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Overview of Chapters 6-9: Atomic Structure, Periodic Trends, Bonding AP Chemistry/1213 Chapter 7 Electronic Structure of Atoms Review: • • • • • • • • • EMR Waves: , 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 Hrxn 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