CHAPTER 7 OUTLINE
		CHEMICAL QUANTITIES
		I. The Mole: A Measurement of Matter
		A. What is a Mole?
		1. Quantitative world
		a. Count -- pair, dozen, etc.
		b. Mass -- lb. of beef, etc.
		c. Volume -- gal. of gas
		2. Relationship between all 3 by conversion factors
		a. Examples on p. 172 (1 doz. apples = 12 apples, 1 doz. apples = 2.0 kg apples, 1 doz. apples = 0.20 bushel apples)
		3. SI counting unit of chemistry = MOLE
		a. Rel. to counting, mass, & volume
		B. The Number of Particles in a Mole
		1. One mole (mol) = 6.02 X 1023 representative particles of a substance
		a. Just like one doz. = 12
		b. 6.02 X 1023 known as Avogadro's Number
		c. Representative Particles -- Atom, molecule, form. unit, or ions
		2. Use as a conversion factor
		3. Find # of atoms in molecule
		C. The Mass of a Mole of an Element
		1. Gram atomic mass (gam) -- atomic mass of an element in grams (Remember amu!)
		a. The ratios are the same for both (C amu:H amu is 12:1 ratio, C grams: H amu is 12:1 ratio!)
		b. The gam of any element = 1 mol = 6.02 X 1023 atoms
		D. The Mass of a Mole of a Compound
		1. Gram molecular mass (gmm) -- mass of 1 mol of a molecular compound
		a. Add atomic mass of atoms in compound
		2. Gram formula mass (gfm) -- mass of 1 mol of a ionic compound
		a. Calculated with the same method as gmm
		II. Mole-Mass and Mole-Volume Relationships
		A. The Molar Mass of a Substance
		1. Molar mass -- mass (g) of one mole of any substance
		a. Which is gmm or gfm per mol
		b. Units are in g/mol
		c. Conversion Factor
		d. Start with mol, then multiply      or      Start with grams, then divide
		B. The Volume of a Mole of Gas
		1. Measured at Standard Temperature and Pressure (STP)
		a. 0oC and 101.3 kPa (1 atm)
		b. At STP, 1 mol of gas = 22.4 L
		c. Molar volume = 22.4 L/mol
		2. Gases have different masses (therefore, different density)
		a. Density to determine molar mass
		C. The Mole Road Map
		1. See page 186
		III. Percent Composition and Chemical Formulas
		A. Calculate the % Composition of a Compound
	1. % by mass of each element in the compound
		2. Total mass of each element divided by the total mass of compound, then multiply by 100%
		B. Using Percent as a Conversion Factor
		C. Calculating Empirical Formulas
		1. The lowest whole # ratio of the atoms of the element in a compound
		a. Used to count atoms or moles
		D. Calculating Molecular Formulas
		1. Simple multiple of Empirical Formula
		Outline based upon:      Matta, M. S., Staley, D. D., Waterman, E. L., & Wilbraham, A. C. (2000). Chemistry, Addison-Wesley. (5th ed.). Menlo Park, CA: Prentice Hall, pp. 171-195.
		Return Home