Download L47-Midterm-EST-Study Guide Enriched 2015

SECONDARY 4
EST MIDTERM STUDY GUIDE
Tips for writing your exam (you should read over these on the day of the exam):
 Look at the appendixes (the last few pages) right when you get your exam so
that you know the ‘tools’ that you have to work with
 ALWAYS include units in your answer when doing a calculation
(otherwise you will lose marks)
 ALWAYS include significant figures in your answer… there is short
description in this study guide if you forget how.
 Don’t leave any questions blank
 Use the amount of space given to you in the answer booklet as a guide for
how much you should be writing for each question
 If you don’t know the answer to a question, move onto the next one, and
come back to it once you’ve finished the exam.. you might find some hints
later on the exam that will help you
What you should do to study for the exam:
 Look at the topics that will be covered in the exam (on the next page).
 Go through the study guide, and complete the questions.
 Look over your notes from throughout the year. You will also need to know
certain concepts from the regular science course (ie. E=Pt, V=IR)
 Do some questions that we have been doing throughout the year.. even if
you have done it before, it helps to try them again so that they are fresh in
your mind. The quicker you can do the questions, the more time you will
have to do the more challenging ones. Print out the formulas at the end of
this sheet so that you get used to using them.
 Go over your old tests and quizzes, make sure that you know how to do the
questions (especially calculations)
 Make sure you know how to use all of the equations on the formula sheet at
the end of this guide
 Look at the formula sheet, there are a few equations missing.. memorize:
 Kirchhoff’s Laws
For Series Circuits: Itotal= I1 =I2 =I3.. Vtotal= V1 +V2 +V3 ..
For Parallel Circuits: Itotal= I1 + I2 +I3 .. Vtotal= V1 = V2 = V3 ..
 Mechanical Energy (Em1 = Em2, and Em= Ek + Epg)
Material World
Chemical Changes
 Oxidation
 Stoichiometry
 Endothermic and exothermic reactions
Living World
Organization of matter
 Simplified atomic model
 Nomenclature and notation rules
 Polyatomic ions
Periodic Table
 Relative atomic mass
 Atomic number
 Isotopes
Electricity and magnetism
 Kirchhoff’s Laws
 Magnetic field of a solenoid
Transformation of energy
 Effective Force
 Relationship between heat energy, specific heat
capacity, mass and temperature variations
 Relationship between kinetic energy, mass and
velocity
 Relationship between travel, force and work
 Relationship between gravitational potential
energy, mass, acceleration and travel
Earth and Space
Technological World
Graphical Language
 Multiview orthogonal projection
 Conduction, insulation and protection
(resistane and coding, printed circuits)
Composition of the exam:

Short Answer questions

Long Answer questions

Opinion question
Materials Permitted:
 Calculator
 Writing Instruments
 Ruler
Significant Figures
It’s very important that you include significant figures in your answer. Here are
some things to think about:
 If you don’t, you will lose marks.
 Most of the questions will involve multiplication (which takes precedence),
so focus on using the same number of significant figures in your answer as
the lowest number of significant figures given to you in your question.
 Don’t round your answer to significant figures until the end of the
calculation. For example, if you are doing a calculation involving
stoichiometry, keep at least 2 decimal places in your numbers until the end.
 Show me your answer, then round it to significant figures.
Multiplication
1. Multiply the numbers that are getting multiplied just as it would have been done without sig
fig's. For instance, 7.6, 9.687, and 44 are multiplied together. The answer (forgetting about sig
fig's) is 3239.3328
2. Count the number of sig fig's in each number. 7.6 has 2 sig fig's, 9.687 has 4 sig fig's, and 44
has 2 sig fig's.
3. Choose the lowest number of sig fig's, and apply that number to the answer in part one. Using
the above example, 3239.3328 has to be converted into 2 sig fig's, which becomes 3200.
Division - see Multiplication and follow the same rules except divide instead of multiply.
Material World
Chemical names and structures
The Periodic Table (pg. 24-26, 28 in textbook)
Atomic number: the number of protons in the element.
Relative atomic mass: mass of an atom of a particular element, including protons,
neutrons and electrons. Measured in a.m.u. (atomic mass units).
Mass number: relative atomic mass rounded to the nearest whole number.
Isotopes:
-
it can be said that all isotopes of the same atom have the same number of
_________________ but a different number of _________________.
-
In nature, not all isotopes of an atom are present in the same proportions. Often, one
isotope type will be more abundant than the other(s). This is referred to as relative
abundance.
Simplified Atomic Model: takes into account the number of neutrons in the
nucleus. The protons and neutrons are indicated, along with the number of
electrons in each shell. See page 28 in textbook for an example. Do question #32
on page 34 for practice.
Nomenclature
-you should know how to name a compound given a chemical formula, and to
write a chemical formula given the name of a compound.
The International Union of Pure and Applied Chemistry (IUPAC)
 Global organization responsible for setting standards in chemistry
 Assigns each compound a unique name
 Should be able to write chemical formula from chemical name
Ionic Compounds
Naming
 Name metal first
 Change ending of non-metal to “ide”
o Ex. hydride, fluoride, chloride, bromide, oxide, sulfide, nitride, etc.
Special Cases – Transition Elements
 Transition elements (metals in Groups 3-12) can form more than one cation → need to know
which one is being used. The charge on the metal will be indicated in brackets.
Molecular Compounds
Naming
 Name left-most non-metal first
 Change ending of right-most non-metal to “ide”
 Add prefixes to both element names to specify number of
atoms in a molecule
Prefix
mono
di
Number
1
2
tri
tetra
penta
hexa
hepta
octa
nona
deca
Polyatomic Ions
 Ion made of two or more different non-metal atoms joined
covalent bonds
 Form ionic compounds
 Only one cation: ammonium ion
 Names of anion and in “ate” not “ide” → except for
hydroxide
3
4
5
6
7
8
9
10
by
 Otherwise, naming is same as for binary ionic compounds
 Formulas is also same → except must use brackets to show more than one polyatomic ion
Examples:
Ammonium sulfide
Copper (II) carbonate
NH4+
S2-
Cu2+
(NH4)2S
CO32Cu2(CO3)2
CuCO3
1. Write the chemical formula for the following compounds. (4)
a. Potassium iodide
b. Dinitrogen trioxide
c. Copper (II) oxide
d. Barium nitrate
Energy (pg 73-79, 83, 88-91 in textbook)
The Law of Conservation of Energy states that energy can not be created or
destroyed, only transferred or transformed. Therefore, the total amount of energy
in a closed system is constant.
See the Chapter 3 Worksheet and Enriched Exam Review for practice questions.
The key to these questions is to obey the Law of Conservation of mass, and to
know which UNITS each variable must be expressed in. For example, other than
thermal energy, mass must be in kg to be put into the equations. Velocity is
always in m/s.
Thermal Energy: Q, heat, is the variation in thermal energy.
Q  mc ΔT Here, mass must be in g, and c is the specific heat capacity in J/goC.
The specific heat capacity is the amount of thermal energy required to raise the temperature of
one gram of a substance by one degree Celsius.
Kinetic Energy: energy of an object in motion.
1
E k  mv2 Remember: mass (m) must be in kg, velocity (v) must be in m/s. (km/h  3.6)
2
Gravitational Potential Energy: energy stored in an object raised above a surface, based on
it’s reference level (usually how far above the Earth it is)
E pg  mgh
(g=9.8N/kg) Mass (m) must be in kg, and height (h) must be in m.
Weight: If you are given the weight of an object, remember that it is the product of the mass and
gravitational field intensity (g). It is expressed in Newtons. Weight is calculated based on the
equation
w = Fg = mg, where w is the weight, Fg is the gravitational force, and m is the mass in kg.
Mechanical Energy: These problems are based upon the Law of Conservation of Energy, that
the energy in a closed system remains constant. Mechanical energy is the sum of the potential
energy and kinetic energy.
E m  E pg  E k and E m1 E m 2 so.. E pg1 E k1 E pg 2  E k 2 ..
Effective force: The effective force is the component of a force that affects the motion of the
object. A force applied at an angle can be broken down into it’s vertical and horizontal
components.. this is done using the basic trig functions (sin, cos, tan). It helps to draw a diagram
for these problems.
Work: Work is done when a force applied to an object causes it to move, in the same direction
as the force or one of it’s components.
W = ΔE, where W is the work, and ΔE is the difference in energy in a system
Also, W = F//d, where: W is the work (in Joules)
F// is the force parallel to the displacement of the object
d is the distance travelled by the object (in meters)
Changes in matter (pg. 112-117, 120)
Stoichiometry (lots of practice problems on Enriched Exam Review)
- the study of quantities of chemical reactions (using ratios in balanced chemical
equations to solve problems relating to those equations)
-you can do these problems in a variety of ways, depending on what you are
comfortable with. However, most problems involve four main steps:
1) Balance the chemical equation.
2) Convert whatever is given to mol.
3) Use ratios from the equation to predict how many mol of the unknown are
produced or needed.
4) Convert these new mol to whatever units are desired [usually mass (g)]
Endothermic/Exothermic Reactions
There are two types of questions here.
A. To find reaction energy, add up the energy in the bonds between the molecules
in the products, then in the reactants. Subtract the total bond energy of the
products from the bond energy of the reactants. If this value (the reaction energy)
is negative, it is exothermic, meaning it releases energy. If the value is positive, it
is endothermic, and absorbs energy. Try #14 on page 133. You should know how
to use the tables on page 115.
1. Sketch the graph of an endothermic reaction.
2. Sketch the graph of an exothermic reaction.
B. If given a chemical equation that includes the amount of energy in kJ, and are
asked to determine the amount of energy in a particular experiment, you need to do
a bit of stoichiometry. For example:
2H2O2 2H2O + O2 + 200kJ
Here, if asked to find the amount of energy released based on a certain amount of
O2 , you need to use the ratio of 1 mol of O2 to 200kJ of energy. Try question #16
on page 134.
Oxidation Reaction
1. What is an oxidation reaction?
2. What is an easy way to distinguish it from other reactions?
3. Give an example of an oxidation reaction.
Electricity and Magnetism (pg. 159-162, 169-170 in textbook)
Kirchhoff’s Laws (again, see the worksheet for practice problems)
1. The intensity of a current that flows into a node of a circuit is equal to the
intensity of the current that flows out of it. What this means for circuit diagrams:
For Series Circuits: Itotal= I1 =I2 =I3.. For Parallel Circuits: Itotal= I1 + I2 +I3 ..
2. The total energy from the power supply is equal to the energy transferred
diffused by the elements in the circuit. What this means for circuit diagrams:
For Series Circuits: Vtotal= V1 +V2 +V3 ..For Parallel Circuits: Vtotal= V1 +V2 +V3 ..
Equivalent Resistance
Series Circuits : Req= R1 +R2 +R3 ..
Parallel Circuits: Req 
1
1
1

R1 R2
For Extra practice- pg. 173 #19,20
Electromagnetism
A live wire, that is, a wire that is
conducting electricity, has a magnetic
field around it. When this is coiled
into a certain shape, it is called a
Solenoid (like the ones in your
earphones from woodshop). To
determine the direction of the
magnetic field, you use the right hand
rule, where your fingers point in the direction of conventional current, and the
thumb points toward the north pole of the magnetic field (within the coil). See
page 169 for a better diagram. Remember, conventional current flows from
positive to negative.
To increase the power of an electromagnet or solenoid:
1. increase the current intensity
2. add more loops
3. use a better core
Technological World
Technical Drafting (pg. 402-404 in textbook)
We have done many drawings/projections in the woodshop. You simply need to
remember how to do these.
 Isometric Projection
 Multiview Projection
The most important thing is to include a SCALE for your drawing. So, if one
centimetre on your paper is equal to 10 centimetres on your actual object, your
scale is 1 : 10.
FORMULAS
m
v
C:
m:
V:
concentration
mass
volume
W  ΔE
W: work
E: variation in energy
V  RI
V:
R:
I:
potential difference
resistance
electric current intensity
W  FΔd
W:
F:
d:
work
force
distance travelled
Fg  mg
Fg:
m:
g:
gravitational force
mass
gravitational field
intensity
Ep:
h:
gravitational potential
energy
mass
gravitational field
intensity
height
1
E k  mv 2
2
Ek:
m:
v:
kinetic energy
mass
velocity
Q  mc ΔT
Q:
m:
c:
T:
quantity of heat
mass
specific heat capacity
change in temperature
C
Req  R1  R2  ...
1
1
1


 ...
Req
R1 R 2
Req: equivalent resistance
Req: equivalent resistance
E  PΔt
E:
P:
t:
energy consumed
power
time
P  VI
P:
V:
I:
power
potential difference
electric current intensity
Fe :
k:
q:
r:
electrical force
Coulomb’s constant
charge of particle
distance between two
particles
Fe 
kq1q 2
r2
E p  mgh
m:
g:
QUANTITIES
NAME
SYMBOL
VALUE
Coulomb’s constant
k
9  109
Gravitational field intensity
g
9.8 N/kg
Nm 2
C2
Examples of Common Polyatomic Ions
NAME
CHEMICAL FORMULA
Acetate
CH3COO
Ammonium
NH4
Bicarbonate
HCO3
Carbonate
CO32
Chlorate
ClO3
Chromate
CrO24
Hydroxide
OH
Nitrate
NO 3
Phosphate
PO34
Sulphate
SO24