3.1 The periodic table

• Periods, groups, blocks

• Metals, metalloids, non-metals

• Recognize s, p, d, and f blocks

• Period number = outer energy level

• Group = number of valence electrons

• Electron configuration ↔ position (up to Z=36)

• Deduce element position from electron configuration and vice versa

• Trends: atomic radius, ionic radius, IE, electron affinity, electronegativity

• Explain trends across periods and down groups

• Group 1: increasing metallic character

• Group 17: decreasing non-metallic character

• Reactions: Group 1 metals with water, Group 17 with halide ions

• Describe and explain displacement reactions using periodic trends

• Oxides: basic (metal) → amphoteric → acidic (non-metal)

• Oxide reactions with water

• Deduce equations for oxides of group 1, group 2, carbon, and sulfur with water

• Number of electrons transferred in bonding

• Charge if compound were ionic

• Deduce oxidation states in compounds and ions

• Evidence for energy sublevels

• Explain discontinuities using energy sublevels and electron pairing

• Incomplete d-sublevels

• Variable oxidation states, high melting points, magnetic properties

• Catalytic properties, colored compounds, complex ions with ligands

• Recognize ligands and complex ions as characteristic transition element chemistry

• Successive IE values close together

• Deduce electron configurations of first-row transition element ions

• Light absorption promotes electron between split d-orbitals

• Complementary colors (use color wheel)

• Use the color wheel to link absorbed and observed colors