April 7 - Ca2+, Mg2+ Al3+, Zn2+, Ag1+, Cd2+ 4. Oxygen is...

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All Chapter 8 Chapter 11: Sect 1-3 Chapter 4: Sect. 10-11 Chapter 11 Electrochemistry Have to study redox reactions. Reduction Reaction Is the gain of electrons Decrease in oxidation # Oxidation Reaction Is the loss of electrons. Increase in oxidation # Rules: 1. All elements in their neutral state have an oxidation number of 0 Examples: O2, H2, N2, Fe(s) 2. All monatomic ions have oxidation number equivalent to charge on ion. Fe2+ = +2 Cl- = -1 S2- = -2 3. Some elements are “one trick ponies” and only have one oxidation state available. Group 1 metals Na+, K+ Group 2 metals
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Unformatted text preview: Ca2+, Mg2+ Al3+, Zn2+, Ag1+, Cd2+ 4. Oxygen is always , -2 , when combined with other stuff. Oxide state. 5. H is always +1, when combined (unless a previous rule is in effect) Hydride H H-NaH : 1+, 1-MnO4- + Fe2+ Fe3+ + Mn2+ In aqueous free to add H2O to either side (use as needed) Acidic: Free to add H+ to either side Basic: Free to add OH-*make sure to check charge balance Right way: MnO4- + Fe2+ Fe3+ + Mn2+ MnO4- Mn2+ , +7 +2, ADD 5electrons Fe2+ Fe3+, +2 +3, LOSE one electron...
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This note was uploaded on 11/18/2010 for the course CH 302 taught by Professor Holcombe during the Spring '07 term at University of Texas at Austin.

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April 7 - Ca2+, Mg2+ Al3+, Zn2+, Ag1+, Cd2+ 4. Oxygen is...

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