CHEM 110 Lecture Notes - Electronegativity
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CHEM 110 Full Course Notes
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Transition metals are their ionic form and in a variety of oxidation states. Electrons are lost from the 4s orbital before the 3d orbitals. Remember electronegativity: increase from left to right and from bottom to top; power of an atom to hold on to its atoms tightly (how effectively) Low electronegativity will mean lose electrons readily. Maximum possible oxidation state results from losing all 4s and 3d electrons. Oxidation state increases from sc to mn: 3+ to 7+ Oxidation state decrease from mn to zn: mn7+ and ni2+ and cu2_ 2+ oxidation state becomes more stable as we go from left to right in the first series of transition metals. It is too difficult to remove d electrons as they become lower in energy as the nuclear charge increases.