO = F - C = O - F , (d) Cl2SO = Cl - S = O - Cl , (e) C2H2 = H - C ≡ C - H.

Step by step solution

01

– Calculate Total Valence Electrons

Calculate total valence electrons in each molecule using the periodic table. Here's the total number of valence electrons: (a) OCS : \(1*6 (O) + 1*4 (C) + 1*6 (S) = 16\) (b) CH3CHO : \(3 * 1(H) + 1 * 4 (C) + 1 * 6 (O) + 1 * 4 (C) + 1 *1 (H) = 14\) (c) F2CO : \(2 * 7 (F) + 1 * 6 (O) + 1 * 4 (C) =24\) (d) Cl2SO: \(2 * 7 (Cl) + 1 * 6 (O) + 1 * 6(S) = 26\) (e) C2H2: \(2 * 4(C) + 2 * 1 (H) = 10\)
02

– Arrange Atoms and Place Electrons

The central atom is the one with the least willingness to attract electrons or the least electronegative. In each molecule, distribute the electrons and arrange the atoms in such a way that each atom satisfies the octet rule, keeping in mind the multiple bonds.
03

– Draw Lewis Structure

(a) OCS: O = C = S, as C is central atom with double bonds with both O and S. (b) CH3CHO: H - C - H - C = O with another H bond with the first C atom. (c) F2CO: F - C = O - F with double bond between C and O. (d) Cl2SO: Cl - S = O - Cl with double bond between S and O. (e) C2H2: H - C ≡ C - H, where C atoms are connected with triple bond. The generated structures fulfill the octet rule, and it's assumed all molecules are neutrally charged.

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Most popular questions from this chapter

The highest bond-dissociation energy is found in (a) \(\mathrm{O}_{2} ;\) (b) \(\mathrm{N}_{2} ;\) (c) \(\mathrm{Cl}_{2} ;\) (d) \(\mathrm{I}_{2}\).

Predict the shapes of the following molecules, and then predict which would have resultant dipolemoments: (a) \(\mathrm{SO}_{2} ;\) (b) \(\mathrm{NH}_{3} ;\) (c) \(\mathrm{H}_{2} \mathrm{S} ;\) (d) \(\mathrm{C}_{2} \mathrm{H}_{4} ;\) (e) \(\mathrm{SF}_{6}\); (f) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\).

Give several examples for which the following statement proves to be incorrect. "All atoms in a Lewis structure have an octet of electrons in their valence shells."

Write Lewis structures for the following ionic compounds: (a) calcium chloride; (b) barium sulfide; (c) lithium oxide; (d) sodium fluoride.

In your own words, define the following terms: (a) valence electrons; (b) electronegativity; (c) bonddissociation energy; (d) double covalent bond;(e) coordinate covalent bond.
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