Ionic Bonds

Force that holds two atoms together

How easy an atom loses it's electron

How much attraction the atom has for it's electron

Valence electrons

So they can acquire a stable 8 electron structure in their outermost layer

• Noble Gases
• Because they are already chemically stable because they have a full outermost shell

A positively charged ion

A negatively charge ion

-ide

Force that holds oppositely charged particles together in an ionic compound

Compounds that contain ionic bonds

• Binary
• Meaning they contain only two different elements

A metallic cation and a nonmetallic anion

• Structure of alternating cations and anions
• Large numbers of ions together in ratio according to how many electrons needed to be transfered
• Vary in shape according to the size and relative numbers of the ions bonded

• 3-D geometric arrangement of particles
• Each anion is surrounded by cations and visa versa

• High melting and boiling point
• Hard
• Rigid
• Brittle
• Bad conductors of electricity in solid state
• Conductors of electricity in aqueous state

When energy is absorbed during a chemical reaction

• When energy is released during a chemical reaction
• Formation of ionic compounds from positive and negative ions

Individual ions have more energy because ions that are bonded are more stable

If the amount of energy released during bond formation is added to the ionic compound, the bond breaks

The energy required to separate one mole of the ions of an ionic compound

• Size: smaller ions have higher lattice energy
• Charge of the ion: ionic bond formed by ions with a larger positive or negative charges have higher lattice energy

The simplest ratio of the ions represented in an ionic compound

A one-atom ion

Is the charge of a monatomic ion

Ions made up of more than one atom