Section 1: Water, Solubility & ph

Transcription

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 Cohesion DEFINE Has + charge (Hydrogen) and charges (Oygen) Like magnet Water molecules attracted to each other creating surface tension Adhesion Surface Tension Water molecules are attracted to other substances such as glass, soil, and plant tissues tightness across the surface of water caused by cohesion Capillary Action Ability of water to climb up against gravity High Specific Heat Amount of heat (energy) required to raise the temperature of water by 1⁰ C Universal Solvent dissolves more substances than any other liquid Less Dense as a Solid and Floats Water in a liquid state keeps rebonding and changing its shape 3. Compare and contrast acid to base scientifically. Give two examples of each. Substance high in H + ions example: battery acid, stomach acid, coke 4. Why does your stomach have enzymes with the ph of 2? Is your stomach more acidic or basic? Acidic 5. Would an acid or base have more H + ions? Acid 6. Would an acid or base have more OH- ions? Base 7. Where on a ph scale would acids be located? On the left 8. Where on the ph scale would bases be located? On the right 9. What is the sum of the ph and poh in a substance?14

2 10. Why is water said to be polar? Why is this an important property of water? Because it has + and charges. It dissolves polar substances. 11. What type of chemical bond holds the oxygen and hydrogen molecules together in a water molecule? Is this a strong or weak bond? Hydrogen Weak 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? A) Have one hydrogen atom and 2 oxygen atoms B)hydrogen C)weak 13. How does water dissolve other substances? Are these substances polar or non-polar? Why? Use the solubility graph below to answer questions 14. How many grams of NaCl dissolves at 70 C? 45 g 15. At what temperature will 140 grams of KI dissolve? Around 13 degrees 16. How many grams of KNO3 can be dissolved in 200 g of water at 50 C? 80 g at 100 g So 80+80= 160

3 Section 2: Biomolecules 1. List the organic molecules. Why are they considered organic? A. Carbohydrates, Lipids, Fats, Nucleic Acids B. Contained in living things 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. Dehydration synthesis- Hydrolyosis - 3. Name the 3 parts that make up a nucleotide. phosphate, sugar and nucleotide 4. Deoxyribose is a sugar found in DNA or RNA? DNA 5. What does RNA stand for? Ribonucleic Acid 6. Explain the structure and function of an enzyme and state which biomolecule it is. Complex structure of substrate, active site and enzyme that fits together like lock and key -it is a protein 7. What does denature mean? What happens to proteins when they are denatured? uncoiled protein, they no longer work 8. Using the following diagram, LABEL active site, substrate, enzyme, lock and key fit, and product. X- substrate Y- enzyme Lock and key Step 2 Z- products

4 9. Complete the following chart: Elements in biomolecule/polymer CHON Protein Nucleic Acids Carbohydrates Lipids CHONP CHO CHO Where synthesized (made) in cell Ribosome Nucleus Chloplasts Smooth ER Function Defense, repair, growth Code for your genes Insulation Long term energy Short term energy Monomer Glucose DNA, RNA phospholipid Glycerol Examples enzymes, antibodies DNA, RNA Glucose Fatty acids, steroids 10. Compare and contrast DNA to RNA in a Venn diagram. (five differences and two similarities)

5 11. Be able to recognize these functional groups. Draw each one and label. 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.) 3 times= 1 pie 9/3=3 3 times= 3 pies 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! 1 hr= 3600 s 3 x 3600 = 10, 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? 30,0000 cg

6 Conversions to be used in problems How many slices will be eaten by 45 people? 45 people x 4 slices per person = 180 slices 16. How many people could you invite to a party if you could order $ worth of pizza? 103,46/ $14.78= 7 pizzas 12 slices/1 pizza= 84 slices. 84/4 people = 21 people 17. If you had 3 parties last month, how many slices of pizza did you serve? 1 party= 15 persons 15 x 3= 45 persons 45/4= 11 pieces 18. How many centimeters are in 7.4 meters? 7.4 /100= 740c m 19. What is 450 milliliters in liters? 450/1000=.450 L 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? 1550/1000=.1550kg 21. The distance from a Port Huron to the Indiana State line is approximately kilometers (via I-94). Express this distance in meters km x 1000= m 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!!! Volume= 3 cm x 6 cm x 4 cm = 72 D= m/v 80/72=1.1 g/cm3 So would be right below top of water 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. D= g/ 45 ml=

7 24. What is the density of a 100 g object with a volume of 250 ml? D= 100/250 =.25g/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? D= 454g/ 2270 =.2 g/cm3 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? D=m/v.6g/cm3= X/1.2cm3 =.72g 27. A 800 g boulder has a density of 8 g/cm3. What is the volume of the boulder? D=m/v volume= mass/density 800g/8cm3= 100 cm3 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. Charge Location in Atom Size Proton + Nucleus Neutron 0 Nucleus Electron - Electron or outer shells 3. Compare and contrast metals, nonmetals, and metalloids characteristics Metal- shiny, ductile, conduct electricity Non-metals- dull, no electricity, not ductile Metalloid- properties of metals and non metals 4. Compare and contrast a stable and unstable atom. Are majority of the atoms on the periodic table stable or unstable? Explain. Unstable atom is trying to bond (share or give electrons) Most are unstable 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. Are happy with 8 electrons in outer shell. Effects bonding because every compound wants 8 electrons in outer shell.

8 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? Electrons- either shared or given away electrostatic force is attraction between + and charges. Rules- opposite attract / same repel + and + or and - + and - 7. Compare and contrast intermolecular and intramolecular forces. Give 3 examples of each. Intermolecular force- weak force between molecule H 2O Intramolecular force strong force between atoms table salt 8. Compare and contrast covalent and ionic bonds. Give an example of each. Covalent- share electrons and are nonmetals only Ionic give electrons away and are metals and nonmetal 9. Compare and contrast polar covalent and nonpolar covalent bonds. Give an example of each. Polar covalent share electrons unequally ex. Water Non-polar- share electrons equally ex. CO2 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? Group give valence e rows give orbitals 12. Define electronegativity and how it affects elements as they increase in atomic number. Which element is the most electronegative? describes the tendency of an atom to attract a shared pair of electrons increases as goes down row Fr 13. Why is water like a magnet? Has + and - charge 14. Compare and contrast a cation and anion. Why do ions have an electrical charge? Cation is positive ion Anion negative What do intramolecular forces hold together? moleculeswhat do intermolecular forces hold together?atoms 16. What is a diatomic element? What are the 7 diatomic elements? Elements that always occur in 2 s in nature H, O, N, F, Cl, Br, I

9 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. Non polar ionic bond Hydrogen bond Section 5: Matter 1. What are 5 indicators (signs) of chemical change? Produces gas, color change, formation of a precipitate, odor change, temperature 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- P Photosynthesis - C Burning gas-c Melting butter - P Vaporization of water-p Dry Ice Sublimating- P Condensation Digestion of proteins into amino acids -C Cutting grass -P Cooking an egg -C Curdling of milk- C Grass growing-p 3. Compare and contrast matter vs non-matter. Give two examples of each. matter makes up everything you can see( such as clothes, water, food, plants, and animals) 4. Compare and contrast pure substances vs. mixtures. Give two examples of each. Pure substance- Elements and Compounds ex) silver Ag, NaCl can not be broken down by physical means Mixture- can be broken down ex. Coffee, pizza 5. List the two categories of pure substances. Give one example of each and explain their differences. - Elements and Compounds ex) silver Ag, NaCl can not be broken down by physical means 6. List the two categories of mixtures. Give one example of each and explain their differences. Homogeneous- solution ex. Milk, coke Hetergeneus- trail mix

10 7. What are the parts of a solution? What type of mixture is a solution? Solute substance that dissolve (like sugar) b) Solution is homogeneous Solvent- what helps it dissolve (tea) 8. What is a Balanced Chemical Equation? Equations where both sides have same amount 9. What are coefficients? What are subscripts? Can they be changed? # in front of formula, number of molecules in formula. Can change coefficients 10. Balance the following reaction: NaOH + HCl NaCl + H 2O Equation is balanced 11. Balance the following reaction: CO 2 + H 2O H 2CO 3 Equation is balanced 12. What is the Law of Conservation of Matter (LCM)? Matter is neither created or destroyed. 13. What are you calculating in a LCM problem? Amount of product produced or used. 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? A + B C + D ? = = D D=2 15. What are the types of chemical reactions discussed in this section? Synthesis #11 and double replacement #10 equation 16. Write the chemical formula for a Combustion Reaction. Give one example of this reaction. CH + O CO 2 + H 2O Using gas to start fire 17. Write the chemical formula for a Synthesis Reaction. Give an example. A + B= AB Table salt 18. Write the chemical formula for a Decomposition Reaction. Give an example. AB A +B 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 C P C P p Chemical or Physical Change

11 20. What are the 4 phases of matter? Solid, liquid, gas, plassa 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? sublimation

12 23. Heat is added between points D and E. All of the heat being added is going to do what to the substance? gas 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? B to C increases 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. C to B

13 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. Have to be equal on both sides II