1. Matter

2. Intro to Matter
Matter and its Properties

3. Matter is anything that has mass and takes up space
Not matter:

4. What is matter made of?
All matter is composed of tiny particles called atoms.
An atom is the smallest unit of matter that still maintains its properties.
How small is an atom?
Roughly 7.8 x atoms in 1 grain of sand!

5. Properties of Matter
We can classify or sort matter based on its properties and characteristics.
Physical properties are descriptive of the matter and can be observed without changing the identity.
Chemical properties describe the matter’s ability to change into another substance.

6. Physical Properties of Matter
Shape
Color
State (Solid, Liquid, or Gas)
Boiling Point/Melting Point
Texture
Solubility: ability of a substance to dissolve at a given temperature
Temperature
Density: ratio of an object’s mass to its volume
Conductivity: ability to conduct electrical current

7. Chemical Properties of Matter
Flammability: ability to burn
Reactivity: ability to form compounds with other materials
Rust
Tarnish
Corrosion: when a material is “eaten away” by an acid

8. Changing Matter
Physical and Chemical Changes

9. Changing Matter
Physical Change: changes the appearance or form but not the substance itself
Chemical Change: a change that results in the production of a new substance

10. Physical Changes
Tearing
Bending
Crushing
Changing state
Dissolving

11. Chemical Changes
Burning
Rotting
Rusting
Cooking
Tarnishing
Corroding

12. Chemical Changes
Chemical reaction is a change in matter that produces one or more new substances.
Chemical changes occur when bonds (attractions that holds compounds together) break and new bonds form.

13. Clues to Chemical Change
There are a few clues we can look for to see if a chemical change has occurred
fizzing/foaming/bubbling
Change in color
Odor
Formation of a precipitate (solid produced when two liquids are mixed)
Heat or light produced

14. Heat Production/Loss Endothermic: energy is brought into the reaction
Feels cold
Exothermic: energy is released during the reaction
Feels warm

15. Types of Matter
Elements, Compounds, and Mixtures

16. Matter Matter can be classified by its purity.
Element: pure substance made of only 1 type of atom
Gold, silver, oxygen, hydrogen, etc.
Compound: substance made of more than 1 type of atom chemically combined.
Salt, sugar, baking soda
Mixture: substances are mixed together but not chemically combined
Salad, Kool-Aid, cereal

17. Mixtures Mixtures can be broken down into two major groups
Homogeneous: uniform properties and composition
Cannot see the different parts of the mixture
Heterogeneous: physically unique substances with different properties
Different parts of the mixture are clearly visible

18. Mixtures
Three Types of Mixtures:
Solutions
Colloids
Suspensions

19. Solution Particles are too small to be seen Same properties throughout
Examples: kool-aid, salt water

20. 2 Parts of a Solution
Solvent: largest part, dissolves the solute, and can be a solid, liquid, or gas
Water is the “Universal Solvent”
This is because it is the most commonly used solvent
Solute: smallest part, too small to be seen in solution, dissolved by the solvent

21. Colloids Particles are larger than those in a solution
Small, undissolved particles that do not settle to the bottom
Examples: fog, milk, mayonnaise
Tyndall Effect: When a the particles in a colloid scatter light that is shown through it

22. Suspension Has the largest particles
particles can easily be seen and easily separated
do not have the same properties throughout
Examples: sand in water, cereal, soup

23. Solubility

24. Solubility
Ability of one substance to dissolve in another at a given temperature.
It is expressed in terms of the amount of solute that will dissolve in a given amount of solvent to produce a saturated solution
Insolubility is the inability of one substance to dissolve in another substance

25. Solubility
Saturated Solution: solution that contains the maximum amount of dissolved solute
Unsaturated solution: substance that contains less solute than a saturated solution under the same conditions
Supersaturated solution: solution that contains more dissolved solute than a saturated solution under the same conditions

26. Factors that affect Solubility
Temperature
The higher the temperature, the more soluble the solute
sugar in tea
Pressure
If the pressure of a gas solute is higher, more of the solute can be dissolved in the solvent
Ex: CO2 in soda
Agitation
Stirring or shaking will cause the solute to dissolve more rapidly
Surface Area
The greater the surface area, the more rapidly the solute can dissolve
Type of Material
Polar and ionic compounds dissolve in water because water is polar and attracts the charges
Non-polar compounds dissolve non-polar substances

27. Solubility Curves
Solubility curves show how much solute can dissolve in a solvent at a given temperature.
Above the line is supersaturated
On the line is saturated
Below the line is unsaturated

28. Solubility Curve Practice
What is the solubility of KNO3 at 55OC?
A solution is prepared by adding 50 grams of KNO3 to 100 ml of water at 50OC. Is this solution saturated, unsaturated supersaturated?
A solution is prepared by adding 50 grams of KNO3 to 100 ml of water at 30OC. Is this solution saturated, unsaturated, or supersaturated?