Chapter 2: Ionic and Molecular Compounds

This set of vocabulary flashcards covers the fundamental definitions, naming conventions, and charge characteristics of ionic and molecular compounds as discussed in the General Chemistry 1 lecture.

Ionic Compound

A compound formed between metals and non-metals, wherein the metal serves as a cation and the non-metal serves as an anion.

Molecular Compound

Also referred to as a covalent compound, it is formed between two nonmetals or between a nonmetal and a metalloid.

Cation

A positively charged ion, typically formed by metals.

Anion

A negatively charged ion, typically formed by nonmetals.

Representative Elements

Elements found in Group 1 through Group 8 (specifically Group 1 through Group 7 for the context of this lecture) that form specific charges based on their group.

Transition Metal

Elements located between Group 2 and Group 3 that have the ability to form more than one kind of cation charge state.

Group 1 Charge

Representative metals in this group form a $+1$ cation.

Group 2 Charge

Representative metals in this group form a $+2$ cation.

Group 3 Charge

Representative metals in this group form a $+3$ cation.

Group 5 Charge

Nonmetals in this group form a $-3$ anion.

Group 6 Charge

Nonmetals in this group form a $-2$ anion.

Group 7 Charge

Nonmetals in this group form a $-1$ anion.

Empirical Formula

The simplest formula of a compound where the ratio of components cannot be reduced further; a requirement for ionic formula units.

Ionic Formula Requirement (Charge)

The sum of the charges on the cations and the anions in each formula unit must equal zero.

Polyatomic Ion

An ion consisting of multiple atoms that functions as a single charged unit, such as Nitrate $NO_3^-$ or Carbonate $CO_3^{2-}$.

Monoatomic Ion

An ion consisting of a single atom, such as Sodium $Na^+$ or Chlorine $Cl^-$.

Stokes System

A naming system for transition metal ionic compounds that requires the use of Roman numerals to indicate the charge state of the cation.

-ide suffix

The ending added to the base name of a nonmetal when naming an ionic or simple molecular compound (e.g., Chlorine becomes Chloride).

Parentheses (in formulas)

Used in chemical formulas to indicate that a subscript applies to all elements within a polyatomic ion.

Molecular Prefixes

Terms like mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, and deca- used to indicate the number of each kind of atom in a molecular compound.

Dinitrogen Monoxide

The chemical name for the molecular compound $N_2O$, demonstrating the use of prefixes for both elements when the first has a subscript.