Name___________________________________ Per. ______

The Mole (Ch. 3 & 7)

OTHS Academic Chemistry

Objectives: Define and use the concept of a mole

Express & manipulate chemical quantities using dimensional analysis, scientific notation, and sig figs

Calculate the number of atoms, ions, formula units or molecules in a sample of material

Calculate percent composition and empirical and molecular formulas

Vocabulary: Dimensional analysis, significant figures, mole, particle, atom, molecule, formula unit, diatomic element, molar mass, percent composition, empirical formula, molecular formula

Memorize: 1. All nomenclature from the last test 2. Mole conversion factors (see table to right) 3. Empirical Formula Calculations Poem:

4. Percent composition formula

Provided: Periodic Table

CHECKLIST: How to be successful in OTHS Academic Chemistry

Pay attention and take notes in class Ask questions in class on material that is not clear Work every page in the practice packet for the unit Check answers to the practice packet online at http://othschem.weebly.com/ Come to tutorials with any chemistry teacher Do the online homework and check solutions once they become available Always do the practice test for every test & ask good questions on review day Keep up with the calendar for the class/be aware of approaching quizzes, tests, & other deadlines Use videos posted on website as a quick and convenient tutorial Read the chapter in the book

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Quick Guide to Understanding Mole Conversions

Mole Conversion Factors 1 mole = 6.02 x 1023 particles 1 mole = “X” grams (where “X” = molar mass) 1 mole = 22.4 L (for any gas at STP)

Circle which conversion factor you would use for converting:

1. 3.20 moles of O2 to L of O2? 1 mole = 6.02 x 1023 particles, 1 mole = X grams, 1 mole = 22.4 L

2. 0.75 moles of CO2 to molecules of CO2? 1 mole = 6.02 x 1023 particles, 1 mole = X grams, 1 mole = 22.4 L

3. 23 g of NaCl to moles of NaCl? 1 mole = 6.02 x 1023 particles, 1 mole = X grams, 1 mole = 22.4 L

4. 3.40 x 1026 atoms of Hg to moles of Hg? 1 mole = 6.02 x 1023 particles, 1 mole = X grams, 1 mole = 22.4 L

5. 7.5 x 1019 formula units of ZnO to moles ZnO? 1 mole = 6.02 x 1023 particles, 1 mole = X grams, 1 mole = 22.4 L

Okay- now set up the following equations and solve:

6. 3.20 moles of O2 = ??? L of O2

3.20 moles O2 x ___________________ = ___________________ L O2

7. 3.40 x 1026 atoms of Hg = ??? moles of Hg

3.40 x 1026 atoms of Hg x ___________________ = ___________________ moles of Hg

8. 75.0 L of NH3 = ??? molecules of NH3

75.0 L of NH3 x ___________________ x___________________ = ___________________ molecules of NH3 1

"Particles" can be atoms, molecules, or formula units.*

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