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
Membrane
Transport
Passive
Transport
Simple
Diffusion
Facilitated
Transport
Osmosis
Active
Transport
Protein
Pumps
Endocytosis
Exocytosis
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
6H2O(l) + 6CO2(g)
Glucose + Oxygen
Chlorophyll + light
C6H12O6(aq) + 6O2(g)
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Science 10 Final Review
Cellular Respiration
Glucose + Oxygen
C6H12O6(aq) + 6O2(g)
Water + Carbon Dioxide
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
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Science 10 Final Review
Phototropism
Know what phototropism is and how it effects the growth of plants.
Darwin’s experiment on phototropism
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Science 10 Final Review
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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Science 10 Final Review
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
Elements
Compounds
Mixtures
Solutions
Mechanical
Mixtures
Suspensions
Colloids
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Science 10 Final Review
5 Atomic Models
Picture of Model
Scientist Name
Model Characteristics
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Science 10 Final Review
The Periodic Table
Atomic Number
Ion Charge
8
2-
O
Atomic
Molar Mass
Oxygen
16.00
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
Families/Groups – Columns:
-
Metalloids
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
30
3
4
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Science 10 Final Review
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
Octet Rule: The outermost energy level likes to be completely full
meaning it contains 8 electrons.
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Science 10 Final Review
Naming & Formulas
~ Ionic Compounds
Metal
Cation (positive)
I.e.
Na 1+
Sodium has less
Electron
+
+
Non-metal
Anion (negative)
=
=
Ionic Bond
Giving or
receiving of
electrons.
+
Cl 1Chlorine has 1
extra electron
=
NaCl
Therefore, Na
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.
2.
3.
4.
Identify the ions and their charges.
Determine the total charges needed to balance.
Note the ratio of cations to anions.
Use the subscripts to write the formula, if needed.
I.e. aluminum chloride
1. aluminum: Al3+
chloride: cl2.
Al +
+
+
Cl – Cl – Cl –
3. Al need 1
Cl need 3
Therefore Ratio is 1 to 3
4. AlCl3
Total Charge = 0
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Science 10 Final Review
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
Anion (negative)
+
+
Non-metal
Anion (negative)
=
=
Covalent Bond
Sharing of
Electrons
O2
O
16+
OO
16+
16+
Sharing
Electrons
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Science 10 Final Review
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
Solubility of Molecular Compounds
Acids & Bases
Properties of an Acid
Properties of a Base
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Science 10 Final Review
Naming Acids:
Rules are listed in your data booklet as well.
Ionic Name
Acid Name
Example
Formula
hydrogen ----ide
hydro ----ic acid
HCl
hydrogen ----ate
----ic acid
H3PO4
hydrogen ----ite
----ous acid
H3PO3
Ionic Name
hydrogen
chloride
hydrogen
phosphate
hydrogen
phosphite
Acid Name
hydrochloric
acid
phosphoric
acid
phosphorous
acid
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
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.
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Science 10 Final Review
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
phosphate
sodium nitrate + iron (II)
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
Fe – 1
N–2
O – 6 + 4 = 10
Na – 3
P–1
Products
Fe – 3
N–1
O – 3 + 8 = 11
Na – 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)
Reactants
Fe – 1 x 3 = 3
N–2x3=6
O – (6 x 3) + (4 x 2) = 26
Na – 3 x 2 = 6
P–1x2=2
6NaNO3(aq)
+
Fe3(PO4)2(s)
Products
Fe – 3
N–1x6=6
O – (3 x6) + 8 = 26
Na – 1 x 6 = 6
P-2
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Science 10 Final Review
Five Common Type of Reactions
1. Formation Reactions = two elements combine to form a compound.
Element + Element
Compound
A
AB
I.e.
+
S8(s) +
B
O2(g)
SO2(g)
2. Decomposition Reactions = a compound breaks down into two
elements
Compound
Element + Element
AB
A
I.e. NaCl(s)
+
Na(s) +
B
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
A
I.e.
+
Cl2(g)
BC
Compound + Element
AC
+ 2AgBr(s)
+
B
2AgCl(s) + Br2(l)
4. Double Replacement Reaction: Two ionic compounds react
together switching their elements to make two new compounds.
Compound + Compound
AB
+
CD
I.e. Pb(NO3)2(aq) + 2NaI(aq)
Compound + Compound
AD +
CB
PbI2(s) + NaNO3(aq)
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Science 10 Final Review
5. Hydrocarbon Combustion Reaction: contain hydrogen, carbon and
oxygen and always result in carbon dioxide and water as your
products.
Hydrocarbon + Oxygen
CxHy
+
Carbon dioxide + Water
O2(g)
CO2(g) + H2O(g)
I.e. CH4(g) + 2O2(g)
CO2(g) + 2H2O(g)
Predicting Products:
1.
2.
3.
4.
Classify the Reaction
Predict the names of the products
Write the skeleton equation
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)
4. 3Cu(s)
+
Au(ClO3)3(aq)
Cu(ClO3)2(aq)
+ 2 Au(ClO3)3(aq)
+
3Cu(ClO3)2(aq) +
Au(s)
2Au(s)
The Mole
Avogadro’s Number = 6.02 x 1023 molecules
n= m
M
n = number of moles
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
M = 108 g/m0l
n = 486 g
108 g/mol
n = 4.5 mols
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Science 10 Final Review
PHSYICS
Significant Digits
Scientific Notation
Manipulating Formulas
Motion
Uniform Motion (constant velocity i.e. constant speed and
direction)
Non-Uniform Motion
Speed
Average speed = distance traveled
change in time
v =d
= dfinal – dinitial
t
d (m)
tfinal – tinitial
Rise
v (m/s)
Run
t (s)
t (s)
Slope = Rise = d
Run t
Slope = speed
Scaler & Vector Quantities
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Science 10 Final Review
Distance vs. displacement/ speed vs. velocity
Velocity
Average velocity = displacement
change in time
v = d
= dfinal – dinitial
tfinal – tinitial
t
d (m)
Rise
v (m/s)
Run
t (s)
t (s)
Slope = Rise = d
Run t
Area = b x h
=vxt
Slope = speed
Area = distance
Acceleration
speed
distance
time
Positive acceleration
because the slope is
increasing.
time
Negative acceleration
because the slope is
decreasing.
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Science 10 Final Review
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
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=Fxd
Energy
Work = Joules
Energy = Joules
Work = Change in Energy
W = ΔE
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Science 10 Final Review
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
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 work
Work done on an object will change the object’s energy
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Science 10 Final Review
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.
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
total work input
x 100%
No process is 100% efficient. Some energy will always remain
in the form of thermal energy (heat).
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Science 10 Final Review
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.
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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