INTRODUCTION TO CHEMISTRY – CHAPTER 1



Name: ________________________________________________Period #: _____Summative Review Packet for IDS Chemistry 2009-2010INTRODUCTION TO CHEMISTRY – CHAPTER 11-1. Chemistry is the study of:1-2. What are ozone (O3) and chlorofluorocarbons (CFCs) and how do they relate to climate change?1-3. Compare and contrast mass and weight. MassBoth Mass and WeightWeight1-4. Put the following steps of a Scientific Method in the correct order:____ Construct a hypothesis____ Develop a theory____ Make an observation____ Design and conduct experiments____ Revise hypothesis (if needed)____ Analyze results and draw a conclusionAnswer the Simpson’s questions about experimental design. You may need to look up some definitions! Make sure you understand the parts of an experiment!1-5. Bart believes that mice exposed to microwaves will become extra strong (maybe he's been reading too much Radioactive Man). He decides to perform this experiment by placing 10 mice in a microwave for 10 seconds. He compared these 10 mice to another 10 mice that had not been exposed. His test consisted of a heavy block of wood that blocked the mouse food. He found that 8 out of 10 of the microwaved mice were able to push the block away. 7 out of 10 of the non-microwaved mice were able to do the same. Identify the:A. Control Group:B. Independent Variable:C. Dependent Variable:D. What should Bart's conclusion be?E. How could Bart's experiment be improved? ANALYZING DATA – CHAPTER 22-1. State whether the units below are used to measure length (L), volume (V), mass (M), temperature (T), pressure (P), or energy (E).____ K____ grams____ liters____ kg____ Celsius____ atm____ inches____ mm Hg____ millimeters____ cm3____ Joule____ cm2-2. What 2 factors affect something’s density? What is the equation for density?2-3. Given the following liquids and their densities, draw the layers they would form in a beaker.LiquidDensityWater1.000Corn syrup1.37Ethyl alcohol0.789 PROPERTIES OF MATTER – CHAPTER 33-1. What does the law of conservation of matter state?3-2. Assume that the test tube shown on the picture started out having 20.0 g of mercury (II) oxide. After heating the test tube briefly, you find 1.35g of mercury (II) oxide left and 8.0 g of liquid mercury. How much oxygen gas was produced by the chemical reaction? Show your work.3-3. Suppose your heat some mercury (II) oxide in a test tube similar to the one shown in the picture above. After the chemical reaction, you find 12.5 g of liquid mercury and 1.0 g of oxygen gas. There is no mercury (II) oxide left in the test tube. How much mercury (II) oxide did you start with? Show your work.3-4. Label each substance below as a mixture or a pure substance. If classify as a mixture specify homogeneous or heterogeneous. If classify as a pure substance specify compound or element. A. air ____________________B. lemonade (with pulp) _______________________C. oatmeal raisin cookie _______________________D. vinegar ___________________________E. pure water ___________________________F. gasoline ___________________________3-5. A table spoon of salt is dissolved in 250 mL of water. What type of mixture is formed (homogeneous or heterogeneous)? Which compound in the mixture is the solute and which is the solvent?3-6. Label each drawing below with one of these words: Solid, Liquid or Gas.3-7. Write True or False for each of the following statements, if false write correct statement.A. ______ A solid has defined shape and volume.B. ______ A liquid had define shape and takes on the volume of its container.C. ______ A gas has both shape and volume of its container.D. ______ The particles in a gas cannot be compressed into a smaller volume.E. ______ The particles in a solid are spaced far apart.F. ______ Solids tend to expand when heated.3-8. Compare and contrast intensive and extensive properties. Provide at least 2 examples of each.Intensive PropertiesBothExtensive PropertiesSTRUCTURE OF THE ATOM – CHAPTER 44-1. Compare and contrast ions and isotopes. Show what the ion and isotope of Nitrogen would be under the appropriate column.IonsBoth Ions and IsotopesIsotopes4-2. Determine the atomic number, and the number of protons, electrons, and neutrons for each isotope describe below.Atomic NumberMass NumberNumber of ProtonsNumber of ElectronsNumber of Neutrons193928144021ELECTRON CONFIGURATION – CHAPTER 55-1. Given Boron’s electron configuration of [He]2s22p1, which of the following represents the Lewis electron-dot structure?a. ·Be· b. ·B: c. :B: d. Be:5-2. Define the following which relate to electron configuration:A. Aufbau principal – B. Pauli exclusion principal – C. Hund’s rule – 5-3. Write the electron configuration (you may use noble-gas notation if you wish) and draw the orbital diagram for the following elements:A. OxygenB. AluminumC. MagnesiumPERIODIC TABLE – CHAPTER 6 AND ELEMENT HANDBOOKUse the 4 periodic tables at end of packet for these questions. Be sure to assign a number to each periodic table!Table 1 – Title: Groups and PeriodsColor (and provide a key) for each group of elements.List the names and 1-2 unique characteristics of each group on the back of the periodic tables.Next to each row (to the left of Group 1), state the number of orbitals each row has.Table 2 – Title: Electrons and IonsIn black ink, write the number of valence electrons each group of elements has on top of each group.In red ink, describe what charge an ion of these elements will form.Color the metals light blue, the metalloids green, and the non-metals yellow.Table 3 – The BlocksColor and label the blocks the following colors: s = blue, p = purple, d = yellow, f = greenShow how many electrons each block can hold in a given orbital.Table 4 – TrendsDraw an arrow going across the table from left to right (arrowhead pointing right).Draw an arrow going from top to bottom alongside Group 1 (arrowhead pointing down).Describe the trends for the following as you move across the arrows:Atomic radius:Ionization energy:Ionic radius:IONIC BONDING – CHAPTER 7Circle the letter of the choice that best completes the statement or answers the question.7-1. The overall charge of a formula unit for an ionic compounda. is always zero.b. is always negative.c. is always positive.d. may have any value.7-2. The formation of a stable ionic compound from ionsa. is always exothermic.b. may be either exothermic or endothermic.c. is always endothermic.d. neither absorbs nor releases energy.7-3. Underline the word that correctly describes each property in ionic compounds.a. Melting point low highb. Boiling pointlow highc. Hardnesshard softd. Brittlenessflexible brittlee. Electrical conductivity in the solid state lowhighf. Electrical conductivity when dissolved in water.lowhigh7-4. For each of the following chemical formulas, write the correct name of the ionic compound represented.A. CaCl2 _________________________________B. K2S ___________________________________C. MgO __________________________________D. Fe2O3 __________________________________E. Li2SO4 _________________________________F. NaBr __________________________________7-5. Draw the Lewis electron-dot structure for the chemical formulas A. and C. in question 7-4.COVALENT BONDING – CHAPTER 88-1. For each of the items in column A, write the letter of the matching item in column B._____ COa. bromic acid_____ CO2b. dinitrogen tetroxide_____ HBrc. carbon monoxide_____ N2O4 d. ammonia_____ NH3e. carbon dioxide8-2. Draw the Lewis electron-dot structure for CO2, N2O4, and NH3.CHEMICAL REACTIONS – CHAPTER 99-1. Balance and classify (single replacement, double replacement, synthesis, decomposition, or combustion) each of the following chemical equations.____ HgO(s) ____ Hg(l) + ____ O2(g) _____________ __________________ H2(g) + ____ O2(g) ____ H2O(l)_ __________________________ ____ Na(s) + ____ H2O(g) ____ NaOH(s) + ___H2(g) _______________________________ CH4(g) + ____ O2(g) ____ CO2(g) + ___H2O(g) ________________________________ MgSO4(ag) + ____ CaCl2(ag) ___ MgCl2(ag) + ___ CaSO4(ag) _____________________ THE MOLE AND STOICHIOMETRY – CHAPTER 10 AND CHAPTER 1110-1. What is the numerical value of a mole and what is the significance of this number? (Why do scientists care about it?)10-2. What is molar mass?10-3. Use the equation below to solve the following problems. Show your work on the space provided. 2 Na2O2(s) + 2 H2O(l) 4 NaOH(s) + O2(g)a. How many moles of sodium hydroxide (NaOH) are produced when 1 mole of sodium peroxide (Na2O2) reacts with water (H2O)? b. How many moles of water (H2O) are needed to produce 10 moles of oxygen gas (O2)? 10-4. Use the equation below to solve the following problems. Show your work on the space provide. Fe2O3(S) + 3C(s) 2Fe(s) + 3CO(g)Fe2O3 has a molar mass of 159.7g/mol and CO has a molar mass of 28.01g/mol. a. If 150g of iron(III) oxide (Fe2O3) react with excess carbon (C), how many grams of carbon monoxide (CO) will be produced?b. How many grams of iron (Fe) will be needed to produce 20 moles of carbon monoxide (CO)?STATES OF MATTER – CHAPTER 1212-1. Identify each process (melting, vaporization, sublimation, condensation, freezing, and deposition) involved during the phase changes below: A. solid to a liquid ________________D. liquid to a solid _________________B. solid to a gas __________________E. gas to a solid ____________________C. liquid to a gas __________________12-2. Classify each of the following phase changes process that require energy (endothermic) or release energy (exothermic)A. liquid water to ice ________________________B. water vapor to liquid water ______________________C. boiling water _________________________D. melting of an ice cube _________________________GAS LAWS – CHAPTER 1313-1. Fill the following table with one of these terms: increase, decreases, constant, Boyle’s law, Charles’s laws, Gay-Lussac law: P1V1 = P2V2, P1 = P2, V1 = V2 T1 T2 T1 T2VolumePressureTemperatureGas LawFormulaincreaseconstantCharles’s lawincreaseconstantP1V1=P2V2constantincreaseincreaseconstantconstantincreaseV1 = V2 T1 T2constantincreasedecrease constantdecreaseconstantBoyle’s lawconstantdecreaseconstantdecreaseconstant decrease13-2. Apply Boyle’s law to explain why air enters your lungs when you inhale and leaves when you exhale.Explain why passengers experience popping sounds in their ears as the airplane ascends. Name the gas law that explains this phenomenon. (Think about what variables are changing!)MIXTURES AND SOLUTIONS – CHAPTER 14Use Figure 1 to answer questions 14-1 to 14-4.14-1. Compare the solubility of potassium bromine (KBr) and potassium nitrate (KNO3) at 80°C.14-3. If you dissolve 25g of potassium nitrate (KNO3) in 100g of water at 30°C, producing an unsaturated solution. How much more potassium nitrate (in grams) must be added to form a saturated solution at 30°C?14-4. A supersaturated solution of potassium nitrate (KNO3) is formed by adding 150g of KNO3 to 100g water,heating until the solute completely dissolves and then cooling the solution to 55°C. If the solution is agitated, how much potassium nitrate will precipitate? ENERGY AND HEAT – CHAPTER 1515-1. What does the law of conservation of energy state?15-2. Explain how the chemical potential energy stored in octane, a principal component of gasoline, is converted when gasoline burns in an automobile’s engine. 15-3. What is enthalpy and what instrument is typically used when measuring it?ACIDS AND BASES – CHAPTER 1818-1. The pH scale is used to rank hydronium ion concentration of a given substance. Which of the following sequences shows these solutions from least to most acidic? a. Gastric juice, vinegar, human blood, baking soda. b. Baking soda, human blood, vinegar, gastric juice. c. Baking soda, vinegar, human blood, gastric juice. d. Gastric juice, human blood, vinegar, baking soda.18-2. Buffers in your body are constantly working to prevent harmful increases or decreases in the pH of your blood, urine, and other fluids. In order to resist such changes, a buffer is composed of a. a strong acid and a strong base.b. a weak acid and its conjugate base, or a weak base and its conjugate acid.c. a strong acid and weak base.d. a strong base and weak acid ................
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