1. The Nature of Matter
Mr. Halfen
Sept. 2016

2. Characteristics Properties
Independent of volume
Useful for identifying a substance
Useful for designing mixture separation techniques
examples:

3. States of Matter Solid - Definite Shape, Definite Volume
Liquid - Indefinite Shape, Definite Volume
Gas - Indefinite Shape, Indefinite Volume

4. Changes in State Addition of Heat (Energy) Melting Boiling Sublimation
Loss of Heat (Energy)
Condensation
Freezing (Solidification)

5. Substances Copy Figure 2.22 into your notes.
Add the following info under mixtures-
heterogeneous - mixture not identical throughout (e.g., salad or fruit loops in a bowl of milk)
homogeneous - identical throughout (aka “solution”)
alloy - homogeneous mixture of metals (e.g., steel, brass, bronze)

6. Substances - definitions
solution -
solute -
solvent -
suspension -
miscible -

7. Separation Techniques
Solid in Liquid - Suspensions
Decanting -
Filtration -
Centrifugation -

8. Separation techniques
Dissolved Solids in Liquids
Distillation -
Evaporation -
Chromatography -

9. Separation Techniques
Solid & Solid
Density -
Magnetism -
Differences in Solubility -

10. Separation Techniques
Liquid & Liquid
Density -
Separation Funnel -
Fractional Distillation -

11. Solubility
Maximum amount of a substance (solute) that can be dissolved in another substance (solvent)
Depends on substances and temperature
In general,
solubility of solids incr. w/ incr’g temp.
solubility of gases decr. w/ incr’g temp.

12. Atoms and Elements - Definitions
Compound -
Shell -

13. Atomic Structure Subatomic Particle Relative Mass Relative Charge
Location
Protons
Neutrons
none
Electrons
~ zero

14. Atomic Structure (cont.)
atomic number (Z) = no. of protons (aka proton number)
mass number (A) = no. of protons + no. of neutrons (aka nucleon number)
isotope -

15. Atomic Structure - practice
symbol Z A
protons
neutrons
electrons
Hydrogen 2
helium 3 C 14 8 18
silver
107
Uranium U 92
235
143

16. Atomic Structure (cont.)
Compare your data from the last slide to table 2.8 on p. 52. Why are some of them different?
Which of the following pair are isotopes?
A) Atom 1: Z=12 & A=26; atom 2: Z=13 & A=26
B) Atom 1: Z=12 & A=27; atom 2: Z=12 & A=26
C) Atom 1: Z=12 & A=26; atom 2: Z=13 & A=27

17. Relative atomic Mass Relative atomic mass -
calculate the relative atomic mass for:
Isotope
Relative abundance
12C
99%
13C
0.99%
14C
0.01%

18. Symbols – get atomic symbols for these elements
Aluminum Al
Bromine
Chromium
Mercury
Nitrogen
Lead
Tin
Silver
Carbon
Cesium
Iodine
Sodium
Platinum
Strontium
Argon
Calcium
Copper
Iridium
Neon
Rubidium
Titanium
Gold
Cadmium
Iron
Potassium
Nickel
Radon
Uranium
Boron
Chlorine
Hydrogen
Lithium
Oxygen
Sulfur
Vanadium
Beryllium
Cobalt
Helium
Magnesium
Phosphorus
Silicon
Zinc Zn

19. Electron Arrangement Copy the Bohr model from figure 2.37
Draw Bohr models for the following: 2H
23Na
15O
40K
28Si
39Ca

20. Radioactivity radioactivity - radioactive dating - industrial uses -
medical uses -