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A chemical formula describes a chemical compound by identifying its constituent elements using chemical symbols and indicating the number of atoms or ions of each element through subscript numbers. For example, sucrose (C12H22O11) shows it contains carbon, hydrogen, and oxygen atoms in specific proportions. This notation allows chemists to communicate compound composition accurately and concisely.

A molecular formula shows the exact number of atoms of each element in a molecule, such as glucose (C6H12O6). An empirical formula displays the simplest whole-number ratio of atoms, so glucose's empirical formula is CH2O. The molecular formula is always a whole-number multiple of the empirical formula; multiplying CH2O by six yields C6H12O6.

A structural formula graphically represents how atoms are connected in a molecule using chemical symbols and lines to denote bonds. Single, double, and triple lines represent single, double, and triple bonds respectively. Extended models like ball-and-stick and space-filling models provide three-dimensional perspectives of molecular shape, offering more detailed information than molecular or empirical formulas alone.

Elements in chemical formulas are arranged by electronegativity rather than alphabetically, with more positively charged or metallic elements listed first, followed by more negatively charged or nonmetallic elements. For example, potassium hydroxide is written KOH, not HKO or OHK. This convention ensures consistent, standardized representation across chemistry.

H2 is a molecular formula representing a diatomic hydrogen molecule with two atoms chemically bonded together. In contrast, 2H indicates two separate, unbound hydrogen atoms. The expression 2H2 represents two distinct diatomic hydrogen molecules. Understanding this distinction is critical for accurately interpreting chemical formulas and reactions.

The molecular formula is derived by multiplying the empirical formula by a whole number determined from experimental measurements of molecular mass. For benzene, the empirical formula CH is multiplied by six (based on its molecular mass) to yield the molecular formula C6H6. This process requires experimental determination of both empirical formula and molecular mass.

The structural formula provides the most information, revealing both atomic composition and three-dimensional molecular geometry through graphical representation of bonds and atomic arrangement. The molecular formula ranks second in informativeness, showing exact atom counts. The empirical formula is least informative, displaying only the simplest whole-number ratio of atoms present.