1. The nature of matter

2.  Differentiate between an element, compound, and mixture  Determine if a change is chemical or physical  Correlate between changes of state and energy  Explain the law of conservation of mass for an equation  Understand and apply the importance of density

3. What we think we knowWhat we want to know

4.  Matter  Atoms are matter  Elements  Atom  Compound  Molecule  Chemical formula

5.  C 6 H 12 O 6  H 2 O  Fe 2 O 3  If I were to put a 2 in front of C 6 H 12 O 6 making it 2C 6 H 12 O 6 how many of each element would I then have?  3H 2 O  45Fe 2 O 3

6.  Pure substance  Cannot be broken down by physical actions  Elements  Compounds  Mixture  Can be separated  Homogeneous  Heterogenous  Miscible  immiscible

7.  Copper  Water  Wet pancake mix  Carbon dioxide  Salad  Air

8.  Soda  Meringue pie

9.  Kinetic theory  All matter is made of atoms and molecules that act like tiny particles  These tiny particles are always in motion  The higher the temperature the faster they move  At the same temperature the more massive particles move slower than less massive particles  viscosity

10.  Evaporation  Condensation  Sublimation Mrzimmerman.org

11.  Law of conservation of mass  Law of conservation of energy

12. 4P + 5O 2  P 4 O 10 (Yes) 14 Atoms on each side KClO 3  KCl + O 2 (No) 5 and 4 H 2 + O 2  H 2 O (No) 4 and 3 2Na + Cl 2  2NaCl (Yes) 4 Atoms on each side S 8 + O 2  SO 3 (No) 10 and 4

13. 2Al + 3FeO  Al 2 O 3 + 3Fe 6CO 2 + 6H 2 O  C 6 H 12 O 6 + 6O 2 2H 3 PO 4  H 4 P 2 O 7 + H 2 O

14. Chemical changes/property  reactivity  Chemical composition changes Physical changes/property  Melting and boiling point  Density  Buoyancy

15.  Digesting food  Ripping paper up  A car exploding  Boiling water  Dissolving sugar in water  Cutting up watermelon  Baking a cake

16.  What exactly is dentistry?  Write down on your handout what you believe density is and then discuss it with the person sitting next to you.

17.  g/mL or g/cm 3  same bc mL is volume and v=l x w x h (cm x cm x cm)  D=m/v  M=vD  V=M/D

18.  What is the density of carbon dioxide gas if 0.196 g occupies a volume of 100 mL?g.  A block of wood 3.0 cm on each side has a mass of 27 g. What is the density of this block?

19.  An irregularly shaped stone was lowered into a graduated cylinder holding a volume of water equa to 2.0 mL. The height of the water rose to 7.0 mL. If the mass of the stone was 25 g, what was its density? Incorrect numbers, but an example.

20.  Five mL of ethanol has a mass of 3.9g and 5.0 mL of benzene has a mass of 4.4 g. Which liquid is more dense?  The density of silver is 10.5 g/mL. What will be the volume of apiece of sliver with a mass of 42.0 g?

21.  An object has a density of 54.76 g/mL and a volume of 3.40 mL. What is the mass?  A piece of metal has the mass of 42.07g and a density of 5.3 g/cm 3. What is the volume of this metal?