1 / 15

T he Mole and Avogadro’s Number

T he Mole and Avogadro’s Number. Mole ( n ): the amount of substance 6.02x10 23 particles (atoms or molecules) of a substance The same number of particles as atoms in 12 grams of carbon-12. Review. How many atoms are there in 1.2 moles of oxygen?

brady-miller
Télécharger la présentation

T he Mole and Avogadro’s Number

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. The Moleand Avogadro’s Number

  2. Mole (n): the amount of substance • 6.02x1023 particles (atoms or molecules) of a substance • The same number of particles as atoms in 12 grams of carbon-12

  3. Review • How many atoms are there in 1.2 moles of oxygen? • Calculate the number of moles of nitrogen equal to 3.45x1015 atoms of nitrogen.

  4. Counting Atoms • CO • CO2 • Fe(NO3)3 • C6H12O6 • potassium carbonate

  5. How many molecules in 5 moles of water? • How many hydrogen atoms in 5 moles of water? • How many atoms in 5 moles of water?

  6. 1. How many chloride ions are there in zinc chloride? 2. A sample of zinc chloride contains 3.1x1019 molecules. a. How many moles is this? b. How many zinc ions? c. How many chloride ions?

  7. Stop.

  8. Masses of Compounds

  9. Atomic mass (A): the mass of an atom of an element relative to (compared to) other elements (g/mol)

  10. Ionic: formula unit • Molecular (covalent): molecule

  11. Formula mass: sum of the atomic masses of the atoms in the compound’s formula (IONIC) (g/mol) • Molecular mass: sum of the atomic masses of all the atoms in one molecule (COVALENT) (g/mol)

  12. Molar mass (M): the mass of one mole of any substance (g/mol) • atoms, molecules, ions, etc.

  13. Ionic Formula Mass Molar Mass Covalent Molecular Mass

  14. Calculating Molar Mass • Stop.

  15. Calculate the mass of 1.98 moles of iron (II) nitrate. • How many molecules are there in 1.00 grams of iron (II) nitrate? • Calculate the mass of one molecule of iron (II) nitrate.

More Related