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 3.1 The periodic table: Classification of elements
Structure 3.1.1 and 3.2.2
Understandings:
  • The periodic table consists of periods, groups and blocks (3.1.1).
  • The period number shows the outer energy level that is occupied by electrons. Elements in a group have a common number of valence electrons (3.2.2).
Learning outcomes:
  • Identify the positions of metals, metalloids and non-metals in the periodic table (3.1.1).
  • Deduce the electron configuration of an atom up to Z = 36 from the element’s position in the periodic table and vice versa (3.2.2).
Additional notes:
  • The four blocks associated with the sublevels s, p, d, f should be recognized.
  • A copy of the periodic table is available in the data booklet.​
  • Groups are numbered from 1 to 18.
  • The classifications “alkali metals”, “halogens”, “transition elements” and “noble gases” should be known.
Linking question(s):
  • Structure 1.2 How has the organization of elements in the periodic table facilitated the discovery of new elements?
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This video covers groups, periods and the names of the groups. 
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This video covers the blocks of the periodic table and electron configurations. 
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This video covers the properties of metals and non-metals. 

This video covers the metalloids. 

Structure 3.1.3
Understandings:
  • Periodicity refers to trends in properties of elements across a period and down a group.
Learning outcomes:
  • Explain the periodicity of atomic radius, ionic radius, ionization energy, electron affinity and electronegativity.​
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This video covers electron shielding and effective nuclear charge.
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This video covers atomic radius.
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This video covers ionic radius.
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This video covers ionisation energy.
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This video covers electron affinity.
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This video covers electronegativity.

Structure 3.1.4
Understandings:
  • Trends in properties of elements down a group include the increasing metallic character of group 1 elements and decreasing non-metallic character of group 17 elements.
Learning outcomes:
  • Describe and explain the reactions of group 1 metals with water, and of group 17 elements with halide ions.​
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This video covers metallic character.
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This video covers the group 1 metals. 
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This video covers the group 17 elements. 

Structure 3.1.5
Understandings:
  • Metallic and non-metallic properties show a continuum. This includes the trend from basic metal oxides through amphoteric to acidic non-metal oxides.
Learning outcomes:
  • Deduce equations for the reactions with water of the oxides of group 1 and group 2 metals, carbon and sulfur.
Additional notes:
  • Include acid rain caused by gaseous non-metal oxides, and ocean acidification caused by increasing CO2 levels.
Linking questions:
  • Structure 2.1, 2.2 How do differences in bonding explain the differences in the properties of metal and non-metal oxides?
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This video covers the acid-base properties of the period 3 oxides. 
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This video covers acid deposition (acid rain). 
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This video covers ocean acidification. 

Structure 3.1.6
Understandings:
  • The oxidation state is a number assigned to an atom to show the number of electrons transferred in forming a bond. It is the charge that atom would have if the compound were composed of ions.
Learning outcomes:
  • Deduce the oxidation states of an atom in an ion or a compound.
  • Explain why the oxidation state of an element is zero.
Additional notes:
  • Oxidation states are shown with a + or – sign followed by the Arabic symbol for the number, e.g. +2, –1.
  • Examples should include hydrogen in metal hydrides (–1) and oxygen in peroxides (–1).
  • The terms “oxidation number” and “oxidation state” are often used interchangeably, and either term is acceptable in assessment.
  • Naming conventions for oxyanions use oxidation numbers shown with Roman numerals, but generic names persist and are acceptable. Examples include nitrate, nitrite, sulfate, sulfite.
Linking questions:
  • Reactivity 3.2 How can oxidation states be used to analyse redox reactions?
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This video covers how to determine oxidation states. 

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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)