1. Atomic Structure
Unit 3

2. History of the Atom
Watch the Brain Pop on Atomic Model!

3. Atomic Structure Electrons- outside the nucleus Protons Neutrons+ + N N -
Neutrons
Outside the nucleus

4. Complete the following table:
Subatomic Particle
Location
Charge
Mass
Electron
Proton
Neutron

5. Complete the following table:
Subatomic Particle
Location
Charge
Mass
Electron
Electron Cloud
(-)
0 amu
(teeny tiny!)
Proton
Nucleus
(+)
1 amu
Neutron
Neutral

6. Reading the Periodic Table
* Atomic #: The number of _protons_ in an atom. It equals the number of _electrons_ in a neutral atom. * Mass number = __protons__ + neutrons * # of neutrons = _Mass_#___ - ___atomic number_____ * Atomic Mass: The _average__of all naturally occurring isotopes.

8. Observe the models of atoms at your Lab stations.
Use the results and your periodic table to complete the chart and the following questions.
Homework: Complete page 6

9. NOTES: Isotopes and Ions
Warm-up:

10. Isotopes:
Isotopes - is a version of an atom with the same number of PROTONS, but different number of NEUTRONS.
-If an atom is an isotope you name it using the element name followed by the mass number.
* Ex: carbon – 12 and carbon -14
- Writing Isotope Symbols:
Write the atomic symbol for the element
To the top left of the symbol write the mass # of the isotope.
Beneath that (to the bottom left of the symbol). Write the atomic number of the element.

11. Ex: Label the following
Carbon-14 is written like this: C
Mass # 14
Element Symbol 6
Atomic #

12. C and C 14 12 6 6 Isotope Examples:
How many protons does Carbon-14 contain?
How many protons does Carbon-12 contain? 6
How many neutrons does Carbon-14 contain?
How many neutrons does Carbon-12 contain?
14-6 = 8
12-6= 6

13. Ions are charged atoms (+ or -)
* Atoms as a rule are all neutral in charge, meaning that the number of protons and electrons in the atoms are equal.
Ions:
Ions are charged atoms (+ or -)
Formed when an atom GAINS or LOSES electrons

14. Ions Examples Lithium - 7 + Protons: 3 Neutrons: 4 Charge: 1+
Cations
Positively (+) charged atoms
Form by LOSING electrons
Usually formed by metals
Examples Lithium - 7 +
Protons: 3
Neutrons: 4
Charge: 1+
Electrons: 2

15. 2- Ions Protons: 16 Neutrons: 16 Charge: 2- Electrons: 18 Anions
Negatively (-) charged atoms
Form by GAINING electrons
Usually formed by nonmetals
Examples Sulfur - 32 2-
Protons: 16
Neutrons: 16
Charge: 2-
Electrons: 18

16. Page 9 -10 Complete the table as directed on Pg. 9.
Complete the chart and answer the questions on Pg. 9 in group of 2 (no larger!).
Homework: Pg. 10

17. Atom#
Isotope Symbol
Atom name with mass #
#Protons
#Neutrons
#Electrons
Atomic Number
Mass Number
Neutral/Isotope/Ion
Charge 1
Neutral 2 3 4 5 6 7 8 9 10 11 12

18. Isotopes and Average Atomic Mass
Isotopes and Average Atomic Mass * Compare & contrast Mass Number and Atomic Mass:

19. Atomic Mass Calculations
Atomic mass is the weighted average of the masses of all naturally occurring isotopes.
Atomic Mass=
Σ[(Percent Abundance) x (Mass of Isotope)]
Σ = take the sum of; add them all up at the end!
Sample Calculations together.. 

20. Atomic Structure- Inside the Nucleus
Protons
Positively (+) charged particles
Equal to the atomic number
Identity of atoms is based on # of protons in Nucleus
Contribute to the mass of the atom
Proton mass = 1amu
amu= atomic mass unit

21. Atomic Structure- Inside the Nucleus
Neutrons
Neutral particles (no charge)
Help hold nucleus together; contribute to stability
Neutrons + Protons= mass number
Neutron mass = 1amu

22. Atomic Structure- Outside the Nucleus (Electron Cloud)
Electrons
Negatively (-) charged particles
Responsible for the CHEMICAL PROPERTIES of the atom
In a neutral atom (no charge), protons=electrons
Very little mass
~0 amu

23. Reading the Periodic Table Elements
Atomic number 6
= # Protons
(element identity!) C
Element Symbol
Last page of notes!!! Students will have to flip their packets to the back to complete, before returning to the back of page 2 to complete their content frame. 
= weighted average of isotope atomic masses
12.01
Atomic Mass
Carbon

24. Complete the following table:
Complete Symbol
Mass Number
Atomic Number
Protons
Neutrons
Electrons 16 14 Se 70 34

25. Si 14 16 70 34 Se 14+16 = 30 70-34 = 36 30 14 70 34 Complete Symbol
Mass Number
Atomic Number
Protons
Neutrons
Electrons Si
14+16 = 30 14 16 Se 70 34
70-34 = 36 30 14 70 34

26. +=
= Cations