What is Matter? Anything that takes up space (volume) and has mass. Anything on EARTH.

What is Matter? Anything that

takes up space (volume) and has mass.

Anything on EARTH.

Types of Matter Homogeneous

Matter that is made up of the same or alike particles.

SAME THROUGHOUT Can’t see the particle

HeterogeneousMatter that is

made up of different types of particles.

DIFFERENT THROUGHOUT

Can see the particles

Homogeneous Materials

Kool aidTeaClear sodasRubbing alcoholWaterElementsCompoundsAcids

Heterogeneous Materials

CerealSaladSnack mixKabobsItalian dressingsUncooked pizzaM & M’sSkittlesVegetable soupMilk

Now it is your turn… you tell me:

Homogeneous or Heterogeneous Flat soda pop

Cherry vanilla ice cream Sugar (C2H3O2)

Salt (NaCl) City Air Iron (Fe) Beach Sand Spaghetti Sauce

Mixtures vs. Pure Substances MIXTURES

Heterogeneous or Homogeneous

Easily separated

EXAMPLES

Any Heterogeneous or homogeneous examples

PURE SUBSTANCESHomogeneousHard to separateIn it simplest form

EXAMPLES

Elements and compounds

Types of Pure

Substances Elements: Purest

substance known that can’t be broken downNeon: Ne

Compounds: 2 or more elements chemically combinedWater: H2O

Atoms are the counting units or quantity of the

element.

Properties of Mixtures

Easily separated Physically combined to

easily separate. Amounts vary when

mixed Changes only in

physical appearance when dissolved.

Types of Mixtures

Heterogeneous Mixtures

SuspensionsColloids

Homogeneous Mixtures

Solutions

Solution

Homogeneous Mixture: Same throughout

Examples: Ice teaSugar waterKool aidSprite

Solutions and Its Properties Particles are individual atoms,

molecules, or ions (charged particles)

Clear Can’t be filtered Particles are evenly spread out Can’t see the particles Homogeneous

Parts of a Solution Solute – Part being

dissolved in the solvent.ex: Sugar, Hot Chocolate, Salt

Solvent – Part that does the dissolving.ex: Water – universal solvent

Aqueous vs. Tincture Solution Aqueous – water

is the solvent

Tincture – alcohol is the solvent

Combinations of Solutions

SOLUTES

1. Solid

2. Solid

3. Solid

SOLVENT

Solid

Liquid

Gas

EXAMPLES

Alloy (pots)

Sea water

Soot in air

4. Liquid

5. Liquid

6. Liquid

Solid

Liquid

gas

Dental fillings

Antifreeze

Humid air

7. Gas

8. Gas

9. Gas

Solid

Liquid

Gas

Gas mask

Sodas

Air

Special Activities of Solutions

Dissociation – splitting ions to form charges

Ionization – gaining or losing electrons to form ions

Electrolyte – Solution that produce electricity(Salt and Water)

Non-electrolyte – solution that does not produce electricity (Sugar and Water)

Special Solutions Miscible – when a liquid is dissolved

into a liquid Example: Antifreeze, alcohol and water

Alloy – when a solid is dissolved into a solidExamples: Stainless steel pots and

pans, bronze, brass, jewelry

Rates of Solutions (how to speed up a solution)

Stirring Heating Powdering-

increasing the surface area

Solubility and Its Factors Solubility – ability of a solute to

dissolve into a solvent. Factors that affect solubility of a gas in a

solution Temperature – decreasing temperaturePressure – increasing pressure

Dilute vs. Concentrated

Dilute – weak solution

“watered down”

ConcentratedStrong solution

Levels of Solutions

Saturated – Holding as much solute at a given temperature

Supersaturated – UNSTABLE – more solute in the solvent at a high temp.

Colloid Properties

Heterogeneous Mixture

Can’t see particles Particle size is larger

than those in solutions

Scatters light – Tyndall Effect

Examples of Colloids Fog- clouds Smoke- smoke Foam- whipped

cream Emulsion-

mayonnaise Sol- paints Gel- butter

Suspension Properties

Heterogeneous Mixture

Can see the particles Easily separated EXAMPLES

waste

oil and water

trail mix

eggs

cereals

Ways to Separate Mixtures Filtering – Suspensions

Evaporation – Solution, Colloids, Suspensions

Distillation – Solutions, Colloids, Suspensions

Chromatography - Solutions

Physical Properties and Changes Physical Properties

Characteristic you can observe without changing the substance

Examples:○ Appearance: color, shape, …○ Measurements: mass, length,

volume…○ Behavior: attracted by magnet,

soluble…○ Changes of State: melting point,

boiling point…

Physical Changes Change made to material

that does not change the substances

Usually, the change can be reversed Examples:

○ Tearing, shredding crushing…○ Boiling, melting, freezing…○ Dissolving

Chemical Properties

Characteristic of a substance that undergoes a certain chemical changeExamples:

○ Flammability or combustibility○ Reactivity

Chemical Change Change of one substance in a

material to a different substance Usually the change can’t be

reversed Signs of a chemical change:

SmellColorFoaming or gas productionPrecipitate – solid forming when two items

are mixed togetherLight or explosion (release of energy)

Examples: rusting, burning, …

Law of Conservation of Mass Matter is neither created nor destroyed

during a chemical change or physical change

original mass = final mass