MSJChem - Tutorial videos for IB Chemistry
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  • SL Syllabus (last exams 2024)
    • Topic 1 Stoichiometric relationships
    • Topic 2 Atomic structure
    • Topic 3 Periodicity
    • Topic 4 Bonding
    • Topic 5 Energetics
    • 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
  • HL syllabus (last exams 2024)
    • 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
    • Topic 21 Measurement and data processing
  • 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)
  • New syllabus (first exams 2025)
    • Structure 1.1 Models of the particulate nature of matter
    • Structure 1.2 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 >
      • 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)
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Structure 1.4 Counting particles by mass: The mole
Structure 1.4.1
Understandings:
  • The mole (mol) is the SI unit of amount of substance. One mole contains exactly the number of elementary entities given by the Avogadro constant.
Learning outcomes:
  • Convert the amount of substance, n, to the number of specified elementary entities.
Additional notes:
  • An elementary entity may be an atom, a molecule, an ion, an electron, any other particle or a specified group of particles.
  • The Avogadro constant NA is given in the data booklet. It has the units mol–1. ​
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This video covers the mole concept. 

Structure 1.4.2
Understandings:
  • Masses of atoms are compared on a scale relative to 12C and are expressed as relative atomic mass Ar and relative formula mass Mr .
Learning outcomes:
  • Determine relative formula masses Mr from relative atomic masses Ar .
Additional notes:
  • Relative atomic mass and relative formula mass have no units.
  • The values of relative atomic masses given to two decimal places in the data booklet should be used in calculations.
Picture
This video covers relative atomic mass and relative molecular mass / relative formula mass. 
Please note that the IB now uses the term relative formula mass for both molecular and ionic compounds. 

Structure 1.4.3
Understandings:
  • Molar mass M has the units g mol–1
Learning outcomes:
  • Solve problems involving the relationships between the number of particles, the amount of substance in moles and the mass in grams.
Additional notes:
  • The relationship n =  m/M is given in the data booklet.
Picture
This video covers how to calculate the molar mass of a compound. 
Picture
This video covers how to calculate the amount (in mol) of a substance. Using the equation n = CV will be covered later in this section. 
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This video covers how to convert between amount (in mol) and mass (in g). 

Structure 1.4.4
Understandings:
  • The empirical formula of a compound gives the simplest ratio of atoms of each element present in that compound.
  • The molecular formula gives the actual number of atoms of each element present in a molecule.
Learning outcomes:
  • Interconvert the percentage composition by mass and the empirical formula.
  • Determine the molecular formula of a compound from its empirical formula and molar mass.
​
Picture
This video covers how to determine the percent composition by mass of an element in a compound. 
Picture
This video covers empirical and molecular formulas.
Picture
This video covers how to determine an empirical formula from percent composition by mass data. 

Structure 1.4.5
Understandings:
  • The molar concentration is determined by the amount of solute and the volume of solution.
Learning outcomes:
  • Solve problems involving the molar concentration, amount of solute and volume of solution.​
Additional notes:
  • The use of square brackets to represent molar concentration is required.
  • Units of concentration should include g dm–3 and mol dm–3 and conversion between these.
  • The relationship n = CV is given in the data booklet.
Picture
This video covers calculations involving concentrations of solutions. 

Structure 1.4.6
Understandings:
  • Avogadro’s law states that equal volumes of all gases measured under the same conditions of temperature and pressure contain equal numbers of molecules.
Learning outcomes:
  • Solve problems involving the mole ratio of reactants and/or products and the volume of gases.
Picture
This video covers Avogadro's law.

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  • Home
    • About
    • Blog
    • Online tutoring
    • Privacy policy
  • Member's Area
  • SL Syllabus (last exams 2024)
    • Topic 1 Stoichiometric relationships
    • Topic 2 Atomic structure
    • Topic 3 Periodicity
    • Topic 4 Bonding
    • Topic 5 Energetics
    • 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
  • HL syllabus (last exams 2024)
    • 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
    • Topic 21 Measurement and data processing
  • 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)
  • New syllabus (first exams 2025)
    • Structure 1.1 Models of the particulate nature of matter
    • Structure 1.2 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 >
      • 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)