The Mole Unit Acc Chemistry 14-15 http://rhsaccchem.sfinstructionalresources.wikispaces.net/home Name: A. Lab Bead Mania B. Lesson 1 - The Mole and Molar Mass C. Practice The Mole and Molar Mass D. Lesson 2 Significant Digits E. Practice Significant Digits F. Lesson 3 - Converting between particles, moles and grams G. Practice - Converting between particles, moles and grams H. Lab - Chalk Talk I. Lab How Many Molecules of Water are in Lake Erie J. Quiz 1 K. Lesson 4 - Percent Composition L. Practice - Percent composition M. Lab - How Sweet You Are N. Quiz 2 - Percent Composition O. Lesson 5 - Empirical Formulas P. Practice - Empirical Formulas Q. Lab - The Strange Case of Moles Airline R. Lesson 6 - Molecular Formulas S. Practice - Molecular formulas T. Quiz 3 - Empirical vs. Molecular Formulas U. The Mole Unit Review V. The Mole Unit Test A. Lab Bead Mania B. Lesson 1 - The Mole and Molar Mass C. Practice The Mole and Molar Mass (pg 309) 1. Define mole. 2. How is a mole similar to a dozen? 3. The mole represents an enormous number called Avogadro s number. Write this number. a. Explain why Avogadro s number is so huge. b. The smallest piece that makes up a substance is dependent on the type of substance. This is called a representative particle. i. For elements the representative particle is an, for compounds the representative particle is a. Page 1 of 10 MM
4. 1 mole of any substance contains particles. 5. Explain why chemists use the mole. 6. Which has a larger mass a dozen limes or a dozen eggs? Justify your answer. 7. Explain what is meant by molar mass. Determine the molar mass for each of the following compounds. Show your work. No work = no credit 8. CaCl 2 10. C 2 H 5 OH 9. (NH 4 ) 3 PO 4 11. C 12 H 22 O 11 (sucrose) Mixed Review Answer the following questions: 12. Which are there more of on the periodic table: Metals, nonmetals or metalloids? 13. Which type of element loses electrons to create positive ions? 14. Name the shapes that can produce polar molecules. 15. Which of the types of substance (elements, compounds or mixtures) can be separated by physical means? 16. Which element will have the smaller atomic radius: Arsenic or Phosphorus? D. Lesson 2 Significant Digits Page 2 of 10 MM
E. Practice Significant Digits Determine the number of significant digits in each number. 1) 0.012 2) 100 3) 120. 4) 0.2070 5) 0.0102 6) 12,000 7) 12,000. 8) 15.0 9) 5.56 x 10-4 10) 0.00010 11) 98.06501 12) 1.0 x 10-9 Round each number to the specified significant digits. 13) 790,001.01 1 sig. dig. 14) 665.001 2 sig. digs. 15) 15,984,123 4 sig. digs 16) 789.65 3 sig. digs. Atomic Structure Unit Review Fill in the chart. # Element protons # neutrons M/NM/ML? Noble gas notation Sodium 23 Phosphorus 31 Antimony - 75 F. Lesson 3 - Converting between Particles, Moles and Grams G. Practice - Converting between Particles, Moles and Grams 1. What is the relationship between the following a. 1 mole Li = atoms Li b. 1 mole Li = grams Li c. 1 mole NaCl = grams NaCl d. 1 mole NaCl = molecules NaCl Page 3 of 10 MM
Complete the following conversions. You MUST show your dimensional analysis. No work = no credit Mole - Particles 2. Fill in the dimensional analysis conversion factor for converting from representative particles to moles 1.23 x 10 23 atoms Ca = 0.204 mols Ca 3. Fill in the dimensional analysis conversion factor for converting from moles to representative particles 1.25 mols H 2 O = 7.53 x 10 23 molecules H 2 O 4. Determine the number of atoms in 2.50 mol Zn. 5. How many moles contain 5.75 x 10 24 atoms Al? Mole Grams 6. Determine the mass in grams of 3.57 mol Ag. 7. Determine the number of moles in each of 23.7 g S. 8. What is the mass of 0.0535 moles of (NH 4 ) 3 PO 4? 9. How many moles are in 45.0 g CaCl 2 Page 4 of 10 MM
Mole Particles Grams 10. Fill in the dimensional analysis conversion factor for converting from representative particles to grams 1.23 x 10 23 atoms Ca = 8.18 grams Ca 11. Fill in the dimensional analysis conversion factor for converting from moles to representative particles 22.5 grams H 2 O = 7.52 x 10 23 molecules H 2 O 12. How many atoms are in 76.63 g Li? 13. What is the mass in grams of 8.62 x 10 24 atoms Mn? Reactions Unit Review Balance the following reactions 14. PH 3 P 4 + H 2 15. H 2 + O 2 H 2 O 16. N 2 + H 2 NH 3 17. Al + Pb(NO 3 ) 2 Al(NO 3 ) 3 + Pb 18. KOH + H 3 PO 4 K 3 PO 4 + H 2 O 19. Cu + AgNO 3 Cu(NO 3 ) 2 + Ag 20. Na + Cl 2 NaCl H. Lab - Chalk Talk I. Lab How Many Molecules of Water are in Lake Erie? Page 5 of 10 MM
J. Quiz 1 Perform conversion between all units including mass, moles, and particles (atoms and molecules). K. Lesson 4 - Percent Composition L. Practice - Percent Composition 1. Define percent composition. Complete the following math calculations to determine percent composition. No work = no credit 2. Determine the percent composition of calcium chloride, CaCl 2. 3. Calculate the percent composition of sodium sulfate, Na 2 SO 4. 4. Which has the larger percent by mass of sulfur, H 2 SO 3 or H 2 S 2 O 8? 5. Which has the higher percent by mass of hydrogen - phosphoric acid (H 3 PO 4 ) or hydrochloric acid (HCl)? Page 6 of 10 MM
Mixed Review 6. When completing a single replacement reaction, metals always replace. 7. The products of a combustion reaction are. 8. How does an ion differ from an atom? 9. Ionic compounds are made up of. 10. For a bond to be polar, the electronegativity difference must be higher than. M. Lab - How Sweet You Are N. Quiz 2 - Percent Composition Calculate the percent composition for each element in a molecule. Analyze compounds to compare the percent composition of a single element. O. Lesson 5 - Empirical Formulas P. Practice - Empirical Formulas 1. What is an empirical formula? Complete the math calculations to figure out the empirical formulas. No work = no credit. 2. The pain reliever morphine contains 17.900 g C, 1.680 g H, 4.255 g O and 1.228 g N. Determine the empirical formula. Page 7 of 10 MM
3. A blue solid is found to contain 36.84% nitrogen and 63.16% oxygen. What is the empirical formula for this solid? 4. A solid compound decomposes when heated in the laboratory. Given the following data, determine the empirical formula for the initial compound. Reaction Equation Item Mass A x B y(s) ---------> xa (s) + yb (g) Solid Product Gas Product 4.20 g 0.59 g Molar mass element A is 84.0 g/mol element B is 23.7 g/mol Properties of Elements Review: Give the special name to the following groups on the periodic table. Group 1 Group 2 Group 17 Group 18 The groups (columns) on the periodic table are also called. The rows on the periodic table are called. Q. Lab - Strange Case of Moles Airline Page 8 of 10 MM
R. Lesson 6 - Molecular Formulas S. Practice - Molecular Formulas 1. What is the difference between a molecular formula and an empirical formula? 2. Can an empirical formula also be a molecular formula? (YES or NO) Complete the math calculations to figure out the molecular formulas. No work = no credit. 3. Analysis of a chemical used in photography indicates an empirical formula of C 3 H 3 O. The molar mass is found to be 110.0 g/mol. Determine the molecular formula. 4. A compound was found to contain 49.98 g carbon and 10.47 g hydrogen. The molar mass of the compound is 58.12 g/mol. What is the molecular formula? 5. Azobenzene is an important intermediate in the manufacture of dyes. It contains 79.1% carbon, 5.55% hydrogen, and 15.4% nitrogen. It has a molar mass of 182 g/mol. What is the molecular formula? Page 9 of 10 MM
Bonding Review Write the correct compound formulas. Identify them as covalent of ionic. 6. Methane (IONIC or COVALENT) 7. Zinc hydroxide (IONIC or COVALENT) 8. Copper (I) sulfide (IONIC or COVALENT) 9. Oxygen difluoride (IONIC or COVALENT) T. Quiz 3: Empirical & Molecular Formulas Calculate the empirical formulas from percent composition or from mass composition. Calculate molecular formulas when given empirical formulas and molecular mass. * You may need to calculate the empirical formula. U. The Mole Unit Review V. The Mole Unit Test Page 10 of 10 MM