(also written as) is the formula for the acetate ion. Most polyatomic ions tend to follow certain naming trends, but acetate is one of the ions that does not follow those naming trends, so memorize this one since it shows up frequently in chemistry.

The alcohol functional group is -OH

We know that by definition, all amino acids contain a carboxylic acid functional group (), and an amino functional group (). Therefore the additional functional group canonlycontain sulfur and hydrogen.

氨基官能团有点基础,the carboylic acid functional group is slightly acidic. The -SH functional group will also be acidic, but because sulfur and oxygen are in the same group on the periodic table, the -SH group will have similar acidic properties to an -OH group, and alcohols are less acidic than carboxylic acids.

Amides contain both oxygen and nitrogen in the functional group. The oxygen forms a double bond with a carbon, and the carbon bonds to a nitrogen. This forms the structure, where the nitrogen is also bound to the carbon.

is an alcohol functional group.

is an amine functional group.

is a carboxylic acid functional group.

is an aldehyde functional group.

A nitrile group contains a carbon-nitrogen triple bond, while all of the other groups contain a carbon-oxygen double bond.

Nitrile:

Ester:

Ketone:

Carboxylic acid:

Aldehyde:

An organic compound is typically defined as one that contains carbon. Though there some small exceptions to this rule (for example, cyanide is not considered organic), in general most compounds follow it.

Though water, oxygen, and sodium chloride, may seem organic, they are not for they do not contain any covalent bonds to carbon. The only gievn compound that contains carbon is glucose, a sugar.

The simplest way to begin these types of problems is to assume that we are starting out with 100 grams of the sample compound. This allows us to simplify things, since we know the mass percentages of the elements that make up out unknown compound.

Next, we must convert amount of each element from grams into moles.

This gives us a formula of

Now, we need to simplify this formula by dividing each of the terms by the greatest common denominator, 3.33, which gives us:

This is our empirical formula. To obtain the molecular formula, we must first find the mass of our empirical formula, which is.

Next, we need to divide the molecular weight of the compound by the empirical weight to obtain an integer of. Finally, we multiply the empirical formula by this integer in order to obtain the molecular formula, which is: