1. THE ATOM AND THE PERIODIC TABLE

2. STATE STANDARD  SPI 0807.9.9 Use the periodic table to determine the properties of an element.

3. OBJECTIVES  I can identify the parts of an atom  I can compare and contrast the relative masses of the different parts of an atom  I can calculate atomic mass

4. REPRESENTATION OF AN ATOM

5. ELEMENT TILE

6. STATE STANDARD  SPI 0807.9.9 Use the periodic table to determine the properties of an element.

7. OBJECTIVES  I can calculate atomic mass correctly 8 out of 10

8. Calculating Atomic Mass APE Atomic# = #of Protons = #of Electrons For Oxygen, O, the atomic # is 8 So, O has 8 Protons and 8 Electrons.

9. Calculating Atomic Mass MAN (Mass #) - (Atomic#) = ( # of Neutrons)

10. Calculating Atomic Mass Oxygen has an Atomic # of 8 Therefore O has:  8 Protons  8 Electrons To calculate # of Neutrons:  First round the atomic mass from 15.99 to 16  Then subtract the number of Protons. 16 Mass # - 8 Atomic # 8 # Neutrons

11. ISOTOPES  ISOTOPES are atoms that have the same number of protons but different number of neutrons.

12. ISOTOPES  Isotopes of an element share the same chemical properties and most of the same physical properties.

13. STATE STANDARD  SPI 0807.9.9 Use the periodic table to determine the properties of an element.

14. OBJECTIVE  I CAN ACCURATELY DRAW THE BOHR ATOMIC MODEL FOR THE FIRST 20 ELEMENTS

15. BOHR’S MODEL OF THE ATOM  Niels Bohr (1913): studied the light produced when atoms were excited by heat or electricity.  Bohr proposed that electrons are in orbits & when excited jump to a higher orbit. When they fall back to the original they give off light.

16. BOHR’S MODEL OF THE ATOM

18. BOHR’S ATOMIC MODEL  Bohr's model: -electrons orbit the nucleus like planets orbit the sun  Each orbit can hold a specific maximum number of electrons ORBIT (n)MAX # OF ELECTRONS 12 28 318 432

19. BOHR ATOMIC MODEL FOR NEON