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Mrs. Kay Chemistry 11 Course Outcomes Unit One: Introduction 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 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 Mrs. Kay Chemistry 11 Course Outcomes 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 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 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 Mrs. Kay Chemistry 11 Course Outcomes 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 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 a unbalanced equation supply the necessary coefficients to balance it Define: skeleton, balanced and word equations Unit Five: The Mole! 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 Mrs. Kay Chemistry 11 Course Outcomes Unit Six: Organic chemistry 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