SCH 3U1
Culminating Performance Task
Introduction:
This task will test your abilities to perform a brief lab procedure, collect
data and answer questions on previously given topics.
The lab itself is found on page 606-7 in the textbook. The lab is based on
the reaction of magnesium metal with hydrochloric acid and the resulting gas
being collected. While in the lab, make sure you obey all safety procedures
and use the lab equipment properly and with care. As a class, we will go over
the brief procedure beforehand so you will not need any written procedures
at the lab desk. Complete the procedure accurately and concisely because
you still need time to answer questions. You may bring one blank piece of
paper into the lab station and record and write anything pertaining to the
lab. You and your lab partners are free to discuss anything during the data
collection but may not consult with other groups.
The questions that are being asked will take approximately 40 – 45 minutes
to answer. The 10-13 questions in the written portion of the CPT will be
based directly on the lab and the topics of the questions will be given
beforehand (eg. Ionic equations, Boyle’s Law). The questions will include all
the units. The only question that is not based directly on the lab is the last
question which will be an organic molecule that you will have to give the
correct IUPAC name. Answer all the questions on the response sheet and
then submit all papers for marking (test copy, answer sheet, data sheet).
The Culminating Performance Task is a final evaluation and the questions,
answer sheet and data sheet will not be returned to you. You may see it on
the exam review day if you would like to check them. The CPT is worth 5%
of your overall grade.
Materials:
Bring pencil, calculator, ruler, sheet of blank paper
Culminating Performance Task:
Possible Topics
Unit 1 – Nature of Matter
Unit 4 – Solutions
-
significant digits and place value
measurement and uncertainty
Bohr-Rutherford diagrams
p+, no, e1mass number and atomic number
isotopes and calculations (% to
mass, mass to %)
Periodic Table
groups and periods
Lewis dot diagrams (metal-nonmetal; non-metal-non-metal)
Periodicity (radius, ionization
energy, electronegativity,
reactivity)
Bonding
Nature and properties of ionic and
covalent compounds
intermolecular forces
∆electronegativity to determine
bonding
octet rule
Lewis structures (metal-non-metal;
non-metal-non-metal)
Polar vs. non-polar molecules
Naming of ionic and covalent
molecules
Unit 2 – Chemical Reactions
Chemical Reactions
word, skeleton and balanced
chemical equations
balancing reactions
reaction types (5)
metal activity series (you do not
have to memorize the chart)
name one hydrocarbon that will be
presented in class
Unit 3 – Chemical Quantities
-
calculation of moles, molar mass, #
of particles
per cent composition
limiting reactants
per cent error and per cent yield
Classification of Solutions
solution types (9 types) and
classification (3 types)
dissolving and particle attractions
molar concentration (M = n/V) and
dilutions (M1V1 = M2V2)
solubility, ionic equations, net ionic
equations, spectator ions
identifying ions in solution
solution stoichiometry
Acids and Bases
properties of acids and bases
pH scale
Arrhenius acids and bases
Strong vs. weak acids and bases
Acid-base neutralization and
titrations
Unit 5 – Gases
Gas Behaviour
the solid, liquid and gas state
forces between particles
Kinetic Molecular Theory
STP
Boyle’s Law
Charles’ Law
Gay-Lussac’s Law
Combined Gas Law
Real vs. ideal gases
Gases and the Mole
molar volume of 22.4 L/mol at STP
Avogadro’s Law
Ideal Gas Law and the Universal
Gas Constant
Density and molar mass
Dalton’s Law of Partial Pressure
Gas stoichimetry