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Chemistry dât tables
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Transcript of Chemistry dât tables
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Appendix E
MHR 595
Appendix E
Table E.4 Conversion Factors
Quantity Relationships between units
length
mass
temperature
volume
pressure
energy
bp of H 2O = 373 .15 K (100 C)
1 m = 10 3 km
1 pm = 10 12 m
1 u = 1.66 10 27 kg
1 kg = 10 3 g
T (C) = T (K) 273.15
mp of H 2O = 273.15 K (0 C)
= 10 3 mL
1 mL = 1 cm3
= 10 3 g/mL= 1 g/L
1 J = 6.24 1018 eV
= 10 2 cm= 10 3 mm
= 10 3 t
0 K = 273.15 C
T (K) = T (C) + 273.15
= 10 3 m31 L = 1 dm 3
1 kg/m 3 = 10 3 g/m 3
= 760 mm Hg= 760 torr= 1 atm
101 325 Pa = 101.325 kPa
density
Chemistry Data TablesTable E.1 Useful Math Relationships
Table E.2 Fundamental Physical Constants (to sixsignicant digits)
Table E.3 Common SI Prexes
tera (T) 1012
giga (G) 109
mega (M) 106
kilo (k) 103
deci (d) 10 1
centi (c) 10 2
milli (m) 10 3
micro ( ) 10 6
nano (n) 10 9
pico (p) 10 12
9.806 65 m/s 2
6.022 14 1023/mol
9.109 38 10 31 kg
1.674 93 10 27 kg
1.672 62 10 27 kg
8.314 47 J/mol K
22.414 0 L/mol
2.997 92 108 m/s
1.660 54 10 27 kg
mass of electron ( m s)
mass of neutron ( m n)
mass of proton ( m p)
molar gas constant ( R
molar volume of gas at STPspeed of light in vacuo ( c
unified atomic mass ( u
acceleration due to gravity ( g
Avogadro constant ( N a)
charge on one mole ofelectrons (Faraday constant)
96 485.3 C/mol
)
)
)
)
D = mV
P =F
A
= 3.1416
Volume of sphere V = 43 r 3
Volume of cylinder = r2h
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596 MHR
Appendix E
Table E.6 Summary of Naming Rules for Ions
Table E.7 Summary of Naming Rules for Acids
Modern name ExampleClassical acid nameaqueoushydrogen ___ide
hydro___ic acid
HNO2, aqueoushydrogen nitriteor nitrous acid
HCl, aqueoushydrogen chlorideor hydrochloric acid
H2CO3, aqueoushydrogen carbonateor carbonic acid
___ic acid
___ous acidaqueoushydrogen ___ite
aqueoushydrogen ___ate
Type of ion ExamplePrefix or suffix
if the ion is the mostcommon oxoanion
-ate chlorate, ClO3
if the ion has the higherpossible charge
cuprous, Cu+
if the ion has one Oatom less than the mostcommon oxoanion
-ite
-ous
if the ion has two Oatoms less than the mostcommon oxoanion
if the ion has 1 Oatom more than themost common oxoanion
if the ion has 1 H atomadded to the mostcommon oxoanion
if the ion has 1 O atomless and 1 S atom morethan the most commonoxoanion
hypo-___-ite
per-___-ate
bi-
thio-
-ic
if the ion has the lowerpossible charge
chlorite, ClO2
hypochlorite,ClO
perchlorate,ClO4
bicarbonate,HCO3
thiosulphate,S2O32
titanic, Ti4+
Note: According to theStock system, metallicions are named usingRoman numerals.
The Romannumeral showsthe charge onthe metal ion
titanium(IV) Ti 4+copper(I), Cu+manganese(VII),
Mn 7 +
Polyatomic Ions
Metallic Ions
Table E.5 Alphabetical Listing of Common Polyatomic Ions
acetate
ammonium
arsenate
benzoate
borate
bromate
carbonate
Most common ion
CH3COO
NH4+
AsO 43
C6H5COO
BO33
BrO33
CO32
Common related ions
arsenite
tetraborate
AsO 33
B4O72
HCO3 bicarbonate
(hydrogencarbonate)
perchloratechloritehypochlorite
peroxide
iodide
nitrite
dichromate
cyanatethiocyanate
ClO4
ClO2
ClO
Cr2O72
glutamate
hydroxide
iodate
nitrate
oxalate
permanganate
phosphate
O2
2
I
NO2
OCN
SCN
C5H8NO4
OH
IO3
NO3
OOCCOO 2
MnO 4
PO43 phosphite
tripolyphosphate
ClO3chlorate
chromate
cyanide
CrO42
CN
PO33
P3O105
SO42sulfate
bisulfide(hydrogensulfide)
HSO4
SO32
HSO3
S2O32
bisulfate(hydrogensulfate)sulfite
bisulfite(hydrogensulfite)thiosulfate
S2sulfide HS
silicate
stearate
SiO32
C17H35COO
orthosilicate SiO44
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Appendix E
MHR 597
Table E.8 Standard Molar Enthalpies of Formation
Note: The enthalpy of formation of an element in itsstandard state is de ned as zero.
Table E.9 Ionization Constants for Acids
c o n t i n u e d
acetic acid
benzoic acid
chlorous acid
cyanic acid
formic acid
Acid Formula Conjugate base K a
CH3COOH
C6H5COOH
HClO 2HOCN
HCHO 2
HBr
CH3COO
C6H5COO
ClO2
OCN
CHO2
Br
1.8 10 5
6.3 105
1.1 10 2
3.5 10 4
1.8 10 4
1.0 109
1.3 106hydrochloricacid
hydrobromicacid
HCl Cl
hydrocyanicacid
hydrofluoricacid
hydrogen oxide
hypobromousacid
H2O
HOBr
HCN
HF
CN
OH
BrO
F
6.2 10 10
2.8 10 9
6.3 10 4
1.0 10 14
Al2O3(s)CaCO3(s)CaCl2(s)Ca(OH)2(s)CCl4( )CCl4(g)CHCl3( )CH4(g)C2H2(g)C2H4(g)C2H6(g)C3H8(g)C6H6( )CH3OH ( )
C2H5OH ( )CH3COOH ( )CO(g)CO2(g)COCl2(g)CS2( )CS2(g)CrCl3(s)Cu(NO 3)2(s)CuO (s)CuCl (s)
CuCl 2(s)
H
f(kJ/mol)Substance
1675.7 1207.6
795.4985.2128.2
95.7134.1
74.6+227.4
+ 52.4 84.0
103.8+ 49.1
239.2
277.6484.3110.5393.5219.1
+ 89.0+116.7556.5302.9157.3137.2
220.1
Substance
HBr(g)HCl(g)HF (g)HCN(g)H2O( )H2O(g)H2O2( )HNO 3( )H3PO4(s)H2S(g)H2SO4( )FeO (s)Fe2O3(s)Fe3O4(s)
FeCl 2(s)FeCl 3(s)FeS 2(s)PbCl 2(s)MgCl2(s)MgO(s)Mg(OH)2(s)HgS(s)NaCl (s)NaOH (s)Na2CO3(s)
36.3 92.3
273.3+ 135.1 285.8 241.8 187.8 174.1
1284.4 20.6
814.0 272.0 824.2
1118.4
341.8 399.5 178.2 359.4 641.3 601.6 924.5
58.2 411.2 425.6
1130.7
H
f(kJ/mol) Substance
NH3(g)N2H4( )NH4Cl(s)NH4NO3(s)NO(g)NO2(g)N2O(g)N2O4(g)PH3(g)PCl3(g)P4O6(s)P4O10(s)KBr(s)KCl(s)
KClO3(s)KOH(s)Ag2CO3(s)AgCl(s)AgNO 3(s)Ag2S(s)SF6(g)SO2(g)SO3(g)SnCl 2(s)SnCl 4( )
45.9+ 50.6
314.4365.6
+ 91.3+ 33.2+ 81.6+ 11.1
+ 5.4287.0
2144.3 2984.0
393.8436.5
397.7424.6505.8127.0124.4
32.6 1220.5
296.8395.7325.1511.3
H
f(kJ/mol)
Table E.10 Ionization Constants for Polyprotic Acids
Table E.11 Ionization Constants for Nitrogen Bases
1,2-diaminoethane(ethylenediamine)
Base FormulaConjugate
acid K b
dimethylamine(N-methylmeth-anamine)
NH2CH2CH2NH2 NH2CH2
(CH3)2NH
8.4 105
5.4 104(CH3)2NH2+
CH2NH3+
ethanamine
methanaminetrimethylamine(N-N-dimethyl-methanamine)
C2H5NH2
CH3NH2(CH3)3N
C2H5NH3+
CH3NH3+
(CH3)3NH+
4.5 104
4.6 104
6.4 105
ammonia
hydrazine
hydroxylamine
pyridine
aniline
urea
NH3N2H4NH2OH
C5H5N
C6H5NH2NH2CONH 2
NH4+
N2H5+
NH3OH+
C5H5NH+
C6H5NH3+
NH2CONH 3+
1.8 105
1.3 106
8.8 109
1.7 109
7.5 1010
1.3 1014
boric acid(aqueoushydrogen borate)
Acid Formula Conjugate base K a
5.4 10 10
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598 MHR
Appendix E
Table E.12 Solubility Product Constants in Water at 25 C
Table E.13 Standard Reduction Potentials
c o n t i n u e d
F2(g) + 2e 2F (aq)
Co3+ (aq) + e Co2+ (aq)
H2O2(aq) + 2H+
(aq) + 2e 2H2O( )
Ce4+ (aq) + e Ce3+ (aq)
PbO 2(s) + 4H+
(aq) + SO42
(aq) + 2e PbSO 4(s) + H2O( )
MnO 4
(aq) + 8H+
(aq) + 5e Mn 2+ (aq) + 4 H2O( )
Au 3+ (aq) + 3e Au (s)
PbO 2(s) + 4H+
(aq) + 2e Pb2+ (aq) + 2H2O( )
Cl2(g) + 2e 2Cl (aq)Cr2O72
(aq) + 14H
+(aq) + 6e
2Cr3+ (aq) + 7H2O( )O2(g) + 4H
+(aq) + 4e
2H2O( )MnO 2(s) + 4H
+(aq) + 2e
Mn 2+ (aq) + 2 H2O( )IO3
(aq) + 6H
+(aq) + 6e
I (aq) + 3 H2O( )Br2( ) + 2e
2Br (aq)AuCl 4
(aq) + 3e
Au (s) + 4Cl
(aq)
NO3
(aq) + 4H+
(aq) + 3e NO (g) + 2 H2O( )
2Hg2+ (aq) + 2e Hg22
+(aq)
Reduction half reaction E
(V)
2.866
1.92
1.776
1.72
1.691
1.507
1.498
1.455
1.358
1.232
1.229
1.224
1.085
1.066
1.002
0.957
0.920
AgBrCuBr
PbBr 2
AgBrO 3TlBrO 3
Ag2CO3BaCO3CaCO3MgCO3PbCO 3
AgClCuCl
Ag2CrO4BaCrO4PbCrO
4
AgCNCuCN
BaF2CdF2CaF2FeF 2
Bromides
Carbonates
Chlorides
Chromates
Cyanides
Fluorides
5.38 10 51.10 10 4
5.35 10 136.27 10 9
6.60 10 6
8.46 10 122.58 10 93.36 10 96.82 10 67.40 1014
1.77 10 101.72 10 9
1.12 10 121.12 10 10
2.3 1013
5.97 10 173.47 10 20
1.84 10 76.44 10 33.45 10 112.36 10 6
4.01 10 9
6.47 10 6
1.14 107
1.12 10 10
AlPO 4Ca3(PO4)2Co3(PO4)2Cu3(PO4)2Ni3(PO4)2
Ba(IO3)2Ca(IO3)2Sr(IO 3)2Y(IO3)3
CuIPbI2AgI
1.27 10 129.8 10 9
8.52 10 17
9.84 10 212.07 10 332.05 10 351.40 10 374.74 10 32
BaSO4CaSO4Hg2SO4
1.08 10 104.93 10 5
6.5 10 7
CuSCNPd(SCN) 2
1.08 10 134.39 10 23
Iodides
Phosphates
Sulfates
Thiocyanates
Ca(OH)2Co(OH)2Eu(OH) 3Fe(OH) 2
Fe(OH) 3Pb(OH) 2Mg(OH)2Ni(OH) 2Sn(OH) 2Zn(OH) 2
5.02 10 65.92 10 159.38 10 274.87 10 17
2.79 103 9
1.43 10 205.61 10 125.48 10 165.45 10 27
3 10 17
Iodates
Hydroxides
Be(OH)2Cd(OH) 2
6.92 10 227.2 10 15
Bromates Ag+ (aq) + e Ag(s)
Hg22+
(aq) + 2e 2Hg( )
Fe3+ (aq) + e Fe2+ (aq)
O2(g) + 2H+
(aq) + 2e H2O2(aq)
I2(s) + 2e 2I (aq)
Cu+ (aq) + e Cu (s)O2(g) + 2H2O( ) + 4e
4OH (aq)Cu2+ (aq) + 2e
Cu (s)AgCl(s) + e
Ag(s) + Cl
(aq)
4H + (aq) + SO42
(aq) + 2e H2SO3(aq) + H2O( )
Cu2+ (aq) + e Cu + (aq)
2H + (aq) + 2e H2(g)
Fe3+ (aq) + 3e Fe (s)
Pb2+ (aq) + 2e Pb (s)
Sn 2+ (aq) + 2e Sn (s)
Ni2+ (aq) + 2e Ni (s)
Cd2+ (aq) + 2e Cd (s)Cr3+ (aq) + e
Cr2+ (aq)Fe2+ (aq) + 2e
Fe (s)Cr3+ (aq) + 3 e
Cr(s)Zn 2+ (aq) + 2e
Zn (s)2H2O( ) + 2e
H2(g) + 2OH
(aq)
Al3+ (aq) + 3e Al (s)
Mg2+ (aq) + 2e Mg(s)
La3+ (aq) + 3e La(s)
Na+ (aq) + e Na (s)
Ca2+ (aq) + 2e Ca(s)
Ba2+ (aq) + 2e Ba(s)
K+ (aq) + e K(s)
Li+ (aq) + e Li(s)
0.800
0.797
0.771
0.695
0.536
0.5210.401
0.342
0.222
0.172
0.153
0.000 0.037 0.126 0.138 0.257 0.403 0.407 0.447 0.744 0.762 0.828 1.662 2.372 2.379 2.711 2.868 2.912 2.931 3.040
Reduction half reaction E
(V)
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Appendix E
MHR 599
Table E.14 Speci c Heat Capacities of VariousSubstances
Table E.15 Average Bond Energies
c o n t i n u e d
HH
HC
HN
HO
HF
HSi
HP
HS
HCl
HBr
HI
HMg
436
338
339
460
570
299
297
344
432
366
298
126
Energy(kJ/mol)Bond
CC
CN
CO
CF
CSi
CP
CS
CCl
CBr
CI
347
305
358
552
305
264
259
397
280
209
Energy(kJ/mol)Bond
NN
NO
NF
NSi
NP
NS
NCl
NBr
NI
160
201
272
330
209
464
200
276
159
Energy(kJ/mol)Bond
PP
PS
PF
PCl
PBr
PI
SS
SF
SCl
SBr
SI
210
444
490
331
272
184
266
343
277
218
170
Energy(kJ/mol)Bond
Hydrogen Carbon NitrogenPhosphorusand sulfur
SubstanceSpecific heat capacity
(J/g C at 25 C)
aluminum
carbon (graphite)
copper
gold
hydrogen
iron
ammonia (liquid)
ethanol
water (solid)
water (liquid)
water (gas)
0.900
0.711
0.385
0.129
14.267
0.444
4.70
2.46
2.01
4.184
2.01
Element
Compound
Other material
air
concrete
glass
granite
wood
1.02
0.88
0.84
0.79
1.76
Note: The values in this table represent average valuesfor the dissociation of bonds between the pairs of atomslisted. The true values may vary for different molecules.
Table E.16 Average Bond Lengths
Note: The values in this table are average values. Thelength of a bond may be slightly different in differentmolecules, depending on the intramolecular forceswithin the molecules.
HH
HC
HN
HO
74
109
101
96
Length(pm)Bond
CC
CN
CO
CF
154
147
143
133
Length(pm)Bond
NN
NO
NF
NSi
146
144
139
172
Length(pm)Bond
PP
PS
PF
PCl
221
210
156
204
Length(pm)Bond
Hydrogen Carbon NitrogenPhosphorusand sulfur
HF
HSi
HP
HSHCl
HBr
HI
HMg
OO
OF
OSi
OP
OS
OCl
OBr
OI
92
148
142
134127
141
161
173
CSi
CP
CS
CClCBr
CI
186
187
181
177194
213
NP
NS
NCl
NBrNI
177
168
191
214222
PBr
PI
SS
SFSCl
SBr
SI
222
243
204
158201
225
234
148
142
161
160
151
164
172
194
SiSi
SiP
SiS
SiF
SiCl
SiBr
SiI
234
227
210
156
204
216
240
FCl
FBr
FI
ClBr
ClI
BrI
FF
ClCl
BrBr
II
166
178
187
214
243
248
143
199
228
266
C
C
C
N
N
O
C
C
C
N
134
127
123
122
120
121
121
115
113
110
Oxygen Silicon Halogens Multiple bonds
O
C
N
O
N
O
C
N
O
N
OO
OF
OSi
OP
OS
OCl
OBr
OI
204
222
368
351
265
269
235
249
SiSi
SiP
SiS
SiF
SiCl
SiBr
SiI
Si
226
364
226
553
381
368
293
640
FCl
FBr
FI
ClBr
ClI
BrI
FF
ClCl
Br Br
II
256
280
272
217
211
179
159
243
193
151
C
C
C
N
N
O
C
C
C
N
607
615
745
418
631
498
839
891
1077
945
Oxygen Silicon Halogens Multiple bonds
O
C
N
O
N
O
O
C
N
O
N
Energy(kJ/mol)Bond
Energy(kJ/mol)Bond
Energy(kJ/mol)Bond
Energy(kJ/mol)Bond
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