Periodic Table of the Elements

Transcript

1 Period Periodic Table of the Elements 1 I A 18 VIII A s 4s , ,3, ,4, ,3,6, ,4, , , , s Rb Sr 4d Y Zr Nb Mo Tc Ru Rh Pd Ag Cd 5p In Sn Sb Te I Xe rubidium strontium yttrium zirconium niobium molybdenum technetium ruthenium rhodium palladium silver cadmium indium tin antimony tellurium iodine xenon , ,4, ,6, ,3, , , , , , , , s 5d 6p cesium barium lutetium hafnium tantalum tungsten rhenium osmium iridium platinum gold mercury thallium lead bismuth polonium astatine radon s 1 ±1 # 29 +2,1 ions commonly formed 2 H hydrogen 2 II A symbol English element name Cu copper 13 III A 14 IV A 15 V A 16 VI A 17 VII A mass (rounded) s Li Be 2p B C N O F Ne lithium beryllium boron carbon nitrogen oxygen fluorine neon Gases Liquids Metalloids s Na Mg p Al Si P S Cl Ar sodium magnesium III B IV B V B VI B VII B VIII B VIII B VIII B I B II B aluminum silicon phosphorus sulfur chlorine argon ,3, ,2,3, ,2, ,3,4,6, , , , , , K Ca 3d Sc Ti V Cr Mn Fe Co Ni Cu Zn 4p Ga Ge As Se Br Kr potassium calcium scandium titanium vanadium chromium manganese iron cobalt nickel copper zinc gallium germanium arsenic selenium bromine krypton Cs Fr francium Ba Ra radium d Lu Hf Ta W Re Os Ir Pt Au Lr Rf Db Sg Bh lawrencium rutherfordium dubnium seaborgium bohrium Hs hassium Mt meitnerium Ds darmstadtium 281 Rg roentgentium 272 Hg Cn copernicum 285 7p Tl Nh nihonium Pb Fl flerovium Bi Mc moscovium Po Lv livermorium At Ts tennessine He helium Rn Og oganesson lanthanides (rare earth metals) actinides 4f 5f , , , , , , ,2 La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb lanthanum cerium praseodymium neodymium promethium samarium europium gadolinium terbium dysprosium holmium erbium thulium ytterbium , ,3,4, ,3,4, ,3,5, ,4,5, , , ,3 Ac Th Pa actinium 227 U thorium protactinium uranium Np Pu Am neptunium plutonium americium Cm curium Bk berkelium Cf californium Es einsteinium Fm fermium Md mendelevium No nobelium 259 ammonium NH 4 +1 hydronium H 3 O +1 acetate C 2 H 3 O 2 1 CH 3 COO 1 chlorite ClO 2 1 ClO 1 Common Poly Ions hydrogen sulfate permanganate periodate hydrogen hydroxide nitrate cyanide CN 1 nitrite 1 NO 2 carbonate cyanate thiocyanate OCN 1 SCN 1 bromate iodate 1 BrO 3 1 IO 3 dihydrogen phosphate OH 1 perchlorate chlorate hypochlorite ClO 4 1 ClO 3 1 NO 3 1 HSO 4 1 MnO 4 1 IO 4 1 HCO 3 1 H 2 PO 4 1 sulfate sulfite phthalate chromate dichromate carbonate hydrogen phosphate 2 SO 4 2 SO 3 2 C 8 H 4 O 4 peroxide CrO 4 2 Cr 2 O 7 2 CO oxalate C 2 O 4 silicate tetraborate borate arsenate 2 SiO 3 2 O 2 B 4 O BO 3 3 AsO phosphate PO 4 HPO 4 orthosilicate SiO 4 4 Copyright Jeff Bigler. This document is licensed under a Creative Commons Attribution-Share Alike 3.0 United States License. You are free to share and/or adapt this work, with appropriate attribution, under an identical, similar, or compatible license. See for more information.

2 Chemistry Reference Tables 1 Table A. Standard Temperature and Pressure... 2 Table B. Selected Units... 2 Table C. Selected Prefixes... 2 Table D. Physical Constants for Water... 3 Table E. Vapor Pressure and Density of Water... 3 Figure F. Phase Diagram for Water... 3 Table G. Solubility Guidelines... 4 Table H. K sp Values for Some Insoluble Salts at 25 C... 4 Figure I. Solubilities of Selected Compounds... 4 Table J. Number Prefixes... 5 Table K. Poly Ions... 5 Table L. Flame Test Colors... 5 Table M. Aqueous Ion Colors... 5 Table N. Colors of Assorted Compounds... 5 Table O. Common Acids... 6 Table P. pk a Values for Common Acids... 6 Table Q. Common Bases... 6 Table R. Common Acid-Base Indicators... 6 Table S. Symbols Used in Nuclear Chemistry... 7 Table T. Selected Radioisotopes... 7 Table U. Constants Used in Nuclear Chemistry... 7 Figure V. Neutron/Proton Stability Band... 7 Table W. Activity Series... 8 Table X. Std. Reduction Potentials... 8 Table Y. Selected Properties of the Elements... 9 Figure Z. Bonding Triangle Table AA. Bond Dissociation Energies & Bond Lengths Table BB. Thermodymanic Data Table CC. Some Common & Equivalent Units and Approximate Conversions Table DD. Selected Formulas and Equations Table A. Standard Temperature and Pressure Table B. Selected Units Name Values Name Symbol Quantity Standard Pressure 1 atm 760 torr kpa meter (SI) m Standard Temperature 0 C 32 F K centimeter cm length atm = atmosphere kilogram (SI) kg Torr = millimeter of mercury (mm Hg) gram g mass kpa = kilopascal Pascal (SI derived) Pa C = degree Celsius atmosphere atm F = degree Fahrenheit mm of mercury mm Hg pressure K = kelvin Torr Torr Kelvin (SI) K Table C. Selected Prefixes degree Celsius C temperature Factor Number of Units Prefix Symbol amt of substance (SI) mol mole ,000,000 mega- M Joule (SI derived)) J ,000 kilo- k kilocalorie kcal energy deci- d second (SI) s time centi- c liter L, l volume milli- m part per million ppm concentration micro- (or u) molarity mol M, concentration 1 adapted from: The University of the State of New York. The State Education Department. Albany, NY Edition. Reference Tables for Physical Setting/Chemistry.

3 Chemistry Reference Tables p. 3 Table D. Physical Constants for Water Freezing 1 atm 0 C = K Boiling 1 atm 100 C = K Heat of Fusion J/g Heat of Vaporization 2270 J/g Specific Heat Capacity (C p ) J/g C Freezing Point Depression Constant (K f ) 0.52 C/m Boiling Point Elevation Constant (K b ) 1.86 C/m Table E. Vapor Pressure and Density of Water Temp P vap density ( C) (kpa) (g/cm 3 ) Figure F. Phase Diagram for Water

4 Chemistry Reference Tables p. 4 Table G. Solubility Guidelines Ions That Form Ions That Form EXCEPT with SOLUBLE Compounds INSOLUBLE Compounds EXCEPT with Group I ions (Li +, Na +, etc.) carbonate (CO 2 3 ) ammonium (NH + 4 ) chromate (CrO 2 4 ) Group I ions, nitrate (NO 3 ) phosphate (PO 3 4 ) ammonium (NH + 4 ) hydrogen carbonate (HCO 3 ) sulfite (SO 2 3 ) chlorate (ClO 3 ) sulfide (S 2 Group I ions, ) + perchlorate (ClO 4 ) Group II ions, NH 4 acetate (C 2 H 3 O 2 or CH 3 COO ) Ag + hydroxide (OH ) Group I ions, halides (Cl, Br, I ) Ag +, Cu +, Pb 2+ 2+, Hg 2 oxide (O 2 ) NH + 4, Ba 2+, Sr 2+, Tl + sulfates (SO 2 4 ) Ca 2+, Sr 2+, Ba 2+, Ag +, Pb 2+ Table H. K sp Values for Some Insoluble Salts at 25 C Compound K sp MgCO PbCl BaF CuCl PbI AgOH BaCO CaCO SrCO AgCl BaSO CaF Mg(OH) Ag 2 CrO CuI AgBr PbSO PbCO Mn(OH) PbCrO Fe(OH) AgI Zn(OH) FeS HgCl ZnS PbS CdS Al(OH) CuS Fe(OH) Ag 2 S HgS Figure I. Solubilities of Selected Compounds

5 Chemistry Reference Tables p. 5 Table J. Number Prefixes Number Inorganic Organic Number Inorganic Organic 1 mono- meth- 6 hexa- hex- 2 di- eth- 7 hepta- hept- 3 tri- prop- 8 octa- oct- 4 tetra- but- 9 nona- non- 5 penta- pent- 10 deca- dec- Table K. Poly Ions ion formula ion formula ion formula ion formula americyl 2+ AmO 2 ammonium + NH 4 cyanate OCN dichromate 2 Cr 2 O 7 carbonyl CO 2+ hydronium H 3 O + thiocyanate SCN imide NH 2 thiocarbonyl CS 2+ iodyl + IO 2 selenocyanate SeCN molybdate 2 MoO 4 neptunyl 2+ NpO 2 nitrosyl NO + tellurocyanate TeCN peroxide 2 O 2 plutoryl 2+ PuO 2 thionitrosyl NS + hydroxide OH oxalate 2 C 2 O 4 selinyl SeO 2+ phosphoryl PO + iodate IO 3 phthalate 2 C 8 H 4 O 4 selenoyl 2+ SeO 2 thiophosphoryl PS + methanolate CH 3 O selenate 2 SeO 4 thionyl / SO 2+ + phospho PO 2 methanethiolate CH 3 S 2 disulfide S 2 sulfinyl acetate CH 3 COO ethanolate C 2 H 5 O 2 sulfate SO 4 sulfonyl / 2+ amide NH SO 2 permanganate MnO 4 thiosulfate sulfuryl 2 hydroxylamide NHOH nitrate NO 3 dithionate 2 S 2 O 3 2 S 2 O 4 uranyl UO 2+ azide N 3 superoxide O 2 silicate 2 SiO 3 vanadyl VO 2+ hydrazide N 2 H 3 tetraborate 2 B 4 O 7 borate 3 BO 3 mercury (II) Hg 2+ bromate BrO 3 carbide 2 C 2 arsenate 3 AsO 4 mercury (I) 2+ Hg 2 chlorate ClO 3 carbonate 2 CO 2 phosphate 3 PO 4 cyanide CN chromate 2 CrO 4 orthosilicate 4 SiO 4 Table L. Flame Test Colors Element Color Element Color Element Color Ba yellow-green K pink Pb blue Ca orange-red Li fuchsia Sb pale green Cu blue-green Mg bright white Sr red Fe gold Na yellow Zn blue-green Table M. Aqueous Ion Colors Ion Color Ion Color Cu + green V 2+ violet Cu 2+ blue V 3+ blue-green Fe 2+ yellow-green 2 CrO 4 yellow Fe 3+ orange-red 2 Cr 2 O 7 orange Cr 3+ violet [Cr(NO 3 ) 3 ] to green [CrCl 3 ] 2+ Cu(NH 3 ) 4 dark blue Ni 2+ green FeSCN 2+ red-brown (wine-red to dark orange) Mn 2+ pink Co 2+ pink Mn 7+ purple (e.g., the MnO 4 ion) 2 CoCl 4 blue Pb 3+ blue-green (Pb 2+ and Pb 4+ are clear) 3+ Ti(H 2 O) 6 purple Table N. Colors of Assorted Compounds Compound Color Compound Color F 2 pale yellow gas NO colorless gas Cl 2 green-yellow gas NO 2 brown gas Br 2 red-brown liquid metallic sulfides of transition metals I 2 dark metallic solid; dark violet vapor sulfides S 8 yellow odorous solid metallic PbI 2 bright yellow precipitate oxides Fe 2 O 3 reddish-brown (rust) tend to be black oxides of colored transition metals tend to be colored

6 Chemistry Reference Tables p. 6 Table O. Common Acids Table P. pk a Values for Common Acids Formula Name Acid pk a Conj. Base HCl (aq) hydrochloric acid H 2 O 15.7 OH HNO 3 (aq) nitric acid 2 HPO PO 4 H 2 SO 4 (aq) sulfuric acid HCO CO 3 H 3 PO 4 (aq) phosphoric acid + NH NH 3 H 2 CO 3 (aq) carbonic acid HCN 9.1 CN 2 HC 2 H 3 O 2 (aq) ethanoic acid H 2 PO HPO 4 or CH 3 COOH (aq) (acetic acid) H 2 S 7.0 HS H 2 CO HCO 3 Table Q. Common Bases CH 3 COOH 4.8 CH 3 COO Formula Name HCOOH 3.7 HCOO NaOH (aq) sodium hydroxide HNO NO 2 KOH (aq) potassium hydroxide HF 3.2 F Ca(OH) 2 (aq) calcium hydroxide C 6 H 8 O 7 NH 3 (aq) aqueous ammonia (citric acid) 3.1 C 6 H 7 O 7 H 3 PO H 2 PO 4 Table R. Common Acid-Base Indicators HSO SO 4 Indicator ph Range of HNO NO 3 Color Change Color Change H 3 O H 2 O bromophenol blue yellowpurple HCl 7.0 Cl methyl orange redyellow HBr 9.0 Br bromocresol green yellowblue HI 10 I methyl red redyellow HClO 4 10 ClO 4 litmus redblue H 2 SO 4 12 HSO 4 bromothymol blue yellowblue phenol red yellowred Any acid with a pk a value less than 0 is a thymol blue yellowblue phenolphthalein clearpink strong acid; any base with a pk a value greater than 14 is a strong base.

7 Chemistry Reference Tables p. 7 Table S. Symbols Used in Nuclear Chemistry Table T. Selected Radioisotopes Decay Name Notation Symbol Nuclide Half-Life Mode 4 alpha particle 2 He or H y beta particle (electron) gamma radiation neutron proton positron 0-1e or C 5730 y 0 N 7.2 s 0 n n Ne 17.2 s H or 1 p p 24 Na 15 h 0 1e or Mg 9.5 min 32 P 14.3 d Table U. Constants Used in Nuclear Chemistry Constant Value mass of an electron (m e ) amu mass of a proton (m p ) amu mass of a neutron (m n ) amu Bequerel (Bq) 1 disintegration/second Curie (Ci) 3.7 x Bq Figure V. Neutron/Proton Stability Band 36 Cl y 37 K 1.23 s + 40 K y + 42 K 12.4 h 37 Ca s 51 Cr 27.7 d 53 Fe 8.51 min 59 Fe 46.3 d 60 Co 5.26 y 85 Kr y 87 Rb y 90 Sr 28.1 y 99 Tc 2.13 x 10 5 y 131 I 8.07 d 137 Cs y 153 Sm 1.93 d 198 Au 2.69 d 222 Rn 3.82 d 220 Fr 27.5 s 226 Ra 1600 y 232 Th 1.4 x y 233 U 1.62 x 10 5 y 235 U 7.1 x 10 8 y 238 U 4.51 x 10 9 y 239 Pu 2.44 x 10 4 y 241 Am 432 y

8 Chemistry Reference Tables p. 8 Table W. Activity Series Metals Reacts with cold H 2 O and acids, replacing hydrogen. Reacts with O 2, forming oxides. Reacts with steam (not cold H 2 O) and acids, replacing hydrogen. Reacts with O 2, forming oxides. Does not react with H 2 O. Reacts with acids, replacing hydrogen. Reacts with O 2, forming oxides. Reacts with O 2, forming oxides. Fairly unreactive, forming oxides only indirectly. Arrows indicate direction from LEAST to MOST active elements. An element can replace any element below itself on the activity series. Note that the order of elements in the activity series is similar to, though not quite identical with, the order of elements/ions in the table of Std. Reduction Potentials (Table X). Table X. Std. Reduction Potentials Nonmet als Half-Reaction E 0 (V) Cs F 2 Li + + e Li(s) Rb Cl 2 Cs + + e Cs(s) K Br 2 Rb + + e Rb(s) 2.98 Na I 2 K + + e K(s) Li Ba e Ba(s) Ba Sr e Sr(s) Sr Ca e Ca(s) Ca Na + + e Na(s) 2.71 Mg Mg e Mg(s) Be Be e Be(s) 1.85 Al Al e Al(s) 1.66 Mn Mn e Mn(s) Zn Cr 2 H 2 O + 2 e H 2 (g) + 2 OH Fe Zn e Zn(s) Cd Cr e Cr(s) 0.74 Co Fe e Fe(s) 0.44 Ni Cr 3+ + e Cr Sn Cd e Cd(s) 0.40 Pb Co e Co(s) 0.28 H 2 Ni e Ni(s) 0.25 Sb Sn e Sn(s) 0.13 Bi Pb e Pb(s) 0.13 Cu 2 H e H 2 (g) Ag S(s) + 2 H e H 2 S(g) Hg Sn e Sn Au Cu 2+ + e Cu Pt Cu e Cu(s) Cu + + e Cu(s) I 2 (s) + 2 e 2 I Fe 3+ + e Fe Ag + + e Ag(s) Hg e 2 Hg(l) Hg e Hg(l) Hg e Hg Br 2 (l) + 2 e 2 Br Pt e Pt(s) O 2 (g) + 4 H e 2 H 2 O Cl 2 (g) + 2 e 2 Cl Au e Au(s) Co 3+ + e Co F 2 (g) + 2 e 2 F E o values at 1M concentration and 1 atm.

9 Chemistry Reference Tables p. 9 Table Y. Selected Properties of the Elements # symbol element name mass (IUPAC 2005) Melting Point, C Boiling Point, C density g/ml electroneg ativity (Pauling) 1 st ionization potential (kj/mol) Electron Affinity (kj/mol) radius (pm) 89 Ac actinium Al aluminum common oxidation states 95 Am americium ,4,5,6 51 Sb antimony ,5 18 Ar argon < As arsenic ±3,+5 85 At astatine Ba barium Bk berkelium ,4 4 Be beryllium < Bi bismuth ,5 107 Bh bohrium B boron Br bromine ±1,+5 48 Cd cadmium < Ca calcium Cf californium C carbon ±4 58 Ce cerium ,4 55 Cs cesium Cl chlorine Cr chromium ,2,6 27 Co cobalt ,3 112 Cn copernicum Cu copper ,1 96 Cm curium Ds darmstadtium Db dubnium Dy dysprosium Es einsteinium Er erbium Eu europium ,2 100 Fm fermium F fluorine Fr francium Gd gadolinium Ga gallium Ge germanium ,2 79 Au gold ,1 72 Hf hafnium Hs hassium He helium < Ho holmium H hydrogen ±1 49 In indium I iodine ,+5,7 77 Ir iridium ,3,6 26 Fe iron ,2

10 Chemistry Reference Tables p. 10 # symbol element name mass (IUPAC 2005) Melting Point, C Boiling Point, C density g/ml electroneg ativity (Pauling) 1 st ionization potential (kj/mol) Electron Affinity (kj/mol) radius (pm) 114 Fl flerovium Kr krypton < La lanthanum Lr lawrencium common oxidation states 82 Pb lead ,4 116 Lv livermorium Li lithium Lu lutetium Mg magnesium < Mn manganese < ,3,4,6,7 109 Mt meitnerium Md mendelevium ,2 80 Hg mercury < ,1 42 Mo molybdenum ,3,5 60 Nd neodymium Ne neon < Np neptunium ,3,4,6 28 Ni nickel ,3 41 Nb niobium ,3 7 N nitrogen < No nobelium ,3 76 Os osmium ,6,8 8 O oxygen Pd palladium ,4 15 P phosphorus Pt platinum ,2 94 Pu plutonium ,3,5,6 84 Po polonium ,2 19 K potassium Pr praseodymium ,4 61 Pm promethium Pa protactinium ,4 88 Ra radium Rn radon < Re rhenium ,4,6 45 Rh rhodium ,4,6 111 Rg roentgentium Rb rubidium Ru ruthenium ,3,6,8 104 Rf rutherfordium Sm samarium ,2 21 Sc scandium Sg seaborgium Se selenium ,2,+6 14 Si silicon ±4 47 Ag silver Na sodium Sr strontium

11 Chemistry Reference Tables p. 11 # symbol element name mass (IUPAC 2005) Melting Point, C Boiling Point, C density g/ml electroneg ativity (Pauling) 1 st ionization potential (kj/mol) Electron Affinity (kj/mol) radius (pm) 16 S sulfur Ta tantalum common oxidation states 43 Tc technetium ,4,6 52 Te tellurium ,6,2 65 Tb terbium ,4 81 Tl thallium ,3 90 Th thorium Tm thulium ,2 50 Sn tin ,2 22 Ti titanium ,3,2 74 W tungsten ,4 118 Uuo ununoctium Uup ununpentium Uut ununtrium U uranium ,3,4,5 23 V vanadium ,2,3,4 54 Xe xenon < Yb ytterbium ,2 39 Y yttrium Zn zinc < Zr zirconium Figure Z. Bonding Triangle EN average electronegativity EN electronegativity difference

12 Chemistry Reference Tables p. 12 Table AA. Bond Dissociation Energies & Bond Lengths Values given are homolytic bond dissociation energies, meaning that the electrons are divided equally between the two atoms. Hydrogen Compounds Group IVA Compounds Group VA Compounds Bond D r D r D r Bond Bond (kj/mol) (pm) (kj/mol) (pm) (kj/mol) (pm) H H C C N N H B C = C N = N H C C C N N H Si C Si N O H Ge C Ge N = O H Sn C Sn N F H N C Pb N Cl H P C N P P H As C = N P O H O C N P = O H S C P P = S H Se C O P F H Te C = O P Cl H F C O P Br 264? H Cl C B 356? P I 184? H Br C S As As H I C = S As O C F As F C Cl As Cl Group VIIA Compounds C Br As Br Bond D r C I As I (kj/mol) (pm) Si Si Sb Sb 121? F F Si N 355? Sb F 440? Cl Cl Si O Sb Cl (5) 248? Br Br Si S Sb Cl (3) I I Si F At At 116? Si Cl I O 201? Si Br Group VIA Compounds I F Si I D r Bond I Cl Ge Ge (kj/mol) (pm) I Br 175? Ge N 257? O O Ge F O = O Ge Cl O F Group IIIA Compounds Ge Br S = O Bond D r Ge I 212? S S (8 ) (kj/mol) (pm) Sn F 414? S = S B B 293? Sn Cl S F B O 536? Sn Br S Cl B F 613? Sn I Se Se 172? B Cl Pb F 331? Se = Se B Br 377? Pb Cl Pb Br 201? Pb I

13 Chemistry Reference Tables p. 13 Table BB. Thermodymanic Data Standard enthalpy of formation ( ) & standard entropy ( S ) for selected compounds. Note that standard H f enthalpy values are in kilojoules per mole, whereas entropy values are in joules per mole Kelvin. Substance State Δ ( H f kj ) mol S J ( ) K Substance State Δ ( H f kj ) mol S J ( ) K Substance State Δ ( H f kj ) mol S J ( ) K mol mol mol Ag s Cr 2 O 3 g MnO 2 s Ag + aq Cu s N 2 g AgCl s Cu + aq NH 3 g AgBr s Cu +2 aq NH 4 aq AgNO 3 s CuO s NO 2 aq Al s Cu 2 O s NO 3 aq Al +3 aq Cu(OH) 2 s N 2 H 4 l AlCl 3 s CuS s NH 4 Cl s Al 2 O 3 s Cu 2 S s NH 4 NO 3 s Al(OH) 3 s 1277 CuSO 4 s NO g Ba s F aq NO 2 g BaCl 2 s F 2 g N 2 O g BaCO 3 s Fe s N 2 O 4 g Ba(NO 3 ) 2 s Fe(OH) 3 s Na s BaO s FeO s Na + aq Ba(OH) 2 s Fe 2 O 3 s Na 2 CO 3 s BaSO 4 s Fe 3 O 4 s NaHCO 3 s Be s 0 10 FeSO 4 s NaCl s BeO s H 2 g NaF s Br 2 l H + aq NaNO 3 s Br aq HBr g NaOH s C s HCO 3 aq Ni s CCl 4 l HCl g NiCl 2 s CHCl 3 l HF g NiO s CH 4 g HI g OH aq C 2 H 2 g HNO 3 aq O 2 g C 2 H 4 g HPO 4 aq P 4 s C 2 H 6 g HSO 4 aq PCl 3 g C 3 H 8 g H 2 O l PCl 5 g CH 3 OH l H 2 O g PH 3 g C 2 H 5 OH l H 2 PO 4 aq PO 4 aq C 6 H 12 O 6 s H 2 S g Pb s CO g Hg l Pb +2 aq CO 2 g Hg +2 aq PbBr 2 s aq HgO cr PbCl 2 s Ca s I aq PbO s Ca +2 aq I 2 s PbO 2 s CaCl 2 s K s PbS s CaCO 3 s K + aq PbSO 4 s CaO s KBr s S s Ca(OH) 2 s KCl s SO 2 g Ca 3 (PO 4 ) 2 s KClO 3 s SO 3 g CO 3 2 CaSO 4 s KClO 4 s SO 4 aq Cd s KNO 3 s S - 2 aq Cd +2 aq Mg s Si s CdCl 2 s Mg +2 aq SiO 2 s CdO s MgCl 2 s Sn s Cd(OH) 2 s MgCO 3 s Sn +2 aq CdS s MgO s SnO 2 s CdSO 4 s Mg(OH) 2 s Zn s Cl 2 g MgSO 4 s Zn +2 aq Cl aq Mn s ZnI 2 s ClO 4 aq Mn +2 aq ZnO s Cr s MnO s ZnS s

14 Chemistry Reference Tables p. 14 Table CC. Some Common & Equivalent Units and Approximate Conversions Some Common & Equivalent Units Length 1 in (inch) = 2.54 cm 12 in = 1 ft (foot) 3 ft = 1 yd (yard) 5,280 ft = 1 mi (mile) = 1,760 yd Mass 1 lb (pound) = 16 oz ~ 454 g 1 ton = 2000 lb 1 tonne = 1000 kg Volume 1 pinch = 8 teaspoon 3 teaspoons = 1 tablespoon (Tbsp) 2 tablespoons = 1 ounce 8 oz. (ounces) = 1 cup 2 cups = 1 pint 2 pints = 1 quart 4 quarts = 1 gallon Some APPROXIMATE Conversions Length 1 cm ~ width of a small paper clip 6 in ~ length of a (US) dollar bill 1 ft ~ 30 cm 1 m ~ 1 yd 1 mi ~ 1.6 km 0.6 km ~ 1 mi Volume 1 pinch ~ 8 teaspoon 1 ml ~ 10 drops 1 teaspoon (tsp) ~ 5 ml ~ 60 drops 1 tablespoon (Tbsp) = 3 tsp ~ 15 ml 2 Tbsp. = 1 fl. oz. ~ 30 ml 1 C (cup) = 8 fl. oz. ~ 250 ml 1 qt (quart) ~ 1 L Mass 1 small paper clip ~ 1 gram (g) 1 nickel (5 coin) ~ 5 g 1 oz ~ 30 g 1 pound (lb) = 16 oz ~ 0.5 kg 1 ton = 2000 lb ~ 1 tonne Speed 60 mi / h ~ 100 km / h ~ 30 m / s Density air ~ 1 g / L water ~ 1 g / ml ~ 8 lb / gal ~ 1 tonne / m 3 ~ 1 ton / yd 3

15 Chemistry Reference Tables p. 15 Table DD. Selected Formulas and Equations M Density V D D = density M = mass V = volume 1 mol = [molar mass] g (molar mass = formula weight = gram formula mass) Mole Conversions 1 mol = 22.4 L of gas at 0 C and 1 atm 1 mol = molecules, atoms, or particles measured value- accepted value Percent Error % error *100% accepted value mass of part Percent Composition % composition *100% mass of whole moles of solute (moles of solute)(dissociation factor) molarity ( M ) normality ( N ) liter of solution liter of solution moles of solute Concentration molality ( m) kg of solvent moles of A mole fraction ( ) grams of solute parts per million (ppm) 1,000, 000 A total moles grams of solvent P1 V1 P2 V2 P = pressure n = moles Gases T1 T2 V = volume (L) T = temperature (K) Pressure Titration Colligative Properties PV = nrt R L atm LkPa 4 Ltorr molk molk molk 1 atm = kpa = 760 torr = 760 mm Hg = in. Hg = bar = 14.7 psi P A = χ A P T P A = partial pressure of A χ A = mole fraction of A P T = P A + P B + P C + P T = total pressure N A V A = N B V B N = normality of H O + A 3 V A = volume of acid N = normality of OH B V B = volume of base T f = imk f T f = freezing point depression ( C) T b = boiling point elevation ( C) K f = freezing point depression constant (H 2 O = 0.52 C/m) T b = imk b K b = boiling point elevation constant (H 2 O = 1.86 C/m) i = van t Hoff factor (dissociation factor) π = osmotic pressure π = im RT = N RT m = molality M = molarity (mol/l) N = normality (mol/l) R = ideal gas constant T = temperature (K) Acid-Base ph = log[h 3 O + ] [H 3 O ][A ] Ka pk a = log(k a ) poh = log[oh ] [HA] base ph pk a log ph + poh = 14 [H B][OH ] acid K b pk b = log(k b ) K w = K a K b = [B] Equilibrium K p = K c (RT) Δn K p = gas press. K c = molar conc. Δn = change in equil. const. equil. const. # moles q = m C p T q = heat T = change in temperature Heat q = m H f m = mass H f = heat of fusion q = m H v C p = specific heat capacity H v = heat of vaporization Thermodynamics ΔG = ΔH TΔS G = standard free energy S = standard entropy ΔG = RT ln K H = standard enthalpy T = temperature (K) q = charge q I = current (amperes) t = time (seconds) I (Coulombs) Electrochemistry t F = Faraday s constant = 96,000 Coulomb per mole electrons ΔG = nfe n = moles of electrons E = standard reduction potential Temperature K = C K = Kelvin C= ( F32) * 5/9 C = degrees Celsius F = degrees Fahrenheit Radioactive Decay A A t 1 ½ o 2 A = amount left A o = original amount t = total elapsed time τ ½ = half-life number of half-lives = t ½