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)There’s 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?

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?

Scientific Notation Way to simplify BIG and small numbers

Scientific Notation Coefficient x 10 exponent can be 6.02 x exponent coefficient

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)

Scientific Notation Convert the following into of scientific notation = ____________

Your turn! = ___________ = ________ = ___________

Scientific Notation Convert the following out of scientific notation x 10 4 = ________ x = ________ Hi Mrs. Duley!

Dimensional Analysis Used to convert between units You need to use a conversion factor

Conversion Factor Ratio equal to “1” Contains the unit that you currently have and the unit that you want to convert to

Examples: 12 inches = 1 foot 12 inches 1 foot 12 inches 1 foot OR

Dimensional Analysis Conversion Unit that you have Unit that you have Unit that you want = Unit that You want X  T-diagram Conversion Factor

Single-step conversions 30 seconds = ? minutes

Example #2 How many inches are in 3.7 feet? (12 inches = 1 ft)

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.

You can do this! How many minutes are in 2 days? (given) 2 days

One more… How many milligrams are in 160 pounds?

Double deckers!!! Convert 8.89 g/mL into kg/gallon.

Page 33 Title: 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 grams of carbon x objects or particles in one mole ( )

+ One mole is an amount of substance One dozen = 12 objects One ream = 500 objects One pair = 2 objects One mole = 6.02 x objects

+ 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!

+ 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 = amu g in one mole g/mole

+ Mole Mercury: Atomic mass = amu g in one mole g/mole

+ Conversion Factors – KNOW THIS! 1 mole = 6.02 x representative particles aka atoms/molecules = 22.4 L of gas = molar mass (in grams)

+ MOLAR ROAD MAP draw this in your spiral

+ Example 1 How many molecules are there in 3 moles of water?

+ Example 2 How many atoms are in 3.65 g of iron?

+ HOMEWORK! You have to watch the internet (shut up!). Go to my website & click “Unit 2 – Measurement.” Watch the Metric Video and follow instructions. I’ll remind you with a text. Weren’t here that day? See me after class to get into my Remind 101 app.

+ 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 molecules 1 mol Br 2 = grams

+ Example 3 How many liters are in 5.50 grams of hydrogen (H 2 ) gas?