Unit Organizer - Mrs. Rhee Science - Home



Topic 1: Data CollectionWhat is chemistry? How do we make accurate and precise observations of our world?VocabularyTermDefinitionOrganic ChemistryInorganic ChemistryAnalytical ChemistryPhysical ChemistryBiochemistryQualitative ObservationQuantitative ObservationPrecisionAccuracyDependent VariableIndependent VariableScientific MethodMajor prefixes of the Metric System (kilo-milli)SI SystemDensityIntensive propertyExtensive propertyDimensional AnalysisConversion FactorSignificant FigureUncertaintyTopic 1: Data Collection (cont)What is chemistry? How do we make accurate and precise ob3servations of our world?ObjectivePractice ProblemIdentify the proper names and uses of common laboratory materials.Label the following materials with their proper names and uses Read laboratory measuring instruments to the nearest degree of precision and record data with correct number of significant figures.44951657620Use the picture to the right to answer the following questions.Each mark represents __________ mL.The device shown is precise to what decimal place? ________According to the measuring device, what is the volume of water?____________Name and use basic SI units.Label each of the following measurements with the proper SI unit.Length _______________Volume ______________Mass ______________Label the values below with the correct metric prefixes___________1000 ___________1/1000 ___________1/100 ___________1/10Distinguish between qualitative and quantitative observations.Classify each of the following as either a qualitative or quantitative observation:________________The candle weighs 4.00 grams. ________________ The candle is round.________________The candle burned brightly. ________________ The candle is 2.00cm.Perform mathematical operations involving dimensional analysis.Convert using proper dimensional analysis: 25.4ft/day = ? cm/minDetermine the number of significant figures in measurements.Underline and state the number of significant figures in each of the following values:1.201 ___________ 12.0 x 104___________0.012___________ 1200 ___________Round each of the following numbers to 3 significant figures:125.32 ________________ 124.500________________23.523 ________________ 0.0010101________________Perform mathematical operations involving significant figures.Solve the following. Report answers with correct units and significant figures:6.5 cm / 2.1 cm =_____________________ 2.33 K + 18.1 K _______________________0.00032 m x 12 m =_____________________ 44.25 kg – 2.25 kg ________________________Topic 1: Data Collection (cont)What is chemistry? How do we make accurate and precise ob3servations of our world?Perform mathematical operations involving significant figures AND use basic SI units. Convert the following (while maintaining the same number of significant figures): 42.1 g = ___________ kg 0.450 L = ___________ mL 2.25 L = ___________ mL 5.4 ft/day =___________ cm/min 3.2 °C = ___________ °F 126 K =___________ CPerform mathematical operations involving scientific notation.Express the following numbers in scientific notation:52,000 = 0.000175 =Perform the computations below expressing the answers in scientific notation(7.1x 109)(55) = 10,500 ÷ (4.0 x 10-4) =Differentiate between a precise and an accurate set of data.Distinguish between intensive and extensive properties.Label the following as intensive or extensive properties of matter:Density_________________Volume_________________Mass _________________Temperature_________________Topic 2: Chemical and Physical Properties of SubstancesWhat are the characteristics by which matter can be classified?VocabularyTermDefinitionmatterchemical changechemical propertyphysical changephysical propertychanges of state (phase change)solid, liquid, gas, plasmapure substanceatomelementcompoundmixtureheterogeneous mixturehomogeneous mixturesolutionsolutesolventaqueous solutiondensityTopic 2: Chemical and Physical Properties of SubstancesWhat are the characteristics by which matter can be classified?ObjectivePractice Problemdistinguish between chemical and physical properties; chemical and physical changes.Classify each of the following as either a physical or chemical change or propertyRelease of Odor _________________Reactivity_________________ Paper Burning _________________Crushing Chalk _________________ Color Change _________________Melting Butter_________________Cutting Paper _________________Stirring_________________distinguish between and classify types of matterTopic 2: Chemical and Physical Properties of Substances (continued)distinguish between and classify types of matterComplete the following table using the terms element, compound, mixture, heterogeneous, homogeneous, and pure substance.A group of two or more substances that are physically combined are called aa. mixture.b. compound.c. element.Mixtures that are not evenly mixed throughout are called a. pure substances. b. homogeneous.c. heterogeneous.Classify the following substances as a: heterogeneous mixture, solution, compound, or element.a. iron shavings (Fe) _________________c. brewed tea_________________b. neon gas (Ne)_________________d. water (H2O) _________________e. granite _________________ f. nitrogen_________________g. salt (NaCl) _________________h. energy drink _________________describe the characteristics of phase states in terms of particle arrangement and motion.Which of the following has a definite shape? Circle all that applya. Solidsb. Liquidsc. Gases Which of the following has a low density? Circle all that applya. Solidsb. Liquidsc. Gases Label each of the following with A-I as given in the diagram to the right _____Melting_____Evaporation_____Liquid_____Solid3683635-1425575_____Gas_____Condensation _____Freezingdescribe the relationship between energy, particle motion and change of phase.Label A, B, and C with the proper phase states.Label 1,2,3,4 with the proper phase changes600075-1744345At point 3 on the graph above,the heat added increases and the temperature increases.the heat added decreases and the temperature decreases.the heat added decreases and the temperature stays the same.the heat added increases and the temperature stays the same.Use derived properties to identify substancesUse the diagram below to answer the next three questions Which line in the graph above represents lead? The density of lead is 11.4 g/mL. The density of gold is 19.3 g/mL.Line A Line BLine A if the piece of lead is larger than the piece of gold.3209290200025Line A if the piece of gold is larger than the piece of lead.Which of the following has the greatest volume?80 g of substance A80 g of substance B both have the same volumenot enough information to tellThe independent variable in the graph isvolume in mL.mass in gline A.line ic 3: Atomic TheoryWhat is all matter made of?VocabularyTermDefinitionatomatomic massatomic numberisotopemass numberneutronprotonnucleusatomic orbitalelectronphotonAufbau principleHund’s rulePauli exclusion principleatomic emission spectrumelectromagnetic spectrumcontinuous spectrumline spectrumquantaGround stateExcited stateTopic 3: Atomic TheoryWhat is all matter made of?ObjectivePractice ProblemsState the position of protons, neutrons and electrons in the atom.State the relative masses and relative charges of protons, neutrons and electrons.Draw a bohr model of an atom of Sodium-23, labeling the number of protons, neutrons, electrons and their charges.Determine the number of protons, neutrons and electrons in atoms and ions from the mass number, atomic number and plete the following table:SymbolAtomic #Mass ## Protons# Electrons# NeutronsIonic Charge34800Define the term isotope.Write the symbolic notations used to represent isotopes.Calculate the atomic mass for an element given the mass of its isotopes and the percent abundance for each.How many neutrons do each of the following isotopes contain?(a) chlorine-32 ___ (b) gold- 169 _______ c) lead-182 _______ Given the following information for element "X",IsotopeMass (amu)Percent Abundance1 34.9775.77%2 36.9724.23%(a) Calculate the atomic mass for element “X”(b) Identify element X : Describe the electromagnetic spectrum.?Draw two waves with the wavelengths representing the relative energies of red light and of blue light.Label one “more energetic,” the other “less energetic.”Describe how the frequencies of light emitted by an atom are a unique characteristic of that atom.Summarize the main features of the Bohr model of the hydrogen atom.Which of the following does the Quantum Mechanical model of the atom propose?The atom contains protons and electrons.Electrons orbit the nucleus of the atom. Electrons orbit the nucleus in specific patterns.Electrons emit energy in the form of plete the following table:Principal Energy Level Total number of sublevelsTotal number of orbitalsTotal number of electrons2425Write labeled orbital diagrams for each of the following elements:Calcium ArgonApply the Aufbau principle, Hund’s rule and the Pauli Exclusion Principle to write electron configurations for an atom.Write electron configuration and ion configurations of elementsWrite the electron configurations for the following elements using noble gas notation.Mn ZnP PbWrite the full electron configurations for the following ions:P-3 Al 3+Determine which of the following electron configurations represent an atom in theexcited state and identify that element. (Circle choice and name the element)a. 1s22s32p63s23p6 b. 1s22s12p63s23p5 c. 1s23s22s22p63p6element name_______________________________Topic 4: Periodic TrendsWhat trends are used to identify the properties of elements and compounds?VocabularyTermDefinitionDiatomic elementPeriodicityElectronegativityDimitri MendeleevPeriodic LawGroup/FamilyPeriodValence ShellValence Electron(s)Octet RuleThe shielding effectAtomic RadiusIonic RadiusIonization EnergyTopic 4: Periodic TrendsWhat trends are used to identify the properties of elements and compounds?ObjectivePractice ProblemsIdentify the diatomic elements.List the formulas of the diatomic elements: H2 ,Discuss the relationship between an element's electron configurations its location on the periodic table.An atom is found to have the electron configuration of [Kr]5s24d105p5Identify this element:How many valence electrons does it have?What family does this element belong to? What charge do all of elements in this family have and why?Compare the periodic trends of atomic and ionic radius, ionization energy, and electronegativity.Explain how the shielding effect influences atomic radius, ionization energy, and electronegativity.Classify the phase state of an element as a solid, a liquid, or a gas.Describe the main features of our modern periodic table.Locate and name the s, p, d and f- blocks on the periodic table.Using the periodic table below,Circle the only noble gas that does not have a p orbital.Number the groups 1A-8ANumber the periods 1-7Box and Label the 2-s block, the 3p-block, 5d-block, and the 4-f-block. Label the halogens, transition elements, alkaline earth metals, alkali metals, and the noble gases.Label groups 1A, 2A and 7A with their ionic chargePut an X through all seven elements that are naturally diatomic.Label the arrows to show the trends for electronegativity both along a period and a groupLabel the appropriate arrows to show the trends for atomic radius both along a period and a groupLabel the appropriate arrows to show the trends for ionization energy both along a period and a group744855-44450054990911398250050272948655050089154014668500Topic 5: BondingHow do elements combine to form new matter?How does the type of bond affect the properties of the compound?VocabularyTermDefinitionIonAnionCationIonic bondLattice energyMetallic bondOxidation numberCovalent bondLewis structureResonance structureVSEPRPolar covalentNon-polar covalentDispersion forceDipole-dipole Hydrogen bondPi bondOrbital hybridizationBond lengthBond strengthBond energyTopic 5: BondingHow do elements combine to form new matter?How does the type of bond affect the properties of the compound?ObjectivePractice ProblemsProperly write the chemical formulas of ionic compounds when given the nameProperly write the chemical formulas of molecular compounds when given the name Properly write the chemical formulas of acids when given the nameWrite the correct formula for the following compounds:sulfur trioxide____________________ calcium sulfate____________________phosphoric acid____________________ hydrofluoric acid____________________aluminum fluoride ____________________ lead(II)nitrate____________________aluminum hydroxide ____________________ ammonium carbonate______________gold(III)chloride dinitrogen pentaoxide Properly name ionic compounds when given the chemical formulaProperly name molecular compounds when given the chemical formula Properly name acids when given the chemical formulaWrite one proper name for each of the following compounds. PbCl4_____________________________________________NCl3_____________________________________________S2F10_____________________________________________Hg(NO3)2_____________________________________________HNO3_____________________________________________H2S_____________________________________________Fe(OH)3_____________________________________________Sn3(PO4)4_____________________________________________PREDICT the type of chemical bond formed using electronegativity differencesAn ionic bond exists when the electronegativity difference is greater than _________A covalent bond exists when the electronegativity difference is _______A polar covalent bond exists when the electronegativity difference is between _______________DESCRIBE the characteristics of ionic and covalent compoundsCircle the words that complete the sentence. (Molecular/Ionic) bonds are usually (strong/weak) and (do/ do not) conduct electricity, are volatile and have a low melting ic 5: Bonding(Continued)DRAW Lewis Diagrams of Ionic and Covalent Bonds based on the Octet RuleDraw resonance structuresDETERMINE the direction of a dipole moment in a polar moleculePREDICT the molecular geometry of a molecule using the VSERP ModelPredict the polarity of a moleculeLewis StructureElectro-negativity DifferenceBond PolarityMolecular Shape(VSEPR)Shape NameMolecular PolarityCBr4H2OPH3SO3NH4+Brackets!BH3Classify the intermolecular forces that exist between atoms and molecules.Identify the type of bonding that occurs between the atoms/molecules/ions listed below.(Select: Ionic, polar covalent, nonpolar covalent, dipole-dipole, hydrogen bonding, dispersion forces.)___________________________Between atoms of hydrogen and oxygen in a water molecule___________________________Between molecules of water___________________________Between atoms of bromine in a bromine molecule___________________________Between molecules of bromine___________________________Between ions of sodium and chlorine in sodium chloride___________________________Between molecules of fluoromethaneTopic 6: The MoleHow do chemists quantify matter?VocabularyTermDefinitionEmpirical FormulaMolecular FormulaStructural FormulaFormula unitMoleMolar massAvogadro’s principlePercent CompositionObjectivePractice ProblemsDefine mole, Avogadro's number, and molar mass, and state how all three are related.Calculate the number of atoms in a sample of any chemical element.Perform mole-mass conversions.How many atoms are in one mole of sulfur? _______________________________How much volume does one mole of any gas at STP occupy? __________Calculate the molar mass of the following compounds:Ca(OH)2 = Sulfur trioxide = FeCl3 = Iron(III) sulfide=How many moles are in 10.0g of potassium chlorate?How many grams are in 2.2 moles of hydrosulfuric acid?How many molecules are present in 2.50 moles of sulfur dioxide? How many oxygen atoms are contained in 13.5 grams of carbonic acid?What is the mass of 4.32 x 1025 molecules of ammonia (NH3)?Topic 6: The Mole (continued)Calculate the percent composition of a compound.Calculate the percentage composition by mass of C12H22O11.Determine the empirical formula and molecular formula of a compound.An unknown compound is composed of 71.0% silver, 7.9% carbon, and 21.1% oxygen.Determine the empirical formula for this compound.What is the molecular formula and name of this compound if it has been determined to have the molar mass of 303.8 grams?Determine the chemical formula of a hydrate.Experimentally?determine?the chemical formula of a hydrate.Use the data below to determine the formula and name for the aluminum bromide hydrate, AlBr3?XH2O.Mass of empty crucible and lid: 4.26 gMass of crucible, lid, and hydrate: 8.60 gMass of crucible, lid, and anhydrate (i.e., after heating): 7.35 gTopic 7: Chemical ReactionsHow do chemists quantify matter?VocabularyTermDefinitiondecomposition (analysis)combination (synthesis)single-replacementdouble-replacementcombustion of a hydrocarbonneutralization reactionPrecipitateActivity SeriesTopic 7: Chemical ReactionsObjectivePractice ProblemsSTATE the reasons why a chemical reaction must be balanced. A balanced equation verifies the law of conservation of matter becausethe molar masses of all substances are the samethe coefficients on both sides of equation are the samethe moles of reactants equals the moles of productsthe mass of reactants equals the mass of productsREAD a chemical reaction properly and identify the major parts, such as products, reactants, yields, and phase states.The equation that correctly describes the reaction at right is Al2 + 3 Cl2 --> Al2Cl62 Al + 3 Cl --> 2 AlCl32 Al + Cl2 --> 2 AlCl2 Al + 3 Cl2 --> 2AlCl32785745-887095Identify the products above:Identify the reactants above:Aqueous solutions of magnesium chloride and sodium hydroxide are mixed together to produce solid magnesium hydroxide. Write a complete balanced equation for this reaction (include phases).What type of reaction is this? ________________________________APPLY the rules for balancing chemical reactions to a given list of chemical reactions.Balance the following equations: N2 + H2 NH3Cs + H3PO4 Cs3PO4 + H2MnO2 + HCl MnCl2 + H2O + Cl2C4H10 + O2 CO2 + H2OIDENTIFY and NAME the major types of chemical reactions- synthesis, single replacement, double replacement, combustion or decomposition.PREDICT the products or reactants of a chemical reaction when given one or the other.Properly predict the products, balance and name each of the reactions below. Assume all reactions occur (phases not needed)ReactantsProductsReaction TypeCa(OH) 2 + H2SO4Mg(ClO3) 2+ O2K + O2C7H16 + O2Li + I2Al + HClCaOZn + FeCl3Al2 SO4)3 + MgCl2Determine an activity series and predict whether or not a reaction will occurPredict whether a reaction will occur for each of the following. If a reaction takes place, write a balanced chemical equation (including phases). If a reaction does not take place, write No RXN.Cl2 (g) + KBr (aq) NaOH (aq) + AlCl3 (aq) Fe(NO3)2 (aq) + MgCl2 (aq) H2CO3 (aq) + Ba(OH)2 (aq) Topic 8: StoichiometryHow do chemists predict the amount of products that can be produced by a chemical reaction?VocabularyTermDefinitionstoichiometryLimiting reactantExcess reactantTheoretical yieldPercent YieldPrecipitateTopic 8: StoichiometryHow do chemists predict the amount of products that can be produced by a chemical reaction?ObjectivePractice ProblemsPREDICT the amount of a substance being used or produced by a reaction using the method of stoichiometryDetermine the moles of hydrogen gas produced when 50 grams of aluminum are reacted with sulfuric acid.Calculate the volume of hydrogen gas that must be burned with oxygen gas to form 4.0 moles of water at STP.When 234 grams of HgO is heated until decomposition, what mass of mercury will be formed?Topic 8: Stoichiometry (continued)How do chemists predict the amount of products that can be produced by a chemical reaction?DETERMINE the limiting reactant in a chemical reactionCALCULATE percent yield of a reaction. 2Al(s) + 3H2SO4(aq) Al2(SO4)3(aq) + 3H2(g)According to the above balanced chemical equation, if you place 5.00 grams of aluminum into 5.00 grams of sulfuric acid….a. How many grams of aluminum sulfate can be produced?b. What is the limiting reactant? ___________________c. Which reactant is in excess and by how much?d. If the actual yield of the aluminum sulfate is 5.35 grams, what is the percent yield?Determine the activity series of a set of reactions.From the data below, determine the activity series of these six elements: X, Y, Z, H, Ba, and Hg, placing the most active one first in the box provided below. Reactants ObservationsX + HClBubbles formY + HClNo ReactionZ + BaCl2No ReactionY + HgCl2A liquid metal begins to appearZ + HClBubbles formZ + XCl3A dark substance begins to form on the Z metalWork space: (if needed)Activity Series: most active ------------------------------------------------------------------>least activeTopic 9: Acids/ Bases/ MolarityHow do acids and bases react in solution?VocabularyTermDefinitionSoluteSolventSaturated SolutionSolutionSolubilityMolarityBronsted-Lowry Acid: Bronsted-Lowry Base: Titration: Salt: Buffer: pHObjectivePractice ProblemsGiven two of the following values (molarity, mass, and volume), CALCULATE the third value.How many grams of K2SO4 will be required to prepare 250mL of 0.5 M potassium sulfate?How many grams of NaOH will be required to prepare 500mL of 0.25 M sodium hydroxide?CALCULATE and DESCRIBE how to prepare a solution and perform a dilutionDescribe how you would prepare 100mL of 0.1 M HCl from 1M HCl?DIFFERENTIATE between an Arrhenius acid/base and a Bronsted-Lowry acid/base. Label and connect the conjugate acid-base pairs in the following reactions:NH4+ + OH- NH3 + H2O_________ _________ _________ _________ C2H3O2- + H2O HC2H3O2 + OH-_________ _________ _________ _________Which reaction(s) above don’t fit Arrhenhius’s definition of an acid/base and WHY?Topic 9: Acids/ Bases/ Molarity (continued)EXPLAIN the differences among an acid, a base, and a salt, and write balanced chemical equations for neutralization plete and balance the neutralization reactions shown below. Include the intermediate acid-base ions. Your completed reactions must be balanced..HCl + Mg(OH)2 H3PO4 + Ga(OH)3 HNO3 + Ba(OH)2 RELATE the ideas of Ka, pH, and conductivity to acid-base chemistry, and describe the relationship among, Ka, pH and conductivity, and acid-base strength.Given that HNO3, is a strong acid,Would you expect the Ka value for nitric acid, HNO3, to be large or small? _______Would the equilibrium mixture for nitric acid, HNO3, contain mainly products or mainly reactants? _______When 4 moles of nitric acid dissolve in 1 liter of water, what will be the approximate concentration of H3O+ ion formed? ________Would HNO3 have a high or a low conductivity? __________Would HNO3 have a high or a low pH value? __________Below you are given three values for the concentration of H+ ions of three different acids. Based on your knowledge of the relationship between [H+], pH, and conductivity, determine which of the three given pH values and relative conductivities best matches each of the concentrations of H+. [H+] pH (9.2, 6.9, or 1.4) Conductivity (high, medium, or low) 5.7 X 10-10M __________________________ 1.3 X 10-7M__________________________ 4.4 X 10-2M__________________________A solution has a hydrogen ion concentration of 3.42 x 10-10 M.What is [OH-] of the solution?What is the pH of the solution?Is the solution acidic or basic?__________________EXPLAIN the principles involved in the titration of acids and bases, and use unit analysis to calculate concentrations or volumes in titration problems.What is the molarity of a nitric acid solution if 43.3 mL of 0.100 M KOH solution is needed to neutralize 20.0 mL of the acid? Based on the data gathered below after titrating an solution of sodium hydroxide of unknown concentration, calculate the average concentration of the unknown sodium hydroxide solution. Show all of your work.Trial 1Trial 2Trial 3Initial burette HCl reading015.029.2Final burette HCl reading15.029.245.5mL of acid addedVolume of NaOH solution10.0 mL10.0 mL10.0 mLConcentration of HCl1.001.001.00Concentration of Unknown NaOHCalculation Trial 1:Calculation Trial 2:Calculation Trial 3:Average concentration of unknown NaOH solution:Concluding questionsIf you were graded on the overall effort you put into this class, what grade do you think you would deserve? (Please answer this as honestly as possible!)That’s it... You’re Done! Good Luck on the Final!!! ................
................

In order to avoid copyright disputes, this page is only a partial summary.

Google Online Preview   Download