Naming Ionic Compounds

Ionic compounds are solids composed of positive ions (cations) and negative ions (anions) held by electrostatic attraction.
Formulas list the cation followed by the anion.
Compounds are electrically neutral; the sum of positive and negative charges in a formula unit must equal zero.

Binary compounds contains ions from only two different elements: a metal and a nonmetal.
Rule: Name the metal cation followed by the nonmetal anion with the suffix modified to "-ide".
Examples: - $NaCl$ : sodium chloride - $CaCl_2$ : calcium chloride - $CsBr$ : cesium bromide

Transition metals and certain other elements can form ions with multiple possible charges (e.g., $Fe^{2+}$ and $Fe^{3+}$ ).
A Roman numeral in parentheses must follow the cation name to indicate its specific charge.
The charge of the metal is calculated based on the known charge of the anion to ensure a neutral formula unit.
Examples: - $FeBr_3$ : iron (III) bromide (Three $Br^-$ at $-1$ each requires an $Fe^{3+}$ ion). - $TiCl_4$ : titanium (IV) chloride (Four $Cl^-$ at $-1$ each requires a $Ti^{4+}$ ion).

Prompt: "you try n a two o"
Response: Sodium is the cation and oxide is the anion; the name is sodium oxide ( $Na_2O$ ).
Prompt: "You try. Six, MnF two"
Response: The compound contains two fluoride ions ( $F^-$ ), each with a $-1$ charge. To maintain electrical neutrality, the manganese ion must have a charge of $+2$ . The name is manganese (II) fluoride ( $MnF_2$ ).