Unit 2: Compound Structure and Properties
2.1 Types of Chemical Bonds.
Apply Coulomb’s Law and electronic structure to compare
electronegativity values for two elements.
Classify a bond as ionic, non-polar covalent, polar covalent, or
metallic using periodic trends or electronegativity values.
Assign partial charges to atoms in a bond based on electronegativity.
Recognize that ionic and covalent bonds exist on a continuum, with polar
covalent bonds in between.
Describe the nature of bonding in terms of electron donation,
acceptance, sharing, or delocalization.
2.2 Intramolecular Force and Potential Energy.
Examine a potential energy vs. distance graph to determine bond length
and bond energy.
Identify the bond order of a bond.
Compare the relative strength and length of single, double, and triple
bonds.
Apply Coulomb’s Law to compare the strength of given bonds.
2.3 Structure of Ionic Solids.
Sketch a simple lattice structure for an ionic solid.
2.4 Structure of Metals and Alloys.
Sketch a simple model of a metallic solid.
Determine if two metals will form an interstitial or substitutional
alloy based on their relative sizes.
Compare the main properties of interstitial and substitutional alloys.
2.5 Lewis Diagrams.
Draw a Lewis structure that obeys the octet rule given a molecular
formula.
Evaluate a Lewis structure to determine if it is valid.
Complete a partial Lewis structure so that it obeys the octet rule.
2.6 Resonance and Formal Charge.
Draw a Lewis structure with resonance when multiple valid configurations
exist.
Complete a partial Lewis structure so that it minimizes formal charges.
Choose the best Lewis structure from several valid options based on
formal charge.
2.7 VSEPR and Hybridization.
Identify the VSEPR geometry for a given molecule.
Assign bond angles based on hybridization (up to sp³).
Quantify the number of pi and sigma bonds in a molecule.
Identify two molecules as geometric isomers.
Compare the bond strength of sigma and pi bonds.