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Tips for Studying:
Take responsibility for yourselfRecognize that in order to succeed you need to make decisions about your priorities, your time, and your resources.
Center yourself on your values and principlesDon't let friends and acquaintances dictate what you consider important.
Put first things firstFollow 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 placesMorning, 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 situationwhen 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 problemsFor 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!
BIOLOGY
FINAL REVIEW PACKAGE~ SCIENCE 10 ~
Microscopes
Be able to label a microscope diagram! (see following page)
Be able to explain all of the following:
Hans and Zacharias JanssenRobert HookeAntoni van Leeuwenhoek
Transmission Electron MicroscopeScanning Electron Microscope
Cell Theory – Spontaneous Generation
Be able to explain all of the following:
Franseco RediJohn NeedhamLazzaro SpallanzaniFrench Academy of SciencesLouis Pasteur
Robert BrownM.J. Schleiden & Schwann
Controlled VariablesManipulated VariablesResponding Variables
Cell Organelles
Know all of the following cell organelles and be able to explain their functions.
Cell Membrane Transport
Be able to explain in detail each of the following cell membrane transport systems and draw diagram explaining it’s process.
Is bigger better?
CellMembra
neTranspor
ActiveTransport
PassiveTransport
Simple Diffusion
Osmosis
Facilitated
TransporEndocytosi Protein
Pumps
Exocytosis
Plant Structure
Know the following parts of the plant and their functions:
- Shoot System- Root System- 3 Types of Tissue:
1. Dermal Tissuea. cuticleb. epidermis
2. Ground Tissue
3. Vascular Tissuea. Xylem Tissueb. Phloem Tissue
Science 10 Final Review
Photosynthesis
Water + Carbon Dioxide Glucose + Oxygen
6H2O(l) + 6CO2(g) C6H12O6(aq) + 6O2(g)
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Chlorophyll + light
Chlorophyll + light
Science 10 Final Review
Cellular Respiration
Glucose + Oxygen Water + Carbon Dioxide
C6H12O6(aq) + 6O2(g) 6H2O(l) + 6CO2(g)
Gas Exchange
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Science 10 Final Review
Cr0ss-section of a Plant Diagram
Root to Leaf Water Transport
Tonicity in Plants
Phototropism
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Science 10 Final Review
Know what phototropism is and how it effects the growth of plants.
Darwin’s experiment on phototropism
Gravitropism
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Science 10 Final Review
Know what gravitropism is and how it effects the growth of plants.
Know how the chemical substance auxin affects plant growth.
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Science 10 Final Review
CHEMISTRY
Safety in the Lab:
Safety Hazard SymbolsWHMIS Symbols
Properties of Matter
Physical 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 Matter
HomogeneousHeterogeneous
Be able to define and classify each of the following:
5 Atomic Models
Picture of Model Scientist Name Model Characteristics
Matter
Pure Substances Mixtures
Elements Compounds Solutions Mechanical Mixtures Suspensions Colloids
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Science 10 Final Review
Atomic Molar Mass = # of protons + neutronsAtomic Number = # of protonsIon Charge = most common charge the element takes on tocomplete its energy levels.
Metals - Non-metals - Metalloids
Families/Groups – Columns: Alkali MetalsAlkaline Earth MetalsTransition MetalsHalogensNoble Gases
Periods – Rows
Subatomic Particles: Electrons, Protons, Neutrons
Complete the following Table:Element
NameIUPAC Symbol
Atomic Number
Group Number
Period Number
Metal (m) Nonmetal
(nm)
SATP State
Family Name
Chlorine
Magnesium
30
3 4
In an atom: # of electrons can change, becomes an ion# of neutrons can change, becomes an isotope# of protons can NOT change
Energy Level Diagrams
Atom:
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Atomic Molar Mass
Science 10 Final Review
0 Charge
11 Protons 12 Neutrons23 = Atomic Number
Ion: 1+ Charge
11 Protons 12 Neutrons23 = Atomic Number
Octet Rule: The outermost energy level likes to be completely full meaning it contains 8 electrons.
Naming & Formulas
~ Ionic Compounds
Metal + Non-metal = Ionic Bond
Cation (positive) + Anion (negative)= Giving orreceiving of electrons.
I.e. Na 1+ + Cl 1- = NaCl
Sodium has less Chlorine has 1 Therefore, Na Electron extra electron gives Cl his
electron.
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Na
281
Na
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Science 10 Final Review
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 chloride
Writing 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 chloride
1. aluminum: Al3+
chloride: cl- 2. Al + + +
Cl – Cl – Cl –
Total Charge = 0
3. Al need 1Cl need 3Therefore Ratio is 1 to 3
4. AlCl3
Multivalent Elements
Elements 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 chloride
Polyatomic Ions
Ions 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 Compounds
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Science 10 Final Review
Non-metal + Non-metal = Covalent Bond
Anion (negative) + Anion (negative)= Sharing ofElectrons
Naming Rules for Molecular Compounds
1. Name the first element2. Name the second element adding “ide” to the end.3. Add prefixes indicating the number of atoms.
I.e. N2O dinitrogen monoxide
P4O10 tetraphosphorus decaoxide
Writing Formulas for Molecular Compounds:
So easy! The prefixes in the names indicate the number of each element.
I.e. carbon tetrachloride CCl4
dinitrogen trioxide N2O3
Properties of Ionic Compounds and Molecular Compounds
Sharing Electrons
O 16+
O 16+O
16+
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O2
Science 10 Final Review
Solubility of Molecular Compounds
Acids & Bases
Properties of an Acid Properties of a Base
Naming Acids:
Rules are listed in your data booklet as well.
Ionic Name Acid Name ExampleFormula Ionic Name Acid Name
hydrogen ----ide
hydro ----ic acid HCl hydrogen chloride
hydrochloric acid
hydrogen ----ate
----ic acid H3PO4 hydrogen phosphate
phosphoric acid
hydrogen ----ite
----ous acid H3PO3 hydrogen phosphite
phosphorousacid
Chemical Reactions
Exothermic Reactions
Release Energy, usually in the form of heat!
C(s) + O2(g) CO2(g) + energy
coal + oxygen carbon dioxide + energy
Endothermic Reactions
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Science 10 Final Review
Absorb 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 Mass
Diatomic and Polyatomic Elements
Certain 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 Reactions
Example: 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) phosphate
2. 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.
Reactants ProductsFe – 1 Fe – 3N – 2 N – 1O – 6 + 4 = 10 O – 3 + 8 = 11Na – 3 Na – 1P – 1 P - 2
4. Now balance by adding coefficients to the front of certain formulas. Remember you can NOT change the subscripts only the coefficients.
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Science 10 Final Review
3Fe(NO3)2(aq) + 2Na3PO4(aq) 6NaNO3(aq) + Fe3(PO4)2(s)
Reactants ProductsFe – 1 x 3 = 3 Fe – 3N – 2 x 3 = 6 N – 1 x 6 = 6O – (6 x 3) + (4 x 2) = 26
O – (3 x6) + 8 = 26
Na – 3 x 2 = 6 Na – 1 x 6 = 6P – 1 x 2 = 2 P - 2
Five Common Type of Reactions
1. Formation Reactions = two elements combine to form a compound.
Element + Element Compound
A + B AB
I.e. S8(s) + O2(g) SO2(g)
2. Decomposition Reactions = a compound breaks down into two elements
Compound Element + Element
AB A + B
I.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 + Element
A + BC AC + B
I.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.
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Science 10 Final Review
Compound + Compound Compound + Compound
AB + CD AD + CB
I.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 + Water
CxHy + O2(g) CO2(g) + H2O(g)
I.e. CH4(g) + 2O2(g) CO2(g) + 2H2O(g)
Predicting Products:
1. Classify the Reaction2. Predict the names of the products3. Write the skeleton equation4. Balance the skeleton equation
I.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 Mole
Avogadro’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
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Science 10 Final Review
M = 108 g/m0l 108 g/mol
PHSYICS
Significant Digits
Scientific Notation
Manipulating Formulas
MotionUniform Motion (constant velocity i.e. constant speed and direction)Non-Uniform Motion
Speed
Average speed = distance traveledchange in time
v =d = dfinal – dinitial
t tfinal – tinitial
Slope = Rise = d Run t
Slope = speed
Scaler & Vector QuantitiesDistance vs. displacement/ speed vs. velocity
Velocity
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d (m)
t (s)
v (m/s)
t (s)
RiseRun
Science 10 Final Review
Average velocity = displacement change in time
v = = dfinal – dinitial
tfinal – tinitial
Slope = Rise = d Area = b x h Run t = v x t
Slope = speed Area = distance
Acceleration
Positive acceleration Negative acceleration because the slope is because the slope is increasing. decreasing.
Force
Force = Newtons = kg . m/s2
Net Force = mass x acceleration
Fnet = m x a
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d (m)
t (s)
v (m/s)
t (s)
RiseRun
distance
time
speed
time
Science 10 Final Review
Weight
Weight = force due to gravity = Newtons = kg . m/s2
Weight = mass x gravitational acceleration
Fg = mg
g = acceleration due to gravity on Earth’s surface = 9.81 m/s2
Work
For work to be done force and movement must both be going in the same direction.
ForceMovement
Work = Joules = Newton . m = kg . m/s2 . m
Work = force x distance
W = F x d
Energy
Work = JoulesEnergy = JoulesWork = Change in Energy
W = ΔE
Types of Energy
Potential Energy
Potential 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 height
Ep = m g h
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Science 10 Final Review
Kinetic Energy
Kinetic energy is energy of motion.Kinetic energy = Joules = kg . m/s2 . m
Kinetic energy = 1 mass x (velocity)2
2 Ek = ½ mv2
Mechanical Energy
Total mechanical energy of an object in motion is potential and kinetic energy combined.Mechanical energy = Joules = kg . m/s2 . m
Mechanical energy = Potential energy + Kinetic energy Em = Ep + Ek Em = m g h + ½ mv2
Energy is the ability to do workWork done on an object will change the object’s energy
Pendulum Energy Conversions
Imagine a pendulum swinging between points A & C. Label the types of energy (Ep, Ek or both) present at points A, B & C.
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C
B
A
Science 10 Final Review
Laws of Thermodynamics
1. 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.
Efficiency
Efficiency = useful work output x 100% total work input
No process is 100% efficient. Some energy will always remain in the form of thermal energy (heat).
Energy Conversions in Technological Systems
2. 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.
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Science 10 Final Review
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.
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