Overview of Chapters 6-9: Atomic Structure, Periodic Trends, Bonding
AP Chemistry/1213
Chapter 7 Electronic Structure of Atoms
Review:
• EMR Waves: l, n and E relationships
• Older theories of the atom
• Basics of Bohr’s theory
• Heisenberg’s Uncertainty Principle
• Erwin Schrödinger’s idea about the wave function/probabilities of finding an electron, quantum numbers
• Use of orbital names – s, p, d, f – in quantum numbers
• Electron configuration and orbital diagrams, including the application of Aufbau, Hund’s and Pauli’s rules/principles
• s, p, d, f blocks in the periodic table
• Anomalous electron configurations
New Material:
• Use of numbers for quantum numbers
• The presence of nodes in relation to orbitals
• Degenerate orbitals vs energy levels in multi-electron atoms
Chapter 7 - Periodic Trends
Review:
• Predict and explain:
• Periodic trends in atomic radius
• Trends in ionic radius, especially comparing neutral atom with its respective ion
• Isoelectronic series
• Ionization energy – both periodic trends in first ionization energy and successive IEs
New Material:
• Use effective nuclear charge to explain trends in atomic radius and ionization energy
• Predict and explain periodic trends in electron affinity
• Describe and compare properties of metals, nonmetals and metalloids
• Apply group trends in terms of reactions
Chapter 8 – Basics of Chemical Bonding
Review:
• types of chemical bonds – ionic, covalent, metallic
• relate bond polarity and the type of bond to differences in electronegativity
• Lewis structures of covalently-bonded molecules and polyatomic ions, including exceptions to the octet rule
• predict formation of single, double and triple bonds
• name molecules
New Material:
• lattice energy
• quantify bond polarity using dipole moments
• relate bond lengths, electronegativity differences and dipole moments to each other in molecules
• use of formal charge to determine most likely Lewis structure
• resonance structures
• bond energies (enthalpies) and their use in determining DHrxn and their relation to bond length
Chapter 9 – Molecular Geometry
Review:
• the basics of VSEPR theory – the reasoning (valence electrons repel one another)
• shapes based on VSEPR - linear (two electron domains), trigonal planar (three domains), tetrahedral (four domains), trigonal bipyramidal (five domains) and octahedral (six domains)
• use Lewis Structures to predict molecular geometry
• predict polarity of simple molecules, knowing their shapes, presence of lone pairs and differences in electronegativity
New Material:
• the use of electron domains, and especially nonbonding pairs of electrons (lone pairs) to determine a molecule’s shape, including shapes based on trigonal bipyramidal and octahedral
• the effect of lone pairs on bond angles due to their greater repulsion than bonded pairs of electrons
• application of VSEPR to larger molecules
• express molecular polarity in terms of dipole moments
• valence bond theory
• hybrid orbitals
• sigma and pi bonds in multiple bonds and resonance structures