The Mole -just as a _____ is always ____, a _______ is always _______, a ______ is always ____, and a _____ is always ____, a _____ is always ____________________________, or __________, and just like it is sometimes easier to buy things by the _______ or by the _____, it is sometimes easier to consider numbers of _________ of _______ by the _____ I. Converting Moles to Particles and Particles to Moles

The Mole I. Converting Moles to Particles and Particles to Moles How many molecules in 4.5 moles of sucrose? How many moles in 1.75 x 1025 molecules of water?

The Mole II. Molar Mass -the _______ of ______ are established ________ to the mass of one __________ atom, which has ____ _________ and ____ __________ -____-________ of the mass of a __________ atom, or about the mass of a _______ or a ________, is called an _______ _____ _____, or _____ -the ______ _____ is the _____ of one _____ of an element, and is numerically equal to the ________ _____, but with units of ______ per _____, so the _______ _____ of a Carbon-12 atom is ___ ____, and the ______ _____ of Carbon-12 is ___ ______ per _____

The Mole II. Molar Mass A. Converting Mass to Moles and Moles to Mass What is the mass of 0.415 moles of Vanadium? How many moles of Tantalum are in 75 grams of Tantalum ?

The Mole II. Molar Mass A. Converting Mass to Atoms and Atoms to Mass How many atoms are there in 99.838 g Uranium? What is the mass, in grams, of 1.1703 x 1024 atoms of Niobium?

The Mole II. Molar Mass A. Converting Mass to Molecules and Molecules to Mass How many molecules are there in 456 g Silicon dioxide? What is the mass, in grams, of 1.75 x 1026 molecules of cyclohexane?

The Mole III. Empirical and Molecular Formulas A. Calculating Percent Composition What is the percent composition of Sodium, Sulfur, and Oxygen in Sodium Sulfate?

The Mole III. Empirical and Molecular Formulas A. Calculating Percent Composition What is the percent composition of Carbon, Hydrogen, and Oxygen in fructose, C6H12O6?

The Mole III. Empirical and Molecular Formulas B. Determining Empirical Formula from Percent Composition What are the empirical and molecular formulas for Ibuprofen if the molar mass is 206 g/mole and the percent composition of 75.7% C, 8.80% H, and 15.5% O?

The Mole III. Empirical and Molecular Formulas B. Determining Empirical Formula from Percent Composition What are the empirical and molecular formulas for Glycerol if the molar mass is 92.11 g/mole and the percent composition of 39.12% C, 8.75% H, and 52.12% O?

The Mole III. Empirical and Molecular Formulas B. Determining Empirical Formula from Percent Composition What are the empirical and molecular formulas for Naphthalene if the molar mass is 128 g/mole and the percent composition of 93.7% C and 6.3% H?

The Mole III. Empirical and Molecular Formulas B. Determining Empirical Formula from Percent Composition What are the empirical and molecular formulas for a Lead chloride compound if the molar mass of the compound is 349.0 g/mole and the percent composition is 59.37% Pb?

The Mole III. Empirical and Molecular Formulas A. Calculating Percent Composition -lab 1. Hypothesis 2. Prediction 3. Gathering Data

The Mole III. Empirical and Molecular Formulas A. Calculating Percent Composition -lab 3. Gathering Data -procedure 4. Analyzing Data 5. Drawing Conclusions

-hydrates are __________ that have a specific number The Mole IV. Hydrates -hydrates are __________ that have a specific number of ______ molecules attached to them A. Naming Hydrates Formula Name

The Mole IV. Hydrates B. Calculating the Formula for a Hydrate What is empirical formula and for a hydrated compound of Copper(II) sulfate, if 2.50 grams of blue CuSO4·nH2O is heated in a crucible until 1.59 grams of white anhydrous CuSO4 remains ?