1. States of Matter/ Mixtures of Matter
Glencoe: Chapters 3, 13, & 15

2. Matter Anything that has mass and volume
Mass is a measure of the quantity of matter in a sample of any material.
Volume is a measure of the amount of space an object takes up.
Sunlight, ideas, dreams, energy and heat are not matter.
Anything you can see is matter, desk, paper, chair, etc. Including air, you can fill a balloon to see air, it is matter.
Law of Conservation of Mass
Mass is not created nor destroyed during a chemical reaction.

3. The state of matter is the form in which the matter is naturally found based on temperature and pressure.

4. Solids have a definite shape and definite volume
the particles in it are closely packed together
High intramolecular attraction among the particles in the solid (this is why they are close together – they are attracted to each other)

5. Properties of Solids
Have very strong attractive forces between the particles. Limits the motion of particles to mere vibrations.
Most solids are more dense than most liquids, as a result. When the liquid and solid states of such a substance co-exist, the solid almost always sinks in the liquid. There is a 10% difference in density between solid and liquid states of a substance.

6. Liquids takes on shape of container
Indefinite shape and definite volume
form of matter that “flows”
particles are closely packed, but move around more freely than those of a solid.

7. Properties of Liquids
Density of liquids are related to the intermolecular forces that hold particles together.
Liquids can be compressed, though it requires an enormous amount of pressure to do so.
Liquids exhibit fluidity, and can diffuse through another liquid.
Viscosity is a measure of the resistance to flow. The stronger the attractive forces, the higher the viscosity. Inversely related to temperature.

8. Gases
have NO definite shape and NO definite volume (indefinite shape and indefinite volume)
expand to fill container; random organization
easily compressed
particles are very far apart and fast moving
low intramolecular attraction (not attracted to each other – so far apart)

9. Plasma Not found naturally on Earth EXCEPT in lightning bolts.
It is found naturally in the sun and stars.

10. What is a state change
A state change means a substance has changed from one state of matter to another.
Example: Water freezing involves a change from the liquid state of matter to the solid state of matter. We can show this as:
H2O (l)  H2O (s)

11. ALL STATE CHANGES ARE PHYSICAL!
So . . .
Are state changes physical or chemical changes?
PHYSICAL!!
Why?
When the water is in liquid form it is H2O (water). When it is in the solid form as ice, it is STILL H2O (water). The identity of the substance did NOT change!
H2O (l)  H2O (s)
ALL STATE CHANGES ARE PHYSICAL!

12. Elements, Compounds, and Mixtures
Elements – simplest form of pure substance. They cannot be broken into anything else by physical or chemical means. Elements are pure substances. (ex: Cl, H, O, Br, Fe)
Compounds – pure substances that are combined, contains two or more elements. They can be broken into simpler substances by chemical means. (Ex: H2O, NaCl, KBr, etc)
Mixtures – two or more substances that are not chemically combined with each other and can be separated by physical means. The substances in a mixture retain their individual properties.
Solutions – a special kind of mixture where one substance dissolves in another.

13. A mixture is a combination of two or more substances in which each substance retains its individual chemical makeup.
The composition of a mixture is varied, and the number of mixtures that can be created are infinite. Substances naturally tend to mix.

14. Types of Mixtures Homogenous Has a constant composition
Always has a single phase
Also called solutions
Ex: milk, toothpaste, mayonnaise
Heterogeneous
Do not have a constant composition
Individual substances remain distinct
Ex: salad, vegetable soup, granite

15. Alloys- mixtures of metal elements
Stainless steel is a mixture
of iron and chromium.
(iron and at least one other
Element)
Brass is an alloy of copper
and zinc.

16. Types of Solutions Gas-gas: Air (nitrogen, oxygen & hydrogen gases)
Gas-liquid: Carbonated drinks (contain CO2 gas in a solution)
Liquid-gas: Humid air (water droplets in air)
Liquid-liquid: Vinegar (acetic acid in water)
Solid-liquid: Kool-aid (powder drink contains sugar and other solid ingredients in water)
Solid-solid: Steel (alloy of iron containing carbon)

17. Solutions
A solution is a type of homogeneous mixture formed when one substance dissolves in another.
It is the best mixed of all mixtures.
A solution always has a substance that is dissolved and a substance that does the dissolving.
The substance that is dissolved is the solute and the substance that does the dissolving is the solvent.
Water is the universal solvent. (This means it dissolves most things)

18. Heterogeneous Mixtures
Two types of heterogeneous mixtures are colloids and suspensions. They are compared to solutions, which have a particle size of less than one nanometer (1 nm).
Suspensions are mixtures that contain particles that will settle out if left undisturbed.
Colloids are mixtures that do not settle out, but are not solutions because of particle size.

19. Suspensions
Particle size: > 1000 nm
Can be filtered
Examples: cornstarch in water, muddy water, fine sand in water
Colloids
Particle size:
1 nm < X < 1000 nm
Cannot be filtered
Examples: Milk, gemstones, blood, cheese, smoke, deodorant, marshmallow

21. Separating Mixtures
Because the substances in a mixture are physically combined, processes used to separate them vary with the differences in the physical properties of the substances.

22. Filtration
Mixtures composed of solids & liquids can be separated easily by this method.
Uses a porous barrier to separate a solid from a liquid.
Distillation
Most solutions can be separated by this method.
Based on the differences in the boiling points of the substances involved.

23. Crystallization
Separation technique that results in the formation of pure solid precipitate from a solution containing the dissolved substance.
Produces highly pure solids.
Chromatography
Separates components of a mixture on the basis of the tendency of each to travel or be drawn across the surface of another material.