CHEM 1AA3 Lecture Notes - Lecture 4: Effective Nuclear Charge, Ionic Radius, Alkali Metal
12 Mar 2014
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Chem 1a03 lecture 4 - the periodic table and some atomic. Noble gases, group 18a ns2np6 electron configuration: considered chemically inert until 1962. Non-metals: main group (s and p block) tend to gain electrons, ability to oxidize increases towards the upper period, for instance, cl2 can rip electrons from i-, yet br2 cannot rip from cl-. React with metals to form salts. (search: synthesis of nacl) Metals: main group (s and p block) metals (and h) tend to lose electrons, alkali metals (group 1) oxidize more readily than alkaline earth metals, both oxidize easy in water know: how to write their reactions. General trends in physical properties: across a period, metallic properties decrease. Melting point varies with type of bonding (network covalent>metallic>ionic>molecular) Atomic radius decreases (z increases, but e- are added to the same n valence shell with same o o number of core electrons.
