1. Atomic Structure
Review

2. Outside nucleus in electron cloud
3 Parts of the Atom:
Subatomic Particle
Relative Mass
Charge
Where Found
Proton 1 +1
In Nucleus
Neutron
0(neutral)
Electron -1
Outside nucleus in electron cloud

3. How many electrons can each energy level hold?
1st—2
2nd—8
3rd—18
4th –32

4. Match the Diagram with the Name
Dalton
Bohr
Rutherford
Thomson

5. Properties of the Atom

7. Atomic Number
Chemical Symbol
Element
Average Atomic Mass

8. Atomic # # of protons in an atom
In a neutral Atom, # of protons=# of electrons
Atomic # of a given element will never change, therefore, the # of protons of an element will never change.

9. Mass Number EX) Oxygen Avg. Atomic Mass = 15.999
Sum of the protons and neutrons
Closest whole # to the Avg. Atomic Mass(from periodic table)
WHY?
EX) Oxygen Avg. Atomic Mass =
Therefore, Mass # = 16

10. Average Atomic Mass Mass of atom in Atomic Mass Units
Given on periodic table as average mass of all isotopes of that element.(we’ll discuss isotopes)
The number of neutrons sometimes varies!!!
Atomic Mass Unit—defined as 1/12 the mass of a Carbon-12 atom

11. What is the atomic # of Potassium?
39.10 39 19 20

12. What is the Average Atomic Mass of Magnesium?12
24.31 24
12.31

13. What is the Mass # of Magnesium?12
24.31 24
12.31

14. How many protons are found in Potassium?19 20 39 21

15. Isotopes
Atoms of the same element with the same # of protons, but different # of neutrons.

16. 2 ways of writing Isotopes
H-1 H H-3
Each of these represents Hydrogen
The number represents the mass #
Each of these represents Carbon
The top # represents the mass #
The bottom # represents the Atomic #

17. Isotopes of Carbon

18. A neutron walked into a bar and asked how much for a drink
A neutron walked into a bar and  asked how much for a drink.  The bartender replied,  "for you, no charge." 

19. Ions
Ions
Ions
Ions
Ions
Ions

20. Ions + ions 2. - ions Atoms become (+) by losing electrons
A “charged” atom.
Atoms become charged by gaining or losing electrons.
2 Types of Ions:
+ ions
Atoms become (+) by losing electrons
2. - ions
Atoms become (-) by gaining electrons

22. Determine the Atomic # and Mass # Atomic # = # protons
Using the Periodic Table to determine the # protons, # electrons, and # of neutrons:
Determine the Atomic # and Mass #
Atomic # = # protons
# protons = # electrons
Mass # = # neutrons + # protons

23. # p = 6 # e = 6 # n = 6 A # = 6 M # = 12 Atomic # Atomic Mass
M # = # p + # n
12 = 6 + #n
A # = 6
M # = 12

24. # p = 11 # e = 11 # n = 12 A # = 11 M # = 23 Atomic # Atomic Mass
M # = # p + # n
23 = 11 + #n
A # = 11
M # = 23

25. # p = 19 # e = 19 # n = 20 A # = 19 M # = 39 Atomic # Atomic Mass
M # = # p + # n
39 = 19 + #n
A # = 19
M # = 39

26. # p = 27 # e = 27 # n = 32 A # = 27 M # = 59 Atomic # Atomic Mass
M # = # p + # n
59 = 27 + #n
A # = 27
M # = 59

27. Element
Atomic #
Mass #
# of Protons
# of Neutrons
# of Electrons
Phosphorus 15 31 16
Carbon 6 13 7
Helium 2 4
Beryllium 10
Iodine 53
126 73
Argon 18 40 22
Fluorine 9 19