Chemistry Reference Tables

Chemistry Reference Tables Name Value Avogadro s number 6.0 10 particles/mole 0.081 L atm mole K Gas constant (R) 6. L mmhg mole K 8.1 L kpa mole K Standard pressure 1.00 atm = 101. kpa = 760. mmhg = 760. torr Standard temperature 0C or 7K Volume of 1 mole of any gas at STP. L Thermodynamic Constants Symbol Value (.18 J = 1 cal) Heat of fusion of water Heat of vaporization of water Specific heat of water H f (water) H v (water) C p (water) J/g,60 J/g.05 J for ice,.0 J for steam, g C g C.18 J for liquid g C Metal Specific Heat J g C Density (g/cm ) Melting Point ( C) Aluminum 0.897.70 660 Copper 0.85 8.9 108 Gold 0.19 19.1 106 Iron 0.9 7.86 155 Lead 0.19 11.7 8 Magnesium 1.0 1.7 69 Mercury 0.10 1.599 9 Nickel 0. 8.90 155 Titanium 0.5.5 1660 Zinc 0.88 7.1 0 NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page 1

Organic Substances Name Density Melting Point ( C) Boiling Point ( C) Ethanol (CH CH OH) Glucose (C H O ) 6 1 6 Hexane (C H ) 6 1 Methane (CH ) Methanol (CH OH) Sucrose (C H O ) 1 11 0.789 g/cm 119 79 1.5 g/cm 86 Decompose 0.660 g/cm 95 69 0.716 g/l 18 16 0.791 g/cm 9 65 1.7 g/cm 86 Decompose Inorganic Substances Name *Density @ STP Melting Point ( C) Boiling Point ( C) Chlorine.1 g/l 101 5 Hydrogen 0.0899 g/l 59 5 Hydrogen chloride 1.60 g/l 115 85 Hydrogen sulfide 1.5 g/l 85 61 Nitrogen 1.5 g/l 10 196 Nitrogen monoxide 1. g/l 16 15 Oxygen 1. g/l 18 18 Sodium carbonate Sodium chloride.5 g/cm 851 Decomposes.165 g/cm 801 11 Sulfur dioxide.9 g/l 7 10 *Water (at C) 1.00 g/cm 0 100 NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page

Formulas D = m D = density V K = C + 7 m = mass PV T PV = V = volume T 1 1 t 1 P = P + P + P + K = Kelvin M V 1... = M V P = pressure 1 1 PV = nrt R = gas constant M = moles of solute T = temperature liters of solution q = mc p ΔT M = molarity q = mh v n = number of moles q = mh f q = quantity of heat energy ph + poh = 1 C p = specific heat ph = log[ H + ] H v = heat of vaporization poh = log[ OH ] H f = heat of fusion K = [ H ][ OH ] = 1 10 w [H ] = 10 + ph [OH ] = 10 E=hν c=λν + 1 poh K w = equilibrium constant for the ionization of water E = energy of a photon h = Planck s constant = 6.66 x 10 - Js ν = frequency of light c = speed of light =.00 x 10 8 m/s λ = wavelength of light 1 m = 10 9 nm NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page

NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page 56 Ba Barium 17.8 55 Cs Cesium 1 57 La Lanthanum 18.91 7 Hf Hafnium 178.9 7 Ta Tantalum 180.95 7 W Tungsten 18.8 75 Re Rhenium 186.1 76 Os Osmium 190. 77 Ir Iridium 19. 88 Ra Radium (6) 87 Fr Francium () 89 Ac Actinium (7) 10 Rf Rutherfordium (61) 105 Db Dubnium (6) 106 Sg Seaborgium (6) 107 Bh Bohrium (6) 108 Hs Hassium (69) 109 Mt Meitnerium (68) 7 Rb Rubidium 85.7 5 Rh Rhodium 10.91 Ru Ruthenium 101.07 Tc Technetium (98) Mo Molybdenum 95.9 1 Nb Niobium 9.91 0 Zr Zirconium 91. 9 Y Yttrium 88.91 8 Sr Strontium 87.6 0 Ca Calcium 0.08 19 K Potassium 9.10 1 Sc Scandium.96 Ti Titanium 7.88 V Vanadium 50.9 Cr Chromium 59 5 Mn Manganese 5.9 6 Fe Iron 55.85 7 Co Cobalt 58.9 1 Mg Magnesium.1 11 Na Sodium.99 IVB 5 VB 6 VIB 7 VIIB 8 VIIIB 9 VIIIB IIIB Be Beryllium 9.01 Li Lithium 6.91 1 H Hydrogen 1.008 IIA 1 IA 91 Pa Protactinium 1.0 90 Th Thorium.0 9 U Uranium 8.0 9 Np Neptunium (7) 9 Pu Plutonium () 95 Am Americium () 96 Cm Curium (7) 59 Pr Praseodymium 10.91 58 Ce Cerium 10.1 60 Nd Neodymium 1. 61 Pm Promethium (15) 6 Sm Samarium 150.6 6 Eu Europium 156 6 Gd Gadolinium 157.5 PERIODIC TABLE

NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page 5 78 Pt Platinum 195.08 79 Au Gold 196.97 80 Hg Mercury 00.59 81 Tl Thallium 0.8 8 Pb Lead 07. 8 Bi Bismuth 08.98 8 Po Polonium (09) 85 At Astatine (10) 86 Rn Radon () 110 Ds Darmstadtium (71) 111 Rg Roentgenium (7) 11 Uub Ununbium (77) 8 Cd Cadmium 11.1 7 Ag Silver 107.87 6 Pd Palladium 106. 5 Xe Xenon 1 5 I Iodine 16.90 5 Te Tellurium 17.60 51 Sb Antimony 11.76 50 Sn Tin 118.71 9 In Indium 11.8 8 Ni Nickel 58.69 9 Cu Copper 6.55 0 Zn Zinc 65.9 1 Ga Gallium 69.7 Ge Germanium 7.61 As Arsenic 7.9 Se Selenium 78.96 5 Br Bromine 79.90 6 Kr Krypton 8.80 18 Ar Argon 9.95 17 Cl Chlorine 5.5 16 S Sulfur.07 15 P Phosphorus 0.97 1 Si Silicon 8.09 1 Al Aluminum 6.98 10 VIIIB 11 IB 1 IIB 5 B Boron 10.81 6 C Carbon 1.01 7 N Nitrogen 1.01 8 O Oxygen 16.00 9 F Fluorine 19.00 10 Ne Neon 0.18 He Helium.00 17 VIIA 1 IIIA 1 IVA 15 VA 16 VIA 18 VIIIA 97 Bk Berkelium (7) 98 Cf Californium (51) 99 Es Einsteinium (5) 100 Fm Fermium (57) 101 Md Mendelevium (58) 10 No Nobelium (5) 10 Lr Lawrencium (6) 65 Tb Terbium 158.9 66 Dy Dysprosium 16.50 67 Ho Holmium 16.9 68 Er Erbium 167.6 69 Tm Thulium 168.9 70 Yb Ytterbium 17.0 71 Lu Lutetium 17.97 OF THE ELEMENTS

SOLUBILITY RULES Soluble: All Nitrates, Acetates, Ammonium, and Group 1 (IA) salts All Chlorides, Bromides, and Iodides, except Silver, Lead, and Mercury(I) All Fluorides except Group (IIA), Lead(II), and Iron(III) All Sulfates except Calcium, Strontium, Barium, Mercury, Lead(II), and Silver Insoluble (0.10 M or greater): All Carbonates and Phosphates except Group 1 (IA) and Ammonium All Hydroxides except Group 1 (IA), Strontium, Barium, and Ammonium All Sulfides except Group 1 (IA), (IIA), and Ammonium All Oxides except Group 1 (IA) Guidelines for Predicting the Products of Selected Types of Chemical Reaction Key: M = Metal NM = Nonmetal 1. SYNTHESIS: a. Formation of binary compound: A + B AB b. Metal oxide-water reactions: MO + H O base c. Nonmetal oxide-water reactions: (NM)O + H O acid. DECOMPOSITION: a. Binary compounds: AB A + B b. Metallic carbonates: MCO MO + CO c. Metallic hydrogen carbonates: MHCO MO+ H O (l) + CO (g) d. Metallic hydroxides: MOH MO + H O e. Metallic chlorates: MClO MCl + O f. Oxyacids decompose to nonmetal oxides and water: acid (NM)O + H O. SINGLE REPLACEMENT: a. Metal-metal replacement: A + BC AC + B b. Active metal replaces H from water: M + H O MOH + H c. Active metal replaces H from acid: M + HX MX + H d. Halide-Halide replacement: D + BC BD + C. DOUBLE REPLACEMENT: AB + CD AD + CB a. Formation of a precipitate from solution b. Acid-Base neutralization reaction 5. COMBUSTION REACTION Hydrocarbon + oxygen carbon dioxide + water NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page 6

ACTIVITY SERIES of Halogens: F Cl Br I ACTIVITY SERIES of Metals Li Rb K Ba Sr Ca Na Mg Al Mn Zn Cr Fe Cd Co Ni Sn Pb [ H ] Sb Bi Cu Hg Ag Pt Au Replace hydrogen from cold water Replace hydrogen from steam Replace hydrogen from acids React with oxygen to form oxides + NH BrO CN CHO (CHCOO ) ClO ClO ClO ClO IO MnO NO NO OH HCO HSO SCN CO CrO 7 CrO SO SO PO Polyatomic Ions Ammonium Bromate Cyanide Acetate Perchlorate Chlorate Chlorite Hypochlorite Iodate Permanganate Nitrate Nitrite Hydroxide Hydrogen carbonate Hydrogen sulfate Thiocyanate Carbonate Dichromate Chromate Sulfate Sulfite Phosphate Boling Point Elevation and Freezing Point Depression ΔT = i K b m ΔT = i K f m i = van't Hoff factor Substance K b ( C/m ) K f ( C/m ) benzene.5 5.1 camphor 5.95 0 carbon tetrachloride 5.0 0 ethyl ether water.0 0.5 1.79 1.86 NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page 7

Bohr Model for Hydrogen Atom (measurement in nanometers) n = 6 n = 5 n = n = n = E=hν h = 6.66 x 10 - Js c=λν c =.00 x 10 8 m/s 1 m = 10 9 nm n = 1 UV = Ultraviolet IR = Infrared 18 656 1 97 1875 86 109 10 10 IR Visible UV Electromagnetic Spectrum (measurement in meters) 10 10 10 10 1 10 0 10 1 10 10 10 10 5 10 6 10 7 10 8 10 9 10 10 10 11 10 1 10 1 Microwaves X rays Radio waves Infrared Ultraviolet Gamma rays Longer Wavelength Visible Light Shorter Wavelength Red Orange Yellow Green Blue Violet 7.0 10 7 6.5 10 7 5.9 10 7 5.7 10 7.9 10 7. 10 7.0 10 7 NCDPI Reference Tables for Chemistry (October 006 form A-v1) Stock No. 10569 Page 8

Common Polyatomic Ions +1-1 - - + ammonium C H O - - NH acetate CO - carbonate PO + - H O - hydronium hypochlorite chromate PO ClO - ClO - ClO - chlorite chlorate dichromate sulfate ClO - perchlorate sulfite CN - cyanide peroxide NO - NO - HCO - OH - MnO - nitrate C O - nitrite hydrogen carbonate (bicarbonate) hydroxide permanganate CrO Cr O - 7 SO - SO - O - oxalate phosphate phosphite Prefixes Used in Naming Common Metal Ions Binary Molecular Compounds Ion Systematic Common Name Name Prefix Number Fe + iron (II) ferrous mono 1 Fe + iron (III) ferric di Cu + copper (I) cuprous tri Cu + copper (II) cupric tetra Pb + lead (II) plumbous penta 5 Pb + lead (IV) plumbic hexa 6 Cr + chromium (II) chromous hepta 7 Cr + chromium (III) chromic octa 8 Sn + tin (II) stannous nona 9 Sn + tin (IV) stannic deca 10 Co + cobalt (II) cobaltous Co + cobalt (III) cobaltic + Hg mercury (I) mercurous Hg + mercury (II) mercuric ** ALWAYS: Zn +, Ag +, Cd + **

Periodic Table with Electronegativities 1A A B B 5B 6B 7B 8B 1B B A A 5A 6A 7A 8A 1 H.1 He Li 1.0 Be 1.5 5 B.0 6 C.5 7 N.0 8 O.5 9 F.0 10 Ne 11 Na 0.9 1 Mg 1. 1 Al 1.5 1 Si 1.8 15 P.1 16 S.5 17 Cl.0 18 Ar 19 K 0.8 0 Ca 1.0 1 Sc 1. Ti 1.5 V 1.6 Cr 1.6 5 Mn 1.5 6 Fe 1.8 7 Co 8 Ni 9 Cu 0 Zn 1.6 1 Ga 1.6 Ge 1.8 As.0 Se. 5 Br.8 6 Kr.0 7 Rb 0.8 8 Sr 1.0 9 Y 1. 0 Zr 1. 1 Nb 1.6 Mo 1.8 Tc Ru. 5 Rh. 6 Pd. 7 Ag 8 Cd 1.7 9 In 1.7 50 Sn 1.8 51 Sb 5 Te.1 5 I.5 5 Xe.6 55 Cs 0.7 56 Ba 0.9 57 La 1.1 7 Hf 1. 7 Ta 1.5 7 W 1.7 75 Re 76 Os. 77 Ir. 78 Pt. 79 Au. 80 Hg 81 Tl 1.8 8 Pb 8 Bi 8 Po.0 85 At. 86 Rn. 87 Fr 0.7 88 Ra 0.9 89 Ac 1.1 10 Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 Ds 111 Uuu 11 Uub 11 Uut 11 Uuq 115 Uup 116 Uuh 58 Ce 1.1 59 Pr 1.1 60 Nd 1.1 61 Pm 1. 6 Sm 1. 6 Eu 1.1 6 Gd 1. 65 Tb 1. 66 Dy 1. 67 Ho 1. 68 Er 1. 69 Tm 1. 70 Yb 1. 71 Lu 1. 90 Th 1. 91 Pa 1.5 9 U 1.7 9 Np 1. 9 Pu 1. 95 Am 1. 96 Cm 1. 97 Bk 1. 98 Cf 1. 99 Es 1. 100 Fm 1. 101 Md 1. 10 No 1.5 10 Lr Type of bond Electronegativity difference Nonplar covalent bond Polar covalent bond Ionic bond 0 to 0. 0.5 to 1.7 1.8 and above

150 10 10 10 110 100 0 90 ::c "' O'J 80 0 0... 70 - ~ ::::J 0 60 UI... 0 UI E <U... (.!) 50 0 0 0 10 Solubility Curve I v v / - Kl/ / / ) ~/ v, /j / I ------, gases - NaN0 '---v J solids. v I \ /... / / v / KN0....t j...... HCI. NHCI"" ' "'l. I /.... ~, I /"" \......, ' I / NH..., NaS~ ~ I/ --. ',,... ~...- ' / ~ - ~ KC!>- / I y - '"/ - --- -. - ~KC I0...... - _,,,.........,,,_... ~ " - ' NaCl / / /........ ~ --- - -.....,, so... - 1 -- --.,. - - - ----- -.; --- 0 0 10 0 0 0 50 60 70 80 90 100 Temperature ( C)

Table H Vapor Pressure of Four Liquids 00 propanone ethanol 150 water Vapor Pressure (kpa) 100 101. kpa ethanoic acid 50 0 0 5 50 75 100 15 Temperature ( C) Reference Tables for Physical Setting/CHEMISTRY

Thermodynamic Quan ti ties for Selected Substances at 98.15 K (5 C) Substance Aluminum Al(s) AlClJ(s) Al0J(s) Barium Ba(s) BaC0 (s) BaO(s) Beryllium Be(s) BeO(s) Be(OHh(s) Bromine Br(g) Br-(aq) Br(g) Br(1) HBr(g) Calcium Ca(g) Ca(s) CaC0 (s, calcite) CaC1(s) CaF(s) CaO(s) Ca(OHh(s) CaS0(s) Carbon C(g) C(s, diamond) C(s, graphite) CC1(g) CC1(1) illfo I!::.GJ 50 illfo I!::.GJ 50 (kj/mol) (kj/mol) O/mol-K) Substance (kj/mol) (kj/mol) O/mol-K) CF(g) -679.9-65.1 6. 0 0 8. CH(g) -7.8-50.8 186. -705.6-60.0 109. CH(g) 6.7 09. 00.8-1669.8-1576.5 51.00 CH(g) 5.0 68.11 19. CH5(g) -8.68 -.89 9.5 0 0 6. C H 8 (g) -10.85 -.7 69.9-116. -117.6 11.1 CH1o(g) -1.7-15.71 10.0-55.5-55.1 70. CH10U) -17.6-15.0 1.0 C5H5(g) 8.9 19.7 69. C 6 H 6 (1) 9.0 1.5 17.8 0 0 9. -608. -579.1 1.77 CH 0H(g) -01. -16 7.6-905.8-817.9 50.1 CH 0H(Z) -8.6-166. 16.8 CH 5 0H(g) -5.1-168.5 8.7 CH 5 0H(l) -77.7-17.76 160.7 111.8 8.8 17.9 C5H1P5(s) -17.0-910. 1.1-10.9-10.8 80.71 CO(g) -110.5-17. 197.9 0.71.1 5. C0(g) -9.5-9. 1.6 0 0 15. HCH 0(1) -87.0-9. 159.8-6. -5. 198.9 Cesium Cs(g) 76.50 9.5 175.6 179. 15.5 15.8 Cs(s) 0 0 85.15 0 0 1. CsCl(s) -.8-1. 101. -107.1-118.76 9.88 Chlorine -795.8-78.1 10.6 Cl(g) 11.7 105.7 165. -119.6-1167. 68.87 Ci-(aq) -167. -11. 56.5-65.5-60.17 9.75 Cl(g) 0 0.96-986. -898.5 8. HCl(aq) -167. -11. 56.5-1.0-11.8 106.7 HCl(g) -9.0-95.7 186.69 Chromium 718. 67.9 158.0 Cr(g) 97.5 5.6 17. 1.88.8. Cr(s) 0 0.6 0 0 5.69 Cr0 (s) -119.7-1058.1 81. -106.7-6.0 09. -19. -68.6 1.

100 Appendix C / Thermodynamic Quantities for Selected Substances at 98.15 K (5 C) illfo f1go so M:I/!:t.GJ so f 'f Substance (kj/mol) (kj/mol) (J/mol-K) Substance (kj/mol) (kj/mol) (J/mol-IO Cobalt Magnesium Co(g) 9 9 179 Mg(g) 17.1 11.5 18.6 Co(s) 0 0 8. Mg(s) 0 0.51 MgClz(s) -61.6-59.1 89.6 Copper MgO(s) -601.8-569.6 6.8 Cu(g) 8. 98.6 166. Mg(OHh(s) -9.7-8.7 6. Cu(s) 0 0.0 CuClz(s) -05.9-161.7 108.1 Manganese CuO(s) -156.1-18..59 Mn(g) 80.7 8.5 17.6 Cu0(s) -170.7-17.9 9.6 Mn(s) 0 0.0 MnO(s) -85. -6.9 59.7 Fluorine Mn0(s) -519.6-6.8 5.1 F(g) 80.0 6 158.7 Mn0-(aq) -51. -7. 191. p-(aq) -.6-78.8-1.8 F(g) 0 0 0.7 Mercury HF(g) -68.61-70.70 17.51 Hg(g) 60.8 1.76 17.89 Hg(l) 0 0 77.0 Hydrogen HgC1(s) -0.1-18.0 1.5 H(g) 17.9 0.6 11.60 HgCl(s) -6.9-10.5 19.5 H+(aq) 0 0 0 H+(g) 156. 1517.0 108.9 Nickel H(g) 0 0 10.58 Ni(g) 9.7 8.5 18.1 Ni(s) 0 0 9.9 Iodine NiC1(s) -05. -59.0 97.65 l(g) 106.60 70.16 180.66 NiO(s) -9.7-11.7 7.99 r(aq) -55.19-51.57 111. l(g) 6.5 19.7 60.57 Nitrogen 1(s) 0 0 116.7 N(g) 7.7 55.5 15. Hl(g) 5.9 1.0 06. Nz(g) 0 0 191.50 NH (aq) -80.9-6.50 111. Iron NH (g) -6.19-16.66 19.5 Fe(g) 15.5 69.8 180.5 NH/(aq) -1.5-79.1 11. Fe(s) 0 0 7.15 Fe +(aq) -87.86-8.9 11. Nz~(g) 95.0 159. 8.5 Fe +(aq) -7.69-10.5 9. NHCN(s) 0.0 FeC1(s) -1.8-0. 117.9 N~Cl(s) -1. -0.0 9.6 NHN0(s) -65.6-18.0 151 FeC1 (s) -00-1. NO(g) 90.7 86.71 10.6 FeO(s) -7-55. 60.75 Fez0 (s) -8.16-70.98 89.96 N0 (g).8 51.8 0.5 Fe0(s) -1117.1-101. 16. NzO(g) 81.6 10.59 0.0 FeS(s) -171.5-160.1 5.9 Nz0(g) 9.66 98.8 0. NOCl(g) 5.6 66. 6 Lead HNOJ{aq) -06.6-110.5 16 Pb(s) 0 0 68.85 HN0(g) -1. -7.9 66. PbBr(s) -77. -60.7 161 PbC0(s) -699.1-65.5 11.0 Oxygen Pb(N0 )i(aq) -1. -6.9 0. O(g) 7.5 0.1 161.0 Pb(N0)z(s) -5 0(g) 0 0 05.0 PbO(s) -17. -187.9 68.70 0(g) 1. 16. 7.6 OH-(aq) -0.0-157. -10.7 Lithium H0(g) -1.8-8.57 188.8 Li(g) 159. 16.6 18.8 HzO(l) -85.8-7.1 69.91 Li(s) 0 0 9.09 Hz0(g) -16.10-105.8.9 u+(aq) -78.5-7. 1. H0(l) -187.8-10. 109.6 u+(g) 685.7 68.5 1.0 LiCl(s) -08. -8.0 59.0

Appendix C I Thermodynamic Quantities for Selected Substances at 98.15 K (5 C) 101 i Substance AH/ A.Gl so tjlo A.Gl S (kj/mod (kj/mol) (J/mol-IO Substance (kj/mol) (kj/mol) (J/mol-:K) Phosphorus Sodium P(g) 16. 80.0 16. Na(g) 107.7 77. 15.7 P(g) 1. 10.7 18.1 Na(s) 0 0 51.5 P(g) 58.9. 80 Na+(aq) -0.1-6 59.0 P(s, red) -17.6-1.0.85 Na+(g) 609. 57. 18.0 Pis, white) 0 0 1.08 NaBr(aq) -60.6-6.7 11 PC1(g) -88.07-69.6 11.7 NaBr(s) -61. -9. 86.8 PClJ(l) -19.6-7. 17 NaCOJ(s) -110.9-107.7 16.0 PF 5 (g) -159. -150.7 00.8 NaCl(aq) -07.1-9.0 115.5 PH(g) 5. 1. 10. NaCl(g) -181. -01. 9.8 PP6(s) -160.1 NaCl(s) -10.9-8.0 7. P01 0 (s) -90.1-675. 8.9 NaHCOJ(s) -97.7-851.8 10.1 POC1(g) -5. -50.5 5 NaN0 (aq) -6. -7. 07 POC1(1) -597.0-50.9 NaNOJ(s) -67.9-67.0 116.5 HP0(aq) -188. -11.6 158. NaOH(aq) -69.6-19. 9.8 NaOH(s) -5.6-79.5 6.6 Potassium K(g) 89.99 61.17 160. Strontium K(s) 0 0 6.67 SrO(s) -59.0-56 5.9 KCl(s) -5.9-08. 8.7 Sr(g) 16. 110.0 16.6-91. KC10(s) KCl0 (aq) -9.5-89.9-8.9 1.0 65.7 Sulfur S(s, rhombic) 0 0 1.88-96.9-00. 8.5 K0(s) S0(g) -95. -70. 56. KOi(s) -8.5-0.6 1.5 sol-(aq) -909. -7.5 0.1 KN0(s) -9.70-6. -9.1 -.1 88.1 9.1 S0(g) K0i(s) -95.8-9.8 11.0 SOC!i(l) -5.6 KOH(s) -.7-78.9 78.91 KOH(aq) -8. -0.5 91.6 HS(g) -0.17 -.01 05.6 H S0(aq) -909. -7.5 0.1 Rubidium HS0(1) -81.0-689.9 156.1 Rb(g) 85.8 55.8 170.0 Rb(s) 0 0 76.78 Titanium RbCl(s) -0.5-1.0 9 Ti(g) 68 180. ;_ RbC10(s) -9. -9.0 15 Ti(s) 0 0 0.76 TiC1(g) -76. -76.8 5.9 Scandium TiClil) -80. -78.1 Sc(g) 77.8 6.1 17.7 Ti0(s) -9.7-889. Sc(s) 0 0.6 50.9 Vanadium Selenium V(g) 51. 5.1 18. HSe(g) 9.7 15.9 19.0 V(s) 0 0 8.9 Silicon Zinc Si(g) 68..9 167.8 Zn(g) 10.7 95. 160.9 Si(s) 0 0 18.7 Zn(s) 0 0 1.6 SiC(s) -7. -70.85 16.61 ZnC1(s) -15.1-69. 111.5 SiC~(l) -60.1-57.8 9. ZnO(s) -8.0-18..9 Si0(s, quartz) -910.9-856.5 1.8 Silver Ag(s) 0 0.55 Ag+(aq) 105.90 77.11 7.9 AgCl(s) -17.0-109.70 96.11 Ag0(s) -1.05-11.0 11. AgN0(s) -1. -.1 10.9 f