1. Drawing Atoms CHEMICAL SCIENCE

2. Review: Atomic Structure Subatomic Particle ChargeMass (in au) Location ProtonPositive (+) 1Nucleus NeutronNo Charge (0) 1Nucleus ElectronNegative (-) 0Electron Shell Note: Electrons interact with other atoms during reactions, so it is most important to be able to represent them in diagrams.

3. Bohr Rutherford Diagrams Bohr Rutherford diagrams show the arrangement of all atoms. To draw one we need to know: 1. How many electrons does this element have? 2. How many electrons go in each shell? 3. How do electrons arrange themselves?

4. How many electrons does this element have? Use the periodic table. The number of electrons will equal the atomic number. Example: Lithium’s atomic number is 3. Therefore it has three electrons.

5. How many electrons go in each shell? Note: Although the third shell can hold 18 electrons, it doesn’t always fill up. The first twenty elements only hold 8 electrons in the third shell.

6. How do electrons arrange themselves? In the first, shell they pair up. After the first shell, they pair up after 4 electrons. Note: This is easier to understand as you go, so let’s look at some examples!

7. Hydrogen Has only one electron. Easy! H

8. Helium Has only two electrons which pair up He

9. Lithium Has three electrons The first two pair up on the first shell The last one doesn’t fit on the first shell so it starts to fill the second Li

10. Beryllium Has four electrons The first two pair up on the first shell The next two start to fill the second shell – They do not pair up Be

11. Carbon Has six electrons The first two pair up on the first shell The remaining four start to fill the second shell – They do not pair up C

12. Nitrogen Has seven electrons The first two pair up on the first shell The next four start to fill the second shell – They do not pair up Because there are four electrons in the second shell, the last electron pairs up N

13. Oxygen Has eight electrons The first two pair up on the first shell The next four start to fill the second shell – They do not pair up Because there are four electrons in the second shell, the last two electrons pair up with the pre-existing electrons O

14. Sodium Has 11 electrons The first two pair up on the first shell The next four start to fill the second shell – They do not pair up The next four electrons complete the second shell by creating pairs The last electron does not fit on the second shell. It starts the third shell Na

15. Lewis Structures/Lewis Dot Diagrams Only the electrons on the very outer shells are involved in chemical reactions These electrons are called VALENCE ELECTRONS Lewis Structures allow us to look only at these electrons to predict reactions Element Symbol Valence Electrons

16. Example: Nitrogen N N

17. Hydrogen H H

18. Helium He He

19. Lithium Li Li

20. Oxygen O O

21. Periodic Trends

22. Your turn! COMPLETE WORKSHEET