Tips for Studying

FINAL REVIEW PACKAGE ~ SCIENCE 10 ~Tips for Studying:Take responsibility for yourself Recognize that in order to succeed you need to make decisions about your priorities, your time, and your resources.Center yourself on your values and principles Don't let friends and acquaintances dictate what you consider important. Put first things first Follow up on the priorities you have set for yourself, and don't let others, or other interests, distract you from your goals. Discover your key productivity periods and places Morning, afternoon, or evening? Find spaces where you can be the most focused and productive. Prioritize these for your most difficult study challenges.Consider yourself in a win-win situation when you contribute your best to a class, you, your fellow students, and even your teacher will benefit. Your grade can then be one additional check on your performance.Look for better solutions to problems For example, if you don't understand the course material, don't just re-read it. Try something else! Consult with the professor, a tutor, an academic advisor, a classmate, a study group, or your school's study skills center Look to continually challenge yourself THIS NOTE PACKAGE IS JUST THE BARE BONES! IT IS YOUR RESPONSIBILITY TO KNOW EACH TOPIC IN GREATER DETAIL! BIOLOGYMicroscopesBe able to label a microscope diagram! (see following page)Be able to explain all of the following: Hans and Zacharias Janssen Robert Hooke Antoni van LeeuwenhoekTransmission Electron Microscope Scanning Electron MicroscopeCell Theory – Spontaneous GenerationBe able to explain all of the following: Franseco Redi John Needham Lazzaro Spallanzani French Academy of Sciences Louis PasteurRobert Brown M.J. Schleiden & SchwannControlled Variables Manipulated Variables Responding VariablesCell OrganellesKnow all of the following cell organelles and be able to explain their functions. Cell Membrane TransportBe able to explain in detail each of the following cell membrane transport systems and draw diagram explaining it’s process.Cell Passive Membrane Active Transport Transport TransportFacilitated Simple Protein Endocytosis Transport Diffusion PumpsExocytosis Osmosis Is bigger better?Plant Structure Know the following parts of the plant and their functions:- Shoot System - Root System - 3 Types of Tissue:1. Dermal Tissue a. cuticle b. epidermis 2. Ground Tissue3. Vascular Tissue a. Xylem Tissue b. Phloem Tissue Science 10 Final ReviewPhotosynthesisChlorophyll + lightWater + Carbon Dioxide Glucose + Oxygen Chlorophyll + light6H2O(l) + 6CO2(g) C6H12O6(aq) + 6O2(g)8 Science 10 Final ReviewCellular RespirationGlucose + Oxygen Water + Carbon Dioxide C6H12O6(aq) + 6O2(g) 6H2O(l) + 6CO2(g)Gas Exchange9 Science 10 Final ReviewCr0ss-section of a Plant DiagramRoot to Leaf Water TransportTonicity in Plants10 Science 10 Final ReviewPhototropismKnow what phototropism is and how it effects the growth of plants.Darwin’s experiment on phototropism11 Science 10 Final ReviewGravitropismKnow what gravitropism is and how it effects the growth of plants.Know how the chemical substance auxin affects plant growth.12 Science 10 Final ReviewCHEMISTRYSafety in the Lab:Safety Hazard Symbols WHMIS SymbolsProperties of MatterPhysical Properties – physical appearance and composition of a substance. Examples page 13, Table A1.1 of text.Chemical Properties – the reactivity of a substance. Examples page 13, Table A1.2 of text.Classification of MatterHomogeneous HeterogeneousBe able to define and classify each of the following:MatterPure Substances MixturesMechanical Elements Compounds Solutions Suspensions Colloids Mixtures13 Science 10 Final Review5 Atomic ModelsPicture of Model Scientist Name Model Characteristics14 Science 10 Final ReviewThe Periodic Table Ion Charge Atomic Number 8 2- O Oxygen Atomic Molar 16.00 MassAtomic Molar Mass = # of protons + neutrons Atomic Number = # of protons Ion Charge = most common charge the element takes on to complete its energy levels.Metals - Non-metals - MetalloidsFamilies/Groups – Columns: Alkali Metals Alkaline Earth Metals Transition Metals Halogens Noble GasesPeriods – RowsSubatomic Particles: Electrons, Protons, NeutronsComplete the following Table: Element IUPAC Atomic Group Period Metal (m) SATP Family Name Symbol Number Number Number Nonmetal State Name (nm) ChlorineMagnesium3015 Science 10 Final Review3 4In an atom: # of electrons can change, becomes an ion # of neutrons can change, becomes an isotope # of protons can NOT changeEnergy Level DiagramsAtom: 0 Charge 1 8 2Na11 Protons 12 Neutrons 23 = Atomic Number Ion: 1+ Charge8 2Na11 Protons 12 Neutrons 23 = Atomic Number16 Science 10 Final ReviewOctet Rule: The outermost energy level likes to be completely full meaning it contains 8 electrons. Naming & Formulas~ Ionic CompoundsMetal + Non-metal = Ionic Bond Cation (positive) + Anion (negative) = Giving or receiving of electrons.I.e. Na 1+ + Cl 1- = NaCl Sodium has less Chlorine has 1 Therefore, Na Electron extra electron gives Cl his electron.Naming Rules for an Ionic Compound:1. Name the cation first by using the element’s name. 2. Name the anion second except minus the last syllable and replace it with “ide”I.e. NaCl = sodium chlorideWriting Formulas for Ionic Compounds:1. Identify the ions and their charges. 2. Determine the total charges needed to balance. 3. Note the ratio of cations to anions. 4. Use the subscripts to write the formula, if needed.I.e. aluminum chloride1. aluminum: Al3+ Cl – Cl – Cl – chloride: cl- Total Charge = 0 2. Al + + + 3. Al need 117 Science 10 Final ReviewCl need 3 4. AlCl3 Therefore Ratio is 1 to 3Multivalent ElementsElements with more than one stable ion. I.e. Iron = Fe2+ and Fe3+ Commonly found amongst the Transition Metals.Must use Roman Numerals to distinguish which ion charge you are using.I.e. FeCl3 iron III chloridePolyatomic IonsIons made up of several non-metallic atoms joined together. Found at the top of your Periodic Table in a box labeled Polyatomic Ions. (go figure!) Charge and name (including ending/suffix) are given in this box.Two most common suffixes for polyatomic ions = ‘ate’ and ‘ite’~ Molecular CompoundsNon-metal + Non-metal = Covalent Bond Anion (negative) + Anion (negative) = Sharing of Electrons18 Science 10 Final ReviewO2O O O 16+ 16+ 16+Sharing ElectronsNaming Rules for Molecular Compounds1. Name the first element 2. Name the second element adding “ide” to the end. 3. Add prefixes indicating the number of atoms.I.e. N2O dinitrogen monoxideP4O10 tetraphosphorus decaoxideWriting Formulas for Molecular Compounds:So easy! The prefixes in the names indicate the number of each element.I.e. carbon tetrachloride CCl4 dinitrogen trioxide N2O3Properties of Ionic Compounds and Molecular Compounds19 Science 10 Final ReviewSolubility of Molecular CompoundsAcids & BasesProperties of an Acid Properties of a BaseNaming Acids:Rules are listed in your data booklet as well.Ionic Name Acid Name Example Formula Ionic Name Acid Name hydrogen ----ide hydro ----ic acid HCl hydrogen hydrochloric chloride acid hydrogen ----ic acid H3PO4 hydrogen phosphoric ----ate phosphate acid hydrogen ----ite ----ous acid H3PO3 hydrogen phosphorous phosphite acidChemical ReactionsExothermic ReactionsRelease Energy, usually in the form of heat!20 Science 10 Final ReviewC(s) + O2(g) CO2(g) + energy coal + oxygen carbon dioxide + energyEndothermic ReactionsAbsorb energy! energy + 6CO2(g) + 6H2O(l) C6H12O6 + 6O2(g) energy + carbon dioxide + water glucose + oxygen (where is this chemical reaction most commonly found?)Law of Conservation of MassDiatomic and Polyatomic ElementsCertain elements do not exist by themselves – they require two of themselves to exist (these are non metals). Found at the top of the Periodic Table.Writing Chemical ReactionsExample: Aqueous iron (II) nitrate reacts with aqueous sodium phoshphate. The products are aqueous sodium nitrate and solid iron (II) phosphate.1. First write the word equation for the reaction.Iron (II) nitrate + sodium phosphate sodium nitrate + iron (II) phosphate2. Next write the skeleton equation for the reaction. Fe(NO3)2(aq) + Na3PO4(aq) NaNO3(aq) + Fe3(PO4)2(s)3. First write out the number of reactants and the number of products you have.21 Science 10 Final ReviewReactants Products Fe – 1 Fe – 3 N – 2 N – 1 O – 6 + 4 = 10 O – 3 + 8 = 11 Na – 3 Na – 1 P – 1 P - 24. Now balance by adding coefficients to the front of certain formulas. Remember you can NOT change the subscripts only the coefficients.3Fe(NO3)2(aq) + 2Na3PO4(aq) 6NaNO3(aq) + Fe3(PO4)2(s)Reactants Products Fe – 1 x 3 = 3 Fe – 3 N – 2 x 3 = 6 N – 1 x 6 = 6 O – (6 x 3) + (4 x 2) = O – (3 x6) + 8 = 26 26 Na – 3 x 2 = 6 Na – 1 x 6 = 6 P – 1 x 2 = 2 P - 2Five Common Type of Reactions1. Formation Reactions = two elements combine to form a compound.Element + Element CompoundA + B ABI.e. S8(s) + O2(g) SO2(g)2. Decomposition Reactions = a compound breaks down into two elementsCompound Element + Element22 Science 10 Final ReviewAB A + BI.e. NaCl(s) Na(s) + Cl2(g)3. Single Replacement Reactions = an element reacts with an ionic compound which results with the element ending up in the compound and the original element in the compound being by itself.Element + Compound Compound + ElementA + BC AC + BI.e. Cl2(g) + 2AgBr(s) 2AgCl(s) + Br2(l)4. Double Replacement Reaction: Two ionic compounds react together switching their elements to make two new compounds.Compound + Compound Compound + CompoundAB + CD AD + CBI.e. Pb(NO3)2(aq) + 2NaI(aq) PbI2(s) + NaNO3(aq)5. Hydrocarbon Combustion Reaction: contain hydrogen, carbon and oxygen and always result in carbon dioxide and water as your products.Hydrocarbon + Oxygen Carbon dioxide + WaterCxHy + O2(g) CO2(g) + H2O(g)I.e. CH4(g) + 2O2(g) CO2(g) + 2H2O(g)Predicting Products:1. Classify the Reaction 2. Predict the names of the products 3. Write the skeleton equation23 Science 10 Final Review4. Balance the skeleton equationI.e. copper (II) + gold(III)chlorate 1. An element with a compound will be single replacement.2. copper is a metal so it will have to replace gold(III) which is the metal in the compound.3. Cu(s) + Au(ClO3)3(aq) Cu(ClO3)2(aq) + Au(s)4. 3Cu(s) + 2 Au(ClO3)3(aq) 3Cu(ClO3)2(aq) + 2Au(s)The MoleAvogadro’s Number = 6.02 x 1023 molecules n = m n = number of moles M m = mass (grams) M = Molar mass (grams per mol)I.e. How many moles of silver are in a 486 gram sample? m = 486 g n = 486 g n = 4.5 mols M = 108 g/m0l 108 g/molPHSYICSSignificant DigitsScientific NotationManipulating FormulasMotion Uniform Motion (constant velocity i.e. constant speed and direction)24 Science 10 Final ReviewNon-Uniform MotionSpeedAverage speed = distance traveled change in time v =d = dfinal – dinitial t tfinal – tinitial v (m/s) d (m) RiseRun t (s) t (s)Slope = Rise = d Run tSlope = speedScaler & Vector Quantities Distance vs. displacement/ speed vs. velocity VelocityAverage velocity = displacement change in time v = Vd = dfinal – dinitialVt tfinal – tinitial v (m/s) d (m) Rise Run25 Science 10 Final Review t (s) t (s)Slope = Rise = d Area = b x h Run t = v x tSlope = speed Area = distance Acceleration speed distance time timePositive acceleration Negative acceleration because the slope is because the slope is increasing. decreasing.ForceForce = Newtons = kg . m/s2Net Force = mass x accelerationFnet = m x aWeightWeight = force due to gravity = Newtons = kg . m/s2Weight = mass x gravitational acceleration26 Science 10 Final ReviewFg = mg g = acceleration due to gravity on Earth’s surface = 9.81 m/s2WorkFor work to be done force and movement must both be going in the same direction. Force MovementWork = Joules = Newton . m = kg . m/s2 . mWork = force x distanceW = F x dEnergyWork = JoulesEnergy = JoulesWork = Change in EnergyW = ΔETypes of EnergyPotential EnergyPotential energy is stored energy (due to change in position and restoring force).Potential energy = Joules = kg . m/s2 . mPotential energy = mass x gravitational acceleration x heightEp = m g h 27 Science 10 Final ReviewKinetic EnergyKinetic energy is energy of motion.Kinetic energy = Joules = kg . m/s2 . mKinetic energy = 1 mass x (velocity)2 22 Ek = ½ mvMechanical EnergyTotal mechanical energy of an object in motion is potential and kinetic energy combined.Mechanical energy = Joules = kg . m/s2 . mMechanical energy = Potential energy + Kinetic energyEm = Ep + Ek2 Em = m g h + ½ mvEnergy is the ability to do work Work done on an object will change the object’s energyPendulum Energy ConversionsImagine a pendulum swinging between points A & C. Label the types of energy (Ep, Ek or both) present at points A, B & C.28 Science 10 Final ReviewA CBLaws of Thermodynamics1. Energy cannot be created or destroyed, but can be transformed from one form to another or transferred from one object to another.2. Every energy transformation results in the loss of some useful energy to unusable heat energy. That is, energy flows from an organized to a disorganized state, thus increasing entropy.EfficiencyEfficiency = useful work output x 100% total work inputNo process is 100% efficient. Some energy will always remain in the form of thermal energy (heat).Energy Conversions in Technological Systems29 Science 10 Final Review2. The reservoir stores water at a higher level than the generator below the dam, so the water has gravitational potential energy due to its higher position. 3. Water is the released into the penstock. As it flows down the penstock it loses gravitational potential energy but gains kinetic energy as it increases speed. 4. As water reaches the turbines, its kinetic energy pushes the blades of the turbines. The kinetic energy of the water is converted to kinetic energy of the turbines. 5. The turbines turn a coil of wire in a magnetic field, which converts the turbine’s kinetic energy into electrical energy. 6. This electricity is then distributed from the station to our homes.30

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