Download MATERIAL FOR GRADE 9 FINAL EXAM 2016

MATERIAL FOR GRADE 9 FINAL EXAM 2016-2017
Introduction to chemical bonding p.164-198
• Define chemical bond.
• Explain why most atoms form chemical bonds.
• Differentiate ionic and covalent bonding.
• Explain why most chemical bonding is neither purely ionic nor purely covalent.
• Classify bonding type according to electronegativity differences.
Covalent bonding and molecular compounds
• Define molecule and molecular formula.
• Explain the relationships among potential energy, distance between approaching atoms, bond length, and bond
energy.
• State the octet rule.
• List the six basic steps used in writing Lewis structures.
• Explain how to determine Lewis structures for molecules containing single bonds, multiple bonds, or both.
• Explain why scientists use resonance structures to represent some molecules.
Ionic bonding and ionic compounds
• Compare and contrast a chemical formula for a molecular compound with one for an ionic compound.
• Discuss the arrangements of ions in crystals.
• Define lattice energy and explain its significance.
• List and compare the distinctive properties of ionic compounds and molecular compounds.
• Draw the Lewis structure for a polyatomic ion given the identity of the atoms combined and other appropriate
information.
Metallic bonding
• Describe the electron-sea model of metallic bonding, and explain why metals are good electrical conductors.
• Explain why metal surfaces are shiny.
• Explain why metals are malleable and ductile but ionic-crystalline compounds are not.
Chemical names and formulas P.207 - 238
• Explain the significance of a chemical formula.
• Determine the formula of an ionic compound formed between two given ions.
• Name an ionic compound given its formula.
• Using prefixes, name a binary molecular compound from its formula.
• Write the formula of a binary molecular compound given its name.
Oxidation numbers
• List the rules for assigning oxidation numbers.
• Give the oxidation number for each element in the formula of a chemical compound.
• Name binary molecular compounds using oxidation numbers and the Stock system
Counting atoms
• Explain what isotopes are.
• Define atomic number and mass number, and describe how they apply to isotopes.
• Given the identity of a nuclide, determine its numbers of protons, neutrons, and electrons.
• Define mole, Avogadro’s number, and molar mass, and state how all three are related.
Using chemical formulas
• Calculate the formula mass or molar mass of any given compound.
• Use molar mass to convert between mass in grams and amount in moles of a chemical compound.
• Calculate the number of molecules, formula units, or ions in a given molar amount of a chemical compound.
• Calculate the percentage composition of a given chemical compound.
Describing chemical reactions P. 247 - 270
• List three observations that suggest that a chemical reaction has taken place.
• List three requirements for a correctly written chemical equation.
• Write a word equation and a formula equation for a given chemical reaction.
• Balance a formula equation by inspection.
Types of chemical reactions
• Define and give general equations for synthesis, decomposition, single displacement, and double
displacement reactions.
• Classify a reaction as a synthesis, decomposition, single-displacement, double-displacement, or combustion
reaction.
• List three kinds of synthesis reactions and six kinds of decomposition reactions.
• List four kinds of single-displacement reactions and three kinds of double-displacement reactions.
• Predict the products of simple reactions given the reactants.
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MATERIAL FOR GRADE 10 FINAL EXAMS 2016-2017
The nucleus Study the copybook and sheets given, solve the chapter review
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Explain why nuclear reactions occur, and know how to balance a nuclear equation.
Describe the different types of radioactive decay and their effects on the nucleus.
Define the term half-life, and explain how it relates to the stability of a nucleus.
Explain what a nuclide is, and describe the different ways nuclides can be represented.
Define and relate the terms mass defect and nuclear binding energy.
Explain the relationship between number of nucleons and stability of nuclei. .
Define nuclear fission, chain reaction, and nuclear fusion, and distinguish between them.
Worksheet notes
Describe the mass defect in a nuclear isotope.
Calculate binding energy in a nuclear isotope using E=mc2 in joules, electron volts and million
electron volt
Introduction to organic chemistry study the copybook and the summary notes given, solve the chapter review
 Explain how the structure and bonding of carbon lead to the diversity and number of organic
compounds.
 Compare the use of molecular and structural formulas to represent organic compounds.
 Compare structural and geometric isomers of organic compounds.
 Distinguish among the structures of alkanes, alkenes AND alkynes.
 Write structural formulas and names for alkane, alkene , alkyne and alcohols
 Isomers and naming cyclic hydrocarbons.
 Drawing line structures.
 Reactions of alkanes, and alkenes
 Reactions of alkynes and alcohols.
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MATERIAL FOR GRADE 11 FINAL EXAMS 2016-2017
 Chapter 15: Acids and Bases
 pH, pOH of strong acids and strong bases and acid-base mixture.
 pH, pOH, Ka, pKa, Kb, pKb of weak acids and bases.
 Calculate the pH of a buffer using equilibrium calculations and the
Henderson-Hasselbalch equation.
 Select the appropriate weak acid to make a buffer of given pH.
 Predict the pH of a titration given the type of acid and base (strong or weak).
 Calculate the pH throughout a titration between acids and bases: strong plus
strong or strong plus weak.
 Use a titration curve to identify what type of titration was employed (e.g.
weak acid plus strong base).
 Distinguish between endpoint and equivalence point.
 Chapter 10: Kinetic molecular theory.
 KMT assumptions.
 Deviation of real gases from ideal behavior.
 How KMT accounts for gas, liquid and solid properties.
 Equilibrium vapor pressure.
 Phase diagram.
 Water.
 Chapter 12: Gas Laws.
 Pressure of gases.
 Barometer.
 Manometer.
 Dalton's law.
 Water displacement method.
 Boyle's law.
 Charle's law.
 Gay-Lussac's law.
 Combined Gas law.
 Ideal Gas Law.
 Avogadro's Law.
 Grahams Law.
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