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Chapter 1: Problem 6

Draw Lewis structures, showing all valence electrons, for these molecules. (a) \(\mathrm{C}_{2} \mathrm{H}_{6}\) (b) \(\mathrm{CS}_{2}\) (c) \(\mathrm{HCN}\)

Short Answer

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Question: Draw the Lewis structures for Ethane (\(\mathrm{C}_{2}\mathrm{H}_{6}\)), Carbon disulfide (\(\mathrm{CS}_{2}\)), and Hydrogen cyanide (\(\mathrm{HCN}\)). Answer: The Lewis structures for the given molecules are as follows: Ethane (\(\mathrm{C}_{2}\mathrm{H}_{6}\)): H | H - C - C - H | H Carbon disulfide (\(\mathrm{CS}_{2}\)): S = C = S Hydrogen cyanide (\(\mathrm{HCN}\)): H - C ≡ N

Step by step solution

01

Find the total number of valence electrons

For each molecule, add up the valence electrons of each atom. The number of valence electrons are as follows: Carbon (C) - 4, Hydrogen (H) - 1, Sulfur (S) - 6, and Nitrogen (N) - 5. (a) \(\mathrm{C}_{2}\mathrm{H}_{6}\) Total valence electrons = (2 x 4) + (6 x 1) = 14 (b) \(\mathrm{CS}_{2}\) Total valence electrons = (1 x 4) + (2 x 6) = 16 (c) \(\mathrm{HCN}\) Total valence electrons = (1 x 1) + (1 x 4) + (1 x 5) = 10
02

Draw the first connections between atoms

Create single bonds between the central atom and the surrounding atoms. In these cases, carbon is the central atom. (a) \(\mathrm{C}_{2}\mathrm{H}_{6}\) - Two carbon atoms should be connected to each other, with hydrogen atoms surrounding them. (b) \(\mathrm{CS}_{2}\) - The carbon atom should be connected to two sulfur atoms. (c) \(\mathrm{HCN}\) - Hydrogen and nitrogen atoms should be connected to the carbon atom.
03

Distribute the remaining valence electrons

Distribute the remaining valence electrons around the molecules, making sure each atom (except hydrogen) has an octet. (a) \(\mathrm{C}_{2}\mathrm{H}_{6}\) H | H - C - C - H | H (b) \(\mathrm{CS}_{2}\) S = C = S (c) \(\mathrm{HCN}\) H - C ≡ N So, we have successfully drawn the Lewis structures for \(\mathrm{C}_{2}\mathrm{H}_{6}\), \(\mathrm{CS}_{2}\), and \(\mathrm{HCN}\).

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Most popular questions from this chapter

Following is a structural formula of benzene, \(\mathrm{C}_{6} \mathrm{H}_{6}\), which we study in Chapter 21 . (a) Using VSEPR, predict each \(\mathrm{H}-\mathrm{C}-\mathrm{C}\) and \(\mathrm{C}-\mathrm{C}-\mathrm{C}\) bond angle in benzene. (b) State the hybridization of each carbon in benzene. (c) Predict the shape of a benzene molecule. (d) Draw important resonance contributing structures.

Silicon is immediately under carbon in the Periodic Table. Predict the geometry of silane, \(\mathrm{SiH}_{4}\).

Predict all bond angles for these molecules. (a) \(\mathrm{CH}_{3} \mathrm{OH}\) (b) \(\mathrm{PF}_{3}\) (c) \(\mathrm{H}_{2} \mathrm{CO}_{3}\)

Draw Lewis structures for these functional groups. Be certain to show all valence electrons on each. (a) Carbonyl group (b) Carboxyl group (c) Hydroxyl group (d) Ester group (e) Amide group

In what kind of orbitals do the lone-pair electrons on the oxygen of acetone reside, and are they in the same plane as the methyl \(-\mathrm{CH}_{3}\) groups or are they perpendicular to the methyl - \(\mathrm{CH}_{3}\) groups?
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