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Atomic theory

Atomic theory. Odds and ends. AMU. 1.6 x 10 -27 Kg Mass of 1/12 of carbon – 12 isotope. Masses of particles. Proton plus charge 1.6 x 10 -27 Kg = 1 amu Neutron no charge 1.6 x 10 -27 Kg = 1 amu Electron negative charge

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Atomic theory

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  1. Atomic theory Odds and ends

  2. AMU • 1.6 x 10 -27 Kg • Mass of 1/12 of carbon – 12 isotope

  3. Masses of particles • Proton plus charge 1.6 x 10-27 Kg = 1 amu • Neutron no charge 1.6 x 10-27 Kg = 1 amu • Electron negative charge • 9.11 x 10-31 Kg = 0 amu

  4. Atomic masses • Average mass of various isotopes • Found by multiplying isotope mass by its percentage in nature, then adding them all up.

  5. examples • Oxygen-16 x 99.762% = • Oxygen-17 x 0.038% = • Oxygen – 18 x 0.200% = • Then add them up__________

  6. example • Copper 63 x 69.17% = • Copper 65 x 30.83% = • Then add _________________

  7. example • Argon - 40 99.600% • Argon - 38 .063% • Argon - 36 .337% • then add _________

  8. FINAL EXAMPLE • Naturally occuring Boron is 80.20% boron-11 and and 19.80 % of some other isotope. • The average mass is 10.81. What is the mass of the other isotope?

  9. MORE ATOM STUFF • NOW THAT WE KNOW AN AMU IS 1.6 X 10-27 Kg WHAT CAN WE DO WITH THAT INFO? • IF WE KNOW THE AVERAGE AMU FOR AN ATOM, WE CAN TRANSLATE THAT INTO A QUANTITY WE CAN WORK WITH IN THE LAB!

  10. THE MOLE • The amount of a substance that contain as many particles as there are atoms in exactly 12g of carbon -12. • By experiment that amount is 6.02 x 1023 particles

  11. calculation • Average Amu of carbon = 12.01 • 12.01amux 1.661x10-27 Kgx 1000 g = 1.99486 x 10-23 Amu Kg • 1.99486 x 10 -23 gx 6.023 x 1023 particles = 12.01 g • mole mole

  12. RESULT • WE CAN NOW HANDLE ATOMS IN THE LABORATORY AND KNOW HOW MANY WE HAVE! • IF I HAVE 12.01 GRAMS OF CARBON, I HAVE 1 MOLE OF CARBON, I HAVE 6.023 X 10 23 ATOMS • SAME WITH ANY OTHER MASS ON THE PERIODIC TABLE!!!!!

  13. 3 MAJOR LAWS OF CHEM • CONSERVATION OF MATTER • IN ANY ORDINARY CHEMICAL REACTION, MATT IS NOT CREATED OR DESTROYED • DEFINITE PROPORTIONS • IN A GIVEN COMPOUND, THERE ARE ALWAYS THE SAME ELEMNTS IN EXACTLY THE SAME MASS RATIO

  14. MULTIPLE PROPORTIONS • WHEN DIFFERENT COMPOUNDS ARE FORMED FROM THE SME TWO ELEMENTS, THE RATIOS ARE ALWAYS SMALL WHOLE NUMBERS. • WATER H20 vs peroxide H20 2 • CARBON DIOXIDE CO2vs CARBON MONOXIDE CO

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