Test Bank for Chemistry: An Atoms-Focused Approach , 2nd Edition

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TesTBankChemistry:An Atoms-FocusedApproachseCond editionThomas R. Gilbert, Rein V. Kirss, Natalie FosterDaniel AutreyFAyetteville stAte UniversityScott ReidmArqUette University

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vPrefaceviiChapter 1|Matter and Energy—An Atomic Perspective1Chapter 2|Atoms, Ions, and Molecules—The Building Blocks of Matter42Chapter 3|Atomic Structure—Explaining the Properties of Elements76Chapter 4|Chemical Bonding—Understanding Climate Change120Chapter 5|Bonding Theories—Explaining Molecular Geometry168Chapter 6|Intermolecular Forces—Attractions between Particles216Chapter 7|Stoichiometry—Mass Relationships and Chemical Reactions255Chapter 8|Aqueous Solutions—Chemistry of the Hydrosphere297Chapter 9|Thermochemistry—Energy Changes in Chemical Reactions350Chapter 10|Properties of Gases—The Air We Breathe414Chapter 11|Properties of Solutions—Their Concentrations and Colligative Properties469Chapter 12|Thermodynamics—Why Chemical Reactions Happen510Chapter 13|Chemical Kinetics—Clearing the Air554Chapter 14|Chemical Equilibrium—Equal but Opposite Reaction Rates637Chapter 15|Acid-Base Equilibria—Proton Transfer in Biological Systems682Chapter 16|Additional Aqueous Equilibria—Chemistry and the Oceans717Chapter 17|Electrochemistry—The Quest for Clean Energy754Chapter 18|The Solid State—A Particulate View812Chapter 19|Organic Chemistry—Fuels, Pharmaceuticals, and Modern Materials856Chapter 20|Biochemistry—The Compounds of Life913Chapter 21|Nuclear Chemistry—The Risks and Benefits970Chapter 22|The Main Group Elements—Life and the PeriodicTable1012Chapter 23|Transition Metals—Biological and Medical Applications1040Contents

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vii6.Creating questions—pose questions or objectives thatprompt students to put elements they have learned togetherinto a coherentwhole to generate new ideas. Can studentscreate a new product or point of view based on data?Three DiffiCulTylevels:1.easy questions—require a basic understanding of theconcepts, definitions, and examples.2.moderate questions—direct students to use critical-thinking skills, to demonstrate an understanding of coreconcepts independent of specific textbook examples, andto connect concepts across chapters.3.difficult questions—ask students to synthesize textbookconcepts with their own experience, making analyticalinferences about biological topics and more.each question measures and explicitly links to a specific com-petency and is written with clear, concise, and grammaticallycorrect language that suits the difficulty level of the specificcompetency being assessed.to ensure the validity of thequestions, no extraneous, ambiguous, or confusing materialis included, and no slang expressions are used. In developingthe questions, every effort has been made to eliminate bias(e.g., race, gender, cultural, ethnic, regional, handicap, age) torequire specific knowledge of material studied, not of gen-eral knowledge or experience.this ensures accessibility andvalidity.keyToThe QuesTion MeTa-DaTaeach question in thetest Bank is tagged with five pieces ofinformation designed to help instructors create the mostideal mix of questions for a quiz or exam.these tags are:how DoesiTwork?thetest Bank author listed the learning objectives fromeach chapter believed to be the most important for studentsto learn.the author then developed questions designed totest students’ knowledge of a particular learning objective.By asking students questions that vary in both type and levelof difficulty, instructors can gather different types of evi-dence, which will allow them to more effectively assess howwell students understand specific concepts.six QuesTion Types:1.rememberingquestions—testdeclarativeknowledge,including textbook definitions and relationships betweentwo or more pieces of information. Can students recall orremember the information in the same form it was learned?2.Understanding questions—pose problems in a contextdifferent from the one in which the material was learned,requiring students to draw from their declarative and/orprocedural understanding of important concepts. Canstudents explain ideas or concepts?3.applying questions—ask students to draw from theirprior experience and use critical-thinking skills to takepart in qualitative reasoning about the real world. Canstudents use learned information in another task orsituation?4.analyzing questions—test students’ ability to break downinformation and see how different elements relate to eachother and to thewhole. Can students distinguish amongthe different parts?5.evaluating questions—ask students to assess informationas awhole and frame their own argument. Can studentsjustify a stand or decision?prefaCe

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viii|PrefaceOBJ:this is the learning objective that the question isdesigned to test.MSC:this is the knowledge type (see above) the questionis designed to test.ANS:this is the correct answer for each question.or, in thecase of some short-answer questions, a possible cor-rect answer to the given question.DIF:this is the difficulty assigned to the problem.problemshave been classified aseasy,medium, ordifficult.REF:this is the section in the textbook from which a ques-tion is drawn.

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1•Chapter 1LearningObjeCtivesDescribe what is meant by the termscientific theoryanddistinguish it fromnatural philosophy.Distinguish between elements and compounds.Describe the scientific method and define a law, a theory,and a hypothesis.Describe the law of definite proportions.Describe the law of constant composition.Describe the law of multiple proportions.Write chemical formulas from the ratios of the elementsin a compound.Describe and apply the COAST method.Distinguish between pure substances and mixtures.Definematter and mass.Describe and give examples of extensive and intensiveproperties.Describe and give examples of chemical and physicalproperties.Use density in calculations.Distinguish between molecules and ions.Distinguish between physical and chemical changes.Distinguish between homogeneous and heterogeneousmixtures.Describe the methods that can be used to separate thecomponents of a mixture: distillation, filtration, andchromatography.Distinguish between the states ofmatter: solid, liquid,and gas.Describe how temperature affects the properties ofmatter.Describe the processes of sublimation, melting, vaporiza-tion, condensation, freezing, and deposition.Define energy, work, and heat.Distinguish between potential and kinetic energy.State the law of conservation of energy.Recognize and interpret the different ways of representingmolecules (diatomic, molecular formula, structural for-mula, condensed structural formula, ball-and-stick,space-filling).Describe ionic compounds and identify an empiricalformula.Describe SI and US measurements.Distinguish between exact and uncertain values.Distinguish between precision and accuracy.Apply the rules for significant figures (weak-linkprinciple).Use the unit-factor method to convert measurements.Distinguish between and convert Fahrenheit, Celsius, andKelvin temperatures.Describe the function of a control sample.For a data set, calculate the mean, standard deviation,and confidence interval.Use Grubb’s test to determine if a data point is an outlier.Chapter 1:Matterandenergy—anatomicperspective

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2•Chapter 11Chapter 1: Matter and Energy—An Atomic PerspectiveMULTIPLE CHOICE1.Which step is NOT a part of the scientific method?a.Form a testable hypothesis.b.Make observations.c.Conduct reproducible experiments.d.Identify different factors that affect results.e.Stop experimentation once the desired results are achieved.ANS: EDIF:EasyREF:1.1OBJ:Describe the scientific method and define a law, a theory, and a hypothesis.MSC: Remembering2.For a hypothesis to be considered a valid scientific theory, it must ________a.summarize experimental data without trying to predict future results.b.be impossible to prove wrong by experiment.c.explain widely observed phenomena based on extensive testing.d.never be modified or expanded.e.be voted on by the scientific community and accepted by all.ANS: CDIF:EasyREF:1.1OBJ:Describe the scientific method and define a law, a theory, and a hypothesis.MSC: Understanding3.According to the law of definite proportions, ________a.atoms forming a given compound react in variable proportions depending on conditions.b.different samples of the same compound contain the same proportions of the sameelements.c.all compounds containing the same types of atoms have identical properties.d.all compounds containing the same types of atoms have relative masses that arewhole-number multiples.e.only one type of molecule can be produced when two elements combine.ANS: BDIF:EasyREF:1.1OBJ:Describe the law of definite proportions.MSC: Understanding4.The law of definite proportions states that ________a.compounds such as NO and NO2have identical chemical properties.b.compounds such as NO and NO2must have masses that are whole-number multiples ofeach other.c.nitrogen and oxygen can combine to form a variety of compounds, such as NO or NO2.d.the elements forming a given compound always react in the same proportions.e.only one compound can be produced when two elements combine.ANS: DDIF:EasyREF:1.1OBJ:Describe the law of definite proportions.MSC: Understanding

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3•Chapter 125.Which one of the following is a hypothesis?a.Energy is required to vaporize a liquid.b.The composition of a pure substance is fixed and definite.c.Hydrogen gas and oxygen gas can react to form water.d.A Car’s battery must be dead because the car won’t start.e.Matter is composed of atoms.ANS: DDIF:ModerateREF:1.1OBJ:Describe the scientific method and define a law, a theory, and a hypothesis.MSC: Applying6.Which of the following illustrates the law of multiple proportions?a.The mass ratio of O to N in NO2is twice that in NO.b.NO2always contains one nitrogen atom and two oxygen atoms.c.The mass of NO2is a small whole-number multiple of the mass of NO.d.NO and NO2have similar chemical and physical properties.e.NO2and N2O4are the same compound.ANS: ADIF:ModerateREF:1.1OBJ:Describe the law of multiple proportions.MSC: Understanding7.Which of the following does NOT illustrate the law of multiple proportions?a.The N-to-O mass ratio in NO is 0.875, whereas that in N2O is 1.75.b.C2H2has a 12:1 C-to-H mass ratio, while C2H6has a 4:1 C-to-H mass ratio.c.The ratio of O:C by mass in CO2is twice that of CO.d.If a sample of H2O contains 16 g of oxygen, a sample of H2O2with the same number ofmolecules would contain 32 g of oxygen.e.H2S and H2O contain the same mass of hydrogen.ANS: EDIF:DifficultREF:1.1OBJ:Describe the law of multiple proportions.MSC: Applying8.Which of the following statements is NOT true?a.The relative numbers of each type of atom in a given compound do not vary.b.A compound always contains the same mass percentages of its constituent elements.c.A large sample and a small sample of a given compound contain the same number ofeach type of atom.d.A large sample and a small sample of a given compound contain the same types of atomscombined in the same proportions.e.A large sample and a small sample of a compound share the same chemical formula.ANS: CDIF:DifficultREF:1.1OBJ:Describe the law of constant composition.MSC: Analyzing

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4•Chapter 139.Which of the following statements is NOT true?a.Given that the chemical formula of methanol is CH4O, the number of carbon atoms in asample of methanol will be the same as the number of oxygen atoms.b.If a compound is 75% carbon and 25% hydrogen by mass, 12 g of the compoundcontains 9 g C and 3 g H.c.If a compound contains 76 g of chlorine and 12 g of carbon, it will always have a 6.33:1mass ratio of Cl to C.d.A compound containing 17.1 g of phosphorus and 58.9 g of chlorine has the sameidentity as a compound containing 35.7 g P and 204.3 g Cl.e.A compound containing 106.6 g of copper and 13.4 g of oxygen has the same identity asa compound containing 159.9 g Cu and 20.1 g O.ANS: DDIF:DifficultREF:1.1OBJ:Describe the law of constant composition.MSC: Evaluating10.A pure substance ________a.must be composed of atoms of the same type.b.cannot be separated into simpler substances by physical means.c.must be a compound.d.has different chemical properties depending on its source.e.can have a composition that varies from sample to sample.ANS: BDIF:EasyREF:1.3OBJ:Distinguish between pure substances and mixtures.MSC: Remembering11.Which of the following is NOT a pure substance?a.sparkling waterd.water vaporb.gold metale.dry ice (solid CO2)c.oxygen gasANS: ADIF:EasyREF:1.3OBJ:Distinguish between pure substances and mixtures.MSC: Understanding12.Which of the following is a pure substance?a.seawaterd.table sugar(sucrose, C12H22O11)b.bloode.beerc.brass (an alloy of copper and zinc)ANS: DDIF:EasyREF:1.3OBJ:Distinguish between pure substances and mixtures.MSC: Understanding13.A molecule ________a.must contain at least two types of atoms.b.can be an element or a compound.c.cannot form a solid.d.cannot be broken into its constituent atoms by any means.e.can contain only one type of atom.ANS: BDIF:EasyREF:1.3OBJ:Distinguish between elements and compounds.MSC: Remembering

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5•Chapter 1414.A sample of a compound ________a.breaks into its constituent atoms during phase changes.b.is a homogeneous mixture.c.contains atoms that can be physically separated from each other.d.contains at least two types of atoms in a constant, fixed ratio.e.has a variable composition depending on its temperature.ANS: DDIF:EasyREF:1.3OBJ:Distinguish between elements and compounds.MSC: Remembering15.Which of the following is an element?a.C6H12O6d.CH4b.HNO3e.O3c.NaClANS: EDIF:EasyREF:1.3OBJ:Distinguish between elements and compounds.MSC: Understanding16.Which of the following is NOT an element?a.Csd.Arb.Aue.Coc.CS2ANS: CDIF:EasyREF:1.3OBJ:Distinguish between elements and compounds.MSC: Understanding17.An element ________a.can be separated into its components by physical methods.b.has different chemical properties depending on its state.c.cannot be separated into simpler substances by chemical methods.d.can also be a compound.e.exists only as atoms, not as molecules.ANS: CDIF:EasyREF:1.3OBJ:Distinguish between elements and compounds.MSC: Understanding18.Table sugar (sucrose, C12H22O11) dissolves in water. This process ________a.is a chemical change.b.is a physical change.c.produces a heterogeneous mixture.d.is a chemical property of sucrose.e.converts sucrose to carbon dioxide and water.ANS: BDIF:EasyREF:1.3OBJ:Distinguish between physical and chemical changes.MSC: Understanding

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6•Chapter 1519.Which of the following is a homogeneous mixture?a.an eggb.smokec.beach sandd.dry ice (solid CO2)e.a salt solution (NaCl dissolved in water)ANS: EDIF:EasyREF:1.3OBJ:Distinguish between homogeneous and heterogeneous mixtures.MSC: Understanding20.Which of the following is a heterogeneous mixture?a.concreted.mercury metalb.sweet teae.an intravenous (IV) solutionc.black coffeeANS: ADIF:EasyREF:1.3OBJ:Distinguish between homogeneous and heterogeneous mixtures.MSC: Understanding21.Distillation may be used to separate components in a mixture based on ________a.solubilities.d.densities.b.masses.e.colors.c.volatilities.ANS: CDIF:EasyREF:1.3OBJ:Describe the methods that can be used to separate the components of a mixture: distillation,filtration, and chromatography.MSC: Remembering22.Which of the following is a chemical property of formaldehyde (CH2O)?a.It is flammable.d.It dissolves in water.b.It has a density of 1.09 g/mL.e.It is a gas at room temperature.c.It is colorless.ANS: ADIF:EasyREF:1.3OBJ:Describe and give examples of chemical and physical properties.MSC: Remembering23.Which of the following is a chemical property of copper metal?a.It conducts heat.b.It reacts with nitric acid to produce copper(II) nitrate.c.It melts at 1085°Cd.It conducts electricity.e.It has an orange color.ANS: BDIF:EasyREF:1.3OBJ:Describe and give examples of chemical and physical properties.MSC: Remembering

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7•Chapter 1624.Which of the following represents a physical property of water?a.It boils at 100°C.b.An electrical current decomposes water into hydrogen gas and oxygen gas.c.It reacts with iron metal and oxygen to form rust.d.It reacts with carbon monoxide to form carbon dioxide and hydrogen gas.e.It is used in photosynthesis.ANS: ADIF:EasyREF:1.3OBJ:Describe and give examples of chemical and physical properties.MSC: Remembering25.Which of the following represents a chemical property of iron?a.Its density is 7.84 g/cm3.d.Its melting point is 1538°C.b.It is magnetic.e.It conducts electricity.c.It reacts with oxygen in moist air.ANS: CDIF:EasyREF:1.3OBJ:Describe and give examples of chemical and physical properties.MSC: Remembering26.Which of the following is a chemical property of acetone (C3H6O)?a.It readily evaporates at room temperature.b.It has a pungent, irritating odor.c.It can be ignited in oxygen.d.It boils at 56°C.e.It is miscible with water.ANS: CDIF:EasyREF:1.3OBJ:Describe and give examples of chemical and physical properties.MSC: Remembering27.Which of the following is a chemical property of platinum?a.It conducts heat and electricity.b.It can react with chlorine gas to form platinum(IV) chloride.c.The difference between its melting and boiling points is 2057°C.d.It is a gray-white metal.e.Sound travels through it at a speed of 2680 m/s.ANS: BDIF:EasyREF:1.3OBJ:Describe and give examples of chemical and physical properties.MSC: Remembering28.Extensive properties are ________a.dependent on the amount of substance present.b.identical for all substances.c.independent of a substance’s phase.d.the physical properties of a substance.e.dependent on the reactivity of the substance.ANS: ADIF:EasyREF:1.3OBJ:Describe and give examples of extensive and intensive properties.MSC: Remembering

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8•Chapter 1729.Which one of the following represents a physical change?a.Milk turns sour.d.An egg begins to smell very bad.b.Rust forms on iron nails.e.Sugar melts and forms a syrupy liquid.c.Sugar ferments to form ethanol.ANS: EDIF:EasyREF:1.3OBJ:Distinguish between physical and chemical changes.MSC: Understanding30.Which one of the following represents a chemical change?a.Mercury(II) oxide is heated up and forms mercury metal and oxygen gas.b.Rubbing alcohol evaporates.c.Iodine vapor deposits on a surface.d.Iron metal is separated from sand using a magnet.e.Rock salt is pulverized.ANS: ADIF:EasyREF:1.3OBJ:Distinguish between physical and chemical changes.MSC: Understanding31.Which one of the following is NOT an intensive physical property of a pure liquid?a.boiling pointd.densityb.conductivitye.colorc.massANS: CDIF:ModerateREF:1.3OBJ:Describe and give examples of extensive and intensive properties.MSC: Remembering32.Which statement is true regarding ammonia, NH3?a.It can also be correctly represented as N2H6.b.It cannot be decomposed into simpler substances by any means.c.Its decomposition produces three volumes of hydrogen for every one volume of nitrogen.d.It can be separated into nitrogen and hydrogen atoms using distillation.e.It is not a stable molecule and does not exist at room temperature.ANS: CDIF:ModerateREF:1.3OBJ:Distinguish between elements and compounds.MSC: Understanding33.When copper metal is dropped into nitric acid, a blue solution containing copper(II) ions is producedalong with brown nitrogen monoxide gas. Which of the following is an example of a chemicalproperty?a.copper’s red-orange appearanceb.nitrogen monoxide’s irritating odorc.the blue color of aqueous copper(II) ionsd.the viscosity of nitric acid at room temperaturee.nitric acid’s ability to react with copper metalANS: EDIF:ModerateREF:1.3OBJ:Describe and give examples of chemical and physical properties.MSC: Analyzing

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9•Chapter 1834.If you had equal masses of each of the following substances, which would occupy the greatestvolume?a.ice (d=0.917 g/mL)d.cocoa butter (d=0.910 g/mL)b.water (d=0.997 g/mL)e.aluminum (d=2.70 g/mL)c.beeswax (d=0.960 g/mL)ANS: DDIF:ModerateREF:1.3OBJ:Use density in calculations.MSC: Analyzing35.The densities of glycerol and of mercury are 1.26 g/mL and 13.5 g/mL, respectively. What volume ofglycerol has the same mass as 25.0 mL of mercury?a.268 mLd.1.47 mLb.426 mLe.338 mLc.2.33 mLANS: ADIF:ModerateREF:1.3OBJ:Use density in calculations.MSC: Applying36.Based on values for the volume per gram of the given materials, which of the following would NOTfloat in water (density = 0.997 g/cm3)?Substanceg/cm3Balsa wood0.120Cork0.240Charcoal (from oak)0.571Human fat0.943Ethylene glycol1.11a.balsa woodd.human fatb.corke.ethylene glycolc.charcoalANS: EDIF:ModerateREF:1.3OBJ:Use density in calculations.MSC: Applying37.Calcite has a chemical formula of CaCO3, and 1.0 g occupies approximately 0.369 cm3. Pyrite (FeS2)is 1.8 times denser than calcite. What is the density of FeS2?a.2.7 g/cm3d.2.2 g/cm3b.0.66 g/cm3e.1.5 g/cm3c.4.9 g/cm3ANS: CDIF:ModerateREF:1.3OBJ:Use density in calculations.MSC: Applying

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10•Chapter 1938.Which of the following can be separated by filtration?a.rust particles in waterd.salt dissolved in waterb.air dispersed in whipped creame.nitrogen from airc.alcohol dissolved in waterANS: ADIF:ModerateREF:1.3OBJ:Describe the methods that can be used to separate the components of a mixture: distillation,filtration, and chromatography.MSC: Understanding39.Which process would be a practical and effective way to separate beta-carotene, an orange pigment,from hexane liquid?a.filtrationd.scanning tunneling microscopyb.chromatographye.sublimationc.combustionANS: BDIF:ModerateREF:1.3OBJ:Describe the methods that can be used to separate the components of a mixture: distillation,filtration, and chromatography.MSC: Applying40.Acetone and water mix to form a homogeneous solution. Acetone has a boiling point of 56°C. Whichof the following would be a suitable method for separating acetone from water?a.filtrationd.scanning tunneling microscopyb.combustione.sublimationc.distillationANS: CDIF:ModerateREF:1.3OBJ:Describe the methods that can be used to separate the components of a mixture: distillation,filtration, and chromatography.MSC: Applying41.Which of the following is an intensive property of chlorine?a.It has mass.b.It boils at−34°C.c.Chlorine gas expands to fill a balloon.d.The reaction of chlorine with hydrogen releases a given amount of energy.e.Chlorine gas in a container exerts a given pressure at a given temperature.ANS: BDIF:ModerateREF:1.3OBJ:Describe and give examples of extensive and intensive properties.MSC: Analyzing42.Which represents an extensive property of hydrogen?a.Hydrogen gas is odorless and colorless.b.A hydrogen gas molecule is composed of two hydrogen atoms.c.Hydrogen gas is flammable.d.Hydrogen releases a given amount of energy when it reacts with oxygen.e.Hydrogen gas under normal conditions is nonmetallic.ANS: DDIF:ModerateREF:1.3OBJ:Describe and give examples of extensive and intensive properties.MSC: Analyzing

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