Unit 12: The Periodic Table,
Bonding & Shapes
Key Learning Targets
Define the following quantities, describe their periodic trends, and use them to predict the relative magnitudes of elements: atomic radii, ionic radii, electronegativity, ionization energy, electron affinity.
Describe lattice energy and make comparisons between ionic compounds using lattice energy.
Compare and contrast the distinctive properties of ionic and molecular compounds.
Identify bond type based on the atoms present and on electronegativity differences. (ionic, polar, nonpolar)
Define the octet rule, apply it to Lewis structures and explain its exceptions.
Illustrate bond formation by constructing Lewis structures for simple molecular compounds and polyatomic ions.
Explain multiple bonding in molecular compounds and the difference in strength between single, double and triple bonds.
Explain resonance and draw valid resonance structures using Lewis Structures.
Explain the valence-shell-electron-pair repulsion model (VSEPR) and use it to predict the molecular geometry of simple molecular compounds.
Predict whether a simple molecular compound is polar or non-polar based on its molecular geometry.
Periodic Table & Trends Notes Handout
Ionic Bonding Notes Handout
Covalent Bonding Notes Handout
Molecular Geometry Notes Handout
Electron Dot WS
Lewis Structures & Shapes WS
Bonding Practice WS
Molecular Geometry WS
Chemical Bonding Lab
Unit 12 Notes PDF