Chemical compound: Difference between revisions
imported>Aleksander Stos m (WP credit) |
imported>Robert Winmill m (Fix disambiguation solid) |
||
| Line 17: | Line 17: | ||
==Phases and thermal properties== | ==Phases and thermal properties== | ||
Compounds may have a number of possible [[phases of matter|phases]]. All compounds can exist as [[ | Compounds may have a number of possible [[phases of matter|phases]]. All compounds can exist as [[Solid (state of matter)|Solid]]s, at least at low enough temperatures. [[Molecular compound]]s may also exist as [[liquid]]s, [[gas]]es, and, in some cases, even [[plasma]]s. All compounds decompose upon applying [[heat]]. The [[temperature]] at which such fragmentation occurs is often called the [[decomposition temperature]]. Decomposition temperatures are not sharp and depend on the rate of heating. At sufficiently high temperatures, all compounds, either after they have decomposed somehow or in the act of decomposing, fragment into smaller compounds or to individual [[atom]]s. | ||
==CAS number== | ==CAS number== | ||
Revision as of 18:18, 27 April 2007
A chemical compound is a chemical substance consisting of two or more chemically bonded chemical elements, with a fixed ratio determining the composition. The ratio of each element is usually expressed by chemical formula. For example, water (H2O) is a compound consisting of two hydrogen atoms bonded to every oxygen atom.
The atoms within a compound can held together by a variety of interactions, ranging from covalent bonds to electrostatic forces in ionic bonds. A continuum of bond polarities exist between the purely covalent bond as in H2 and in benzene C6H6. For example H2O is held together by polar covalent bonds. Sodium chloride is an example of an ionic compound.
Molecules vs. compounds
Many compounds are molecular, i.e. composed of molecules. When molecular compounds are crystallized (converted to a solid), the individual molecules interact - or are held together - by van der Waals forces. Most known compounds are molecular, a fact that is attributable to the scope of organic chemistry.
Salts are an important family of compounds, but few are molecular. Molecules of NaCl do not exist.
And of course, intermediate classes of compounds exist, which feature polar covalent bonds. Hydrogen fluoride is one example.
Many compounds have both a covalent and an ionic subunits. The molecule trifluoroacetic acid, CF3CO2H is composed of a covalent CF3CO2 ensemble. The H atom is attached to one oxygen through a polar covalent bond.
Formulas
Chemists describe compounds using formula in various formats. For molecules, the formula for the molecular unit is shown. For polymeric materials, such as minerals and many metal oxides, the empirical formula is given, e.g. NaCl. The order of the elements in molecular and empirical formulas is C, then H and then alphabetical. Trifluoroacetic acid is thus described as C2HF3O2. More descriptive formulas convey structure information, illustrated again with trifluoroacetic acid. CF3CO2H. On the other hand, formulas for inorganic compounds often do not convey structural information, as illustrated by sulfuric acid, H2SO4 for a molecule that has no H-S bonds. A more descriptive presentation would be O2S(OH)2.
Phases and thermal properties
Compounds may have a number of possible phases. All compounds can exist as Solids, at least at low enough temperatures. Molecular compounds may also exist as liquids, gases, and, in some cases, even plasmas. All compounds decompose upon applying heat. The temperature at which such fragmentation occurs is often called the decomposition temperature. Decomposition temperatures are not sharp and depend on the rate of heating. At sufficiently high temperatures, all compounds, either after they have decomposed somehow or in the act of decomposing, fragment into smaller compounds or to individual atoms.
CAS number
Every chemical compound that has been described in the literature carries a unique numerical identifier, its CAS number.