1. Happy Tuesday!
VIP Word: Proton When you’re finished… Take out a piece of paper Write your name Put everything else away Get ready… Pop Quiz! 

2. *Pop* Quiz Draw and label an atom and its subatomic particles.
Underneath each labelled subatomic particle be sure to include: -The Charge -The Mass -The Location

3. *Pop* Quiz Answers

4. Physical Properties of Matter Notes

5. What is a physical property?
Characteristics of a specific substance that can be observed without changing the substance

6. Which physical properties are dependent on the amount of the sample?
Volume
The amount of space an object occupies
Liter
Graduated cylinder
Mass
The amount of matter in an object
Gram
balance
Weight
Measure of the force of gravity pushing on an object
Newton
Spring scale

7. How do you find the volume of an irregular object?
Water Displacement.
Measure the amount of water in a graduated cylinder and record
Drop the object into the graduated cylinder
Record the final volume
Final volume – initial volume= volume of object

8. How are mass and weight different?
Weight- a measure of the force of gravity acting on the mass of the object.
Unit- Newtons
Measured using a Spring Scale
Mass- the amount of matter in an object
Unit- grams
Measured using a triple beam balance
*Mass does not change with location and does not depend on the force of gravity at a given location.

9. Which physical properties are independent of the amount of matter present?
Melting point
The temperature at which a substance melts or freezes
Boiling point
The temperature at which a substance vaporizes or condenses
Density
Solubility

10. What is Density?
the mass (in grams) per unit volume (cubic centimeters or cm3) of a substance
Determined by:
The distance between the particles
The mass of the particles

11. They have the same density!
Why? How?

12. States of matter
Most dense: solids Liquids Least dense: gases

13. What is the density of water?
The density of water is 1 g/cm3.
A substance which is not soluble in water will float in water if its density is less than 1g/cm3.

14. How do you calculate density?
Density is found by dividing mass by volume.
D= m/v
The units for density are g/cm3
These are derived units 

15. What is a mixture?
Consists of two or more substances that are NOT chemically combined (no chemical change has occurred)
Homogeneous: looks the same throughout
Heterogeneous: different components of mixture can easily be seen
Mixtures are examples of a physical change
The contents of a mixture can be separated

16. What Is A Compound?
A compound is a pure substance that is created by 2 or more elements chemically reacting and joining together
Ex: NaCl, H2O, CO2, NH3, NaHCO3, and C6H12O6
Notice that elements combine in many ways to make compounds
Ex: H2O, H2O2, CO, and CO2
This section was left off of your notes sheet. Add this in. Sorry, yal!

17. Why Do Compounds Form?
Compounds form to allow elements to become more stable
Na is flammable when it comes in contact with H2O, and Cl2 is a toxic gas
NaCl is a very stable compound that is neither flammable nor toxic (in normal quantities)
Compounds that are extremely unstable will break down to form the more stable elements
This section was left off of your notes sheet. Add this in. Sorry, yal!

18. How Do Compounds Form?
Compounds form by the interaction between the nuclei and valence electrons of 2 or more elements
THE OCTET RULE: an element is most stable with 8 valence electrons
Elements will join chemically to get 8 valence electrons
Ex: CO2 : oxygen has 6 valence electrons and carbon has 4
If the carbon shares 2 with each oxygen, everyone will have 8 valence electrons!
This section was left off of your notes sheet. Add this in. Sorry, yal!

19. What Do Compounds Have To Do With My Life?
Compounds are the substances that make up ALL living and non-living things
Examples: Where would you be without:
H2O—water
NaCl—table salt
C3H8O—rubbing alcohol
C6H12O6- sugar
This section was left off of your notes sheet. Add this in. Sorry, yal!

20. What is a solution?
A mixture in which a solute is dissolved in a solvent
Solute: the substance that is dissolved
Solvent: substance in which the solute is dissolved
Particles of each substance are evenly spread throughout the solution
Solutions can be:
Solids: Brass (zinc and copper)
Liquids: Antifreeze (alcohol in water)
Gases: dry air (oxygen in nitrogen)
Combination: Soda (Carbon dioxide in water)

21. What is solubility?
The maximum number of grams of solute which will dissolve in 100g of solvent at a specific temperature and pressure
Data can be used to identify substances

22. What is a saturated solution?
A solution is saturated when no more solute can be dissolved in a volume of solvent at a specific temperature or pressure
Additional solute added to a saturated solution collects at the bottom of the container

23. What is a solubility graph (or curve)?
Shows the relationship between solubility and temperature for a given solute in a solvent
The point at which the curve intersects the x- and y- axis is the saturation point of a given substance

25. What is the solubility of KCl at 40 degrees?
Which is more soluble at 30 degrees? CaCl2 or KCl?
What is the solubility of NaCl at 80 degrees?
How much more KCl will dissolve if you heat the water from 10 to 70 degrees?