Lesson 6.2: Ionic Bonding

A complete set of vocabulary flashcards covering the formation, structure, properties, and naming of ionic compounds based on the Year 9 Bonding unit notes.

Ion

An atom or group of atoms with an electrical charge due to the loss or gain of electrons.

Cation

A positively charged ion formed when an atom loses electrons.

Anion

A negatively charged ion formed when an atom gains electrons.

Metal behavior in bonding

Metals achieve stability by losing electrons to form positive ions (cations).

Non-metal behavior in bonding

Non-metals achieve stability by gaining electrons to form negative ions (anions).

Sodium ion formation equation

$$Na \rightarrow Na^+ + e^-$$

Chlorine ion formation equation

$$Cl + e^- \rightarrow Cl^-$$

Ionic bond

The strong electrostatic attraction between oppositely charged ions.

Crystal lattice

A regular, repeating three-dimensional arrangement where each positive ion is surrounded by negative ions and vice versa.

Sodium chloride melting point

Approximately $801\,^{\circ}C$.

Chemical formula of Sulfide Example

$Na_2S$, where two sodium ions are needed to balance one sulfide ion.

Chemical formula

A representation showing the simplest whole-number ratio of ions in a compound, which must have no overall charge.

Naming Rule 1

Name the metal first and the non-metal second.

Naming Rule 2

Change the ending of the non-metal to $-ide$ (e.g., sodium chloride).

Brittleness in ionic compounds

When the crystal shifts, like charges line up and the resulting repulsion causes the crystal to shatter.

Solubility in water

Many ionic compounds dissolve because water is a polar molecule that attracts ions and breaks the crystal lattice apart.

Dissociation

The process by which an ionic compound separates into ions when dissolved in water.

Electrical conductivity (Solid)

Solid ionic compounds do not conduct electricity because the ions are fixed in place and cannot move.

Electrical conductivity (Molten/Solution)

Molten or dissolved ionic compounds conduct electricity because the ions are free to move and carry electrical charge.

Polar molecule

A molecule with a slightly positive end and a slightly negative end, such as water.

Valence electrons

Electrons in the outermost shell of an atom that are involved in bonding.

Electrostatic attraction

The attractive force between oppositely charged ions.