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SubjectGradeStreamTermWeek Unit NumberUnit NameChapter / Module NumberChapter NameSection / Lesson NumberSection / Lesson NameNumber of Periods
(per chapter)		Vocabulary / Key WordsResourcesLearning Outcomes
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SLOs CodesStudent Learning Outcomes (S.L.Os)Key Performance Criteria
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Chemistry12AdvancedTerm 2
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U3Matter, Energy, and equilibriumChapter 4 / Module 17Acids and BasesL1Introduction to acids and basesRefer to the teacher edition of the book
Supplement with digital resources found on LMS such as Al Madrasa, Boclips, Lernatic, Edushare, ALEKS

Please refer to scope and sequence document on LMS where the lessons to be covered had been identified with their type of learning		CHM.5.3.04.001Differentiate between acids and bases based on Arrhenius, Brønsted-Lowery and Lewis theoriesCHM.5.3.04.001.01 List six general properties of aqueous acids (taste, color of indicators, reaction with metals, metal carbonates and bases, and electrical conductivity)
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CHM.5.3.04.001.02 List five general properties of aqueous bases (taste, color of indicators, how it feels, reaction with acids and electrical conductivity)
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CHM.5.3.04.001.03 Differentiate among acidic, basic and neutral solutions (in terms of the relative amounts of hydrogen ions and hydroxide ions)
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CHM.5.3.04.001.04 Identify the color change of different indicators (phenolphthalein, methyl orange, Litmus paper) in acidic, basic and neutral mediums
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CHM.5.3.04.001.05 Perform an experiment to investigate the color of different indicators in neutral, acidic and basic solutions
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CHM.5.3.04.001.06 Compare between binary acids and oxyacids; while writing the chemical name and chemical formula of some common binary acids and oxyacids
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CHM.5.1.01.012Use the periodic table and a list of some common polyatomic ions in writing ionic compounds, molecular compounds, hydrates and some acids chemical formulasCHM.5.1.01.012.02 Write the chemical name and chemical formula of some acids commonly used in industry and the laboratory
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CHM.5.1.01.012.03 Write the chemical name and chemical formula of some common bases
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CHM.5.3.04.001Differentiate between acids and bases based on Arrhenius, Brønsted-Lowery and Lewis theoriesCHM.5.3.04.001.07 Use the Arrhenius model to write the conceptual definition of acids and bases (Examples, particulate models, space-filling models and ionization equations are required)
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CHM.5.3.04.001.08 Define acids and bases according to Brønsted-Lowry theory, indicating the acid, base, conjugate acid, conjugate base and conjugate acid-base pairs, when chemical equations, formula or space-filling models are given
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CHM.5.3.04.001.09 Describe the amphoteric behavior of water, H2O, and ammonia, NH3 (Using chemical equation, particulate diagram and space-filling models)
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CHM.5.3.04.001.10 Distinguish among monoprotic, diprotic and triprotic acids using ionization equations, examples and particulate diagrams
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CHM.5.3.04.001.11 Define acids and bases according to Lewis theory
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CHM.5.3.04.001.12 Explain why many Lewis acids and bases are not classified as Arrhenius or Brønsted-Lowry acids and bases
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L2Strengths of acids and basesCHM.5.3.04.003Compare between the properties of strong and weak acids and bases using the concept of dynamic equilibriumCHM.5.3.04.003.01 Compare between strong and weak acids (using examples, particulate diagrams and ionization equations)
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CHM.5.3.04.006Express the common equilibrium constants of weak acids and bases (Ka, Kb) CHM.5.3.04.006.01 Define acid ionization constant, Ka, while writing the ionization constant expression for different weak acids
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CHM.5.3.04.003Compare between the properties of strong and weak acids and bases using the concept of dynamic equilibriumCHM.5.3.04.003.02 Relate the strength of weak acids to the numerical values of Ka
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CHM.5.3.04.003.03 Compare between strong and weak bases (using examples, particulate diagrams and ionization equations)
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CHM.5.3.04.003.04 Identify the relationship between the strength of an acid and its conjugate base and the strength of a base and its conjugate acid
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CHM.5.3.04.006Express the common equilibrium constants of weak acids and bases (Ka, Kb) CHM.5.3.04.006.02 Define base ionization constant, Kb, while writing the ionization constant expression of different weak bases
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CHM.5.3.04.003Compare between the properties of strong and weak acids and bases using the concept of dynamic equilibriumCHM.5.3.04.003.05 Relate the strength of weak bases to the numerical values of Kb
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L3Hydrogen Ions & pHCHM.5.3.04.005Explain the concept of pH and ionization water constant (Kw)CHM.5.3.04.005.01 Define the ion-product constant for water, Kw, while writing its expression and value at 25℃
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CHM.5.3.04.007Use the ionization constant of water (KW) to calculate pOH, pH, [H3O+] and [OH-] in the aqueous solutionCHM.5.3.04.007.01 Use Kw to calculate the hydronium ion and hydroxide ion concentration at a given temperature and vice versa
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CHM.5.3.04.005Explain the concept of pH and ionization water constant (Kw)CHM.5.3.04.005.03 Define pH and write its mathematical formula
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CHM.5.3.04.005.04 Know what the pH scale is
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CHM.5.3.04.005.05 Define pOH and write its mathematical formula
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CHM.5.3.04.007Use the ionization constant of water (KW) to calculate pOH, pH, [H3O+] and [OH-] in the aqueous solutionCHM.5.3.04.007.02 Describe the relation between pH and pOH and perform calculations involving this relation
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CHM.5.3.04.006Express the common equilibrium constants of weak acids and bases (Ka, Kb) CHM.5.3.04.006.03 Relate the acidity and basicity of an aqueous solution to the hydronium and hydroxide ion concentration and pH at 25oC or 298 K
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CHM.5.3.04.007Use the ionization constant of water (KW) to calculate pOH, pH, [H3O+] and [OH-] in the aqueous solutionCHM.5.3.04.007.03 Calculate pH of a solution when the [H+] or [OH‒] is given and vice versa
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CHM.5.3.04.007.04 Calculate pOH when the [H+] or [OH⁻] is given and vice versa
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CHM.5.3.04.007.05 Calculate the pH and pOH from [OH‒]
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CHM.5.3.04.007.06 Calculate [H+] and [OH⁻] from pH
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CHM.5.3.04.007.07 Calculate the pH of a strong acid given its concentration
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CHM.5.3.04.007.08 Calculate the pH of a strong base given its concentration
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CHM.5.3.04.006Express the common equilibrium constants of weak acids and bases (Ka, Kb) CHM.5.3.04.006.04 Calculate the acid dissociation constant, Ka, given acid concentration, [H+] and pH
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CHM.5.3.04.006.05 Calculate the base dissociation constant, Kb, given acid concentration, [OH-] and pH
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CHM.5.3.04.005Explain the concept of pH and ionization water constant (Kw)CHM.5.3.04.005.07 List different methods used to measure the pH of a solution
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CHM.5.3.04.007Use the ionization constant of water (KW) to calculate pOH, pH, [H3O+] and [OH-] in the aqueous solutionCHM.5.3.04.007.09 Perform an experiment to investigate the pH of different solutions
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CHM.5.3.04.006Express the common equilibrium constants of weak acids and bases (Ka, Kb) CHM.5.3.04.006.06 Express the equilibrium constant (Keq) of a reaction between an acid and a base while calcualting its value
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L4NeutralizationCHM.5.3.04.004Calculate the concentration of the acid or base in a solution using the acid-base titration techniqueCHM.5.3.04.004.01 Define neutralization reaction while writing the neutralization equation (Complete ionic and net ionic equations)
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CHM.5.3.04.004.02 Define titration, and titrant
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CHM.5.3.04.004.03 Explain how to carry out an acid-base titration
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CHM.5.3.04.004.04 Explain the difference between the equivalence point and the end point of titration process
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CHM.5.3.04.009Solve problems related to acid-base equilibrium, using acid-base titration data and the pH at the equivalence pointCHM.5.3.04.009.01 Describe the titration curve of a strong acid with a strong base with respect to type of salt formed, pH and nature of solution at equivalence point, indicator used and its color change and volume of titrant needed for changing color of indicator
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CHM.5.3.04.009.02 Describe the titration curve of a weak acid with a strong base with respect to type of salt formed, pH and nature of solution at equivalence point, indicator used and its color change and volume of titrant needed for changing color of indicator
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CHM.5.3.04.004Calculate the concentration of the acid or base in a solution using the acid-base titration techniqueCHM.5.3.04.004.05 Define acid-base indicator and its function
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CHM.5.3.04.009Solve problems related to acid-base equilibrium, using acid-base titration data and the pH at the equivalence pointCHM.5.3.04.009.03 Perform a titration experiment
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CHM.5.3.04.004Calculate the concentration of the acid or base in a solution using the acid-base titration techniqueCHM.5.3.04.004.06 Calculate the molarity (concentration) and volume of a solution using titration data
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CHM.5.3.04.022Investigate the types of a solution obtained from salt hydrolysis while determining the concentration of its componentsCHM.5.3.04.022.01 Define salt and salt hydrolysis
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CHM.5.3.04.022.02 Identify the type of salt (acidic, basic or neutral) and its constituent acid and base with their strengths
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CHM.5.3.04.010Describe the chemical properties of the buffer solutions and their applicationsCHM.5.3.04.010.01 Define buffer while identifying its importance to the human body
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CHM.5.3.04.010.02 Describe the composition of buffer while explaining how it works
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CHM.5.3.04.010.03 Explain, using equations, what happens when a strong acid is added to a buffered solution (example HX/X⁻) and the change the occurs to the pH
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CHM.5.3.04.010.04 Explain, using equation, what happens when a strong base is added to a buffered solution (example HX/X⁻) and the change the occurs to the pH
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CHM.5.3.04.010.05 Explain what is meant by buffer capacity
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CHM.5.3.04.010.06 Explain the factors that influence the effectiveness of a buffer
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U4Oxidation and reduction reactionsChapter 5 / Module 18Redox ReactionsL1Oxidation & ReductionRefer to the teacher edition of the book
Supplement with digital resources found on LMS such as Al Madrasa, Boclips, Lernatic, Edushare, ALEKS

Please refer to scope and sequence document on LMS where the lessons to be covered had been identified with their type of learning		CHM.5.3.05.001Investigate the oxidation and reduction processes (Redox), while writing chemical equations for each and determining the oxidizing and reducing agentsCHM.5.3.05.001.01 Distinguish between oxidation and reduction in terms of loss and gain of electrons, oxygen and hydrogen
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CHM.5.3.05.001.02 Define oxidation number
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CHM.5.3.05.001.03 Assign oxidation number to atoms, ions and compounds according to a set of rules
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CHM.5.3.05.001.04 Distinguish between oxidation and reduction in terms of change in oxidation number
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CHM.5.3.05.001.05 Define redox reaction while explaining what must be conserved in a redox reaction
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CHM.5.3.05.001.06 Identify a redox reaction from a given list of reactions while indicating the oxidized and reduced species
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CHM.5.3.05.001.07 Define oxidizing agent and reducing agent in a redox reaction
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CHM.5.3.05.001.08 Identify oxidizing agent and reducing agent in a redox reaction
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CHM.5.3.05.001.09 Define half-reaction, oxidation half-reaction and reduction-half reaction
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CHM.5.3.05.001.10 Write oxidation-half reaction and reduction-half reaction for a redox reaction
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CHM.5.3.05.003Investigate the spontaneity of redox reactions based on the activity series, reduction potential and electronegativityCHM.5.3.05.003.01 Describe the role of electronegativity in redox reactions
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CHM.5.3.05.003.02 Identify the most powerful reducing and oxidizing agents based on electronegativity
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CHM.5.3.05.003.03 Describe the relationship between electronegativity, the oxidation potential and reduction potential of elements
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CHM.5.3.05.003.04 Build the activity series according to the reduction potential of elements
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CHM.5.3.05.003.05 Explain the occurrence of redox reactions based on the activity of the different metals
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CHM.5.3.05.003.06 Predict the occurrence of redox reactions based on the relationship between electronegativity and the reduction potential of elements
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CHM.5.3.05.003.07 Analyse experimental  results to build  part of the activity series
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L2Balancing Redox ReactionsCHM.5.3.05.002Balance redox equationsCHM.5.3.05.002.01 Describe the steps for balancing redox reactions, in acidic medium, by the half-reaction method
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CHM.5.3.05.002.03 Balance redox reaction in acidic medium using half-reaction method
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CHM.5.3.05.002.04 Describe the steps for balancing redox reactions, in basic medium, by the half-reaction method
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CHM.5.3.05.002.05 Balance redox reaction in basic medium using half-reaction method
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CHM.5.3.05.002.06 Describe the balancing of redox reaction using the change in oxidation number method
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CHM.5.3.05.002.07 Balance redox equations using the change in oxidation number method.
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Chapter 6 / Module 19ElectrochemistryL1Voltaic CellsCHM.5.3.05.004Investigate the conditions in which a galvanic cell can be produced while illustrating the effect of the reduction potential of electrodes on the electrons flow, cell potential and energyCHM.5.3.05.004.01 Define electrochemistry
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CHM.5.3.05.007Build a galvanic cell, while illustrating the function of its components and the chemical reactions that can occur to calculate its electromotive force (e.m.f)CHM.5.3.05.007.01 Describe an electrochemical cell while specifying its types
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CHM.5.3.05.007.02 Identify components of a voltaic or galvanic cell (anode, cathode, salt bridge or porous barrier, wires, electrolyte compartments); while explaining the role of each component, when does the reaction start and determining the direction of electron and current flow
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CHM.5.3.05.007.03 Write the oxidation and reduction half-reactions occurring at cathode and anode for a voltaic cell
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CHM.5.3.05.004Investigate the conditions in which a galvanic cell can be produced while illustrating the effect of the reduction potential of electrodes on the electrons flow, cell potential and energyCHM.5.3.05.004.02 Describe standard hydrogen electrode (SHE), while identifying the importance of its E° value and writing the half-cell reactions of the two possible reactions that could occur at the hydrogen electrode
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CHM.5.3.05.004.03 Define the reduction potential and standard electrode potential (E°)
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CHM.5.3.05.004.06 Define electrode potential
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CHM.5.3.05.007Build a galvanic cell, while illustrating the function of its components and the chemical reactions that can occur to calculate its electromotive force (e.m.f)CHM.5.3.05.007.04 Write the cell notation and the overall chemical equation for a redox reaction occurring in a voltaic cell
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CHM.5.3.05.007.05 Use the half-cell standard reduction potentials to calculate the electrochemical cell standard potential, while determining whether the redox reactions are spontaneous or non-spontaneous
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CHM.5.3.05.008Predict the occurrence of redox reactions in electrochemical cells through the standard reduction potential valuesCHM.5.3.05.008.01 Use the standard reduction potentials to predict if a reaction occurs or not, while identifying the strongest reducing or oxidizing agent and the substance that is easily oxidized or reduced
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CHM.5.3.05.017Investigate the changes that happen in Voltaic cells during the electrochemical reaction in terms of number of moles, mass, concentration, number of electrons, charges and current, electrons and ions movement.CHM.5.3.05.017.01 Perform an experiment to investigate voltaic cell
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CHM.5.3.05.017.02 Interpret the movement of the ions between the half-cells solutions in an electrochemical cell
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CHM.5.3.05.017.03 Interpret the change in the ion concentration in the half cells solutions during the function of an electrochemical cell
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CHM.5.3.05.017.04 Interpret the change in the mass of the electrodes during the function of an electrochemical cell
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CHM.5.3.05.017.05 Interpret the electron transfer in an electrochemical cell
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CHM.5.3.05.017.06 Interpret the results of a redox titration
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CHM.5.3.05.017.07 Explain the results from the deviation from the standard cell conditions and changes in the cell potential