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SubjectGradeStreamElective ScenarioTermWeek Unit NumberUnit NameChapter / Module NumberChapter NameSection / Lesson NumberSection / Lesson NameNumber of Periods
(per chapter)		Vocabulary / Key WordsResources
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SLOs CodesStudent Learning Outcomes (S.L.Os)SLOs PriorityKey Performance CriteriaComments
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Chemistry12AdvancedScenario ETerm 2Weeks 1 to 2U3Matter, Energy, and equilibriumChapter 3 / Module 16Chemical EquilibriumL3Using Equilibrium Constants4 periodsRefer 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.5.4.02.006Solve problems related to equilibrium by performing calculations involving concentrations of reactants and productsPower OutcomeCHM.5.4.02.006.03 Calculate the equilibrium concentration given the value of the equilibrium constant and equilibrium concentration of reactants and productsDirect learning: Calculating Equilibrium Concentration, Writing solubility product constant expressions, using solubility product constants
Enrichment: Predicting precipiate, calculating ion concentrations, The common ion Effet
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CHM.5.4.02.006.04 Calculate the value of Keq, Kc, or Kp when the concentration or pressure of reactants and products are given at a constant temperature
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CHM.5.4.02.007Describe the concept of the solubility product constant (Ksp),while expressing it by a mathematical formulaSupport Outcome (Basic) CHM.5.4.02.007.01 Explain what is meant by solubility product constant of a substance and what is describes
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CHM.5.4.02.007.02 Write the solubility equilibrium expression for a given reaction equilibrium
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CHM.5.4.02.007.03 Write the solubility for a given reaction equilibrium
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CHM.5.4.02.008Solve problems related to the concept of solubility product constant (Ksp)Power OutcomeCHM.5.4.02.008.01 Calculate the molar solubility (concentration) of a sparingly soluble ionic compound using the solubility product constant, Ksp
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CHM.5.4.02.008.02 Explain the difference between Ksp and Qsp
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CHM.5.4.02.008.03 Describe the relation between Ksp and Qsp
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CHM.5.4.02.008.04 Identify whether a precipitate will form or not (by calculation and using relation between Ksp and Qsp)
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CHM.5.4.02.008.05 Perform and conduct a practical experiment to determine the Ksp of calcium hydroxide
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CHM.5.4.02.009Investigate some applications of the solubility product constant in industry, pollution treatment and environment protection Support Outcome (Supplementary)CHM.5.4.02.009.01 Describe some applications of the solubility product constant in water treatment
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CHM.5.4.02.009.02 Describe some applications of the solubility product constant in soil treatment
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CHM.5.4.02.009.03 Describe some applications of the solubility product constant in waste treatment
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CHM.5.4.02.009.04 Describe some applications of the solubility product constant in metallic ions precipitation
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CHM.5.4.02.010Conduct practical investigation (considering safety rules) to find the value of equilibrium constant for a chemical reactionSupport Outcome (Basic) CHM.5.4.02.010.01 Determine throught a lab experiment the equilibrium constant value of a chemical reaction
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CHM.5.4.02.010.02 Determine throught a lab experiment the products concentrations and Ksp value of a chemical reaction
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CHM.5.4.02.010.03 Determine throught a lab experiment the Ksp value in a chemical reaction or mixture
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CHM.5.4.02.010.04 Determine throught a lab experiment the Qsp value in a chemical reaction or mixture
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CHM.5.4.02.011Assess the impact of chemical equilibrium processes on various biological, biochemical, and technological systems Support Outcome (Supplementary)CHM.5.4.02.011.01 Investigate some reversible chemical reactions that can occur in the human body showing their importance in maintaining the integrity of vital systems
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CHM.5.4.02.011.02 Explore the application of the solubility product constant in medical and pharmacological fields
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CHM.5.4.02.011.03 Explore the application of the solubility product constant in radiology while exploring its effects on human vital systems
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Week 2 to 6U3Matter, Energy, and equilibriumChapter 4 / Module 17Acids and BasesL1Introduction to acids and bases12 periodsRefer 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 theoriesSupport Outcome (Basic)CHM.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)Direct learning
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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 formulasSupport Outcome (Basic)CHM.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 theoriesSupport Outcome (Basic)CHM.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 equilibriumPower OutcomeCHM.5.3.04.003.01 Compare between strong and weak acids (using examples, particulate diagrams and ionization equations)Direct learning
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CHM.5.3.04.006Express the common equilibrium constants of weak acids and bases (Ka, Kb) Support Outcome (Basic)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 equilibriumPower OutcomeCHM.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) Support Outcome (Basic)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 equilibriumPower OutcomeCHM.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)Support Outcome (Basic)CHM.5.3.04.005.01 Define the ion-product constant for water, Kw, while writing its expression and value at 25℃Direct learning
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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 solutionPower OutcomeCHM.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)Support Outcome (Basic)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 solutionPower OutcomeCHM.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) Support Outcome (Basic)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 solutionPower OutcomeCHM.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) Support Outcome (Basic)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)Support Outcome (Basic)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 solutionPower OutcomeCHM.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) Support Outcome (Basic)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 techniquePower OutcomeCHM.5.3.04.004.01 Define neutralization reaction while writing the neutralization equation (Complete ionic and net ionic equations)Direct learning: Reactions between acids and bases
Self learning (experiment +applications)
Enrichment (Salt Hydrolysis)
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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 pointPower OutcomeCHM.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 techniquePower OutcomeCHM.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 pointPower OutcomeCHM.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 techniquePower OutcomeCHM.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 componentsPower OutcomeCHM.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 applicationsPower OutcomeCHM.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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Week 6 to 7U4Oxidation and reduction reactionsChapter 5 / Module 18Redox ReactionsL1Oxidation & Reduction5 periodsRefer 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 agentsPower OutcomeCHM.5.3.05.001.01 Distinguish between oxidation and reduction in terms of loss and gain of electrons, oxygen and hydrogenDirect learning
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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 electronegativityPower OutcomeCHM.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 equationsPower OutcomeCHM.5.3.05.002.01 Describe the steps for balancing redox reactions, in acidic medium, by the half-reaction methodDirect learning : Balancing Net Ionic Redox Equations, Balancing redox equations using Half reactions
Enrichment: Oxidation number 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