I swear I didn’t do it!! Ask Tony over at the Chemistry Lab! Don’t you EVAH mess with Vinnie again, do you undahstand me, Joey? Come on Sal, fuggetaboutit! give the kid a break, he didn’t mean to blow up the toilet with elemental Sodium and water! Hey, Sal-- The coast is clear! Where have you guys been? Livin’ in a hole somewhere?

Intro Questions If you have 12 eggs, what quantity do you have? – _______ If you travel 5,280 feet, how far have you traveled? – ______ How can something like this help us in Chemistry?

Section 11-1: Measuring Matter Mole(mol) – SI unit for ________ of substance 1 mole of any substance = – ________ ______ (periodic table) of that substance in grams – 6.02 x representative particles (Also called Avogadro's number) ________ —elements __________ —covalent compounds ________ _______--ionic compounds Converting moles to _________ – Conversion Factors # moles x 6.02 x particles 1 mol Convert 3.5 moles sucrose to molecules

Section 11-1 continued Converting particles to moles – Conversion Factors # particles x 1 mole = 6.02 x particles Calculate the # moles in 4.50 x atoms Zn More problems – page 311 #1-3; page 312 #4, 5-8

Section 11-2: Mass and the Mole 1 mole is also equal to the ______ _____ or mass of 1 mole molar mass = _______ _______ with the units g/mol *Same as ______ ______ except for units Converting Moles to mass: # moles x # grams 1 mol – How many grams are in 3.00 mol Mn?

Section 11-2: Mass and the Mole mass to moles: mass x 1 mol #grams – How many moles are in 525 g Ca? mass to atoms: mass x 1 molx 6.02 x atoms #grams1 mol – How many atoms of gold in 25.0 g?

Section 11-2: Mass and the Mole atoms to mass: # particles x 1 mol x # grams 6.02 x particles 1 mol – How much mass is in 5.50 x atoms of helium? More problems: – page 316 # 11-12; page 318 # 13&14; page 319 # 15-17

Section 11-3 continued Molar mass of compounds – add up parts #moles x molar mass = # grams – Find the molar mass of K 2 CrO 4 moles to mass # moles x # grams 1 mol Convert 2.50 mol of (C 3 H 5 ) 2 S to grams

Section 11-3 continued mass to moles mass x 1 mol = molar mass mass to particles mass x 1 mol x 6.02 x particles molar mass1 mol particles to mass particles x 1 mol x molar mass 6.02 x particles1 mol More problems: – page 321 # 20-24; page 322 # 25-26; page 323 # 27-29; page 324 # 30; page 326 #31-35; page 327 #36-39

Section 11-4: Empirical and Molecular Formulas percent composition mass of element x 100 = % by mass mass of compound percent always adds up to 100 – Find % of H and O in water – Find the percent by mass of each element in Be 3 (PO 4 ) 2

Section 11-4 continued Empirical formula – smallest whole # mole ratio of the elements * May or may not be actual molecular formula – To get: 1.Change g to mol 2.Get mole ratio by dividing by the smaller 3.The ratios are the subscripts *If you are given % composition: assume % is grams Find the empirical formula of a sample with g S and g O. Do problems: p. 119 # 68 a & c, #69, #70

Section 11-4 continued Molecular formula – specific # of atoms of each element in compound experimentally determined molar mass = n mass of empirical formula multiply n by empirical formula subscripts molecular formula = (empirical formula) n Problem: The empirical formula of a substance is CH. The molecular mass of the compound is 78 amu. What is the molecular formula of the compound?

Sect cont. – Chemical analysis indicates a sample is composed of 40.68% C, 5.08% H and 54.24% O and has a molar mass of g/mol. Determine the empirical and molecular formulas of succinic acid More problems – Page 120, do 73 and 74

Section 11-5: The formula for a Hydrate Hydrate – compound with a specific # of water molecules bound to its atoms Naming: – name salt prefix hydrate CaCl 2 2H 2 O calcium chloride dihydrate – Prefixes are the same as those used for covalent compounds (see page 338 for review) Anhydrous – without water used to store water or as drying agents – Used to store solar energy i.e. sodium sulfate decahydrate