MSJChem - Tutorial videos for IB Chemistry
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  • Videos (first exams 2025)
    • Structure 1.1 Models of the particulate nature of matter
    • Structure 1.2 The nuclear atom >
      • Structure 1.2 HL The nuclear atom
    • Structure 1.3 Electron configurations >
      • Structure 1.3 Electron configurations HL
    • Structure 1.4 Counting particles by mass: The mole
    • Structure 1.5 Ideal gases
    • Structure 2.1 The ionic model
    • Structure 2.2 The covalent model >
      • Structure 2.2 The covalent model (HL)
    • Structure 2.3 The metallic model
    • Structure 2.4 From models to materials
    • Structure 3.1 The periodic table : Classification of elements >
      • Structure 3.1 The periodic table: Classification of elements (HL)
    • Structure 3.2 Functional groups: Classification of organic compounds >
      • Structure 3.2 Functional groups: Classification of organic compounds (HL)
    • Reactivity 1.1 Measuring enthalpy changes
    • Reactivity 1.2 Energy cycles in reactions >
      • Reactivity 1.2 Energy cycles in reactions (HL)
    • Reactivity 1.3 Energy from fuels
    • Reactivity 1.4 Entropy and spontaneity (HL)
    • Reactivity 2.1 How much? The amount of chemical change
    • Reactivity 2.2 How fast? The rate of chemical change >
      • Reactivity 2.2 How fast? The rate of chemical change (HL)
    • Reactivity 2.3 How far? The extent of chemical change >
      • Topic 6 Kinetics
      • Topic 7 Equilibrium
      • Topic 8 Acids and bases
      • Topic 9 Oxidation and reduction
      • Topic 10 Organic chemistry
      • Topic 11 Measurement and data processing
      • Topic 12 Atomic structure HL
      • Topic 13 Periodicity HL
      • Topic 14 Bonding HL
      • Topic 15 Energetics HL
      • Topic 16 Kinetics HL
      • Topic 17 Equilibrium HL
      • Topic 18 Acids and bases HL
      • Topic 19 Redox HL
      • Topic 20 Organic chemistry HL
      • Options (last exams 2024) >
        • SL Option A
        • HL Option A
        • SL Option B
        • HL Option B
        • SL Option C
        • HL Option C
        • SL Option D
        • HL Option D >
          • Exam review (last exams 2024)
      • Reactivity 2.3 How far? The extent of chemical change (HL)
    • Reactivity 3.1 Proton transfer reactions >
      • Reactivity 3.1 Proton transfer reactions (HL)
    • Reactivity 3.2 Electron transfer reactions >
      • Reactivity 3.2 Electron transfer reactions (HL)
    • Reactivity 3.3 Electron sharing reactions
    • Reactivity 3.4 Electron-pair sharing reactions >
      • Reactivity 3.4 Electron-pair sharing reactions (HL)
Picture


Reactivity 3.1 Proton transfer reactions
Reactivity 3.1.1
Understandings: 
  • ​Brønsted–Lowry acid is a proton donor and a Brønsted–Lowry base is a proton acceptor. 
Learning outcomes:
  • Deduce the Brønsted–Lowry acid and base in a reaction.
Additional notes:
  • A proton in aqueous solution can be represented as both H+(aq) and H3O+(aq). The distinction between the terms “base” and “alkali” should be understood.
Picture
This video covers Brønsted–Lowry acids and bases. 

Reactivity 3.1.2
Understandings: 
  • A pair of species differing by a single proton is called a conjugate acid–base pair.
Learning outcomes:
  • Deduce the Brønsted–Lowry acid and base in a reaction.
Linking question(s):
  • Structure 2.1 What are the conjugate acids of the polyatomic anions listed in Structure 2.1?
Picture
This video covers conjugate acid-bases pairs.

Reactivity 3.1.3
Understandings: 
  • Some species can act as both Brønsted–Lowry acids and bases.
Learning outcomes:
  • Interpret and formulate equations to show acid–base reactions of these species.
Linking question(s):
  • Structure 3.1 What is the periodic trend in the acid–base properties of metal and non-metal oxides?
  • Structure 3.1 Why does the release of oxides of nitrogen and sulfur into the atmosphere cause acid rain?
Picture
This video covers amphiprotic species. 

Reactivity 3.1.4
Understandings: 
  • The pH scale can be used to describe the [H+] of a solution: pH = –log10[H+]; [H+] = 10–pH
Learning outcomes:
  • Perform calculations involving the logarithmic relationship between pH and [H+].
Additional information:
  • Include the estimation of pH using universal indicator, and the precise measurement of pH using a pH meter/probe.
  • The equations for pH are given in the data booklet.​
Picture
This video covers the pH scale. 

Reactivity 3.1.5
Understandings: 
  • The ion product constant of water, Kw, shows an inverse relationship between [H+] and [OH–]. Kw = [H+] [OH–]
Learning outcomes:
  • Recognize solutions as acidic, neutral and basic from the relative values of [H+] and [OH–].
Additional information:
  • The equation for Kw and its value at 298 K are given in the data booklet.
Linking question(s):
  • Reactivity 2.3 Why does the extent of ionization of water increase as temperature increases?
Picture
This video covers the ionic product constant of water, Kw. 

Reactivity 3.1.6
Understandings: 
  • Strong and weak acids and bases differ in the extent of ionisation.
Learning outcomes:
  • Recognise that acid–base equilibria lie in the direction of the weaker conjugate.
Additional information:
  • HCl, HBr, HI, H2SO4 and HCl are strong acids, and group 1 hydroxides are strong bases.
  • The distinction between strong and weak acids or bases and concentrated and dilute reagents should be covered.
Linking question(s):
  • Reactivity 2.3 How would you expect the equilibrium constants of strong and weak acids to compare?
  • Reactivity 1.1 Why does the acid strength of the hydrogen halides increase down group 17?
Picture
This video covers strong and weak acids and bases. 
Picture
This video covers how to distinguish between strong and weak acids and bases. 

Reactivity 3.1.7
Understandings: 
  • Acids react with bases in neutralisation reactions.
Learning outcomes:
  • Formulate equations for the reactions between acids and metal oxides, metal hydroxides, hydrogencarbonates and carbonates.
Additional information:
  • Identify the parent acid and base of different salts.
  • Bases should include ammonia, amines, soluble carbonates and hydrogencarbonates; acids should include organic acids.
Linking question(s):
  • Reactivity 1.1 Neutralisation reactions are exothermic. How can this be explained in terms of bond enthalpies?
  • Reactivity 3.2 How could we classify the reaction that occurs when hydrogen gas is released from the reaction between an acid and a metal?
Picture
This video covers the reactions of acids and bases. 

Reactivity 3.1.8
Understandings: 
  • pH curves for neutralization reactions involving strong acids and bases have characteristic shapes and features.
Learning outcomes:
  • Sketch and interpret the general shape of the pH curve.
Additional information:
  • Interpretation should include the intercept with the pH axis and equivalence point.
  • Only monoprotic neutralization reactions will be assessed.
Linking question(s):
  • Structure 1.4 Why is the equivalence point sometimes referred to as the stoichiometric point?
Video coming soon. 

  • Home
    • About
    • Blog
    • Online tutoring
    • Privacy policy
  • Member's Area
  • Videos (first exams 2025)
    • Structure 1.1 Models of the particulate nature of matter
    • Structure 1.2 The nuclear atom >
      • Structure 1.2 HL The nuclear atom
    • Structure 1.3 Electron configurations >
      • Structure 1.3 Electron configurations HL
    • Structure 1.4 Counting particles by mass: The mole
    • Structure 1.5 Ideal gases
    • Structure 2.1 The ionic model
    • Structure 2.2 The covalent model >
      • Structure 2.2 The covalent model (HL)
    • Structure 2.3 The metallic model
    • Structure 2.4 From models to materials
    • Structure 3.1 The periodic table : Classification of elements >
      • Structure 3.1 The periodic table: Classification of elements (HL)
    • Structure 3.2 Functional groups: Classification of organic compounds >
      • Structure 3.2 Functional groups: Classification of organic compounds (HL)
    • Reactivity 1.1 Measuring enthalpy changes
    • Reactivity 1.2 Energy cycles in reactions >
      • Reactivity 1.2 Energy cycles in reactions (HL)
    • Reactivity 1.3 Energy from fuels
    • Reactivity 1.4 Entropy and spontaneity (HL)
    • Reactivity 2.1 How much? The amount of chemical change
    • Reactivity 2.2 How fast? The rate of chemical change >
      • Reactivity 2.2 How fast? The rate of chemical change (HL)
    • Reactivity 2.3 How far? The extent of chemical change >
      • Topic 6 Kinetics
      • Topic 7 Equilibrium
      • Topic 8 Acids and bases
      • Topic 9 Oxidation and reduction
      • Topic 10 Organic chemistry
      • Topic 11 Measurement and data processing
      • Topic 12 Atomic structure HL
      • Topic 13 Periodicity HL
      • Topic 14 Bonding HL
      • Topic 15 Energetics HL
      • Topic 16 Kinetics HL
      • Topic 17 Equilibrium HL
      • Topic 18 Acids and bases HL
      • Topic 19 Redox HL
      • Topic 20 Organic chemistry HL
      • Options (last exams 2024) >
        • SL Option A
        • HL Option A
        • SL Option B
        • HL Option B
        • SL Option C
        • HL Option C
        • SL Option D
        • HL Option D >
          • Exam review (last exams 2024)
      • Reactivity 2.3 How far? The extent of chemical change (HL)
    • Reactivity 3.1 Proton transfer reactions >
      • Reactivity 3.1 Proton transfer reactions (HL)
    • Reactivity 3.2 Electron transfer reactions >
      • Reactivity 3.2 Electron transfer reactions (HL)
    • Reactivity 3.3 Electron sharing reactions
    • Reactivity 3.4 Electron-pair sharing reactions >
      • Reactivity 3.4 Electron-pair sharing reactions (HL)