Section 1: Water, Solubility & ph
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1 IPC Fall Semester 2017 Final Exam Review Complete this review on your own paper and staple your answers to this review. Each completed section is worth 3 points on your semester exam. The more you have finished, the more points you will earn. DUE ON YOUR FINAL EXAM DAY!!! Section 1: Water, Solubility & ph 1. Draw a water molecule and label the hydrogen and covalent bonds. 2. List the properties of water and define each. PROPERTIES OF WATER Polar DEFINE Cohesion Adhesion Surface Tension Capillary Action High Specific Heat Universal Solvent Less Dense as a Solid and Floats 3. Compare and contrast acid to base scientifically. Give two examples of each. 4. Why does your stomach have enzymes with the ph of 2? Is your stomach more acidic or basic? 5. Would an acid or base have more H + ions? 6. Would an acid or base have more OH- ions? 7. Where on a ph scale would acids be located? 8. Where on the ph scale would bases be located? 9. What is the sum of the ph and poh in a substance? 10. Why is water said to be polar? Why is this an important property of water?
2 11. What type of chemical bond holds the oxygen and hydrogen molecules together in a water molecule? Is this a strong or weak bond? 12. How many water molecules will attach themselves to a single water molecule? Why do they do this? What chemical bond causes this to happen? Is this a strong or weak bond? 13. How does water dissolve other substances? Are these substances polar or non-polar? Why? Use the solubility graph below to answer questions How many grams of NaCl dissolves at 70 C? 15. At what temperature will 140 grams of KI dissolve? 16. How many grams of KNO3 can be dissolved in 200 g of water at 50 C?
3 Section 2: Biomolecules 1. List the organic molecules. Why are they considered organic? 2. Differentiate the processes of dehydration synthesis and hydrolysis. Explain what biomolecule helps catalyze the reaction to happen. Give one example of where each process happens in the real world. 3. Name the 3 parts that make up a nucleotide. 4. Deoxyribose is a sugar found in DNA or RNA? 5. What does RNA stand for? 6. Explain the structure and function of an enzyme and state which biomolecule it is. 7. What does denature mean? What happens to proteins when they are denatured? 8. Using the following diagram, LABEL active site, substrate, enzyme, lock and key fit, and product. 9. Complete the following chart: Protein Nucleic Acids Carbohydrates Lipids Elements in biomolecule/polymer Where synthesized (made) in cell Function Monomer Examples
4 10. Compare and contrast DNA to RNA in a Venn diagram. (five differences and two similarities) 11. Be able to recognize these functional groups. Draw each one and label. Hydroxyl Amine Sulfhydryl Carboxyl Methyl Phosphate Section 3: Process Skills 12. Every three times I clean my bedroom, my mother makes me an apple pie. I cleaned my bedroom 9 times. How many apple pies does she owe me? (What?! Your mother doesn t reward you for cleaning your bedroom? To make up for that injustice, you may have this very easy problem.) 13. Time flew by when you were on that bike ride. Your mom and dad are going to get onto you because you were out for a total of 3 hours. They are worried because they don t know if you are putting enough effort into school. To make sure you are being responsible, they ask you how long you were out in seconds. Let s see if you got grounded! 14. Right before you go to sleep, you decide to weight yourself. You see that you have lost 3 kilograms! You want to brag to your friends but 3 sounds like a pretty low number. To make this number larger, you converted this number to centigrams. What is the correct conversion to centigrams?
5 Conversions to be used in problems How many slices will be eaten by 45 people? 16. How many people could you invite to a party if you could order $ worth of pizza? 17. If you had 3 parties last month, how many slices of pizza did you serve? 18. How many centimeters are in 7.4 meters? 19. What is 450 milliliters in liters? 20. The mass of a premature baby is usually given in units of grams. If a baby weighs 1550 g, what is the mass in kilograms? 21. The distance from a Port Huron to the Indiana State line is approximately kilometers (via I-94). Express this distance in meters. 22. A piece of wood that measures 3.0 cm by 6.0 cm by 4.0 cm has a mass of 80.0 grams. What is the density of the wood? Would the piece of wood float in water? (volume = L x W x H) Show all work!!! 23. The volume of a solution was measured in a graduated cylinder (shown on the right). If the mass of solution is measured to be grams, what is the density of the solution? Show all work. 24. What is the density of a 100 g object with a volume of 250 ml? 25. A loaf of bread has a volume of 2270 cm3 and a mass of 454 g. What is the density of the bread? 26. A block of wood has a density of 0.6 g/cm3 and a volume of 1.2 cm3. What is the mass of the block of wood? 27. A 800 g boulder has a density of 8 g/cm3. What is the volume of the boulder?
6 Section 4: Periodic Table, Models, and Bonding 1. Label the groups, periods, metals, nonmetals, and metalloids. Be able to identify the most reactive and least reactive elements. Be able to identify characteristics of each element by its placement on the periodic table. Label the trends (reactivity and atomic radius) as you proceed across the periodic table from left to right, and from top to bottom. 2. Draw and fill in chart with the correct answers. Proton Neutron Electron Charge Location in Atom Size 3. Compare and contrast metals, nonmetals, and metalloids characteristics 4. Compare and contrast a stable and unstable atom. Are majority of the atoms on the periodic table stable or unstable? Explain. 5. What is the duet-octet rule and how does it affect bonding? Draw a Bohr s models of a Sodium atom and a Neon atom and compare to each other. 6. What subatomic particles are responsible for bonding and how do they affect the bonding process? Define electrostatic force. What are the rules of attraction and repulsion between electric charges? 7. Compare and contrast intermolecular and intramolecular forces. Give 3 examples of each. 8. Compare and contrast covalent and ionic bonds. Give an example of each. 9. Compare and contrast polar covalent and nonpolar covalent bonds. Give an example of each. 10. Draw a Lewis dot structure of Sodium & Chlorine. Why would Sodium bond with Chlorine? What type of bond would it be? What are the charges (oxidation numbers) on Sodium Chloride? Use the Drop and Switch Method to find the chemical compound created when Sodium and Chlorine Bond. 11. What on the periodic table gives information for the # of valence electrons, # of orbitals, and electronegativity? 12. Define electronegativity and how it affects elements as they increase in atomic number. Which element is the most electronegative? 13. Why is water like a magnet? 14. Compare and contrast a cation and anion. Why do ions have an electrical charge?
7 15. What do intramolecular forces hold together? What do intermolecular forces hold together? 16. What is a diatomic element? What are the 7 diatomic elements? 17. Label the following polar covalent bond, nonpolar covalent bond, ionic bond, or hydrogen bond. Label whether they are an intramolecular force or intermolecular force. Section 5: Matter 1. What are 5 indicators (signs) of chemical change? 2. Which of the following words or phrases are a physical change (PC)? Which are a chemical change (CC)? Label each word or phrase with the correct one. Dissolving sugar in water Photosynthesis Burning gas Melting butter Vaporization of water Dry Ice Sublimating Condensation Digestion of proteins into amino acids Cutting grass Cooking an egg Curdling of milk Grass growing 3. Compare and contrast matter vs non-matter. Give two examples of each. 4. Compare and contrast pure substances vs. mixtures. Give two examples of each. 5. List the two categories of pure substances. Give one example of each and explain their differences. 6. List the two categories of mixtures. Give one example of each and explain their differences. 7. What are the parts of a solution? What type of mixture is a solution? 8. What is a Balanced Chemical Equation? 9. What are coefficients? What are subscripts? Can they be changed? 10. Balance the following reaction: NaOH + HCl NaCl + H 2O 11. Balance the following reaction: CO 2 + H 2O H 2CO 3
8 12. What is the Law of Conservation of Matter (LCM)? 13. What are you calculating in a LCM problem? 14. You have this Chemical Reaction: A + B C + D. You are given two reactants, A is 15.3 g and B is 5.1 g. Product C has a mass of 18.4 g. What is the mass of the second product in this reaction? 15. What are the types of chemical reactions discussed in this section? 16. Write the chemical formula for a Combustion Reaction. Give one example of this reaction. 17. Write the chemical formula for a Synthesis Reaction. Give an example. 18. Write the chemical formula for a Decomposition Reaction. Give an example. 19. Digestion involves both chemical and physical changes. Write the type of change that occurs in the digestive system in each stage of digestion below. Stage of Digestion Saliva breaking starch into simple sugars Teeth chewing steak Enzymes breaking down proteins into amino acids Intestines draining water from digested food Small intestine pushing digested material toward the colon for removal from the body Chemical or Physical Change 20. What are the 4 phases of matter? 21. Name the phase changes of matter. Draw a Concept Map below that shows the relationship between all of the phases of matter and each type of change. 22. Which phase of matter occurs when a solid turns into a gas directly without going through a liquid phase?
9 23. Heat is added between points D and E. All of the heat being added is going to do what to the substance? 24. The curve above represents the Heating Curve of Water. In which section of the graph will frozen water melt into a liquid? What happens to the temperature in this section of the graph? Why? 25. Heat is removed from liquid water starting at 85 C until all of the liquid has become frozen into ice at 0 C. Which parts of the water curve above represent this process? Explain why the sections you chose represent each process in the question. Analyze the table below, and use it to answer question #26. The following symbols each represent one atom of different elements: 26. Which of the above correctly represents a chemical equation showing the law of conservation of mass in a chemical reaction? Explain your answer.
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