1. Chapter 11 The Mole

2. 11.1 Measuring Matter Objectives
Describe how a mole is used in chemistry
Relate a mole to common counting units
Convert moles to number of representative particles and number of particles to moles

3. 11.1 Measuring Matter
Vocabulary
Mole
Avogadro's Number

4. Measuring Matter
Matter is:
Measured by mass, volume, or “counting” particles.
All matter made of particles:
Atoms
Molecules
Ions
Formula units
Regardless of form, all will be called particles

5. What is a Mole?
Mole- SI base unit used to measure the amount of a substance
Equal to the number of representative particles (carbon atoms) in exactly 12 grams of carbon-12

6. ATOMS ARE SO SMALL THAT 1 MOLE OF THEM WOULD FIT IN YOUR HAND!
1 mole carbon atoms
6.02 x 1023 atoms
Mass of 12.0 grams

7. mole (mol)
The amount of a compound or element that contains x 1023 of that substance.
Called Avogadro’s number
1 mole = 1 molar mass = 6.02 x 1023 particles (atoms, molecules, formula units)
Basically, the molar mass is the MASS of one MOLE of a substance.

8. To comprehend the enormous size of Avogadro’s number, 6
To comprehend the enormous size of Avogadro’s number, 6.02 x 1023, here are some analogies:
1 mole of rice has more grains than the
number grains of all grain grown since
the beginning of time!
Would a mole of rice grains fill our chemistry lab?
1 mole of rice in grams would cover all the land area of the whole world to a depth of 75 meters.

9. A MOLE IS A LOT OF THINGS!
A mole of atoms are needed in order to express to atomic mass in grams.
Ex. Atomic mass of Al = 27 g.
It would take x 1023 atoms in order to have 27 g of aluminum. (This would fit in your hand).

10. CONVERTING MOLES  PARTICLES:
1 mole = 6.02 x 1023 particles
Conversions:
Convert to particles: x x 1023 particles
1 mole
Convert to moles: x mole
6.02 x 1023 particles

11. Conversion Flow Chart # Moles # Particles Given: Given:
Multiply by A.N.
# Particles
Divide by A.N.

12. Molar Mass

13. QUIZ – THE MOLE 1) What is the SI unit for amount of matter?
2) How many particles are in 1 mole?
This is called _____’s number.
3) Can 1 mole of M & M’s fit in your locker?
4) Can 1 mole of gold atoms fit in your locker?
5) Suppose you had 6.02 x 1023 atoms of silver. How many moles?
What is the mass?

14. Problems: 1) Find the number of atoms in 3.60 mol of Zn.
2) How many formula units in 4.50 mol of NaCl?
3) Calculate the number of molecules in15.0 mol H2O.