MSJChem - Tutorial videos for IB Chemistry
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    • 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
    • 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
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Topic 4 Bonding 

4.1 The octet rule
Understandings:
The “octet rule” refers to the tendency of atoms to gain a valence shell with a total of 8 electrons.
Some atoms, like Be and B, might form stable compounds with incomplete octets of electrons.

4.1 Electronegativity and bonding 
This video covers the relationship between the difference in electronegativity between atoms and the type of bonding. 
Understandings: 
Bond polarity results from the difference in electronegativities  of the bonded atoms.

4.1 Ions and ion formation 
Understandings:
Positive ions (cations) form by metals losing valence electrons.
Negative ions (anions) form by non-metals gaining electrons.
The number of electrons lost or gained is determined by the electron configuration of the atom.

Formation of ions worksheet 
Ion sheet - contains every positive and negative ion you're ever likely to need in IB chemistry 


4.1 Ionic bonding 
Understandings:
The ionic bond is due to electrostatic attraction between oppositely charged ions.
Under normal conditions, ionic compounds are usually solids with lattice structures.

topic_4_ionic_bonding.pdf
File Size: 199 kb
File Type: pdf
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4.1 Structure and properties of ionic compounds 
Applications and skills:
Explanation of the physical properties of ionic compounds (volatility, electrical conductivity and solubility) in terms of their structure.





4.1 Writing formulae of ionic compounds 
This video covers how to write formulae for ionic compounds. 



Writing formulae worksheet

4.1 Polyatomic ions 
Applications and skills:
​Deduction of the formula and name of an ionic compound from its component ions, including polyatomic ions.
Guidance:
Students should be familiar with the following polyatomic ions: NH4+ OH- HCO3- CO32- SO42- PO43- NO3-

4.2 Covalent bonding 
Understandings:
A covalent bond is formed by the electrostatic attraction between a shared pair of electrons and the positively charged nuclei.
Bond polarity results from the difference in electronegativities  of the bonded atoms.
Single, double and triple covalent bonds involve one, two and three shared pairs of electrons respectively.

Bond length decreases and bond strength increases as the number of shared electrons increases.
Applications and skills:
Deduction of the polar nature of a covalent bond from electronegativity values.
topic_4_covalent_bonding.pdf
File Size: 209 kb
File Type: pdf
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topic_4_bond_polarity.pdf
File Size: 201 kb
File Type: pdf
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4.2 Polar and non-polar covalent bonds 
Understandings:
Bond polarity results from the difference in electronegativities  of the bonded atoms.
Applications and skills:

Applications and skills:
Deduction of the polar nature of a covalent bond from electronegativity values.


4.2 Coordinate covalent bonds
Guidance:
Coordinate covalent bonds should be covered

4.2 Polar and non-polar molecules 
Applications and skills:
Prediction of molecular polarity from bond polarity and molecular geometry.
topic_4_polar_and_non-polar_molecules.pdf
File Size: 188 kb
File Type: pdf
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4.3 Lewis structures 
Understandings:
Lewis (electron dot) structures show all the valence electrons in a covalently bonded species.
The “octet rule” refers to the tendency of atoms to gain a valence shell with a total of 8 electrons.
Some atoms, like Be and B, might form stable compounds with incomplete octets of electrons.

Applications and skills:
Deduction of Lewis (electron dot) structure of molecules and ions showing all valence electrons for up to four electron pairs on each atom.
topic_4_lewis_structures.pdf
File Size: 349 kb
File Type: pdf
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4.3 VSEPR theory (molecular geometry) 
Understandings:
Shapes of species are determined by the repulsion of electron pairs according to VSEPR theory.
Applications and skills:
Deduction of Lewis (electron dot) structure of molecules and ions showing all valence electrons for up to four electron pairs on each atom.
The use of VSEPR theory to predict the electron domain geometry and the molecular geometry for species with two, three and four electron domains.
Prediction of bond angles from molecular geometry and presence of non- bonding pairs of electrons.

SL molecular geometries summary sheet 

4.3 Structure and properties of covalent compounds 
 Understandings:
Carbon and silicon form giant covalent/network covalent structures.
Application and skills:
Explanation of the properties of giant covalent compounds in terms of their structures.
Explanation of the physical properties of covalent compounds (volatility, electrical conductivity and solubility) in terms of their structure and intermolecular forces.
topic_4_structure_and_properties_of_covalent_compounds.pdf
File Size: 214 kb
File Type: pdf
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4.3 Allotropes of carbon 
Guidance:
Allotropes of carbon (diamond, graphite, graphene, C60 buckminsterfullerene)  should be covered.

4.3 Resonance structures 
Understandings:
Resonance structures occur when there is more than one possible position for a double bond in a molecule.
Guidance:
Deduction of resonance structures, examples include but are not limited to
C6H6 , CO2- and O3.


Resonance structures worksheet

4.4 Intermolecular forces 
Understandings:
Intermolecular forces include London (dispersion) forces, dipole-dipole forces and hydrogen bonding.
The relative strengths of these interactions are London (dispersion) forces < dipole-dipole forces < hydrogen bonds.
Applications and skills:
Deduction of the types of intermolecular force present in substances, based on their structure and chemical formula.
Note: The term van der Waals forces includes London dispersion forces (instantaneous and induced dipoles) and dipole-dipole forces.
topic_4_intermolecular_forces.pdf
File Size: 197 kb
File Type: pdf
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4.4 Solubility and intermolecular forces 
This video covers polar and non-polar solvents and the different types of intermolecular forces that exist in solutions. 

Bonding and electrcial conductivity 

This video covers the electrical conductivity of substances with different bonding (covalent, ionic and metallic).

4.4 Group 16 hydrides
This video covers the bonding and properties of the group 16 hydrides. 

4.5 Metallic bonding 
Understandings:
A metallic bond is the electrostatic attraction between a lattice of positive ions and delocalized electrons.
The strength of a metallic bond depends on the charge of the ions and the radius of the metal ion.
Applications and skills:
Explanation of electrical conductivity and malleability in metals.
Explanation of trends in melting points of metals.




4.5 Alloys 
Understandings:
Alloys usually contain more than one metal and have enhanced properties.
Applications and skills:
Explanation of the properties of alloys in terms of non-directional  bonding.
Guidance:
Examples of various alloys should be covered.

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  • Home
    • About
    • Blog
    • Online tutoring
    • Privacy policy
  • Member's Area
  • SL Syllabus
    • 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
    • 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
    • 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