The Mole.

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Chapter 10 Chemical Quantities

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Presentation transcript:

The Mole

The Mole SI unit for “amount of substance” Chemists use this unit because they deal with such small particles Can be related to: Number of particles Mass Volume

(Avogadro’s number = 6.02 x 1023) Number of Particles 1pair = 2 particles 1 dozen = 12 particles 1 mole = 6.02 x 1023 representative particles (Avogadro’s number = 6.02 x 1023)

Representative Particles refer to the species present in a substance Element Ion Ionic Compound Covalent Compound Rep. Particle Atom Ion Formula Unit Molecule

Representative Particle Examples Atom: Fe, Al, K, S, Na, H, O Ion: Na1+, Cl1-, NO31-, Mg2+ Molecule: H2O, O2, Cl2, CO2, H2, CCl4 Formula Unit: NaCl, K2SO4, AgNO3

Particle Calculation Examples:

Mass Molar mass = the mass of one mole of a substance Gram atomic mass = mass of one mole of an atom Gram molecular mass = mass of one mole of a molecule Gram formula mass = mass of one mole of a formula unit

Will one dozen feathers have the same MASS as one dozen eggs? Explain. What does this tell us about the MASS of one mole of different substances?

Different Substances Have Different Molar Masses… If you have one mole of 2 different substances, they may each have a different mass even though the number of particles (6.02 x 1023) is the same.

Molar Mass Calculations

Converting with Molar Mass Use molar mass to convert from grams  moles or moles  grams 1 mole = molar mass (g)

Volume 1 mole = 22.4 L of a gas at STP Molar Volume – volume of 1 mole of a gas at STP STP = standard temperature (0oC) and standard pressure (1atm) 1 mole = 22.4 L of a gas at STP

Mass/Volume Examples

Percent Composition Percent (by mass) of all elements in a compound Can be calculated by using Molar Mass Can be used as a conversion factor in dimensional analysis

Percent Composition Examples

Empirical Formulas Give the lowest whole-number ratio of all elements in a compound (all of the subscripts in the formula are reduced)

Examples: H2O2 – true formula for hydrogen peroxide HO – empirical formula for hydrogen peroxide CO2 – true formula for carbon dioxide CO2 – empirical formula for carbon dioxide

Calculating Empirical/True Formulas Given the percent composition, it is possible to calculate the empirical formula and the true formula of a substance

Calculation Examples