Name: Period: Final Exam Fall 2017 Video Review +5 points will be added to the final exam score if the entire packet is complete. The packet is due the class period of the final exam NO EXCEPTIONS! The final exam is 20% of your overall grade. Day 1 Online Practice Quiz Reviews: Day 1 Link #1 = 26 Q Day 1 Link #4 = 25 Q Day 1 Link #2 = 20 Q Day 1 Link #5 = 20 Q Day 1 Link #3 = 19 Q Day 1 Link #6 = 20 Q Day 2 & Day 3 Online Video Reviews: Video Lesson # 1: Ionic Formulas; Using Criss-Cross Method 1. Define an Ionic Bonds: 2. Fill in the blanks: Ionic bonds are between a & 3. Fill in the blank: Metals e- 4. Fill in the blank: Nonmetals (NM) e- 5. Use the criss-cross method to write the formula for magnesium fluoride: 6. Does the one need to be written at the bottom of the formula? 7. Use the criss-cross method to write the formula for sodium phosphide: 8. Use the criss-cross method to write the formula for aluminum oxide: 9. Use the criss-cross method to write the formula for barium oxide: 10. Use the criss-cross method to write the formula calcium nitride: 11. Use the criss-cross method to write the formula sodium fluoride: 12. Use the criss-cross method to write the formula aluminum phosphide: Video Lesson#2: Writing Ionic Formulas 1. Give 2 examples, one example of a Chemical Name and another example of a Chemical Formula : a. Chemical Name: Chemical Formula: 1
2. Looking at the periodic table on the video, what are the charges for the following groups: Charge = 3. Lithium Oxide: Write the charges below: 4. The number of positive charges have to balance the number of negative charges. Explain how 5. What is the final chemical formula for Potassium Nitride: 6. Potassium Nitride: Write the charges below: 7. The number of positive charges have to balance the number of negative charges. Explain how 8. What is the final chemical formula for Potassium Nitride: 9. Sodium Chloride: Write the charges below: 10. The number of positive charges have to balance the number of negative charges. Explain how 11. What is the final chemical formula for Sodium Chloride: 12. Aluminum Oxide: Write the charges below: 13. The number of positive charges have to balance the number of negative charges. Explain how 14. What is the final chemical formula for Aluminum Oxide: 15. Circle answer: Correct or incorrect formula? Li 2O 1 Explain: 16. Circle answer: Correct or incorrect formula? Li + 2O 2- Explain: Video Lesson #3: Transition Metals in Ionic Formulas 1. Describe the location of the transition metals: 2. List the 10 most common transition metals that the presenter has written in his periodic table: 3. Explain how the transition metal elements are different from the other Group I, Group II, and Group III metal ions: 4. What type of cation charges will the Group I elements ALWAYS form (e.g.) Li? 5. What type of cation charges will the Group II elements ALWAYS form (e.g.) Ca? 6. List the cation charges that iron can make: 7. List the cation charges that gold can make: 8. List the cation charges that manganese can make: 9. How can one tell the difference between the different charges for the same transition metal? 10. What is the name of the following: Fe 2+ = Fe 3+ = Au 1+ = Mn 4+ = Mn 6+ = Mn 7+ = 2
11. List the three common Roman numerals for transition metals: 12. What type of cation charge will Manganese II Chloride have: 13. What type of cation charge will Iron III oxide have: 14. Explain why we DON T need Roman numerals for the following compounds: Calcium Fluoride & Sodium Sulfide: Video Lesson #4: Naming Ionic Compounds with Transition Metals 1. In what part of the periodic table is the transition metal family located? Circle below: 2. When metals are a transition metal, what is written in the name: 3. Transition metals are metals with multiple charges. List the charges for Iron, Fe: 4. What is the name of the following iron ions? Fe 2+ = and Fe 3+ = 5. In the formula FeCl 3 which element does NOT change its charge? Circle answer: Fe or Cl 6. How many negative chlorides is there in FeCl 3? 7. So which iron criss-crossed to form the ionic compound FeCl 3? 8. What is the name of FeCl 3? 9. Chromium (II) has the ionic formula Cr 2+. Write the ionic formula for the following transition metals: Copper (I) Iron (III) Vanadium (IV) 10. Explain why Potassium, (in the ionic formula Potassium Iodide), does NOT have a Roman numeral after its name? 11. Does Calcium, (in the ionic formula Calcium Nitride), need a Roman numeral? Explain: 12. There are 2 transition metals that DO NOT form more than one charge. Name those 2 transition metals: and 13. Name the following: AgCl = Name the following: ZnCl = Video # 5: Naming Covalent Molecular Compounds 1. Circle the nonmetals located in the periodic table below: 2. Covalent or also known as molecular compounds consist of what 2 type of elements? Circle your answer: metal + metal nonmetal + nonmetal metal + nonmetal 3. Name 2 examples of covalent, molecular compounds: and 3
4. Circle the metals located in the periodic table below: 5. Ionic compounds consist of what 2 type of elements? Circle your answer: metal + metal nonmetal + nonmetal metal + nonmetal 6. Name 2 examples of ionic compounds: and 7. Name: N 2O 3 8. Name: P 4S 10 9. Name: CF 4 10. Name: PCl 5 11. Name: Cl 2O 7 12. Name: P 4O 6 13. Name: CO 14. Which nonmetal has an issue with number prefixes? 15. What is the hint that the instructor gives when name this element? 16. Review: using the number prefix mono- is NEVER used when the first element in a covalent compound has only ONE in the formula. Circle answer: True or False Video Lesson #6: Percent Composition 1. Define percent composition: 2. Calculate the percent composition of %H and %O in H 2O : 3. Write the percent composition formulas: 4. Calculate the percent composition of H 2S: 5. Calculate the percent composition of C 6H 12O 6: 6. Calculate the percent composition of Fe 3(PO 4) 2: Video Lesson #7: Concentration of Solution in Mass Percent 1. How is mass percent signified? 2. Write the formula for mass percent: 3. Remember, solute is the smaller number and solvent is the bigger number and solution is mass of solute + mass of solvent don t forget that!!! Also, water is the universal solvent!!! Calculate the mass percent of 35.6 g KNO 3 and 80 g of solution: 4. Fill-in the blanks: solute + = 5. Calculate the mass percent of 46.5 g NaCl in 75 g H 2O: 6. You will NOT have units in milligrams (mg), all units will be in units of grams (g). Calculate the mass percent of 0.286 g KOH in 4.8 g H 2O: Video Lesson #8: Calculating the % Composition of a Hydrate 1. Using CuCl 2 2 H 2O circle the hydrate salt and then circle the salt alone (anhydrate). 2. Using the words percent, part and whole, write the formula for percent composition: 4
3. Using the words percent mass of water and mass of whole compound, write the formula for percent composition: 4. Define hydrate salt and give 2 examples: 5. Define anhydrous salt and give 2 examples: 6. What color is the anhydrous cobalt salt and the hydrous cobalt salt? 7. Using the given AMU s for each element (notice that the water H 2O is added to the Na 2CO 3 compound What is the total AMU of Na 2CO 3 10 H 2O: 8. What is the total AMU of 10 H 2O: 9. Calculate the percent water in the compound Na 2CO 3 10 H 2O: Video Lesson #9: Atoms, Isotopes, and Ions 1. Define the atom using the 5 given bullets points: 2. List the periodic table info: (list 4 given bullet points); 3. Using the symbol given label the following, chemical symbol, AMU, atomic #, & charge: 40 20Ca +2 4. What s the definition of a stable atom? 5. Which family/group does NOT have a charge (they do not gain or lose electrons): 6. Write the symbol for Calcium with an AMU of 20 and atomic # of 20 without a charge: 7. Define atomic number: 8. Where is the atomic number written on the chemical symbol? 9. Define the mass number (also called the AMU): 10. Where is the mass number (also called the AMU) written on the chemical symbol? 11. Define isotopes: 12. Which subatomic does NOT change?? 13. Which subatomic determines what an atom is? 14. Define ions: 15. What type of charge does the electron have? 16. Define cation: 17. Define anion: 18. 23 11Na + What type of ion? Circle answer: Cation Anion Calculate the p+, n, and e- 19. 16 8O 2- What type of ion? Circle answer: Cation Anion Calculate the p+, n, and e- 20. 35 17Cl - What type of ion? Circle answer: Cation Anion Calculate the p+, n, and e- 21. 14 6C What type of ion? Or is this just an atom? Explain why? Calculate the p+, n, and e- 22. 1 1H + What type of ion? Circle answer: Cation Anion Calculate the p+, n, and e- 23. 2 1H + What type of ion? Circle answer: Cation Anion Calculate the p+, n, and e- 24. List the 2 hydrogen isotopes: and Video Lesson #10: Density 1. Define density: Write the formula for density: 2. Explain how density can be used as a physical property: 3. What are the common units for density: 4. What is the mass of the rubber stopper: 5. What is the Initial volume of the water: 6. What is the final volume of the water: 7. What is the volume of the rubber stopper: 8. Calculate the density of the rubber stopper: 9. Explain how temperature can change density: 5
Final Exam Practice Problems: 1. What is meant by the term chemical change? What is meant by the term physical change? 2. Are all solutions mixtures? Are all mixtures solutions? Explain. 3. What is meant by the term pure substance? 4. What is the difference between a homogeneous mixture and a heterogeneous mixture? 5. What does it mean to say that a compound has a constant composition? 6. Given the following mass, volume, and density information, calculate the missing quantity. a. mass =? g; volume = 124.1 ml; density = 0.821 g/ml b. mass = 142.4 g; volume =? ml; density = 0.915 g/ml 7. Calculate the amu of each compound below and then find the percent composition of the element indicated: a. K2CrO4 (Calculate the % O): b. AuCl3 (Calculate the % Cl): c. SiH4 (Calculate the % Si): d. Ca3(PO4)2 (Calculate the % P): 8. Calculate the percent water in the hydrate: MgSO4 7 H2O 9. Calculate the percent water in the hydrate: Zn(NO3)2 6 H2) 10. Define solution, solute, and solvent: 11. Suppose that 4.25 g of NaCl and 7.50 g of KCl are both dissolved in 125 g of water. Calculate the percent by mass of each component of the solution. 12. What are isotopes? 13. Which general area of the periodic table contains the metallic elements? Which general area contains the nonmetallic elements? 14. What are ions? How are ions formed from atoms? To what do the terms cation and anion refer? 15. To what do the atomic number and the mass number of an isotope refer? How are specific isotopes indicated symbolically? Give an example and explain. 16. Indicate the number of protons, neutrons, and electrons in isolated ions having the following nuclide symbols: a. 19 F 1- b. 24 Mg 2+ c. 56 Fe 3+ 17. Calculate the atomic mass of silicon. The three silicon isotopes have atomic masses and relative abundances of 27.9769 amu (92.2297%), 28.9765 amu (4.6832%) and 29.9738 amu (3.0872%). 18. Calculate the atomic mass of lead. The four lead isotopes have atomic masses and relative abundances of 203.973 amu (1.4%), 205.974 amu (24.1%), 206.976 amu (22.1%) and 207.977 amu (52.4%) 19. A chemist determines that 1.26 g of iron reacts with 0.54 g of oxygen to form rust. What is the percent composition of each element in the new compound? 20. In the lab, a chemist analyzed a sample of methanol and found that it was made of 6.2 g of carbon, 4.1 g of hydrogen, and 15.9 g of oxygen. What is the percent composition of each element? 6