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Chemistry Department
Grade 11
Atomic Theory
1. Provide the meaning of each type of quantum number (principal, angular momentum, magnetic
and electron spin).
2. Apply quantum number rules to determine allowable values for each type of quantum number.
3. Understand the basis of atomic orbitals.
4. Arrange atomic orbitals based upon energy levels.
5. Understand the meaning of the Pauli exclusion principle and how it relates to electron
configurations.
6. Apply Hund’s rule in drawing electron orbital diagrams.
7. Determine the electron configuration of an atom.
8. Use the periodic table to determine the electron configuration of an atom.
Molecular Geometry
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Give in your own words the relevance of VSEPR theory to molecular shapes.
Use the VSEPR model to determine the molecular shape of a molecule.
Explain the difference between electron domain geometry and molecular geometry.
Determine the electron domain geometry and molecular geometry.
Calculate the ideal bond angles for a molecule.
Determine whether a molecule will exhibit ideal bond angles.
Explain how a bond forms in terms of atomic orbitals.
Use the Lewis structure and number of electron domains of a compound to determine the
hybridization of its bonds.
9. Provide the number of sigma and pi bonds in a molecule or around a central atom.
10. Give in your own words the major relevance of the major bonding theories: Lewis-theory,
VSEPR, valence bond theory, hybridization
Periodic Trends
1. Define effective nuclear charge, atomic radius, ionization energy, ionic radius and
electronegativity.
2. Predict differences in effective nuclear charge, atomic radius, ionization energy, energy, ionic
radius and electronegativity. Between elements using periodic trends.
3. Predict the size of the radius of an ion in relation to the unionized species of the same element.
4. Define isoelectronic species and arrange a series of isoelectronic species according to ionic
radius.
5. Determine the polarity of a bond using differences in electronegativity.
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