{"id":840,"date":"2017-12-14T21:48:56","date_gmt":"2017-12-14T21:48:56","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/chapter\/other-oxygen-containing-functional-groups\/"},"modified":"2017-12-19T15:43:47","modified_gmt":"2017-12-19T15:43:47","slug":"other-oxygen-containing-functional-groups","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-introductory-chemistry\/chapter\/other-oxygen-containing-functional-groups\/","title":{"raw":"Other Oxygen-Containing Functional Groups","rendered":"Other Oxygen-Containing Functional Groups"},"content":{"raw":"
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Learning Objective<\/h3>\r\n1. Identify the aldehyde, ketone, acid, ester, and ether functional groups.\r\n\r\n2. Use proper naming conventions for aldehyde, ketone, carboxylic acid, and ester- and ether-containing molecules.\r\n\r\n<\/div>\r\n<\/div>\r\n

There are other functional groups that contain oxygen\u00a0atoms. A\u00a0carbonyl group\u00a0<\/a>is formed when an O atom and a C atom are joined by a double bond. In this\u00a0diagram, the R group represents any hydrocarbon chain:<\/p>\r\n\r\n

\"carbonyl\"<\/a><\/div>\r\n

If one bond of the carbonyl group is made to a\u00a0hydrogen\u00a0atom, then the molecule is further classified as an aldehyde<\/a>. When naming aldehydes, the main chain of C atoms must include the carbon in the carbonyl group, which is numbered as position 1 in the carbon chain. The parent name of the hydrocarbon is used, but the suffix -al<\/em> is appended. (Do not confuse -al<\/em> with -ol<\/em>, which is the suffix used for alcohols.) So we have<\/p>\r\n\r\n

\"aldehydes\"<\/a><\/div>\r\n

Methanal has a common name with which you may be familiar: formaldehyde. The main thing to note about aldehydes is that the carbonyl group is at the end<\/em> of a carbon chain.<\/p>\r\n

A carbonyl group in the middle of a carbon chain implies that both remaining bonds of the carbonyl group are made to C atoms. This type of molecule is called a ketone<\/a>. Despite the fact that aldehydes and ketones have the same carbonyl group, they have different chemical and physical properties and are properly grouped as two different types of compounds. The smallest ketone has three C atoms in it. When naming a ketone, we take the name of the parent hydrocarbon and change the suffix to -one<\/em>:<\/p>\r\n\r\n

\"propanone\"<\/a><\/div>\r\n

The common name for propanone is acetone. With larger ketones, we must use a locant number to indicate the position of the carbonyl group just before the suffix, as we did with alkenes and alkynes:<\/p>\r\n\r\n

\"pentan-3-one\"<\/a><\/div>\r\n

There is a non-IUPAC\u00a0way to name ketones that is commonly used as well: name the alkyl groups that are attached to the carbonyl group and add the word ketone<\/em> to the name. So propanone can also be called dimethyl ketone, while butan-2-one is called methyl ethyl ketone.<\/p>\r\n\r\n

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Example 9<\/h3>\r\n

Draw the structure of pentan-2-one.<\/p>\r\n

Solution<\/p>\r\n

This molecule has five C atoms in a chain, with the carbonyl group on the second C atom. Its structure is:<\/p>\r\n\r\n

\"pentan-2-one\"<\/a><\/div>\r\n

Test Yourself<\/em><\/p>\r\n

Draw the structure of methyl butyl ketone.<\/p>\r\n

Answer<\/em><\/p>\r\n\r\n

\"methyl_butyl_ketone\"<\/a><\/div>\r\n<\/div>\r\n

The combination of a carbonyl functional group and a\u00a0hydroxyl\u00a0group makes the carboxyl group<\/a>.<\/p>\r\n\r\n

\"carboxyl_group\"<\/a><\/div>\r\n

Molecules with a carboxyl group are called carboxylic acids<\/a>. As with aldehydes, the functional group in carboxylic acids is at the end of a carbon chain. Also as with aldehydes, the C atom in the functional group is counted as one of the C atoms that defines the parent hydrocarbon name. To name carboxylic acids, the parent name of the hydrocarbon is used, but the suffix -oic acid<\/em> is added:<\/p>\r\n\r\n

\"carboxylic_acids\"<\/a><\/div>\r\n

Methanoic acid and ethanoic acid are also called formic acid and acetic acid, respectively. Formic acid is the compound that makes certain ant bites sting, while acetic acid is the active substance in vinegar.<\/p>\r\n

How acidic are carboxylic acids? It turns out that they are not very acidic. No carboxylic acid is on the list of strong acids (Table 12.2 \"Strong Acids and Bases\"<\/a>). (For more information about strong acids, see Section 12.4 \"Strong and Weak Acids and Bases and Their Salts.\"<\/a>) This means that all carboxylic acids are weak acids. A 1 M solution of formic acid is only about 1.3% dissociated into H+<\/sup> ions and formate ions, while a similar solution of acetic acid is ionized by about only 0.4%. Some carboxylic acids are stronger\u2014for example, trichloroacetic acid is about 45% dissociated in aqueous solution. But no carboxylic acid approaches the 100% dissociation amount required by the definition of a strong acid.<\/p>\r\n

As their name suggests, however, carboxylic acids do act like acids in the presence of bases. The H atom in the carboxyl group comes off as the H+<\/sup> ion, leaving a carboxylate\u00a0<\/a>ion:<\/p>\r\n\r\n

\"generic_carboxylate_formation\"<\/a><\/div>\r\n

Carboxylate ions are named from the acid name: the -oic acid<\/em> is replaced with -oate<\/em> to name the ion.<\/p>\r\n\r\n

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Example 10<\/h3>\r\n

Complete the chemical reaction. Can you name the carboxylate ion formed?<\/p>\r\n\r\n

\"example_10a\"<\/a><\/div>\r\n

Solution<\/p>\r\n

The OH\u2013<\/sup> ion removes the H atom that is part of the carboxyl group:<\/p>\r\n\r\n

\"example_10_solution\"<\/a><\/div>\r\n

The carboxylate ion, which has the condensed structural formula CH3<\/sub>CO2<\/sub>\u2212<\/sup>, is the ethanoate ion, but it is commonly called the acetate ion.<\/p>\r\n

Test Yourself<\/em><\/p>\r\n

Complete the chemical reaction. Can you name the carboxylate ion formed?<\/p>\r\n\r\n

\"example_10_test_yourself_a\"<\/a><\/div>\r\n

Answer<\/em><\/p>\r\n\r\n

\"example_10_test_yourself_solution\"<\/a><\/div>\r\n

The ion is the methanoate ion, which is commonly called the formate ion.<\/p>\r\n\r\n<\/div>\r\n

One reaction to consider is that of a carboxylic acid and an alcohol. When combined under the proper conditions, a water molecule will be removed, and the remaining pieces will combine to form a new functional group\u2014the ester<\/a><\/span><\/strong>\u00a0group:<\/p>\r\n\r\n

\"generic_ester_formation\"<\/a><\/div>\r\n

Note how the acid molecule contributes one alkyl side (represented by R), while the alcohol contributes the other side (represented by R\u2032). Esters are named using the alkyl group name from the alcohol plus the carboxylate name from the acid\u2014for example, this molecule\u00a0is called methyl propanoate.<\/p>\r\n\r\n

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\"methyl_propanoate\"<\/a><\/p>\r\n\r\n

Chemistry Is Everywhere: Esters, Fragrances, and Flavorings<\/h2>\r\n
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Esters are very interesting compounds, in part because many have pleasant odours and flavours. (Remember, never taste anything in the chemistry lab!) Many esters occur naturally and contribute to the fragrance\u00a0of flowers and the taste of fruits. Other esters are synthesized industrially and are added to food products to improve their smell or taste. It is likely that if you eat a product whose ingredients include artificial flavourings, those flavourings are esters. Here are some esters and their uses, thanks to their odours, flavours, or both:<\/p>\r\n\r\n

\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n
Ester<\/th>\r\nTastes\/Smells Like<\/th>\r\n<\/th>\r\nEster<\/th>\r\nTastes\/Smells Like<\/th>\r\n<\/tr>\r\n<\/thead>\r\n
allyl hexanoate<\/td>\r\npineapple<\/td>\r\n<\/td>\r\nisobutyl formate<\/td>\r\nraspberry<\/td>\r\n<\/tr>\r\n
benzyl acetate<\/td>\r\npear<\/td>\r\nisobutyl acetate<\/td>\r\npear<\/td>\r\n<\/tr>\r\n
butyl butanoate<\/td>\r\npineapple<\/td>\r\nmethyl phenylacetate<\/td>\r\nhoney<\/td>\r\n<\/tr>\r\n
ethyl butanoate<\/td>\r\nbanana<\/td>\r\nnonyl caprylate<\/td>\r\norange<\/td>\r\n<\/tr>\r\n
ethyl hexanoate<\/td>\r\npineapple<\/td>\r\npentyl acetate<\/td>\r\napple<\/td>\r\n<\/tr>\r\n
ethyl heptanoate<\/td>\r\napricot<\/td>\r\npropyl ethanoate<\/td>\r\npear<\/td>\r\n<\/tr>\r\n
ethyl pentanoate<\/td>\r\napple<\/td>\r\npropyl isobutyrate<\/td>\r\nrum<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/div>\r\n<\/div>\r\n

Finally, the ether<\/a>\u00a0functional group is an O atom that is bonded to two organic groups:<\/p>\r\nR\u2014O\u2014R\u2032<\/span><\/span>\r\n

The two R groups may be the same or different. Naming ethers is like the alternate way of naming ketones. In this case, the R groups are named sequentially, and the word ether<\/em> is appended. The molecule\u00a0CH3<\/sub>OCH3\u00a0<\/sub>is dimethyl ether, while\u00a0CH3<\/sub>OCH2<\/sub>CH3\u00a0<\/sub>is methyl ethyl ether. Diethyl ether, another ether, was once used as an anesthetic, but its flammability and toxicity caused it to fall out of favor. Smaller ether molecules that are liquids at room temperature are common solvents for organic chemical reactions.<\/p>\r\n\r\n

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Key Takeaways<\/h3>\r\n