CPC 6.2 Ionic Compounds

Compounds are physical combinations

Compounds are chemical combinations of elements

Compounds are always liquids

Compounds are made of identical atoms

Covalent bond

Metallic bond

Ionic bond

Hydrogen bond

Salts

Acids

Oxides

Bases

Acids

Bases

Salts

Oxides

Two metallic cations

A metallic cation and a nonmetallic anion

Two nonmetallic anions

A metallic anion and a nonmetallic cation

Compounds contain three different elements

Compounds contain only one element

Compounds contain only two different elements

Compounds contain four different elements

Water (H₂O)

Carbon dioxide (CO₂)

Calcium Oxide (CaO)

Ammonia (NH₃)

The size of the ions

The number of protons

The number of electrons transferred

The temperature of the environment

Randomly scattered

In a regular repeating pattern

In a linear sequence

In a circular formation

Weak attractions among ions

Strong attractions among ions

Random arrangement of ions

Low Melting and Boiling Points

A two-dimensional geometric arrangement

A random arrangement of particles

A three-dimensional geometric arrangement of particles

A single layer of ions

The color of the compound

The size of the ions

The strength of electrical forces between particles

The shape of the crystal lattice

Because they are made of small particles

Because ionic bonds are relatively weak

Because ionic bonds are relatively strong

Because they have a low density

Soft, but hard to break

Hard, rigid, brittle

Malleable and ductile

Elastic and flexible

Due to weak magnetic forces

Due to strong attraction between electric charges

Due to gravitational forces

Due to weak chemical bonds

They become more flexible

They melt

They break

They expand

Freely moving charged particles

The color of the material

The temperature of the material

Strength of ionic bonds in the material

Ions are locked in position by strong attractive forces

Ions are free to move

They have a high melting and boiling points

Ionic solids are too small to adequately conduct

In solution or a liquid state

In a crystal or solid state

In a gaseous state

In a plasma state

Electrolyte

Insulator

Conductor

Semiconductor

KCl

Ethanol

Acetic acid solution

Water

Exothermic

Endothermic

Ionic

Combustion

Endothermic

Exothermic

Neutralization

Decomposition

Endothermic

Exothermic

Neutral

Reversible

It increases

It decreases

It remains the same

It fluctuates

Bond energy

Lattice energy

Activation energy

Ionization energy

It decreases

It remains the same

It becomes weaker

It becomes stronger

Exothermic reaction

Endothermic reaction

Neutral reaction

Spontaneous reaction

Larger ions have greater lattice energy.

Smaller ions have greater lattice energy.

Ion size does not affect lattice energy.

Lattice energy is only related to charge.

It decreases.

It remains the same.

It increases.

It becomes zero.

They decrease lattice energy.

They have no effect on lattice energy.

They increase lattice energy.

They make the bond weaker.

Na+

Cl-

Br-

K+

Na+ and Cl-

K+ and Br-

Na+ and Br-

K+ and Cl-

Magnesium oxide

Sodium chloride

Water

Barium sulfate

H₂O

C₆H₁₂O₆

NaCl

Be₃Al₂Si₆O₁₈

a mineral deposit

an ionic molecule

a salt crystal

a crystal lattice

Ionic crystals require a large amount of energy to be broken.

Ionic crystals have low melting points and high boiling points.

Ionic crystals are malleable, not brittle.

Ionic crystals conduct electricity in solid or liquid form, but not gas.

Lattice energy is the energy needed for 1 mol of positive ions to bond with 1 mol of negative ions.

Ions in an ionic compound are arranged in a random pattern.

Ionic compounds are never electrolytes.

Ionic compound properties are related to ionic bonding.