Chapter 11 Notes

Topics: Atom, Molecule, Mole Pages: 3 (879 words) Published: December 2, 2012
Christina Park
2/14/12 pd.3
Chapter 11 Notes
I. Measuring Matter
A. Counting Particles
number of unit for counting is always constant.
a. What is a mole?
mole (mol): the SI unit used to measure the amount of a substance, number of representative particles. representative particle: any kind of particle such as atoms, molecules, formula units, electrons, or ions. Avogadro's number: 6.022 136 7 x 10²³, volume of one mole of a gas determined by Amedeo Avagadro in 1811. B. Converting Moles to Particles and Partciles to Moles

number of moles x 6.02 x 10²³ representative particles /1 mole = number of representative particles number of representative particles x 1 mole / 6.02 x 10²³ representative particles = number of moles II. Mass and the Mole

A. The Mass of a Mole
each atom of carbon-12 has a mass of 12 atomic mass units (amu). atomic masses of all other elements are established relative to carbon-12 molar mass: the mass in grams of any pure substance.

molar mass of any element is numerically equal to its atomic mass and has the units g/mol. B. Using Molar Mass
number of moles x number of grams / 1 mole = mass
III. Moles of Compounds
A. Chemical Formulas and the Mole
the chemical formula for a compound indicates the type of atoms and the number of each contained in one unit of the compound. B. The Molar Mass of Compounds
the mass of a mole of a compound equals the sum of the masses of every particle that makes up the compound. number of moles x molar mass = number of grams
molar mass of a compound demonstrates the law of conservation of mass. C. Converting Mole of a Compound to Mass
calculate molar mass of compound.
convert mol to g by using the molar mass as a conversion factor. moles x number of grams / 1 mole = mass
D. Converting the Mass of a Compound to Moles
calculate molar mass of compound.
use inverse of the molar mass as the conversion factor.
mass x 1 mole / number...
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