2.1: Classifications of Matter
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Matter is anything that has mass and volume. Nearly everything within the known universe, from water, to a fish, to the planets, is composed of matter. It may seem beneficial to have one vocabulary term to describe every substance that exists. However, each of these "things" has its own distinct characteristics and, therefore, can be classified using more specific terminology. Matter can be classified as either a pure substance or a mixture, based on its composition.
Pure Substances
A pure substance is a form of matter that has a definite composition. Furthermore, the physical properties, such as color, shine, density, and melting point, of a pure substance must be consistent throughout the entire sample. Pure substances can be categorized as either elements or compounds.
Elements
An element consists of only one type of atom and cannot be broken down into smaller pieces without changing its properties. Aluminum, which is found in soda cans, is an element. Helium, which is used to inflate balloons, is also an element. Carbon is an element that is essential to life on earth, as it is found in all living systems. "Aluminum," "helium," and "carbon" are all examples of elemental names. While many elemental names are short and (relatively) easy to spell, some, like "praseodymium" or "darmstadtium" are quite long and complex. Therefore, every elemental name has a corresponding abbreviation, called an elemental symbol. As was the case with the physical properties of chemistry that were defined in the previous chapter, specific rules must be followed when writing elemental symbols. While a complete elemental name can be written with its first letter being either capitalized or lower-case, the first letter in an elemental symbol must be capitalized, and any additional letters must be lower-case. Finally, note that some elemental symbols do not seem to match with their elemental name. These seemingly-mismatched elemental symbols actually correspond to a Greek or Latin word that can be used to describe the element. For example, "Hg" is the elemental symbol for the element named "mercury," which contains neither an "h" nor an "g" in its spelling! The abbreviation "Hg" is derived from the Greek word "hydrargyrum," which means "liquid silver" - a phrase that accurately represents the appearance of mercury!
Compounds
A compound or molecule must contain two or more elements that are combined in a specific ratio. Much like elements, each compound has a corresponding chemical name, which can be abbreviated using a chemical formula. The derivation of chemical formulas and chemical names will be the focus of the following chapter. A few simple examples will be mentioned here. "Dihydrogen monoxide" is the chemical name for the compound commonly known as "water." The chemical formula for this incredibly important substance is "H2O". Note that chemical names consist of words that resemble elemental names, and chemical formulas contain elemental symbols. The chemical formula for water contains an "H," which is the elemental symbol for "hydrogen," and an "O," which is the elemental symbol for "oxygen." Whole-number subscripts indicate how many of the previous element are present in the compound. If no subscript is written, an unwritten "1" is understood, as was the case for several of the numerical quantities that were discussed in the previous chapter. Therefore, water contains two hydrogens for every one oxygen.
Changing either the elements that are present or their ratio changes the identity of the compound and, therefore, its properties. For example, water (H2O) is used to extinguish fires, but dihydrogen sulfide (H2S) is highly flammable! Both of these chemicals contain two hydrogens, but exchanging the oxygen for a sulfur results in a chemical that behaves very differently. While water contains two hydrogens for every one oxygen, hydrogen peroxide (H2O2) contains a two-to-two ratio of hydrogen to oxygen. Again, the properties of these chemicals are very different: Water is safe to drink, but hydrogen peroxide, which is commonly used as a mild antiseptic, is definitely not!
Mixtures
A mixture is a blend of two or more elements or compounds, which have their own identities and properties. Mixtures, which can be homogeneous or heterogeneous, can be separated into their individual components because the substances are not chemically-connected or bonded to one another.
Homogeneous Mixtures
A homogeneous mixture has a uniform composition, meaning that if several samples are taken, each would contain the same chemicals in approximately the same ratio. Salt water is an example of a homogeneous mixture, as it contains two distinctive chemicals, a "salt," which is most likely sodium chloride, NaCl, and water, H2O. These compounds can be separated by boiling the water, leaving the salt as a residue. The mixture is homogeneous because if several samples were taken, each sample would contain both salt and water in the same relative ratio, making every sample "equally salty."
Heterogeneous Mixtures
A heterogeneous mixture has a non-uniform composition, meaning that if several samples are taken, each would contain either completely different chemicals or the same chemicals, but in different ratios. A chocolate chip cookie is a heterogeneous mixture, because it contains many different chemicals that form the cookie dough and the chocolate chips, which can be separated by pulling out the chips. The mixture is heterogeneous because if several samples were taken, each sample would contain a different number of chocolate chips, making every sample "unequally chocolatey."
Summary
The vocabulary discussed in this section is summarized below in Figure \(\PageIndex{1}\). This image also includes simple "yes-or-no" tests that can be used to help distinguish a pure substance from a mixture, an element from a compound, and a homogeneous mixture from a heterogeneous mixture.
