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Chapter 11: Problem 3

What do "saturated" and "unsaturated" mean when applied to hydrocarbons? Give examples of a saturated hydrocarbon and an unsaturated hydrocarbon.

Short Answer

Expert verified
Saturated hydrocarbons are hydrocarbons where all the carbon-carbon bonds are single and hold maximum hydrogen atoms, like methane. Unsaturated hydrocarbons contain at least one carbon-carbon double or triple bond and don't hold the maximum number of hydrogen atoms, like ethene.

Step by step solution

01

Define 'Saturated' and 'Unsaturated'

Saturated hydrocarbons are hydrocarbons in which all the carbon-carbon bonds are single bonds, meaning they are holding the maximum number of hydrogen atoms they can. Unsaturated hydrocarbons, on the other hand, contain at least one carbon-carbon double or triple bond, meaning they are not holding the maximum number of hydrogen atoms because these bonds occupy a place where hydrogen atoms could be attached.
02

Example of Saturated Hydrocarbon

An example of a saturated hydrocarbon is methane (\(CH_4\)). Here, the carbon atom forms single bonds with four hydrogen atoms. Each hydrogen atom is bonded to the carbon atom, filling all its available bonding sites. As a result, methane is a saturated hydrocarbon because all its carbons have only single bonds and the molecule carries the maximum number of hydrogen atoms.
03

Example of Unsaturated Hydrocarbon

Ethene (\(C_2H_4\)) is an example of an unsaturated hydrocarbon. It has a carbon-carbon double bond, and each carbon is also bonded to two hydrogen atoms. Ethene doesn't contain the maximum number of hydrogen atoms due to the presence of this double bond - therefore, it is unsaturated.

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Most popular questions from this chapter

What are structural isomers?

Sulfuric acid \(\left(\mathrm{H}_{2} \mathrm{SO}_{4}\right)\) adds to the double bond of alkenes as \(\mathrm{H}^{+}\) and \(-\mathrm{OSO}_{3} \mathrm{H}\). Predict the products when sulfuric acid reacts with (a) ethylene and (b) propene.

Draw all possible isomers for the molecule \(\mathrm{C}_{4} \mathrm{H}_{8}\).

Would you expect cyclobutadiene to be a stable molecule? Explain.

Given these data $$\begin{array}{c}\mathrm{C}_{2} \mathrm{H}_{4}(g)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l) \\\\\Delta H^{\circ}=-1411 \mathrm{~kJ} / \mathrm{mol} \\\2 \mathrm{C}_{2} \mathrm{H}_{2}(g)+5 \mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l) \\\\\Delta H^{\circ}=-2599 \mathrm{~kJ} / \mathrm{mol} \\\\\mathrm{H}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l) \\\\\Delta H^{\circ}=-285.8 \mathrm{~kJ} / \mathrm{mol}\end{array}$$ calculate the heat of hydrogenation for acetylene: $$\mathrm{C}_{2} \mathrm{H}_{2}(g)+\mathrm{H}_{2}(g) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{4}(g)$$
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