NAME PER "ALICE" REFERENCE NOTEBOOK

Transcription

1 NAME PER ACTIVE LEARNING IN CHEMISTRY EDUCATION "ALICE" REFERENCE NOTEBOOK This document may be used (when directed) during tests and quizzes, provided that you do not alter it in any way. Do not add any information to it. R-1 A.J. Girondi

2 NOTICE OF RIGHTS All rights reserved. No part of this document may be reproduced or transmitted in any form by any means, electronic, mechanical, photocopying, or otherwise, without the prior written permission of the author. Copies of this document may be made free of charge for use in public or nonprofit private educational institutions provided that permission is obtained from the author. Please indicate the name and address of the institution where use is anticipated A.J. Girondi, Ph.D. 505 Latshmere Drive Harrisburg, PA Website: R-2 A.J. Girondi

3 Reference Table 1 Common Oxidation Numbers of Selected Elements (Note: Sometimes these elements can assume oxidation numbers other than those listed.) Aluminum Al +3 Lithium Li +1 Antimony Sb +3,+5 Magnesium Mg +2 Arsenic As +3,+5 Manganese Mn +2,+4,+7 Barium Ba +2 Mercury Hg +1,+2 Bismuth Bi +3 Nickel Ni +2 Boron B +3 Nitrogen N -3,+3,+5 Bromine Br -1,+5 Oxygen O -2 Calcium Ca +2 Phosphorus P +3,+5 Carbon C +2,+4 Platinum Pt +2,+4 Cesium Cs +1 Potassium K +1 Chlorine Cl -1,+5,+7 Silicon Si +4 Chromium Cr +2,+3,+6 Silver Ag +1 Cobalt Co +2,+3 Sodium Na +1 Copper Cu +1,+2 Strontium Sr +2 Fluorine F -1 Sulfur S -2,+4,+6 Gold Au +1,+3 Tin Sn +2,+4 Hydrogen H +1 Titanium Ti +3,+4 Iodine I -1,+5 Tungsten W +6 Iron Fe +2,+3 Zinc Zn +2 Lead Pb +2, +4 Reference Table 2 Common Oxidation Numbers of Selected Polyatomic Ions Name Formula Charge Ammonium NH Acetate C2H3O Chlorate ClO Perchlorate ClO Cyanide CN Hydrogen carbonate HCO (or bicarbonate) Hydrogen sulfate HSO Hydroxide OH Nitrate NO Nitrite NO Permanganate MnO Thiocyanate SCN Carbonate CO Chromate CrO Dichromate Cr2O Sulfate SO Sulfite SO Phosphate PO R-3 A.J. Girondi

4 Reference Table 3 Latin Names of Four Selected Elements Element Symbol Latin Name copper (I) Cu 1+ cuprous copper (II) Cu 2+ cupric iron (II) Fe 2+ ferrous iron (III) Fe 3+ ferric mercury (I) Hg 1+ mercurous mercury (II) Hg 2+ mercuric tin (II) Sn 2+ stannous tin (IV) Sn 4+ stannic Reference Table 4 Four Kinds of Decomposition Reactions 1. Metallic carbonates decompose into metallic oxides and carbon dioxide. CaCO3 ----> CaO + CO2 K2CO3 ----> K2O + CO2 H2CO3 ----> H2O + CO2 2. Many metallic hydroxides decompose into metallic oxides and water. 2 KOH ----> K2O + H2O Ca(OH)2 ----> CaO + H2O 2 Al(OH)3 ----> Al2O3 + 3 H2O 3. Metallic chlorates decompose into metallic chlorides and oxygen gas. 2 KClO3 ----> 2 KCl + 3 O2 Ba(ClO3)2 ----> BaCl2 + 3 O2 2 Al(ClO3)3 ----> 2 AlCl3 + 9 O2 4. Many binary (two-element) compounds decompose into pure elements. 2 HgO ----> 2 Hg + O2 2 H2O ----> 2 H2 + O2 2 NaCl ----> 2 Na + Cl2 Note: There are many other kinds of decomposition reactions in addition to those shown above. R-4 A.J. Girondi

5 Reference Table 5 The Activity Series Metals Nonmetals lithium fluorine potassium chlorine calcium bromine sodium iodine magnesium aluminum zinc chromium iron nickel tin lead hydrogen Although hydrogen is copper not a metal, it is mercury compared to metals in silver the activity series. platinum gold Reference Table 6 SOLUBILITY RULES Type of Compound Precipitate? 1. Compounds of nitrates (NO3 1- ), acetates (C2H3O2 1- ), and chlorates (ClO3 1- ) ARE soluble NO 2. All common compounds of Na, K, and NH4 1+ ARE soluble NO 3. Most chlorides, Cl 1-, bromides, Br 1-, and fluorides, F 1-, ARE soluble NO (But those of Ag, Hg, and Pb* are NOT soluble) YES 4. Most sulfate, SO4 2-, compounds ARE soluble NO (But those of Pb, Ba, Sr, and Ca** are NOT soluble) YES 5. Most carbonate (CO3 2- ), phosphate (PO4 3- ), and sulfide (S 2- ) compounds are NOT soluble YES (But those of Na, K, and NH4 1+ ARE soluble) NO 6. Most hydroxides, OH 1-, are NOTsoluble YES (But those of all Group1A metals, and Ca, Ba and Sr ARE soluble) NO *Lead chloride, PbCl2, is fairly soluble in hot water. Consider it a precipitate. **Calcium sulfate, CaSO4, is slightly soluble. Consider it a precipitate. R-5 A.J. Girondi

6 ReferenceTable 7 A SOLUBILITY TABLE For our purposes, the combinations below designated with the letter P, are considered to be insoluble enough to form precipitates. If a P is not listed for a substance, it is soluble in water (it dissolves). If you cannot find the data you need in this table, check the solubility rules. P = PRECIPITATE 1 - acetate, C2H3O chromate, CrO phosphate, PO bromide, Br hydroxide, OH silicate, SiO carbonate, CO iodide, I sulfate, SO chlorate, ClO nitrate, NO sulfide, S chloride, Cl oxide, O aluminum P - - P P P - P ammonium barium - - P - - P P P P P P bismuth - P P P P - P P - P P cadmium - - P P - - P P calcium - - P P - - P P P - P copper(ii) - - P P - - P P P - P hydrogen P - - iron(ii) - - P P - - P P P - P iron(iii) P P - - P P P - P lead(ii) - P P - P P P P - P P P P P magnesium - - P P - - P P P - - manganese(ii) - - P P - - P P P - P mercury(i) P P P - P P - P - P P - P P mercury(ii) - P P - - P P P - P P - P P nickel - - P P - - P P - - P potassium silver P P P - P P - P - P P - P P sodium strontium - - P - - P P P P - tin(ii) - P P P - - P P - - P tin(iv) P - - P P zinc - - P - - P P - - P P P - P (Note that sodium, potassium, and ammonium never form precipitates.) R-6 A.J. Girondi

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8 1s Reference Table 9 The Diagonal Rule 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 7s Reference Table 10 Formulas for Percent Error and Percent Deviation % Error = O - A A X 100% O = observed value; A = accepted value % Deviation = O - M M X 100% O = observed value; M = mean (average) value R-8 A.J. Girondi

9 Reference Table 11 Standard Half-Cell Reduction Potentials Reduction---> <---Oxidation E o red (Volts) Li 1+ + e - <====> Li Rb 1+ + e - <====> Rb K 1+ + e - <====> K Cs 1+ + e - <====> Cs Ba e - <====> Ba Sr e - <====> Sr Ca e - <====> Ca Na 1+ + e - <====> Na Mg e - <====> Mg Al e - <====> Al Mn e - <====> Mn Zn e - <====> Zn Cr e - <====> Cr Cd e - <====> Cd Fe e - <====> Fe Cr 3+ + e - <====> Cr Stronger Co e - <====> Co Reducing Ni e - <====> Ni Agents Sn e - <====> Sn Pb e - <====> Pb H e - <====> H2(g) Sn e - <====> Sn Cu 2+ + e - <====> Cu Stronger Cu e - <====> Cu Oxidizing Cu 1+ + e - <====> Cu Agents I2 + 2e - <====> 2 I Fe 3+ + e - <====> Fe Hg e - <====> Hg(l) Hg e - <====> 2 Hg(l) Ag 1+ + e - <====> Ag Br2(l) + 2e - <====> 2 Br Cl2(g) + 2e - <====> 2 Cl Au e - <====> Au F2(g) + 2e - <====> 2 F Oxidizing Agents Reducing Agents R-9 A.J. Girondi

10 Reference Table 12 Vapor Pressure of Water T ( o C) P (mm) T ( o C) P (mm) Reference Table 13 Selected Metric Equivalents 1 meter (m) = 100 centimeters (cm) 1 centimeter (cm) = 10 millimeters (mm) 1 liter (l) = 1000 milliliters (ml) 1 milliliter (ml) = 1 cubic centimeter (cm 3 ) 1 kilogram (kg) = 1000 grams (g) 1 gram (g) = 1000 milligrams (mg) 1 g of H2O = 1 ml H2O Reference Table 14 Selected English-Metric Equivalents 1 meter (m) = inches (in) 1 inch (in) = 2.54 centimeters (cm) 1 kilogram (kg) = 2.2 pounds (lbs) 1 pound (lb) = grams (g) 1 ounce (oz) = grams (g) 1 gram (g) = grains (gr) 1 liter (l) = 1.06 quarts (qts) 1 cubic foot (cu. ft.) = liters R-10 A.J. Girondi

11 1 H Li Be Na Mg K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Rb Cs Fr Sr Ba Ra (226) Y La Ac Zr Hf Unq Nb Ta Mo W Reference Table R-15 The Periodic Table With Atomic Weights Tc Re Ru Os Rh Ir Pd Pt Ag Au Unp Unh Uns Uno Une Uun Uuu Cd Hg B C Al Si In Ge Sn N (99) P As Sb O S Se Te F Cl Br Tl Pb Bi Po At I 2 He Ne Ar Kr Xe Rn (210) (210) (222) Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu (147) Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr (231) (237) (242) (243) (247) (249) (251) (254) (253) (256) (254) (260) atomic number symbol?? E 261 atomic weight (parentheses indicate atomic mass of most stable isotope) R-11

12 Reference Table R-16 Common Oxidation Numbers of the Elements 1 H +1, (-1 in hydrides like NaH) 39. Y He Zr Li Nb +5, Be Mo +6, +4, B Tc +7, +6, C +4, (less commonly +2, -4) 44. Ru +8, +6, +4, N +5, +4, +3, +2, +1, Rh +4, +3, O -2, (-1 in peroxides like H2O2) 46. Pd +4, F Ag Ne Cd Na In Mg Sn +4, Al Sb +5, +3, Si +4, Te +6, +4, P +5, +3, I -1, +7, +5, +3, S +6, +4, +2, Xe +6, +4, Cl -1, +7, +5, +3, Cs Ar Ba K La Ca Ce through Lu Sc Hf Ti +4, +3, Ta V +5, +4, +3, W +6, Cr +6, +3, Re +7, +6, Mn +7, +6, +4, +3, Os +8, Fe +3, Ir +4, Co +3, Pt +4, Ni Hg +2, Cu +2, Tl +3, Zn Pb +4, Ga Bi +5, Ge +4, Po As +5, +3, At Se +6, +4, Rn Br -1, +7, +5, +3, Kr +4, Rb Sr +2 R-12 A.J. Girondi