MSJChem - Tutorial videos for IB Chemistry
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  • 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
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Topic 14 Bonding HL

14.1 VSEPR (HL)
Understandings:
Exceptions to the octet rule include some species   having incomplete octets and expanded octets. 
Applications and skills:
Deduction using VSEPR theory of the electron domain geometry and molecular geometry with five and six electron domains and associated bond angles.
Deduction of the Lewis (electron dot) structures of molecules and ions showing all valence electrons for up to six electron pairs on each atom.

14.1 Molecular geometry (HL)
Understandings:
Exceptions to the octet rule include some species    having incomplete octets and expanded octets. 
Applications and skills:
Deduction using VSEPR theory of the electron domain geometry and molecular geometry with five and six electron domains and associated bond angles.
Deduction of the Lewis (electron dot) structures of molecules and ions showing all valence electrons for up to six electron pairs on each atom.
topic_14_vsepr_theory_hl.pdf
File Size: 431 kb
File Type: pdf
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14.1 sigma and pi bonds (new version)
Understandings:
Covalent bonds result from the overlap of atomic orbitals. A sigma bond (σ) is formed by the direct head-on/end-to-end overlap of atomic orbitals, resulting in electron density concentrated between the nuclei of the bonding atoms. A pi bond (π) is formed by the sideways overlap of atomic orbitals, resulting in electron density above and below the plane of the nuclei of the bonding atoms.
Applications and skills:
Prediction whether sigma (σ) or pi (π) bonds
 are formed from the linear combination of atomic orbitals.
topic_4_sigma_and_pi_bonds.pdf
File Size: 231 kb
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14.1 sigma and pi bonds (old version)
Understandings:
Covalent bonds result from the overlap of atomic orbitals. A sigma bond (σ) is formed by the direct head-on/end-to-end overlap of atomic orbitals, resulting in electron density concentrated between the nuclei of the bonding atoms. A pi bond (π) is formed by the sideways overlap of atomic orbitals, resulting in electron density above and below the plane of the nuclei of the bonding atoms.
Applications and skills:
Prediction whether sigma (σ) or pi (π) bonds
are formed from the linear combination of atomic orbitals.

14.1 Formal charge 
Understandings: 
Formal charge (FC) can be used to decide which Lewis (electron dot) structure is preferred from several. The FC is the charge an atom would have if all atoms in the molecule had the same electronegativity. FC = (Number of valence electrons)-½(Number of bonding electrons)-(Number of non-bonding electrons). The Lewis (electron dot) structure with the atoms having FC values closest to zero is preferred.
Applications and skills:
Application of FC to ascertain which Lewis (electron dot) structure is preferred from different Lewis (electron dot) structures.
topic_14_formal_charge.pdf
File Size: 427 kb
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14.1 Molecules and ions with delocalised pi electrons 
Understandings:
Delocalization involves electrons that are shared by/between more than two nuclei. 

Resonance involves using two or more Lewis (electron dot) structures to represent a particular molecule or ion. A resonance structure is one of two or more alternative Lewis (electron dot) structures for a molecule or ion that cannot be described fully with one Lewis (electron dot) structure alone.

14.1 Delocalized pi electrons 
Understandings:
Delocalization involves electrons that are shared by/between more than two nuclei. 
Resonance involves using two or more Lewis (electron dot) structures to represent a particular molecule or ion. A resonance structure is one of two or more alternative Lewis (electron dot) structures for a molecule or ion that cannot be described fully with one Lewis (electron dot) structure alone.
topic_14_delocalized_pi_electrons.pdf
File Size: 277 kb
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14.1 Calculating wavelength from bond enthalpy values (O2 and O3)
Applications and skills:
Explanation of the wavelength of light required to dissociate oxygen and ozone.
Click to download worksheet
Click to download worksheet

14.1 Catalytic destruction of ozone 
Applications and skills
Description of the mechanism of the catalysis of ozone depletion when catalysed by CFCs and NOx.

Click to download worksheet

14.2 Hybridization 
Understandings:
A hybrid orbital results from the mixing of different types of atomic orbitals on the same atom.
Applications:
Explanation of the formation of sp3, sp2 and sp hybrid orbitals in methane, ethene and ethyne.
Identification and explanation of the relationships between Lewis (electron dot) structures, electron domains, molecular geometries and types of hybridization.


topic_14_hybridization.pdf
File Size: 193 kb
File Type: pdf
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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