1 / 18

TOPIC: Counting Atoms – The Mole

TOPIC: Counting Atoms – The Mole Do Now: Please take out something to write with and your calculator and get ready for a QUIZ. Using Mass to Count Things. Atoms are so tiny it is impossible to count # atoms in only 1 gram of matter So, chemists use mass to “ count ” atoms. The MOLE.

Download Presentation

TOPIC: Counting Atoms – The Mole

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  1. TOPIC: Counting Atoms – The Mole Do Now: Please take out something to write with and your calculator and get ready for a QUIZ

  2. Using Mass to Count Things • Atoms are so tiny it is impossible to count # atoms in only 1 gram of matter So, chemists use mass to “count” atoms

  3. The MOLE • Is the unit used to “count” # atoms • Defined: # atoms in 12.0 grams of C-12 • This is the STANDARD! • 12.0 g of C-12 has 6.02 X 1023 atoms 602,000,000,000,000,000,000,000 atoms

  4. What is a mole? Let’s check out a video Not this kind of mole!

  5. The MOLE • 1 mole of any element has 6.02 X 1023 particles • This is a really big number – It’s so big because atoms are really small!

  6. The number of particles or representative units represented in 1 mole of a substance is known as Avogadro’s Number.= 6.02 X 1023 • One mole of water = 6.02 X 1023 water molecules • One mole of gorillas is 6.02 X 1023 gorillas • One mole of He atoms is 6.02 X 1023 He atoms • One mole of anything is 6.02 X 1023 of that thing

  7. Similar Words • Pair: 1 pair of shoelaces = 2 shoelaces • Dozen: 1 dozen oranges = 12 oranges • Gross: 1 gross of spider rings = 144 rings • Ream: 1 ream of paper = 500 sheets paper • Mole: 1 mole of Na atoms = 6.02 X 1023 Na atoms

  8. 1 mole is equal to the Formula Mass of each element

  9. What is the mass of 1 mole of Mg (magnesium)? 1 mole of Mg = 24 grams

  10. 1 mole is always equal to 6.02 x 1023

  11. So, how many atoms are in 1 mole of Mg? 1 mole of Mg = 24 grams = 6.02 x 1023

  12. MOLAR mass for any element: molar mass of any element = atomic mass in g/mole 1 mole Ne = 20 g/mol [= 6.02 X 1023 atoms] 1 mole Ar = 40 g/mol [= 6.02 X 1023 atoms] 1 mole Kr = 84 g/mol [= 6.02 X 1023 atoms]

  13. Equalities 1 mole of N-14 = 14.0 grams of N-14 = 6.02 X 1023 atoms of N-14 1 mole of C-12 = 12.0 grams of C-12 = 6.02 X 1023 atoms of C-12

  14. Equalities 0.5 mole of C-12 = 6.0 grams of C-12 = 3.01 X 1023 atoms of C-12 1 mole of C-12 = 12.0 grams of C-12 = 6.02 X 1023 atoms of C-12

  15. 0.25 mole of C-12 = 3.0 grams of C-12 = 1.50 X 1023 atoms of C-12 Equalities 1 mole C-12 = 12.0 g C-12 = 6.02 x 1023 atoms C-12

  16. What is the Molar Mass of CuSO4(hint, it’s just like Formula Mass, just a different unit) Cu = 1 x 64 = 64 S = 1 x 32 = 32 O= 4 x 16 = 64 ________ 160 g/mol

  17. Now Lets Take the QUIZ Let’s check out a video

More Related