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! BIOLOGY
Microscopes
Be 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 Leeuwenhoek
Transmission Electron Microscope Scanning Electron Microscope
Cell Theory – Spontaneous Generation
Be able to explain all of the following:
Franseco Redi John Needham Lazzaro Spallanzani French Academy of Sciences Louis Pasteur
Robert Brown M.J. Schleiden & Schwann
Controlled Variables Manipulated Variables Responding 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.
Cell Passive Membrane Active Transport Transport Transport
Facilitated Simple Protein Endocytosis Transport Diffusion Pumps
Exocytosis 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 Tissue
3. Vascular Tissue a. Xylem Tissue b. Phloem Tissue Science 10 Final Review
Photosynthesis
Chlorophyll + light
Water + Carbon Dioxide Glucose + Oxygen Chlorophyll + light
6H2O(l) + 6CO2(g) C6H12O6(aq) + 6O2(g)
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Cellular Respiration
Glucose + Oxygen Water + Carbon Dioxide
C6H12O6(aq) + 6O2(g) 6H2O(l) + 6CO2(g)
Gas Exchange
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Cr0ss-section of a Plant Diagram
Root to Leaf Water Transport
Tonicity in Plants
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Phototropism
Know what phototropism is and how it effects the growth of plants.
Darwin’s experiment on phototropism
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Gravitropism
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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CHEMISTRY
Safety in the Lab:
Safety Hazard Symbols WHMIS 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
Homogeneous Heterogeneous
Be able to define and classify each of the following:
Matter
Pure Substances Mixtures
Mechanical Elements Compounds Solutions Suspensions Colloids Mixtures
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5 Atomic Models
Picture of Model Scientist Name Model Characteristics
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The Periodic Table Ion Charge Atomic Number 8 2- O Oxygen Atomic Molar 16.00 Mass
Atomic 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 - Metalloids
Families/Groups – Columns: Alkali Metals Alkaline Earth Metals Transition Metals Halogens Noble Gases
Periods – Rows
Subatomic Particles: Electrons, Protons, Neutrons
Complete the following Table: Element IUPAC Atomic Group Period Metal (m) SATP Family Name Symbol Number Number Number Nonmetal State Name (nm) Chlorine
Magnesium
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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: 0 Charge 1 8 2
Na
11 Protons 12 Neutrons 23 = Atomic Number Ion: 1+ Charge
8 2
Na
11 Protons 12 Neutrons 23 = Atomic Number
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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 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 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+ Cl – Cl – Cl – chloride: cl- Total Charge = 0 2. Al + + + 3. Al need 1
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Cl need 3 4. AlCl3 Therefore Ratio is 1 to 3
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
Non-metal + Non-metal = Covalent Bond Anion (negative) + Anion (negative) = Sharing of Electrons
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O2
O O O 16+ 16+ 16+
Sharing Electrons
Naming Rules for Molecular Compounds
1. 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 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
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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 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 acid
Chemical Reactions
Exothermic Reactions
Release Energy, usually in the form of heat!
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C(s) + O2(g) CO2(g) + energy coal + oxygen carbon dioxide + energy
Endothermic Reactions
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.
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Reactants Products Fe – 1 Fe – 3 N – 2 N – 1 O – 6 + 4 = 10 O – 3 + 8 = 11 Na – 3 Na – 1 P – 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.
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 - 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
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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.
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 Reaction 2. Predict the names of the products 3. Write the skeleton equation
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4. 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 M = 108 g/m0l 108 g/mol
PHSYICS
Significant Digits
Scientific Notation
Manipulating Formulas
Motion Uniform Motion (constant velocity i.e. constant speed and direction)
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Non-Uniform Motion
Speed
Average speed = distance traveled change in time
v =d = dfinal – dinitial
t tfinal – tinitial
v (m/s) d (m) Rise
Run
t (s) t (s)
Slope = Rise = d Run t
Slope = speed
Scaler & Vector Quantities Distance vs. displacement/ speed vs. velocity
Velocity
Average velocity = displacement change in time
v = Vd = dfinal – dinitial
Vt tfinal – tinitial
v (m/s) d (m) Rise
Run
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t (s) t (s)
Slope = Rise = d Area = b x h Run t = v x t
Slope = speed Area = distance
Acceleration
speed distance
time time
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
Weight
Weight = force due to gravity = Newtons = kg . m/s2
Weight = mass x gravitational acceleration
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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. Force Movement
Work = Joules = Newton . m = kg . m/s2 . m
Work = force x distance
W = F x d
Energy
Work = Joules
Energy = Joules
Work = 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 . m
Potential energy = mass x gravitational acceleration x height
Ep = m g h
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Kinetic Energy
Kinetic energy is energy of motion.
Kinetic energy = Joules = kg . m/s2 . m
Kinetic energy = 1 mass x (velocity)2 2
2 Ek = ½ mv
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
2 Em = m g h + ½ mv
Energy is the ability to do work Work 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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A C
B
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
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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. 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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