THE MOLE Chapter 10 Who is that Little Guy with Squinty Eyes?
THE MOLE NO, Not this mole, this guy has nothing to do with Chemistry!
THINGS YOU SHOULD KNOW Chapter 10 Section 1 and 2 Know what a mole is. Avogadro's Number. Know how to convert between moles and particle. Know how to convert particles into moles. How to determine molar mass. Calculate mole-to-mass conversions Calculate mass-to-mole conversions
METACOGNITION When Things get harder Piano- Swimming- Tennis- Soccer- Basketball- Cycling-
MEASURING MATTER How else do we measure matter? Gallon- Dozen- Ounce- Bakers Dozen- Pair- Pound- Liter-
MEASURING MATTER The mole- SI unit to measure the amount of particles in substance. 1 mole = 6.022 x 10 23 particles Avogadro's number 6.0221367 x 10 23 particles 1mole of = 6.0221367 x 10 23 of
MEASURING MATTER Although all moles have the same number of particles, their mass wont be the same: Draw a mol of H Draw a mol of U 6.022 x 10 23 particles H 6.022 x 10 23 particles U
SEPS How many moles are in 6.022 x 10 23 particles of copper? How many particles are there in 1 mole of zinc? How many moles are in 6.022 x 10 23 particles of Hydrogen? How many particles are there in 1 mole of uranium?
MEASURING MATTER Converting between moles and Particles: Conversion factor (Relationships) 1 mole = 6.022 x 10 23 particles 6.022 x 10 23 particles = 1 mole Ratios (relationships): 1 mol 6.022 x 10 23 particles or 6.022 x 10 23 particles 1 mol
MEASURING MATTER Moles to Particles: Questions: How many particles are in 2.75 mol of Gold? Solution set up: Solution: Given 6.022 x 10 23 particles 1 mol 2.75 mol of Au 6.022 x 10 23 particles of AU = 1.66 x 10 24 particles 1 mol Au of Au
SEPS If there are 4.2 moles of iron, calculate the number of particles of iron.
SEP Change 3.50 moles of glucose into particles of glucose.
MEASURING MATTER Particles to moles: Questions: How many moles are in 1.3623 x 10 24 particles of C 6 H 12 O 6? Solution set up: Solution: Given 1 mol 6.022 x 10 23 particles 1.3623 x 10 24 pt of C 6 H 12 O 6 1 mol C 6 H 12 O 6 6.022 x 10 23 particles C 6 H 12 O 6 = 2.262 mol of C 6 H 12 O 6
SEPS If there are 4.50 x 10 24 zinc atoms, calculate the number of moles of zinc.
SEP If there are 4.05 x 10 23 particles of gold, how many moles of gold do you have?
10-2 MASS AND THE MOLE Molar Mass- The mass in grams of 1 mole of any pure substance. =g/mol Based on Carbon-12 Carbon -12 has a molar mass of 12g /mol Example: Iron-56 1 mol Fe-56 = 6.022 x 10 23 particles. 1 mol Fe = 56 g/mol Fe
SEP Determine the molar mass of the following elements: Sodium has a mass of 22.989 amus Molar mass= g/mol Oxygen has a mass of 15.99 amus Molar mass= g/mol Magnesium has a mass of 24.305 amus Molar mass = g/mol
MASS AND THE MOLE Copper: 1 mol Cu= particles 1 mol Cu= g/mol Cu Nitrogen: 1 mol Ni = Particles 1 mol Ni = g/mol Ni
MASS AND THE MOLE Molar Mass of Compounds: Add all the elements and their masses together. Example: H 2 O 2 x Hydrogen = 2.00 g/mol 1 x Oxygen = 16.00 g/mol Total Molar Mass (g) = 18.00 g/mol How many particles are in 1 mol H 2 O? 6.022 x 10 23 particles of H 2 O
SEP Determine the molar mass of C 6 H 12 O 6. Determine the molar mass of NaCl.
SEP Determine the molar mass for Fe(OH) 3 Determine the molar mass for CO 2.
MASS AND THE MOLE Converting moles to mass: Times the number of moles of the element or compound by the molar mass. 2Na (s) + Cl 2 (g) 2NaCl (s) What is the mass of sodium in this reaction? 2 mol Na Molar mass of Na =23.0 g/mol Solution: 2 mol Na 23.0 g Na 1 mol Na = 46.0 g Na
SEP moles to mass: 6.7 mol of Ti is how many grams of Ti? How many particles of carbon would be present?
SEP If there are 386.00 g of Carbon, how many moles would that be? How many particles of carbon would there be?
HOMEWORK TIME!!!!
QUIZ TIME 10-2
10-3 MOLES OF COMPOUNDS
10-3 WHAT YOU NEED TO KNOW Relationships (ratios) between compounds and elements of that compound. How to determine the number of moles of an atom in a compound.
CHEMICAL FORMULA AND THE MOLE Chemical formulas can help us understand the number of moles in a compound: CCl 2 F 2 (Freon) # of C atoms= 1 # of Cl aroms = # of F atoms = Moles of CCl 2 F 2-1 mol C 2 2 2 mol Cl or 1 mol of Cl 2 2 mol F or 1 mol of F 2
CHEMICAL FORMULA AND THE MOLE Relationships: Look at the different ratios of moles to compound: 1 mol C 2 mol Cl 2 mol F 1 mol CCl 2 F 2 1 mol CCl 2 F 2 1 mol CCl 2 F 2 Lets say you have 5.5 mole of freon, how many moles of Chlorine are there? Moles CCl 2 F 2 moles Cl 1 mol CCl 2 F 2 5.5 mol CCl 2 F 2 2 mol Cl 1 mol CCl 2 F 2
Moles of a compound to moles of an atom: If you have 3.78 mol CCl 2 F 2, determine the number of moles of Carbon.
SEP If there are 8.7 moles of CCl 2 F 2, how many moles of Cl 2 are present?
10-3 MOLES OF A COMPOUND Molar Mass of Compounds (Review) The sum of the masses of all the particles that make up the compound. Determine the molar mass of K 2 CrO 4. If there are 61.94 grams of K 2 CrO 4, how many moles would that be?
EMPIRICAL AND MOLECULAR FORMULAS Chapter 10 Section 4
PERCENT COMPOSITION Percent by mass of each element in a compound. Percent by mass (element) = Mass of element Mass of Compound X 100
PRACTICE PROBLEM NaHCO 3 is the active ingredient in baking soda. Determine the % composition of Na and O if there are 22.99 g of Na and 48.00 grams of O. Steps: Determine the molar mass of NaHCO 3. Divide the mass of Na by the molar mass of NaHCO 3, then times it by 100. Divide the mass of O by the molar mass of NaHCO 3, then times it by 100.
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EMIRICAL FORMULA The formula with the smallest whole number mole ratio of the elements. Percent composition can be used to determine the formula of a compound. Steps: 1. Find the grams of each element. 2. Find the number of moles of each element. 3. Divide all the number of moles by the smallest mole ratio. 4. Determine the ratios between the elements. If a ratio ends in.5, like 2.5, double all the ratios. 2.5 5 5. Write the formula.
SEP Determine the empirical formula for a molecular compound that is made of 40% sulfur and 60% oxygen. Assume there is 100 grams of the molecular compound.
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MOLECULAR FORMULA Specifies the actual number of atoms of each element in one molecule or formula unit of a substance. Always assume there is a 100.0 gram sample. SEP- A sample composed of 40.68% carbon, 5.08% hydrogen, and 54.24 % oxygen, the molar mass of the compound is 118.1g/mol
SEP Conversion % to grams: C=40.68% = 40.68 g C H=5.08% = 5.08 g H O=54.24% = 54.24 g O Convert grams to moles: 3.387 mol C 5.04 mol of H 3.390 mol of O Divide all moles by the smallest mole amount. 3.387 mol of Carbon
SEP Divide all moles by the smallest mole amount. 3.387 mol of Carbon 1 mol C 1.5 mol H 1.0 mol O Ratio is then: 1:1.5:1 Times it by 2 because to obtain whole number ratios 2:3:2 Formula is C 2 H 3 O 2
SEP Calculate the empirical formula mass using the molar mass of each element: 2 mol C x 12.01 g C = 24.02 g C 3 mol H x 1.01 g H = 3.03 g H 2 mol O x 16.00 g 0 = 32.00 g O Total is = 59.05 g/mol Divide molar mass of compound (118.1) by the molar mass of C 2 H 3 O 2 (59.05) 2.000
SEP Multiply subscripts of the empirical formula by to determine the actual molecular formula. 2 x (C 2 H 3 O 2 ) = C 4 H 6 O 4 Check your answer: Determine the molar mass for.
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SEP CONTINUES Page 350: 66, find molecular formula if morphine has a molar mass of 285.34 g/mol
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