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Chapter 10: The Mole 1 mole = 6.02 x 10 23 particles A mole is also called Avogadros number.

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A paper clip is 3.2 cm in length. How many times can of mole of paper clips go around the Earth? (Circumference of the Earth is 25,000 miles, 1 in = 2.54 cm, 1 foot = 12 inches,1 mile = 5,280 feet)

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6.02 x 10 23 particles – atoms, molecules, formula units P. 287-290

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Conversions: Moles Particles, Particles Moles P.290-291 # of moles x 6.02 x 10 23 particles = particles mole # particles x mole = moles 6.02 x 10 23 particles

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Freon - CCl 2 F 2 study sample problem 10.3 on p. 292 How many Fluorine atoms are in 5.5 moles of Freon? 5.5 mol of CCl 2 F 2 x 2 mol F Atoms = 11 mol of F atoms 1 mol of CCl 2 F 2

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The Mass of a Mole of an Element P. 293-294 Conversions: moles mass, mass moles # of moles x # of grams = grams mole grams x mole = moles # of grams

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The Mass of a Mole of a Compound P. 295-296 What is the molar mass of Potassium Chromate?

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The Mole to Mass Relationship P.297-298 1.Find the molar mass of the compound. 2.Convert moles to grams by using molar mass as a conversion factor. Converting Moles to Mass - P. 298-299

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Converting Mass to Moles of a Compound – P. 299

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Particles Mass, Mass Particles Move through the mole tunnel.

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Mole (tunnel) mass Units (atoms, molecules) 6.02 x 10 23 Molar Mass

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Converting Mass to Particles

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Calculating Percentage Composition P.305-307 % composition of an element = mass of element x 100% mass of compound 1.A compound is formed when 9.03 g of Mg combines with 3.48 g of N. What is the percent composition of the compound? 2.When a 14.2 g sample of mercury(II)oxide is decomposed into its elements by heating, 13.2 g of mercury is obtained. What is the percent composition of the compound? 3.Calculate the percentage composition of dicarbon hexahydride, sodium hydrogen sulfate and phosphoric acid.

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Empirical Formula – The Simplest Formula P.309-310 Convert % grams (Assume 100 g) Convert grams moles Divide each mole quantity by the smallest mole quantity Cant have decimals

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Convert grams moles Divide each mole quantity by the smallest mole quantity.

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Determining Molecular Formula A True Formula P.311-312 1.Determine the empirical formula. 2.Divide the molar mass by the molar mass of the empirical formula.

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Hydrates Opal – Silicon Dioxide an example of a hydrate Water is bonded to the atoms of the compound.

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Desiccators Removes water from the surroundings. Circuitry. Electronics and optics. Calcium Sulfate Not soluble in alcohol Calcium Chloride

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Naming Hydrates State the name of the substance and then add a prefix in front of the word hydrate Ex. Na 2 CO 3 * 10H 2 O – sodium carbonate decahydrate

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Hydrated CoCl 2 11.75 g before heating Anhydrous CoCl 2 w/o water 9.25 g after heating Analyzing Hydrates

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Find the mass of the water. Determine the moles of the compound and water. Divide by the smallest mole ratio.

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Section 10-1 Counting Particles Chemists need a convenient method for accurately counting the number of atoms, molecules, or formula units of a substance.

Section 10-1 Counting Particles Chemists need a convenient method for accurately counting the number of atoms, molecules, or formula units of a substance.

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