Naming Ionic and Covalent Compounds

Comprehensive vocabulary and rules flashcards covering the naming of binary ionic compounds, transition metals, polyatomic ions, and covalent compounds based on the lecture notes.

Mn

Manganese

K

Potassium

Hg

Mercury

Ca

Calcium

Be

Beryllium

NaCl

Sodium chloride

$$NaHCO_{3}$$

Sodium bicarbonate

Cation ($+$)

An ion that loses electrons; usually metals.

Anion ($-$)

An ion that gains electrons; usually nonmetals.

Ionic compounds

Compounds formed by the attraction between a positive ion and a negative ion, usually consisting of a metal and a nonmetal or a metal and a polyatomic ion, with an overall neutral charge.

Rule 1 (Binary Ionic Compounds)

Write the name of the metal first; the cation keeps its element name (e.g., $Na \rightarrow$ Sodium).

Rule 2 (Binary Ionic Compounds)

Name the anion second and change the ending of the nonmetal to -ide (e.g., Chlorine $\rightarrow$ chloride).

Rule 3 (Transition Metals)

Transition metals (Groups 3-12) need Roman numerals to indicate their charge because some can have more than one charge (e.g., $FeCl_{2}$ is Iron(II) chloride).

Exception: Silver ($Ag$)

A transition metal that does not need a Roman numeral because its charge is always $+1$.

Exception: Zinc ($Zn$)

A transition metal that does not need a Roman numeral because its charge is always $+2$.

Exception: Cadmium ($Cd$)

A transition metal that does not need a Roman numeral because its charge is always $+2$.

Exception: Scandium ($Sc$)

A transition metal that does not need a Roman numeral because its charge is always $+3$.

Exception: Yttrium ($Y$)

A transition metal that does not need a Roman numeral because its charge is always $+3$.

Polyatomic ions

Covalently bonded groups of two or more atoms that act as a single charged unit.

Ammonium

A polyatomic cation with the formula $NH_{4}^{+}$.

Hydroxide

A polyatomic anion with the formula $OH^{-}$.

Nitrate

A polyatomic anion with the formula $NO_{3}^{-}$.

Carbonate

A polyatomic anion with the formula $CO_{3}^{2-}$ and a charge of $-2$.

Sulfate

A polyatomic anion with the formula $SO_{4}^{2-}$.

Rule 4 (Polyatomic Ions)

Keep the polyatomic ion name and do NOT change the ending (e.g., $NaNO_{3}$ is Sodium nitrate).

Covalent compounds

Compounds formed when two nonmetals share electrons, also known as molecular compounds.

Characteristics of Covalent Compounds

Composed of nonmetals only, share electrons, usually gases, liquids, or soft solids, have lower melting/boiling points than ionic compounds, and are poor conductors of electricity.

Prefix: Mono-

Greek prefix for 1 atom.

Prefix: Di-

Greek prefix for 2 atoms.

Prefix: Tri-

Greek prefix for 3 atoms.

Prefix: Tetra-

Greek prefix for 4 atoms.

Prefix: Penta-

Greek prefix for 5 atoms.

Prefix: Hexa-

Greek prefix for 6 atoms.

Prefix: Hepta-

Greek prefix for 7 atoms.

Prefix: Octa-

Greek prefix for 8 atoms.

Prefix: Nona-

Greek prefix for 9 atoms.

Prefix: Deca-

Greek prefix for 10 atoms.

Rule 1 & 2 (Covalent Compounds)

Name the first element and use a prefix only if there are two or more atoms.

Rule 3 & 4 (Covalent Compounds)

ALWAYS use a prefix for the second element and change its ending to -ide.

Rule 5 (Covalent Compounds)

Do NOT use 'mono-' for the first element (e.g., Carbon monoxide, not monocarbon monoxide).

Rule 6 (Covalent Compounds)

Drop the last vowel of the prefix when followed by another vowel (e.g., Mono + oxide becomes monoxide).