Lec-41-review - Final Exam, Monday, December 22, 11 AM 1:30...

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1 You will be given Constants/conversions Specific data values Periodic table Complex equations (not ideal gas law) Know: trends , solubility rules, oxidation # rules no need to memorize acid strength table, activity series table, amino acid table Final Exam, Monday, December 22, 11 AM – 1:30 PM 2 Be sure to bring the following: • Stony Brook ID card (or other official photo ID) • 2 or more #2 pencils and a good eraser • Calculator with extra batteries Do NOT bring any of the following: • Cell phones, beepers, iPods, or other communication devices • Textbook, notes, or any aids to taking the exam Violations may result in a course grade of F and a report to the Academic Judiciary.
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3 Review: Final exam • Cumulative- course content from entire semester • 40+2 multiple choice problems • Some conceptual, some numerical • A few quite difficult • Point value same regardless of difficulty! • Review lecture notes • PRACTICE problem solving • Do not work too hard Sunday PM • Do not attempt “new” material 24 hours before exam 4 Chapter 5: Chemical Reactions
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5 Chemical reactions Exchange reactions ± formation of molecular cmpd, gas, insoluble salt ± Know solubility rules Redox reactions ± Exchange of electrons, calculation of oxidation # ± Know oxidation # rules Displacement reactions ± Essentially a redox reaction ± Metal activity series • Acid/base reactions • Organic reactions 6 Exchange Reactions: Precipitation types of exchange reactions : ± Form a precipitate precipitate • an insoluble insoluble ionic compound •AgNO 3 (aq) + KC l (aq) KNO 3 (aq) + AgC AgC l (s) ± Form a molecular compound molecular compound • Often water •H 2 SO 4 (aq) + 2 NaOH(aq) Na 2 SO 4 (aq) + 2 H 2 O( l ) ± Form a molecular gas. gas. •2 HC l (aq) + Na 2 S(aq) 2 NaC l (aq) + H 2 S(g)
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7 When ionic solutions mix, a precipitate may form: AgNO 3 (aq) + NaC l (aq) AgC l (s (s ) + NaNO 3 (aq) Not all ions react The solubility rules help predict reactions. A reaction occurs if a product is insoluble. KNO 3 (aq) + NaC l (aq) No reaction Precipitation Reaction 8 Soluble species (Table 5.1): Soluble species (Table 5.1): • All ammonium and group 1A (Na + , K + ,…. and NH 4 + salts) • All nitrates (NO 3 - ) • Most chlorides, bromides and iodides ± (exceptions: AgX, Hg 2 X 2 , and PbX 2 ; X = C l - , Br - , I - ). • Most sulfates (SO 4 2- ) ± (exceptions: CaSO 4 ,SrSO 4 , BaSO 4 , Ag 2 SO 4 , PbSO 4 , and Hg 2 SO 4 ) • All chlorates (C l O 3 - ) • All perchlorates (C l O 4 - ) • All acetates (CH 3 COO - ) Aqueous Solubility of Ionic Compounds
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9 Insoluble species (table 5.1) Insoluble species (table 5.1) Type Exceptions • All phosphates (PO 4 3- ) Group 1A, NH 4 + • All carbonates (CO 3 2- ) Group 1A, NH 4 + • All hydroxides (OH - ) Group 1A, NH 4 + ± Sr(OH) 2 , Ba(OH) 2 & Ca(OH) 2 are slightly soluble • All oxalates (C 2 O 4 2- ) Group 1A, NH 4 + • All oxides (O 2- ) Group 1A • All sulfides (S 2- ) Group 1A, NH 4 + ± MgS, CaS & BaS are slightly soluble.
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This note was uploaded on 11/14/2010 for the course CHE 131 taught by Professor Kerber during the Spring '08 term at SUNY Stony Brook.

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Lec-41-review - Final Exam, Monday, December 22, 11 AM 1:30...

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