chem6c week 7 handout

chem6c week 7 handout - Chemistry 6C Week 7 Handout...

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Chemistry 6C Week 7 Handout Transition Metals: Physical Trends d orbitals are last to be occupied, but lie in lower energy orbitals 10 transition elements in every period because there are 5 orbitals and 2 e- can be put into each orbital Generally good conductors, high melting point and boiling point Atomic radii – smiley face pattern; atomic density- sad face pattern o Lobes of d orbitals are far apart so they do not repel each other as strongly o Electron density low near nucleus so they are not effect at shielding Lanthanide contraction- decrease in radius along first row of f block because of increase in nuclear charge and the very poor shielding of f orbital electrons o Period 6 atomic radii about the same as that of Period 5 o Reason why Au and Pt are so unreactive- valence electrons are close to the nucleus so they are not readily available to chemical reactions Lower melting point and boiling point for group 12 because of filled d orbitals. Group 11 wants to have filled d orbitals, so 1 e- is stripped from s orbitals Chemical Trends d & s orbital electrons of transition metal can be lost in compound formation=> variety of oxidation states transition metal atoms closer to the center of the row have a greater variety of oxidation numbers Higher oxidation number =>greater ability to be reduced => better oxidizing agent Lower oxidation number =>greater ability to be oxidized => better reducing agent
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The oxides of a given transition element show a shift in acidic character with increasing
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This note was uploaded on 06/07/2009 for the course CHEM 6C taught by Professor Hoeger during the Spring '08 term at UCSD.

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chem6c week 7 handout - Chemistry 6C Week 7 Handout...

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