+Tuesday, 10/14

Get out page 36 to turn in!Lab, page 37 with post-lab questions

due Friday.PSAT & Movie tomorrow!!!Label “Mole Calculations” as page 40Label “Mole Project” as page 41

+Page 39Topic: MOLE CONVERSIONSObj: Define the concept of a mole and use moles to calculate atoms.

ESQ: How is a mole used as a measurement in chemistry?

Avogadro’s Number and the

Mole

Holy Moley! I love moles!

+

Avogadro’s Number and the Mole!!!

+Avogadro’s number

The number of atoms in 12.00 grams of carbon-12

6.02 x 1023 objects or particles in one mole

(602 000 000 000 000 000 000 000)

+Just like in the activity you just did:

One mole is an amount of substanceOne dozen = 12 objectsOne ream = 500 objectsOne pair = 2 objectsOne mole = 6.02 x 1023 objects

+What day do you think Mole day is???October 23!! (1023)And what time do you think it starts and ends???

6:02 am to 6:02 pmProject guidelines given out next week. Make me laugh!

+Mole

The mole is central to science – it lets you determine how many molecules you have by weighting them

+Molar Mass

The mass (in g units!) of one mole of a pure substance

We can use it as a conversion factor

+Mole

Lithium:atomic mass = 6.941 amu6.941 g in one mole6.941 g/mole

+Mole

Mercury: Atomic mass = 200.59 amu

200.59 g in one mole200.59 g/mole

+Conversion Factors – KNOW THIS!

1 mole = 6.02 x 1023 representative particles aka atoms/molecules = 22.4 L of gas = molar mass (in grams)

+MOLAR ROAD MAPdraw this in your spiral

+Example 1

How many PARTICLES are there in 3.55 moles of rubidium?

+Example 2

How many moles in 24.0 grams of carbon?

+Diatomic molecules – go everywhere as a pair

+Example 3

How many atoms are in 3.65 g of chlorine?

+Example 4

How many liters are in 5.500 x 1025 molecules of hydrogen (H2) gas?