Unit 1:Matter and Change – Chapter 2
Describe how to distinguish between a substance and a mixture. (2.1)
Compare heterogeneous and homogeneous mixtures. (2.2 and lab)
Explain the difference between an element and a compound. (2.3)
Distinguish between physical and chemical changes in a specific example. (2.4)
State the law of conservation of matter and describe how it relates to physical changes and chemical reactions. (2.4)
Unit 2: Atomic Theory – Chapters 4-5
Summarize the development of the Modern Atomic Theory incorporating the contributions of Dalton, Thomson, Rutherford, Bohr and Schrodinger. (4.1, 4.2, 5.1)
Distinguish among protons, electrons, and neutrons in terms of their relative masses, charges and location in the atom. (4.3)
Infer the number of protons, electrons, and neutrons using the atomic number, mass number and charge of an element. (4.3)
Differentiate between mass number and atomic mass, and calculate atomic mass given isotope mass and abundance data. (4.3)
Describe changes that occur in the nucleus of an atom when it undergoes radioactive decay. Write a nuclear equation for a and b particle decay. (25.1, 25.2)
Explain the significance of quantized energies of the Quantum Mechanical Model. (5.1, 5.3)
Describe atomic orbitals in terms of shape, size and relative energy. (5.2)
Write electron configurations and orbital diagrams for elements applying the Aufbau principal, Pauli exclusion principal and Hund’s Rule as appropriate. (5.2)
Unit 3: Elements and the Periodic Table, Chapter 6
State the Periodic Law. (6.1)
Explain why elements in a group have similar properties. (6.2)
Identify the s, p, d, f - blocks of the Periodic Table, and give their associated names. Give the special names for Groups 1A, 2A, 7A and 8. (6.2)
Define four important periodic trends, atomic size, ionic size, ionization energy and electronegativity. State the changes in these trends on the periodic table and give an explanation for these changes in terms of the structure and electromagnetic forces of the atom. (6.3)
Unit 4: Names and Formulas of Compounds – Chapters 7-9
Describe the formation of an ionic bond, and then an ionic compound. (7.2)
State the basic properties of ionic compounds. (7.2)
Write the chemical formulas for binary and ternary ionic compounds from the name and write the name given the formula. (9.2)
State a few basic properties of molecular compounds. (8.1)
Differentiate between an ionic compound and a molecular compound in terms of their properties based upon their respective structures. (Summary of Ch. 7 and 8)
Create Lewis electron dot diagrams for covalent molecules containing single, multiple and resonance bonds. (8.2 and GIAs)
Describe the shapes of simple covalent molecules using VSEPR theory. (8.3 pp. 232-233)
Categorize a bond as non-polar covalent, polar covalent, or ionic using electronegativity values, and show the relationship between polar covalent bonds and polar molecules. (8.4)
Draw atomic level pictures that represent states, types and formulas of compounds. (GIAs)
Write the chemical formulas for binary molecular compounds from the name and write the name given the formula. (9.3)
Unit 5: Chemical Quantities and Calculations – Chapters 3 & 10
Determine the number of significant figures in a measurement and in a calculated answer. (3.1, activity)
Define a “mole” and relate it to Avogadro’s number. (10.1)
Define molar mass and tell how it relates to the mass of a substance. (10.1)
Convert among a number of particles, moles and mass of a substance. (10.1)
Convert moles to volume and volume to moles, using the volume of one mole of a gas at STP (22.4 L). (10.2)
Calculate the percent composition of a substance from its chemical formula or experimental data. (10.3)
Derive the empirical and/or molecular formula of a compound from experimental data. (10.3 and lab)
Unit 6: Reactions and Stoichiometry - Chapters 11-12
Interpret the symbols involved in a chemical reaction including identifying reactants and products in a chemical reaction. (11.1)
Balance chemical equations employing a variety of methods. (11.1)
Identify a combination, decomposition, single-replacement, double-replacement, and combustion reactions. (11.2)
Be able to predict the products of a combination, decomposition, single-replacement, double-replacement, or combustion reaction, given the reactants. (11.2)
Use the activity series of metals to predict whether a single-replacement reaction will occur. (11.2)
Predict the product of a double-replacement reaction in which a precipitate is formed and write this equation as a net ionic equation. (11.3)
Draw atomic level pictures that represent chemical reactions in terms of proportions of reactants and products including states, types and formulas of compounds. (GIAs)
Suggested Activities and Timetable for Preparing for Exams.
1) During the Christmas Holiday, get organized.
a) Collect materials from each unit of the 1st semester (units 1-5). This would include: self-tests, quizzes, tests, relevant worksheets and labs.
b) Determine what you are missing and get copies of what you need from the internet, from friends or from me, Mr. Ause.
Reviewing Units:
c) Look over the objectives, refreshing your vocabulary and the components of this unit.
d) Review your quizzes and tests, especially looking at those questions you missed.
e) Write an outline of unit using your notes, book and other sources. If you are going to re-read the textbook, the Christmas vacation is the time to do this and not the night before the exam.
f) Work through the summary questions assigned for review days on Units 1-3 and Units 4 & 5.
g) Bring your questions to me during class and tutorials in the following week.
2) Weekends of January12-13 and 19-21: Review all units (as suggested above)
3) During the week of January 14, 2008 ask your questions. Attend any after exam tutorials with further questions.
4) General Reminders:
a) Focus on the Mastery Objectives; regularly refer to these.
b) Spread out your studying.
c) Ask your questions of your classmates and me.
d) Use your old tests, quizzes and self-tests to test your studying.
