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Catalyst – May 6-4, 2011 Grab a calculator!

Catalyst – May 6-4, 2011 Grab a calculator!. Monday Mystery Element! Used to make batteries Can cause kidney failure and high blood pressure Found in tobacco leaves. Catalyst – May 6-4, 2011. Monday Mystery Element! Used to make batteries Can cause kidney failure and high blood pressure

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Catalyst – May 6-4, 2011 Grab a calculator!

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  1. Catalyst – May 6-4, 2011Grab a calculator! Monday Mystery Element! • Used to make batteries • Can cause kidney failure and high blood pressure • Found in tobacco leaves

  2. Catalyst – May 6-4, 2011 Monday Mystery Element! • Used to make batteries • Can cause kidney failure and high blood pressure • Found in tobacco leaves Discovered by Strohmeyer in 1817…..it is…… CADMIUM!

  3. Today’s Agenda • Catalyst • Welcome to STOICHIOMETRY!!! • Holy Moley! • Moles – Particles/Particles – Moles • Moles – Mass/Mass – Moles • Work Time • Exit Question HOMEWORK: Stoichiometry Worksheet

  4. Today’s Objectives • SWBAT perform mole – particle and particle – mole calculations. • SWBAT calculate the molar mass of chemical substances. • SWBAT performmole-mass and mass-mole calculations.

  5. What is a mole to us chemists? • A benign overgrowth of cells because of a failure in mitosis? • NO! But gross… • A rascly little rodent? • NOOOO! • A TV show featuring celebrities? • NOOOOO! • Then WHAT IS IT?????!!!???!?!?!???!!!!

  6. The Mole Think of the term “a dozen”… How many donuts are in a dozen? How many eggs are in a dozen?

  7. The Mole Just like a dozen refers to 12objects… The mole refers to… 6.02 x 1023 particles

  8. Avogadro’s Number This number is called Avogadro’s number… 6.02 x 1023 EQUALS 602,000,000,000,000,000,000,000 http://molechemistry.info/

  9. Avogadro’s Number Key Point #1: 1 mole (mol) = 6.02 x 1023 atoms OR molecules

  10. Stoichiometry Calculations Part One Moles – Particles and Particles – Moles (Particles = Atoms or Molecules)

  11. Avogadro LOVES Us! • Key Point #2: Avogadro's number (6.02 x 1023) is used to convert between moles and particles (atoms/molecules). • It all relates back to the mole… • Guess what’s coming back…

  12. TRAIN TRACKS!!! • Step 1: • What to what? • Step 2: • Write conversion factor(s) • Step 3: • Train tracks

  13. Avogadro’s Number: Example #1 Write this down!!! How many atoms of Na are in 3.4 moles Na?

  14. Scientific Notation on the Calculator • Don’t forget! When you need to type in a scientific notation number like 6.02 x 1023… • Type 6.02 EE 23 instead SAVE TIME AND LOOK COOL!

  15. Avogadro’s Number: Example #2 Write this down!!! How many moles of N2 are in 250 molecules N2?

  16. Avogadro’s Number: You Try! How many molecules of C12H22O11 are in 2.1 moles of C12H22O11?

  17. Stoichiometry Calculations Part Two Moles – Mass and Mass – Moles

  18. OOOH, I want some more train tracks! • Key Point #3: Molar mass is the number of grams in one mole of a substance. It is used to convert between moles and mass. • But Ms. Stroh, how am I ever going to find out this information?

  19. Molar Mass: Example #1 “What is the molar mass?”means… “How many grams are in one mole of a substance?” 1 mol C = 12.01 g C

  20. Molar Mass: Example #2 Write this down!!! 1 mol Na = 22.99 g Na

  21. Molar Mass: Example #3 Write this down!!! 1 mol CO2= 44.01 g CO2

  22. Molar Mass: You Try! 101.1 g KNO3 1 mol KNO3 =

  23. Molar Mass: Step-Up Problem #1 Write this down!!! If we have 3.5 moles of KNO3, how many grams of KNO3 would we have?

  24. Molar Mass: Step-UpProblem #2 Write this down!!! If we have 20 grams CH4, how many moles of CH4 do we have?

  25. Independent Practice • Worksheet time! Show your work! • Finish for Homework! • Show Train Tracks on #7-14

  26. Exit Question • How many molecules are in 1 mole of NH4? • How many grams are in 2.3 moles of NH4 HW: Finish Worksheet and read 12.1 and 12.2 in book!

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