Chemistry 1 - Nomenclature and Writing Chemical Formulae

A collection of vocabulary flashcards covering chemical formula writing, naming rules for ionic and molecular compounds, and nomenclature for acids based on the lecture transcript.

Chemical Formula

A shorthand way of writing the name of a compound; it is a combination of chemical symbols that shows the composition of a compound where the number of atoms of an element is written as a subscript.

Ionic Compounds

Compounds made up of a cation and an anion that are electrically neutral.

Molecular Compounds

Compounds made up of nonmetals.

Crisscross Rule

A method where the charges of ions are interchanged and written as subscripts of the elements in the formula, excluding the signs; the subscript $1$ is not written.

Polyatomic Ions (Radicals)

Groups of atoms that behave as a single unit; parentheses are used to separate them from a subscript when multiple units are present in a formula.

Type II Cations

Metals that form more than one cation with variable oxidation numbers.

Stock System

A naming system for compounds involving Type II cations that uses Roman numerals in parentheses to indicate the oxidation number of the metal.

Traditional System

An older naming system where the suffix $-ic$ indicates the higher oxidation state and the suffix $-ous$ indicates the lower oxidation state.

Mercury (I) Ion

${Hg_2}^{2+}$; these ions are always bound together in pairs.

Ferric

The traditional name for iron (III) or ${Fe}^{3+}$.

Ferrous

The traditional name for iron (II) or ${Fe}^{2+}$.

Stannic

The traditional name for tin (IV) or ${Sn}^{4+}$.

Plumbous

The traditional name for lead (II) or ${Pb}^{2+}$.

Greek Prefixes

Used in naming molecular compounds (two non-metals) to indicate the number of atoms chemically combined, such as mono-, di-, and tri-.

Systematic Nomenclature

A precise way of naming compounds, generally writing the name of the cation first followed by the anion.

Monatomic Anion naming rule

The root word of the element followed by the suffix $-ide$.

Binary Acids (Aqueous)

Acids named using the format: $\text{hydro-}$ + root word + $\text{-ic acid}$ (e.g., $HCl(aq)$ is hydrochloric acid).

Ternary Acids (-ate ending)

Acids formed from polyatomic ions ending in $-ate$; they are named by changing the suffix to $\text{-ic acid}$.

Ternary Acids (-ite ending)

Acids formed from polyatomic ions ending in $-ite$; they are named by changing the suffix to $\text{-ous acid}$.

Ammonium ion

$${NH_4}^{+}$$

Acetate ion

${CH_3COO}^{-}$ or ${C_2H_3O_2}^{-}$

Carbonate ion

$${CO_3}^{2-}$$

Phosphate ion

$${PO_4}^{3-}$$

Permanganate ion

$${MnO_4}^{-}$$

Iron(II,III) oxide

The Stock/IUPAC name for ${Fe_3O_4}$, where iron exists in two oxidation states ($+2$ and $+3$).