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Chemistry Log Books Preparation for the Gateway and GHSGT INTRODUCTION TO CHEMISTRY LOG BOOKS At the end of second semester this year, all students in the tenth grade attending Gwinnett County Schools must earn the minimum acceptable score on the county’s science Gateway test in order to be granted their diploma from a Gwinnett County High School. During their junior year, all students in Georgia are required to take and pass the Georgia High School Graduation Test (GHSGT) in science. Students must pass this test in order to graduate as well. To help students prepare for these high-stakes tests, log books are being required in many science classes here at Berkmar; these log books can be saved from year to year to help you refresh your memory of the AKS learned in each science class. OBJECTIVES OF THE CHEMISTRY LOG BOOKS 1. To review all the chemistry Academic Knowledge and Skills (AKS). 2. To prepare a chemistry log book that should be saved and used to prepare for the science portion of the Gwinnett County Gateway test given during the sophomore year. 3. To prepare a chemistry log book that should be saved and used to prepare for the science portion of the GHSGT given during the junior year. ORGANIZATION OF THE REVIEW SHEETS At the top of each AKS review sheet page, the appropriate AKS correlations are listed. This enables the students and their parents to understand the state and local requirements. After the solid black line, the review questions for the unit are listed. Students can answer these questions in any format they choose. It is recommended that students use some sort of bulleted list or graphic organizer to answer the question. These tend to be more useful and the student is more likely to use the book to study for the end of semester final exam, the Gateway test, and the GHSGT. STUDENT INSTRUCTIONS FOR THE ASSIGNMENT 1. Students will receive an AKS review sheet for the upcoming unit (usually after the last unit test). This sheet should then be glued/taped to fit the page in the composition log book. Students will read the AKS listed at the top of the page to see what they will be learning in the upcoming unit. 2. Students will answer the AKS review sheet questions located below the solid black line. Questions will be answered in the log book. Answers must be placed on the next blank page following the AKS review sheet questions. Answers are not to be written on the AKS review sheet that is glued/taped to fit the page in the log book. You may write on the back of pages in the log book. 3. Students will handwrite all answers in blue or black ink only; answers are NOT to be typed. 4. Students will need to place tabs between each section and clearly label on the tab what is covered in that section. Placing labeled tabs between each section is an organizational tool that will help you when you begin to study for the Gateway and GHSGT. 5. Students will turn in log books on test days, and the log book will be taken for a daily grade. DO’s and DON’Ts Do place your name on the outer cover in permanent ink! Do be NEAT. Points will be lost for: lack of neatness, overhanging papers, messing cutting, messy taping, etc. Directions must be followed every time – or points will be lost EVERY TIME! Do answer all the questions, and answer them correctly. When second semester of your junior year arrives, and it is time to study for the GHSGT, you will appreciate the fact that you answered all of the questions correctly when you realize how much chemistry you have forgotten and need to “brush-up” on. Don’t use “bungeed” log books or spiral bound log books. Don’t use “pull-out” paper log books. Chemistry Log Books First Semester Topics Note: The topic titles below are what should be placed on the tabs to separate the sections in the log book from each other. Safety in Chemistry Measurement Matter Atomic Structure: The Nucleus and Nuclear Chemistry Atomic Structure: Organization of Electrons Periodic Table Chemical Bonding: Ionic and Covalent Chemical Equations Chemistry Log Books Second Semester Topics Note: The topic titles below are what should be placed on the tabs to separate the sections in the log book from each other. The Mole and Stoichiometry Solutions Acids and Bases Energy (Thermochemistry/Organics) Kinetics Gas Laws AKS Review Safety in Chemistry AKS Correlation 2 apply standard safety practices for all classroom laboratory investigation. _____________________________________________________________________________ 1. Identify and give the function of the teacher-selected scientific apparatus and safety equipment. a. ________________________________________________________ b.________________________________________________________ c.________________________________________________________ d.________________________________________________________ e.________________________________________________________ 2. List five (5) safety rules in your own words 1._______________________________________________________________ ________________________________________________________________ 2._______________________________________________________________ ________________________________________________________________ 3._______________________________________________________________ ________________________________________________________________ 4._______________________________________________________________ ________________________________________________________________ 5._______________________________________________________________ AKS Review Measurement AKS Correlation 5c. Explain the relationship between accuracy and precision 5e. Solve scientific problems by substituting quantitative values, using dimensional analysis and/or simple algebraic functions as appropriate 8a1. Calculate density when given a means to determine mass and volume of a material _____________________________________________________________________________ 1. Using dimensional analysis show how many seconds there are in 5 years. 2. List the instrument and unit for measuring the following. Quantity Instrument Unit (metric, SI) Mass Volume Temperature Length 3. Explain how precision and accuracy are alike and how they differ. 4. What is the formula for density? 5. Determine the missing information in the chart below. Show work. MASS 12 grams b. 2 grams WORK: a. Density = b. Mass = c. Volume = VOLUME 6 ml 5 ml c. DENSITY a. 2.54 g/ml 12.0 g/ml You are given a small rock and a shoe box. Explain how you would determine the density of each. A small rock……. Measuring instruments: Procedure: Sample calculations: _______________________________________________________________________________________________ A shoe box……. Measuring instruments: Procedure: Sample calculations: AKS Review Matter AKS Correlation 8a. Identify substances based on chemical and physical properties/changes _____________________________________________________________________________ 1. How are the solid, liquid, and gas of a substance, such as water, alike? 2. How are the solid, liquid, and gas of a substance, such as water, different? 3. Define the following terms: a. pure substance b. heterogeneous c. homogenous mixtures d. solutions. 4. Classify the following examples as pure substance or heterogeneous mixture, homogeneous mixture, and/or solution. a. pizza ____ b. salt water ____ c. clear red liquid ____ d. granite rock ____ e. copper wire ____ f. sodium chloride ____ g. sugar dissolved in water_____ 5. Define a. physical property b. chemical property 6. Classify the following as examples of either physical properties or chemical properties. a. A piece of metal has a mass of 60.0 g._____ b. Metals react with acids to produce hydrogen gas.____ c. Tommy’s weight on the moon 40 lbs.____ d. Susan’s weight on earth is 45.0 kg.____ e. The density of water is 1.00g per ml.____ f. Litmus turns red in the presence of an acid.___ g. The book burned for 20 seconds.____ h. A metal, such as copper, has a good electrical conductivity.___ i. Water boils at a temperature of 100 degrees Celsius.____ j. When sodium hydroxide dissolves in water, the solution becomes hot.____ k. Combustion____ l. Melting___ m. Fermentation___ n. Metabolism___ o. Boiling___ p. Electrolysis___ AKS Review Atomic Structure AKS Correlation Use the modern atomic theory to explain the characteristics of atoms 10a. discriminate between the relative size, charge, and position of protons, neutrons, and electrons in an atom 10c. explain the relationship of the proton number to the element’s identity 10d. explain the relationship of isotopes to the relative abundance of atoms of a particular element 10d1. differentiate between alpha, beta, and gamma radiation __________________________________________________________________ a. b. Trace the development of the modern atomic theory. Atomic theories Democritus Dalton Thomson Rutherford Bohr Describe the basic structure of the atom as protons, neutrons and electrons in specific arrangements. Identify the relative location, size and charge of subatomic particles. proton neutron electron Location Mass Charge c. How does the number of electrons in the outermost level determine the reactivity of an element? d. Give the electron orbital configuration for each element in periods 1,2,3,4. e. Draw electron Dot formulas for elements in periods 1-4. f. What is quantum number? g. Explain emission spectroscopy as it relates the energy loss by electrons when returning to ground state. FILL OUT THE CHART BELOW. Radiation type Alpha Symbol Mass Penetrating power /Shielding Beta Gamma h. What will tend to happen to elements with 1 to 3 valence electrons? i. What will tend to happen to elements with 6-7 valence electrons? j. What will happen to elements with 8 valence electrons? AKS Review Periodic Table AKS Correlation 11 use the organization of the periodic table of elements to predict the properties of elements _______________________________________________________________________________ 1. DEFINE CLEARLY: Period Actinides Transition elements Group(families) Metal Lanthanides Periodic law Noble gases Metalloid Semiconductor Periodicity Nonmetal Synthetic 2. Give four examples of periodicity. 3. Where would you find a metal on the periodic table? 4 .Which elements are most likely to be used as semiconductors? 5. The father of the periodic table was_______. 6. List the columns of the periodic table 1A-8A, give the valence electrons for each and Lewis dot structure for each? 7. List the three elements predicted by Mendeleev. 8. What are the characteristics of transition element? 9. Define: a. Metallurgyb. Orec. Minerald. Alloye. Allotrope10. What state are most elements in at room temperature?____________ 11. List several characteristics of Metals- Nonmetals- Metalloids- 12. What are the group and period trends for ___? atomic radii group-period-ionization energy group-period-electro negativity group-period-AKS Review Bonding AKS Correlation 8b predict formulas for stable ionic compounds based on balance of charges 8c use IUPAC nomenclature from transition between the chemical names and formulas of ionic compounds, covalent compounds __________________________________________________________________ 1. Describe the formation of ionic and covalent bonds. 2. What type of elements will form ionic bonds? 3. Which types of elements will form covalent bonds. 4. When will a covalent bond be polar? 5. How does polarity effect a molecules interaction with other molecules? 6. Identify each of the following weak bonds. Van de Waals Hydrogen Dipole-dipole Ion-dipole 7. What type of bonding would most likely occur between: a)metal-nonmetal _________________________ b)nonmetal-nonmetal _________________________ Fill in the chart below: Name Formula Ionic Silicon dioxide Chlorine trifluoride Carbon tetrachloride Sulfur difluoride N2F4 SO3 NO SeO2 KClO2 Cu2O Na3N NiCl2 Iron (III) oxide Calcium chloride Sodium bromate Ammonium bromide Covalent AKS Review Chemical equations AKS Correlation 9a identify and balance the following type of equations: synthesis (including condensation that synthesizes carbohydrate, lipids, and proteins), decomposition, single replacement, double replacement, and combustion. __________________________________________________________________ Write and balance the following chemical equations: 1. Aluminum reacting with oxygen to produce aluminum oxide. Type of reaction___________________ 2. Iron(II) chloride and sodium phosphate reacting to form sodium chloride and Iron(II) phosphate. Type of reaction___________________ 3. Methane( CH4 ) combining with oxygen gas producing carbon dioxide and water Type of reaction___________________ 4. Chlorine gas reacts with lithium bromide to produce lithium chloride and bromide gas Type of reaction___________________ 5. Calcium carbonate breaks down to Calcium oxide and Carbon dioxide Type of reaction___________________ AKS Review The Mole and Stoichiometry AKS Correlation 9c. Apply concepts of the mole and Avogadro’s number to conceptualize and calculate: -empirical/molecular formulas -mass, moles, and molecules relationships 9d. Verify Conservation of Mass in a chemical reaction quantitatively by: -identifying and solving different types of stoichiometry problems, specifically relating mass to moles and mass to mass -demonstrating the conceptual principle of limiting reactants __________________________________________________________________ In all calculations that follow, SHOW ALL WORK AND USE SIGNIFICANT FIGURES. 1. Write Avogadro’s number conventionally and in scientific notation. 2. (a) What is molar mass? (b) Find the molar mass of the following: Fe CCl4 Al2(CO3)3 3. Perform the following conversions. (a) Determine the number of atoms in 3.75 mol Fe. (Tech can omit) (b) How many moles of CaCl2 contain 1.26x1024 formula units of CaCl2? (Tech can omit) (c) Determine the number of moles of arsenic in 1.90 g As. (d) Calculate the mass in grams of 42.5 mol of potassium cyanide (KCN). (e) Determine the mass in grams of 5.65 x 1024 atoms Se. (Tech can omit) 4. What is the percent composition by mass of each element in: (a) water (b) sucrose (C12H22O11) 5. (a) Define what an empirical formula is and give an example. (b) Define what a molecular formula is and give an example. 6. A compound is 82.6 % C and 17.4 % H. Its molecular weight is 58.14 g/mol. (CP and Tech can omit) (a) What is the empirical formula for this compound? (b) What is the molecular formula for this compound? (c) Draw 2 possible structural formulas for this compound. 7. (a) What is stoichiometry? (b) How many moles of HCl will react with 0.200 mol Al(OH) 3? Use the following equation.(Tech can omit) Al(OH)3 + 3 HCl AlCl3 + 3 H2O (c) What mass of chromium (III) oxide will be produced when 4.58 moles of chromium react?(Tech can Use the following equation. 4 Cr + 3O 2 2 Cr2O3 omit) (d) How many grams of carbon dioxide will be produced when 2.50g of NaHCO3 react with excess acid according to the following equation: (Tech can omit) 3 NaHCO3 + H3C6H5O7 Na3C6H5O7 + 3 CO2 + 3 H2O 8. (a) Distinguish between limiting reactant and excess reactant. (b) Find the limiting reactant when 4 mol LiOH react with 3 mol CO2 according to the following equation: 2 LiOH + CO2 Li2CO3 + H2O. How many moles of water will be produced? (Tech can omit) (c) 45 g C6H6 react with 45 g Cl2 according to the equation: Cl2 + C6H6 C6H5Cl + HCl. What is the limiting reactant? What mass of HCl will be produced? (Tech can omit) 9. (a) Define actual yield, theoretical yield, and percent yield. (b) 5.00 g of tin reacted with excess iodine according to the equation Sn + 2I2 SnI4. Calculate the percent yield of SnI4 if 25.0 g of SnI4 was recovered. (CP and Tech can omit) AKS Review Solutions AKS Correlation 14a. Explain solubility in terms of substance involved (i.e. solute, solvent) and the process of dissolving a solute by: Observing factors that effect the rate at which a solute dissolves in a specific solvent Demonstrating that solubility is related to temperature by constructing a solubility curve Expressing concentrations in molarity Preparing and properly labeling solutions of specified molar concentrations Relate molality to colligative properties __________________________________________________________________ 1. (a) What is a solution? (b) What are the two parts of a solution? 2. Identify the solute and solvent in an aqueous solution of sugarwater. Solute: ____________ Solvent: ____________ 3. If one liquid is soluble in another liquid, such as food coloring in water, the two liquids are considered ________________. 4. If one liquid is insoluble in another, such as oil in water, the two liquids are _____________. 5. Discuss the two processes that occur during solution formation. 6. (a) Explain the phrase “like dissolves like” using the terms polar and nonpolar. (b) Identify whether the following substances would dissolve in WATER or GASOLINE (OCTANE). NaCl CH4 I2 7. Discuss three factors that affect the rate at which solvent particles dissolve solute particles. 8. What is solubility? 9. Distinguish between saturated solutions, supersaturated solutions, and unsaturated solutions. 10. (a) What happens to solid solutes as temperature increases? (b) What happens to gaseous solutes as temperature increases? 11. What is the percent by mass of 81.0 g of NaCl dissolved in a solution of 525 g? 12. (a) 21.0 moles of sugar are in a solution of 52.0 L. What is the molarity of this sugar solution? (b) Explain the steps you would follow in order to prepare the sugar solution with the molarity you calculated above. Be specific with instructions and be sure to indicate the lab equipment needed. (Tech can omit) 13. (a) What is a colligative property? (b) List the four types of colligative properties. 1. 2. 3. 4. 14. Use a colligative property to explain why salt is often thrown on icy steps and roads in the winter. 15. Use the graph below for the questions that follow. Temperature in C (a) How much ammonium chloride dissolves in 100. g of water at 50.C? (b) At what temperature does 115 g of sodium nitrate dissolve in 100. g of water? (c) Name all the gaseous solutes on the solubility graph above. (d) If 40.0 g of NH4Cl is dissolved in 100. g of water at 90.C, how much more solute can be added before the solution becomes saturated? (e) At 80.C, 52 g of KCl is dissolved in 100. g of water. The temperature is then lowered to How much KCl will precipitate out of solution? (f) What is the mass of Yb2(SO4)3 that can dissolve in 350. g of water at 60.C? 10.C. AKS Review Acids and Bases AKS Correlation 14. Analyze properties that describe solutions and the behavior of acids and bases. 14b. Compare, contrast and evaluate the nature and behavior of acids and bases in terms of Arrhenius, BronstedLowry acids/bases, strong vs. weak acids/bases in terms of percent dissociation and conductivity, hydronium ion concentration, pH, and acid-base neutralization. 14c. Classify common substances as acid, base, or neutral based on chemical properties. __________________________________________________________________ 1. Examine the list of physical and chemical properties in the chart below. Decide if that property describes an acid, base, both, or neither by placing a check in the column that the physical or chemical property matches. You can have more than one check by a property or no checks by a property! Property Acid Base tastes sour tastes bitter pH > 7 PH < 7 good conductors of electricity turns blue litmus red turns red litmus blue reactants in neutralization turns pink in the presence of phenolphthalein donates H+ ions accepts H+ ions contains OH- ions contains H+ ions reacts with metals and carbonates dissolves in water to form aqueous solutions corrosive alkaline commonly used as cleaning agents contains more OH- ions than H+ ions contains more H+ ions than OH- ions associated with hydronium (H3O+) ions 2. Fill in the chart below with the different views on acids and bases according to Arrhenius and Bronsted-Lowry. Arrhenius Bronsted-Lowry Acids Bases 3. (a) Distinguish between strong acids and weak acids in terms of percent dissociation. (Tech can omit) (b) Distinguish between strong bases and weak bases in terms of percent dissociation. (Tech can omit) 4. (a) What is the general chemical reaction for neutralization? Be sure to include the products made from a neutralization reaction! (b) What are always the two products of a neutralization reaction? (c) What type of chemical reaction is a neutralization reaction (i.e. synthesis, decomposition, single displacement, double displacement, or combustion)? 5. Draw a pH scale and label the location of acids, bases, and neutral substances. 6. Fill in the blanks in the following table and then answer the questions that follow. More H+ or OH- ions or Substance [H+] pH Equal Amounts? unknown A 1.0 x 10-6 M unknown B 2.5 x 10-8 M unknown C 1.0 x 10-10 M unknown D 7.8 x 10-5 M unknown E 1.0 x 10-7 M Acid, Base, or Neutral? (a) Show the formula for how you calculated the pH for the unknowns in the chart above. (b) How much stronger is unknown A than unknown C? _____________ How do you know? 7. Examine the data in the following table to determine whether the substance is an acid, base, or neutral. If the substance is already identified as an acid, base, or neutral substance, then fill in the data you would expect to find if you tested it in lab. turns red Reaction with Phenolphthalein stays clear Reaction with Methyl Orange turns red stays blue turns pink turns yellow Substance Red Litmus Blue Litmus Unknown A Unknown B Unknown C stays red turns blue Acid, Base, or Neutral? neutral AKS Review Energy (Thermochemistry and Organics) AKS Correlation 13c. collect data in order to calculate the amount of heat given off or taken in by chemical or physical processes (SC6b) 13d analyzing (both conceptually and quantitatively) flow of energy during change of state (phase) (SC6c) __________________________________________________________________ 1. Energy is defined as the ability to do work or produce heat. How does energy affect the behavior of molecules? 2. (a) Where is energy stored in a molecule? (b) What is chemical potential energy? 3. List the two main forms of energy a. _________________ b. __________________ 4. Are temperature and heat energy the same? Defend your answer. 5. The amount of heat energy required to raise the temperature of 1 g of water 1 degree Celsius is _____. 6. What is the difference between calories and Calories? 7. How do you calculate the number of food calories in a food? 8. One calorie is equal to ____ Calories = _____ kCal 9. What is specific heat? 10. In the formula, q = mc∆T, what does each variable represent? q = ______ m= ______ c = _______ ∆T = ______ 11. If the temperature of 34.4 g of ethanol increases from 25.0˚C to 78.8˚C, how much heat has been absorbed by the ethanol? 12. Examine the Heating Curve Graph below and answer the following questions. Heating Curve Graph for Benzene D 100 b. c. d. What do the plateaus on the heating curve graph indicate? Which letter on the heating curve graph represents the liquid state of benzene? Which letter on the graph represents solidification? Which letter represents the highest amount A of kinetic energy in the molecules? 13. What is thermo chemistry? 80 Temperature (in degrees Celsius) a. 90 C 70 60 50 B 40 30 20 10 0 14. How do you calculate change in enthalpy? 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 Time Heat Added (min) AKS Review Kinetics AKS Correlation 12. Predict how various factors affect the rate of a chemical reaction 12a - demonstrate the effects of changing concentration, temperature and pressure on chemical reactions (GPS) 12b - investigate the effects of a catalyst on chemical reactions and apply it to everyday examples (GPS) 13. Evaluate the motion and behavior of atoms and molecules in chemical and physical processes 13a - compare and contrast atomic/molecular motion of solids, liquids, gases and plasma (GPS) 13b - relate temperature, pressure and volume of gases to the behavior of gases 13c - collect data in order to calculate the amount of heat given off or taken in by chemical or physical processes (GPS) 13d – analyze (both conceptually and quantitatively) the flow of energy during a change of state (phase) (GPS) __________________________________________________________________ 1. (a) What are four factors that can affect the rate at which a reaction occurs? (b) Explain how each factor can speed up a reaction. 2. (a) What is a catalyst? (b) How does a catalyst do its job? 3. Explain what it means for a reaction to be at equilibrium. (Tech can omit) 4. Draw a rate of reaction graph and explain what happens to the rate of the forward reaction and the rate of the reverse reaction over time. (CP and Tech can omit) 5. Explain Le Chatelier's Principle. (Tech can omit) 6. What is the KMT? 7. What are the main points of the KMT? Use this equation for the stresses below: 2 H2(g) + O2(g) 2 H2O(l) + 69.2 kJ 8. Which way would the equilibrium shift if the reaction is heated? Why? (Tech can omit) 9. Which way would the equilibrium shift if pressure is increased? Why? (Tech can omit) 10. Which way would the equilibrium shift if more water is added to the mixture? Why? (Tech can omit) 10. Describe solids, liquids, and gases in terms of their molecular motion and energy. 11. Describe what happens to a substance during the melting phase and during the boiling phase. 12. Explain why there is no change in temperature when a substance changes phase. 13. Why is the Kelvin temperature scale used in science? 14. Label on the graph below the following items by writing the term in the appropriate spot on the graph: a. melting (fusion) c. vaporization Heating Curve Graph b. freezing (solidification) d. condensation Heating Curve Graph For Benzene ees Celsius) 35 30 25 Heat Added Over Time (one second intervals) 15. Label on the graph by writing the term in the appropriate area of the graph where the solid, liquid, and gaseous states of matter are. AKS Review Gas Laws AKS Correlation 13b. Relate temperature, pressure and volume of gases to the behavior of gases __________________________________________________________________ 1. What are the four factors that affect the behavior of gases? a. b. c. d. 2. Define pressure AND give the units in which pressure is measured. 3. (a) State Boyle’s Law. (b) What is the equation stated in Boyle’s Law? (c) What type of relationship occurs in the law: direct or inversely proportional? 4. (a) State Charles’ Law. (b) What is the equation stated in Charles’ Law? (c) What type of relationship occurs in the law: direct or inversely proportional? 5. (a) State the Combined Gas Law. (b) What is the equation stated in the Combined Gas Law? (c) What type of relationship occurs in the law: direct or inversely proportional? 6. What is STP and the values it represents? 7. (a) What is Avogadro’s Principle regarding gases? (CP and Tech can omit) (b) What is the volume of a gas at STP? (CP and Tech can omit) 8. Identify the following as being examples of either Boyle’s Law or Charles’ Law: ____(a) George left his basketball outside on a very cold night. The next morning the basketball was very hard to bounce and appeared to be smaller than it was the night before. ____(b) Felecia opens a can of soda and hears the sound of gas escaping. ____(c) Mario decides to shake his bottle of soda before opening it the first time. He notices bubbles in the bottle. ____(d) Katherine squeezes a balloon. 9. A gas at 55C occupies a volume of 3.6 L. What volume will it occupy at 30.C? Assume pressure and mass remain constant. 10. The pressure of air in a 2.25 L container is 1.20 atm. What is the new pressure if the sample is transferred to a 6.5 L container? Assume temperature and mass remain constant. 11. How many moles of air are in a 6.06 L tire at STP? (CP and Tech can omit)