1. Atoms: The Building Blocks of Matter
Chapter 3
Atoms: The Building Blocks of Matter

2. I.Classes of Matter
-Matter exists as elements, compounds, mixtures, or solutions
*Homogeneous matter:
identical properties throughout.
Ex: salt h20

3. *Heterogeneous matter:
different properties
Ex. Fruit salad, shovel of dirt

4. B. Types of Mixtures 1.Heterogeneous mixture
*particles are large enough to be seen and settle out.
EX: concrete

5. *particles very small and do not settle out. EX: Stainless steel
2. Homogeneous mixture
*particles very small and do not settle out.
EX: Stainless steel
#6(homo and hetero mixtures)

6. *Colloids:
Larger particles but left in suspension
Ex: smoke,

7. *Alloy:
solids dissolved in solids
ex: brass, sterling silver
DEMO

8. III. Elements *Pure Subst:
made of only one kind of material and has definite prop
*Element:
simplest pure subst. ;
cannot be chngd into simpler subst by heating or any chem process
-Ex

9. A.   Elements and Atoms
pp39
*Atom:
smallest particle of an element with the prop. of that element.

10. -The prop of a cmpnd are very diff from the prop of the elements in it.

11. A molecule is the smallest particle of a substance that exists alone.
This is a picture of a water molecule. It is two parts hydrogen and one part oxygen.

12. *Chemical Formulas:
1. What it is
2. How much

13. Chemical equation: description of a chem
 *Chemical equation: description of a chem. rxn using symbols and formulas.

14. Chemical equation:
What you put in
What you get out
How much

15. *Law of conservation of mass:
*Law of conservation of nrg:
*nrg: ability to do work
pp77

16. *Diatomic Molecules: (super 7)
Br, I, N, Cl, H, O, F

17. *Chemical Rxn:
1. Bubbles
2. Formation of a precipitate
3. Heat and light given off
pp184

18. mass (amu) charge location
~proton: 1 + nucleus
~neutron: /- nucleus
~electron: 1/ e- cloud

19.  B. Chem Symbols
*represent elements

20. III. Counting Atoms
*Atomic Mass Unit (amu): measures mass of subatomic part.
 -?? Where does it come from??
1/12 mass of a C-12 atom

21. -Atomic #
*number of + in the nucl
~identifies the element
~never chngs

22. -Atomic Mass
*sum of the + and neutrons in its nucleus
-Isotopes
*same # of +, but diff # of neutrons(same elem, diff mass)
*Nuclide: any isotope of any element
  EX: table 3-3 pg 77

23. -Isotopes of H (pg 76)
1. Protium: most common
1+, 1e-, 0+/- mass# = 1
2. Deuterium:
1+, 1e-, 1+/- mass# = 2
3. Tritium:
1+, 1e-, 2+/- mass# = 3

24. isotope notation mass # H : Nuclear symbol atomic# pg: 77
Hydrogen - mass #
pg 80

25. *Aver Atomic mass: aver of the masses of all the atoms in the sample.
(that’s why Atomic mass is not a nice numb)
~atomic mass - atomic# = #of neutrons

26. Chem videos…..
Video #6(the mole-amadeo avoga)
#7 (chem music video 7)
# 8(Avogadro’s Number song)
# 9(A mole is a unit)

27. *Mole: # of particles in 12 grams of C-12
pg 81
*Avogadro’s #: # of particles in 1 mole of substance.
6.022 X atoms
mole

28.
Video #12(how big is a mole)

29. *Molar Mass: mass of 1 mole of pure substance
units---- g/mole
-Gram/Mole Conversion Examples