3.1 Ionic Compounds and Related Concepts

Vocabulary flashcards covering chemical bonds, types of ions, properties of ionic compounds, periodic trends related to ion formation, the octet rule, and ion naming conventions.

Chemical Bond

An attractive force that holds atoms together, forming due to the interaction of electrons within a molecule (intramolecular bonds).

Ionic Bond

A chemical bond resulting from the transfer of an electron from one atom to another, creating ions of opposite charge which then attract each other.

Covalent Bond

A chemical bond formed through the sharing of electrons between atoms.

Ion

An electrically charged atom or group of atoms, formed when an atom gains or loses an electron.

Cation

An ion with a positive charge, formed when an atom loses one or more electrons, resulting in more protons than electrons.

Anion

An ion with a negative charge, formed when an atom gains one or more electrons, resulting in more electrons than protons.

Ionic Compound

A compound that contains ionic bonds, often referred to as salt or electrolyte, which is overall electrically neutral.

Salt

Another term for an ionic compound, such as NaCl.

Electrolyte

A substance, typically an ionic compound, that conducts electricity when dissolved in water.

Ionization Energy

The energy required to remove one electron from a single atom in the gaseous state; low values indicate an ease of losing electrons to form cations.

Electron Affinity

The energy released when an electron is added to a single atom in the gaseous state; large values indicate atoms gain electrons easily.

Ionic Solid

A crystalline solid held together by ionic bonds, where ions are rigidly held in place but can move freely and conduct electricity when dissolved in water.

Octet Rule

The principle that main group elements tend to undergo reactions that leave them with eight valence electrons, achieving a noble gas configuration.

Main Group Metal Cation Naming (Simple)

Identify the element then add the word 'ion' (e.g., K+ = potassium ion).

Transition Metal Cation Naming (Old System)

The ion with the smaller charge is given the ending -ous, and the ion with the larger charge is given the ending -ic (e.g., Fe2+ = Ferrous ion; Fe3+ = Ferric ion).

Transition Metal Cation Naming (New System)

The charge on the ion is given as a Roman numeral in parentheses right after the metal name (e.g., Fe2+ = Iron(II) ion; Fe3+ = Iron(III) ion).

Anion Naming

Replace the ending of the element name with -ide, followed by the word 'ion' (e.g., Cl- = Chloride ion; O2- = Oxide ion).

Polyatomic Ion

An ion composed of more than one atom, where the atoms are held together by covalent bonds, but the entire group has an overall electrical charge.

Group 1A Cation Charge

For Group 1A metals, the cation charge equals the group number (+1).

Group 2A Cation Charge

For Group 2A metals, the cation charge equals the group number (+2).

Group 3A Cation Charge

For Group 3A metals, the cation charge equals the group number (+3).

Group 6A Anion Charge

For Group 6A nonmetals, the anion charge equals 8 minus the group number (-2).

Group 7A Anion Charge

For Group 7A nonmetals (halogens), the anion charge equals 8 minus the group number (-1).

Transition Metal Ion Formation

Transition metals form cations by losing one or more s electrons and sometimes inner-shell d electrons, and often do not follow the octet rule.