1. ATOM Smallest particle of an element with all its properties

3. Periodic Table

4. H ATOMIC NUMBER SYMBOL ATOMIC MASS 1 1.0079

5. Three main parts +PROTON +NEUTRON +ELECTRON

6. PARTICLELOCATIONCHARGE MASS PROTONNUCLEUS POSITIVE + 1 A.M.U ELECTRONELECTRON CLOUD NEGATIVE - 1/1836 A.M.U NEUTRON NUCLEUSNONE 1 A.M.U

8. Most of an atom is empty space. The nucleus of the atom contans amost all of the mass of the atom. A greatly enlarged atom might look like a marbel (the nuceus)insde an empty football stadium.

9. TO FIND # OF PROTONS ATOMIC NUMBER = NUMBER OF PROTONS NUMBER OF PROTONS = NUMBER OF ELECTRONS

10. NEUTRON Atomic mass (rounded off) -subtract ATOMIC NUMBER _____________________ NUMBER OF NEUTRONS

11. ISOTOPE ATOMS OF THE SAME ELEMENT WITH THE SAME NUMBER OF PROTONS/ELECTRONS BUT A DIFFERENT # OF NEUTRONS

13. CARBON ISOTOPE HOW MANY PROTONS, ELECTRONS AND NEUTRONS

14. HOW MANY PROTONS, ELECTRONS NEUTRONS

15. COMPARE THE TWO CARBONS 1. HOW DOES THE MASS COMPARE 2. HOW DO THE PROTONS COMPARE 3. HOW DO THE NEUTRONS COMPARE

16. BORON PROTONS= ELECTRONS= NEUTRONS= ATOMIC NUMBER= ATOMIC MASS =

17. DEMOCRITUS 440 B.C DEVELOPED THE FIRST ATOMIC THEORY

18. DALTON THEORY 1802 ATOMS CANNOT BE BROKEN INTO SMALLER PIECES IN ANY ELEMENT, ATOMS ARE EXACTLY ALIKE

19. ATOMS OF TWO OR MORE ELEMENTS CAN COMBINE TO FORM COMPOUNDS ATOMS OF EACH ELEMENT HAVE A UNIQUE MASS MASSES OF THE ELEMENTS IN A COMPOUNDS ARE ALWAYS CONSTANT RATIO