On the back of p. 19 ColorName of equipment Marking increments
PrecisionMeasurement Red Orange Yellow Green Blue Purple 1)Set up
your chart to look like this. 2)Write page 21 on top of the Duley
Dimensional Analysis 3)Theres no page # for the little page. Put
behind your table of contents. 4)Grab a thumbtack off my desk and
scratch your name onto the top of your calculator. 5)What are the
increments AND precision for this picture? 6) What is the
measurement for the blue box?
Slide 2
Start a new piece of notebook paper Scientific Notation &
Dimensional Analysis p. 20 OBJ: express quantities using scientific
notation & dimensional analysis ESQ: How can measurements be
converted using dimensional analysis?
Slide 3
Scientific Notation Way to simplify BIG and small numbers
Slide 4
Scientific Notation Coefficient x 10 exponent
602000000000000000000000 can be 6.02 x 10 23 exponent
coefficient
Slide 5
Scientific Notation Coefficient x 10 exponent Coefficient MUST
be between 1 and 9 Exponent can be either positive or negative +
exponent large # (> 1) - exponent small # (< 1)
Slide 6
Scientific Notation Convert the following into of scientific
notation 35893 = ____________
Dimensional Analysis Conversion Unit that you have Unit that
you have Unit that you want = Unit that You want X T-diagram
Conversion Factor
Slide 13
Single-step conversions 30 seconds = ? minutes
Slide 14
Example #2 How many inches are in 3.7 feet? (12 inches = 1
ft)
Slide 15
Multi-Step Conversion The conversion factor does NOT contain
both the unit that you have and the unit that you want. The unit
conversion requires multiple (more than one) steps.
Slide 16
You can do this! How many minutes are in 2 days? (given) 2
days
Slide 17
One more How many milligrams are in 160 pounds?
Slide 18
Double deckers!!! Convert 8.89 g/mL into kg/gallon.
Slide 19
Page 33 Title: Avogadros Number and the Mole Holy Moley! I love
moles!
Slide 20
+ Avogadros Number and the Mole!!!
Slide 21
+ Avogadros number The number of atoms in 12.00 grams of
carbon-12 6.02 x 10 23 objects or particles in one mole (602 000
000 000 000 000 000 000)
Slide 22
+ One mole is an amount of substance One dozen = 12 objects One
ream = 500 objects One pair = 2 objects One mole = 6.02 x 10 23
objects
Slide 23
+ What day do you think Mole day is??? October 23!! (10 23 )
And what time do you think it starts and ends??? 6:02 am to 6:02 pm
Project guidelines given out next week. Make me laugh!
Slide 24
+ Mole The mole is central to science it lets you determine how
many molecules you have by weighting them
Slide 25
+ Molar Mass The mass (in g units!) of one mole of a pure
substance We can use it as a conversion factor
Slide 26
+ Mole Lithium: atomic mass = 6.941 amu 6.941 g in one mole
6.941 g/mole
Slide 27
+ Mole Mercury: Atomic mass = 200.59 amu 200.59 g in one mole
200.59 g/mole
Slide 28
+ Conversion Factors KNOW THIS! 1 mole = 6.02 x 10 23
representative particles aka atoms/molecules = 22.4 L of gas =
molar mass (in grams)
Slide 29
+ MOLAR ROAD MAP draw this in your spiral
Slide 30
+ Example 1 How many molecules are there in 3 moles of
water?
Slide 31
+ Example 2 How many atoms are in 3.65 g of iron?
Slide 32
+ HOMEWORK! You have to watch the internet (shut up!). Go to my
website & click Unit 2 Measurement. Watch the Metric Video and
follow instructions. Ill remind you with a text. Werent here that
day? See me after class to get into my Remind 101 app.
Slide 33
+ Diatomic molecules go everywhere as a pair H 2 O 2 F 2 Br 2 I
2 N 2 Cl 2 1 mol Br 2 = 22.4 L of gas 1 mol Br 2 = 6.02 x 10 23
molecules 1 mol Br 2 = 179.8 grams
Slide 34
+ Example 3 How many liters are in 5.50 grams of hydrogen (H 2
) gas?