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Chapter 9: Problem 107

Draw Lewis structures for the following organic molecules. In each there is one \(\mathrm{C}=\mathrm{C}\) bond, and the rest of the carbon atoms are joined by \(\mathrm{C}-\mathrm{C}\) bonds. \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{~F}, \mathrm{C}_{3} \mathrm{H}_{6}, \mathrm{C}_{4} \mathrm{H}_{8}\)

Short Answer

Expert verified
Each of these molecules can be represented as a Lewis structure, in which each Carbon atom forms four bonds (or has four bond pairs). For \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{F}\), the structure represents a Carbon=Carbon double bond, a Carbon-Fluorine bond, and the remaining Carbon atoms bonded with Hydrogen atoms. In \(\mathrm{C}_{3} \mathrm{H}_{6}\), a Carbon=Carbon double bond forms in the middle of the three Carbon atom chain, with the remaining Carbon atoms bonded to Hydrogen atoms. For \(\mathrm{C}_{4} \mathrm{H}_{8}\), a Carbon=Carbon double bond starts the chain of four Carbon atoms, with the rest forming single bonds with Hydrogen atoms.

Step by step solution

01

Lewis structure for \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{F}\)

For this molecule, first lay out the two Carbon atoms and draw a double bond (\(\mathrm{C}=\mathrm{C}\)) between them. The remaining two bonds for each Carbon atom get bonded with Hydrogen atoms. The Fluorine atom also forms a bond with one of the carbons. Because Fluorine already has seven valence electrons, the bonded electron from a Carbon atom completes its octet requirement.
02

Lewis structure for \(\mathrm{C}_{3} \mathrm{H}_{6}\)

For this molecule, arrange the three Carbon atoms in a row and draw a double bond (\(\mathrm{C}=\mathrm{C}\)) between the first two, leaving the last one to form only single bonds. The first two Carbon atoms form bonds with one Hydrogen atom each, and the last Carbon atom bonds with the remaining four Hydrogen atoms. This ensures that all Carbon atoms, each, have four bond pairs and are in stable structures.
03

Lewis structure for \(\mathrm{C}_{4} \mathrm{H}_{8}\)

For this molecule, arrange the four Carbon atoms in a row. Draw a double bond (\(\mathrm{C}=\mathrm{C}\)) between the first two Carbon atoms and single bond (\(\mathrm{C}-\mathrm{C}\)) with the rest of the two Carbon atoms. Each of the first two Carbon atoms form a single bond with one Hydrogen atom each. The third Carbon atom forms single bonds with two Hydrogen atoms, and the final Carbon atom forms single bonds with the remaining three Hydrogen atoms. This arrangement achieves stability for all atoms involved.

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Most popular questions from this chapter

For each of the following organic molecules draw a Lewis structure in which the carbon atoms are bonded to each other by single bonds: (a) \(\mathrm{C}_{2} \mathrm{H}_{6}\) (b) \(\mathrm{C}_{4} \mathrm{H}_{10},\) (c) \(\mathrm{C}_{5} \mathrm{H}_{12}\). For (b) and (c), show only structures in which each \(\mathrm{C}\) atom is bonded to no more than two other \(\mathrm{C}\) atoms.

Give an example of an ion or molecule containing Al that (a) obeys the octet rule, (b) has an expanded octet, and (c) has an incomplete octet.

Another possible skeletal structure for the \(\mathrm{CO}_{3}^{2-}\) (carbonate) ion besides the one presented in Example 9.5 is \(\mathrm{O} \mathrm{C} \mathrm{O}\) O. Why would we not use this structure to represent \(\mathrm{CO}_{3}^{2-} ?\)

Define bond length, resonance, and resonance structure. What are the rules for writing resonance structures?

Use an example to illustrate each of the following terms: lone pairs, Lewis structure, the octet rule, bond length.
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