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Chapter 12

Liquids, Solids, and attraction between molecules.

The states of matter: Solid, Liquid, and Gas.

Gas: no fixed shape and no fixed volume

Liquid: fixed shape, no fixed volume

Solid: fixed shape, fixed volume

Changes in states of matter upon changing temperature

 

Types of solids:

Crystalline

Amorphous

 

 Amorphous structure:

Disordered arrangement of structural units with not well-defined structural parameters (bond angle).

Example: Glass

Types of crystalline solid:

Atomic solid

Metallic solid

Covalent network solid

Molecular solid

Ionic solid

Crystalline solid:

Chapter 13

Solutions

Homogeneous solution: a mixture of two or more substances giving one phase (layer).

All the substances should dissolve.

Solute, Solvent, Solution

Solute + Solvent = Solution

Concentration

Concentration: the amount of solute (moles or grams) dissolved in a given amount of solution or solvent at a given temperature.

Example: the concentration of KCl is 36.7 g/ L.

There are 36.7 g KCl in 1 liter of solution.

Molarity = M : moles of solute in 1 L. solution

Chapter 14

Reaction rates and Chemical equilibrium

Reaction rates

How fast the chemical reaction is occurring.

Or the length of time for proceeding the chemical reaction

To study the rate of reaction:

Types of reactants

Concentration of reactants

Temperature

Pressure if the reactants are in gas state.

Catalyst

Reaction rate:

Collision theory and activation energy

The reaction between molecules can occur if the molecules come together or a collision between reactant molecules can be taken place.

The collisions need to have enough energy (activation energy) to break the chemical bonds.

Chemical equilibrium

 

                   forward

Reactants   ========   Product      

                   Reverse

 At equilibrium:

 

Rate of forward reaction = rate of reverse reaction

 

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