Chapter 11:
The Mole
11.1 Measuring Matter
counting particles, Avogadro’s Number 6.02 x 10
^{23}, mole,
 mole ↔ particle equations
 # moles x 6.022 x 10^{23} particles/mole = # of particles
 # particles x 1 mole / 6.022 x 10^{23} particles = # of moles
11.2 Mass and the Mole
mass of a mole, molar mass,
 mass ↔ mole equations
 # of moles x # of grams / mole = # of grams
 mass (in grams) / molar mass (grams / mole) = # of moles
11.3 Moles of Compounds
chem formulas & mole, molar mass of compounds,
mole ↔ mass of compound
mass ↔ particles (molecules) of compound
11.4 Empirical and Molecular Formulas
Percent composition of compound, empirical formula, determining molecular formula
% by Mass = Mass of Element / Mass of Compound x 100
11.5 Formula of a Hydrate
Naming hydrates Na_{2}CO_{3} · 10 H_{2}O is a decahydrate (10 waters per molecule)
Empirical formula, molecular formula
Molecular formula = (empirical formula subscripts) n
Section 11.1 Measuring Matter
 3/4/2019 p312 4 a,b,c,d  must use format shown in class
 3/4/2019 VIDEO LINK  Tyler DeWitt on x & ÷ significant figures


Section 11.2 Mass and the Mole
 3/5/2019 p 316 12 a,b,c,d  format as shown in class
 3/5/2019 VIDEO LINK  x and divide with powers of 10 and significant figures (shown in class today)
 3/6/2019 p318 13 a,b,c,d,e
 3/11/2019 p. 318 14 a,b,c,d,e (8 pts)


Section 11.3 Moles of a Compound

Section 11.4 Empirical and Molecular Formulas

Section 11.5 The Formula for a Hydrate
 

Section 11.1 Measuring Matter
 3/4/2019 p311 13  must format as shown in class

Section 11.2 Mass and the Mole
 3/7/2019 p318 13 a,b,c,d,e and p319 15,16,17

Section 11.3 Moles of a Compound

Section 11.4 Empirical and Molecular Formulas

Section 11.5 The Formula for a Hydrate
 

Section 11.1 Measuring Matter

Section 11.2 Mass and the Mole
Standard 3 c  Conservation of Matter and Stoichiometry
View Standard 3 State Standard: One mole equals 6.02x10^23 particles (atoms or molecules).
Students Will be able to:Use the mole concept to calculate the number of particles within a giving mass of a substance Book Reference Pages: 317319
Standard 3 d  Conservation of Matter and Stoichiometry
View Standard 3 State Standard: How to determine molar mass of a molecule from its chemical formula and a table of atomic masses, and how to convert the mass of a molecular substance to moles, number of particles of volume of gas at standard temperature and pressure.
Students Will be able to:Calculate the molar mass from a chemical formula. Convert mass to moles to volume Book Reference Pages: 313319


Section 11.3 Moles of a Compound
Standard 3 c  Conservation of Matter and Stoichiometry
View Standard 3 State Standard: One mole equals 6.02x10^23 particles (atoms or molecules).
Students Will be able to:Use the mole concept to calculate the number of particles within a giving mass of a substance Book Reference Pages: 325327
Standard 3 d  Conservation of Matter and Stoichiometry
View Standard 3 State Standard: How to determine molar mass of a molecule from its chemical formula and a table of atomic masses, and how to convert the mass of a molecular substance to moles, number of particles of volume of gas at standard temperature and pressure.
Students Will be able to:Calculate the molar mass from a chemical formula. Convert mass to moles to volume Book Reference Pages: 322327


Section 11.4 Empirical and Molecular Formulas

Section 11.5 The Formula for a Hydrate
Standard 3 D  Conservation of Matter and Stoichiometry
View Standard 3 State Standard: How to determine molar mass of a molecule from its chemical formula and a table of atomic masses, and how to convert the mass of a molecular substance to moles, number of particles of volume of gas at standard temperature and pressure.
Students Will be able to:Calculate the molar mass from a chemical formula. Convert mass to moles to volume Book Reference Pages: 338343

 

 Tutorial for calculating mass <> moles: Summary box and 2 detailed examples of converting moles to other units Std 3e
 Avogadro’s Number in Calculations: Detailed examples and practice problems that use Avogadro's # in calculations Std 3c
 Relating amu to g, # of atoms and gmw: Explanation of the atomic mass unit (AMU) & relating it to mass Std MISC
 Converting grams to moles to atoms: Another way to explain converting g <> moles <> atoms using bridge analogy Std 3
 Grams <>Moles<>Atoms (Handwritten): summary of how to make these conversions with insert from p. 327 Fig 118 (Ch 11.3)
 Multiply and Divide Powers of 10: Multiply & Divide powers of 10 in this tutorial. It guides you through how to multiply and divide numbers attached to 10^{x}
 Mole <> rep. particle Conv. Practice: This tutorial is a worksheet that has 2 examples and 10 problems  Mole <> representative particle Conversion Practice  Tutorial
 Formula of a Hydrate  how to calculate: Formula of a Hydrate  how to calculate, including one example with complete solution
Formula of Hydrate
● Examples of several hydrates and how to calculate formula of hydrate from lab results Visit Site

General
● Introduction to the mole and its meaning and use (Visionlearning) Visit Site
● Professor Mole's Visit Site
● Khan academy vid showing what a mole actually is. Very well done Visit Site

Mole Conversions
● Mole conversion tutorial & help  uses grids Visit Site
● Calculator to figure gram molecular weight Visit Site
● Tutorial on Limiting Reagent, Theoretical Yield, and % Yield (UW Oshkash) Visit Site

Stoichiometry  Ch 11.2
● Problem Solving Skills with moles (CHP) Visit Site
● Tutorial useful in 5 areas of stoichiometry & the mole Visit Site
● Sodium  Scroll down to "Sodium Party". Lots of videos & background how Na reacts with water and also O_{2}. These guys are crazzy!!! Visit Site

Wigger Vids
● Formula of a Hydrate calculated for p. 349 prob. 152. Detailed discussion of how solve this problem. Visit Site
● BASIC CONVERSIONS  A graphic from page 319 of our textbook is used as a visual representation of the process of converting particles <> mol and g <> mol. Lecture 1 Visit Site
● BASIC CONVERSIONS  Conversions are show for one substance only. We are first changing moles > particles in our first example, and then changing g > mol. Lecture 2 Visit Site
● g molecule > mol molecule > mol atom > atoms in problem 31 a p.326 Visit Site
 
