Download Chemistry 11 – Course Outcomes

Chemistry 11 – Course Outcomes
Unit One: Introduction
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Define and give example of empirical, authoritative, rational, intuitive and revealed
knowledge.
Distinguish between observation and inference
Define scientific model
Distinguish between a chemical property (or change) and a physical property (or
change)
Define: Pure substance, impure material, mixtures, homogeneous and heterogeneous,
atoms, elements, compounds, molecules
State the characteristics of a solution and how they differ from pure substances
Distinguish purity from their melting point curves
Describe the characteristics of states of matter
Describe the following methods of physical separation: filtering, distillation,
chromatography and sifting
Use instruments in lab to record measurements
Explain the difference between precision and accuracy
Given a measurement determine the number of significant digits present
Use significant digit rules (rounding, adding/subtracting and multiplying/dividing) to
perform calculations
Use scientific notation to express numbers
Unit Two: Atomic Theory and Periodic Table
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State the postulates of Dalton’s atomic theory
List which statements of Dalton’s theory we now believe to be incorrect
Give observable evidence to support the idea that there are positive and negative
charges.
Describe force between like charges and opposite charges
Explain how J.J. Thomson changed the view of the atom
Use Rutherford’s gold foil experiment to support the model that protons in the atom are
concentrated in the nucleus and positive.
Give the relative mass of the following: electrons, protons, neutrons
Define mass number and atomic number of an isotope, determine the number of
protons, electrons and neutrons for a given isotope
Calculate average atomic mass, given atomic masses and heir abundance.
Locate in periodic table and state the properties of metals, non metals and metalloids
State periodic law
Use formulas of oxides, fluorides, hydrides to organize elements into families
Locate and describe the properties of the noble gases, halogens, transition metals,
alkaline earth metals and alkali metals in the periodic table
Given some properties for elements in a family, predict the corresponding properties
for a missing element of hypothetical element of the same family.
Distinguish between atoms and ions (cations and anions and their formation)
Unit three: Electron Configuration and Periodic Trends
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Give assumptions of Bohr Model
Explain the hydrogen line spectrum in terms of Bohr Model of the atom
State two differences between the Bohr model and the quantum mechanical model of
the atom
Draw an energy level diagram for a given atom
Define valence shell and valence electrons
Label the sublevels on an energy level diagram with s, p, d, f
Describe maximum number of electrons associated with each sublevel
Use the periodic table to predict number of valence electrons
Use the periodic table to predict the electron configuration of an element
Indicate the probable pattern of electrons around the nucleus of any atom using the
electron configuration notation
Distinguish between s and p orbitals
Distinguish between orbit and orbital
State the: Aufbau principle, Hund’s rule, and Pauli Exclusion principle
Define: ionization energy, atomic size (radius) and electron affinity
State and explain trends in the periodic table for ionization energy, electron affinity and
atomic size
Define and describe first ionization energy. Write an equation showing first ionization
energy
Use successive ionization energy to determine number of valence electrons for an
unknown atom
Unit Four: Bonding and Nomenclature
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Define and explain isoelectronic
Use electron affinity to explain formation of ions and explain how the formation of ionic
compounds occurs
State octet rule
Give an electron dot diagram (Lewis dot diagram) of atoms forming ions and ionic
bonding (3 equations)
Use model for the structure of an ionic compound to explain its properties
Define molecular (covalent bonding) and give structural formula of molecular
compounds.
State properties of ionic compounds and molecules (hardness, melting point,
conductivity, odour…)
Describe coordinate covalent bonding and provide example
Define metallic bonding and distinguish its properties form ionic and molecular
(covalent bonds)
Using VSEPR (valence shell electron pair repulsion) theory, predict the shape of a
molecule.
Assign charges (oxidation numbers) to atoms within a compound
Distinguish between molecular and ionic compounds
Use periodic table (ionic table) and polyatomic ionic table to correctly write chemical
formula from a given name.
Apply rules for nomenclature for ionic and molecular compounds if given chemical
formula
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Given the name for an ionic or molecular formula, write the formula
Be able to recognize and name acids
Distinguish between subscripts and coefficients
Properly interpret the meaning of a chemical formula (i.e. Number of atoms)
Identify the 5 main types of chemical reactions: synthesis, decomposition, double
displacement, single displacement, and combustion
Given a word equation for a reaction write a complete balanced chemical equation.
Given an unbalanced equation supply the necessary coefficients to balance it
Define: skeleton, balanced and word equations
Unit Five: The Mole!
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Define the term “mole”
Define the molar mass of a pure substance as the mass of 6.02 x 1023 atoms,
molecules or formula units.
Find the molar mass of a compound using the periodic table
Understand and apply relationship between moles, atoms and formula units with the
molar mass of a substance.
Define “empirical formula”
Solve for empirical formula if given masses or percentage composition of each
component of the compound.
Solve for molecular formula if given percentage composition and molar mass of the
compound
Identify mole ratios of reactants and products from balanced chemical equations
Perform mole to mole conversion, mole to mass conversion, mass to mass conversion
Define “percent yield” and how it can be maximized or minimized
Define “theoretical and actual yields” and how they obtain percent yields through
calculations
Given the amounts of two reactants, identify the limiting reagents and solve the
theoretical yield for the problem
Unit Six: Organic chemistry
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Describe organic chemistry and hydrocarbons
Describe, draw/name and identify the following: alkanes, alkenes, cyclic and alkynes
using IUPAC rules
Know general formulas for alkanes, alkenes, alkynes and cyclic
Define saturated and unsaturated compounds
Define and give examples of isomers (Be able to draw all isomers for alkanes for up to
6 C and for alkenes for up to 4 C)
Name all the prefixes from 1 to 10 carbon groups (alkyl groups)
Define “aromatics” and be able to draw/identify them as compounds containing
benzene ring
Define the term “functional group” and identify/name/draw alcohols, esters, carboxylic
acids
Identify and give examples of addition, substitution, esterification, combustion and
addition reactions of hydrocarbons