1. Atoms

2. You will need: The vocab cards for
Atom, nucleus, electron, element, isotope, compound , ionic bond, ion, covalent bond, molecule, van der Waals forces.
2. 2 Pieces of paper
3. A baggie with 3 colors of holes.
Write the number on the baggie here__________

3. Atomic Particles I. Protons – positive; determines the element;
power of Atomic bomb
(fission); Hydrogen bomb (fusion)
II. Neutron – neutral; determines the isotope
III. Electron – negative; determines the charge; power of electricity

4. Size Nucleus: Protons + neutrons Protons = neutrons in size
Orbitals – electrons
Protons = electrons in charge,
electron size – tiny

5. Determining the number of protons, neutrons, and electrons.
  Protons – is the atomic number
Electrons – is the atomic number
Neutrons –
Round the atomic mass number to the nearest ones.
Subtract the number of protons from the atomic mass

6. Periodic Table O 8 symbol Atomic number = # of protons, # of electrons
Oxygen
15.994
symbol
Atomic Mass = Protons + Neutrons
Element Name

7. On each piece of paper, please draw the circle below
On each piece of paper, please draw the circle below. Fill the paper with the drawing.
Please make each ring a different color.
Color in the center circle ONLY – use the same color as the line.

8. Use blue for protons, green for neutrons, and orange for electrons.
Used the punched holes to show oxygen on your drawing. For now, put the electrons anywhere on the outer 3 rings
Example: Oxygen
Protons: 8
Electrons: 8
Neutrons: 16 – 8 = 8 (not all elements will have the same number of neutrons as protons)
Use blue for protons, green for neutrons, and orange for electrons.

9. Practice: build the following atoms on your drawing.
Lithium – Li Aluminum – Al Sodium – Na Potassium – K Chlorine - Cl

10. Arranging the electrons
Note: This is a very simplified arrangement. You will get a more accurate one in chemistry. 2 electrons fit in the 1st (inner) level. 8 electrons fit in the 2nd level. 8 electrons fit in the 3rd level.

11. Please draw in where the electrons will go.

12. Now build the atoms with the electrons in the correct level.
Lithium – Li Aluminum – Al Sodium – Na Potassium – K Chlorine - Cl

13. Isotopes
I. All of the atoms of the same elements HAVE THE SAME # OF PROTONS II. An isotope has a different number of NEUTRONS THAT THE MOST COMMON. A. The most common is the number of neutrons in the atom that has the atomic mass rounded to the 1s.

14. Use the electrons to fill the orbitals starting from the inside.
EX: Hydrogen – Protons-1 so electrons- 1
Since Hydrogen has one electron in its outermost shell it has a dot structure of H

15. Li Example: Lithium 3 electrons
Since lithium has 1 electron in the outermost shell its dot structure is
Li

16.   N Example: Nitrogen 7 electrons
Since nitrogen has 5 electron in the outermost shell its dot structure is 
 N

17.  Al Example: Aluminum - 13 electrons
Since aluminum has 3 electron in the outermost shell its dot structure is 
Al

18. The electrons in the outer most shell determines how the element will react.

19. Atoms want to be “happy”.
A happy atom has a full outer shell
It can LOSE electrons and become more +
Li· has 1 electron so it will lose the 1 and become Li+ (do not write a “1”).
It can GAIN electrons and become more –
Oxygen has 6 electrons so will add 2 electrons so will become 2-, O2-.

20. The elements in the 1st column have 1 electron in the outer shell and so will lose 1 electron and give those elements a charge of 1+ (but the 1 is not written).
This can be predicted from the Periodic Table. The column number shows the number of electrons in each element’s outermost shell. +

21. The elements in the 2nd column have 2 electron in the outer shell and so will lose 2 electrons and give those elements a charge of 2+. 2+

22. The elements in the 7th column have 7 electron in the outer shell and so will GAIN 1 electron and give those elements a charge of 1-. -

23. The elements in the 6th column have 6 electron in the outer shell and so will gain 2 electrons and give those elements a charge of 2-. 2-

24. The elements in the 5th column have 5 electron in the outer shell and so will gain 3 electrons and have a charge of 3-. 3-

25. The elements in the 4th column have 4 electrons in the outer shell and so could gain or lose 4 electrons. This is so many that elements in this column share electrons rather than give or take electrons.
4+4-