MOLAR ROAD MAP

# of atoms
N
𝑎𝑡𝑜𝑚𝑠
𝑥
𝑚𝑜𝑙𝑒𝑐𝑢𝑙𝑒
𝑎𝑡𝑜𝑚𝑠
÷
𝑚𝑜𝑙𝑒𝑐𝑢𝑙𝑒

# of particles
N m

x NA
xM
÷ NA ÷M
qrxn
x H

 H
÷F
MOLES
qelecton = It

xF

PV = RT
xV
x VM
÷V
÷ VM

Vgas
c or [solution]

LIST OF MOLAR EQUATIONS

𝑁
𝑁𝑎𝑡𝑜𝑚𝑠 = 𝑁𝑚𝑜𝑙𝑒𝑐𝑢𝑙𝑒𝑠 𝑥 𝑁𝑎𝑡𝑜𝑚𝑠 𝑝𝑒𝑟 𝑚𝑜𝑙𝑒𝑐𝑢𝑙𝑒 𝜂=
𝑁𝐴
𝐼𝑡 𝑉 𝑚
𝜂𝑒 − = 𝜂= 𝜂=
𝐹 𝑉𝑚 𝑀

𝑞𝑟𝑥𝑛 = 𝜂∆𝐻 PV=RT 𝜂 = 𝑐𝑉

SCH CHEMICAL EQUATIONS & CONSTANTS

POTENTIALLY USEFUL EQUATIONS:

|𝑇ℎ𝑒𝑜𝑟𝑒𝑡𝑖𝑐𝑎𝑙 − 𝐴𝑐𝑡𝑢𝑎𝑙| 𝐸𝑌
Percent Error %𝐸 = 𝑥100 Reaction Yield 𝑅𝑌 = × 100
𝑇ℎ𝑒𝑜𝑟𝑒𝑡𝑖𝑐𝑎𝑙 𝑇𝑌

∑(𝑚𝑖𝑠𝑜𝑡𝑜𝑝𝑒 )(%𝐴𝑏𝑢𝑛𝑑𝑎𝑛𝑐𝑒)
Average Atomic Mass 𝐴𝐴𝑀 =
100

pH & Molarity 𝑝𝐻 = −log[𝐻3 𝑂+ ] [𝐻3 𝑂+ ] = 10−𝑝𝐻

Percent Composition 𝑚𝑒𝑙𝑒𝑚𝑒𝑛𝑡 𝑖𝑛 𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑

% 𝐶𝑜𝑚𝑝𝑜𝑠𝑖𝑡𝑖𝑜𝑛 = 𝑥100
(Mass Percent) 𝑚𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑

𝑎𝑚𝑜𝑢𝑛𝑡 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒
% 𝑠𝑜𝑙𝑢𝑡𝑒⁄𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 = 𝑥 100
𝑎𝑚𝑜𝑢𝑛𝑡 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛
Percentage Concentration
𝑚𝑠𝑜𝑙𝑢𝑡𝑒 𝑚𝑠𝑜𝑙𝑢𝑡𝑒
𝑝𝑝𝑚 = 𝑥106 𝑝𝑝𝑏 = 𝑥109
𝑚𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 𝑚𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛

% 𝑚/𝑚 𝑥 10 × 𝜌𝑠𝑜𝑙𝑢𝑡𝑒
Molar Conversion [𝑠𝑜𝑙𝑢𝑡𝑒] =
𝑀𝑠𝑜𝑙𝑢𝑡𝑒

𝑃𝑇𝑜𝑡𝑎𝑙 = ∑(𝑃𝑃𝑎𝑟𝑡 )𝑛 𝑃𝑇𝑜𝑡𝑎𝑙 = 𝑃𝐷𝑟𝑦 𝐴𝑖𝑟 + 𝑃𝑤𝑎𝑡𝑒𝑟 𝑣𝑎𝑝𝑜𝑢𝑟

Dalton’s Law of Partial
Pressures
𝑃𝑃𝑎𝑟𝑡 = (𝑃𝑇𝑜𝑡𝑎𝑙 )(%𝐶𝑜𝑚𝑝𝑜𝑠𝑖𝑡𝑖𝑜𝑛)

𝑚
Dilution 𝑐𝑉 = 𝑐2 𝑉2 Density  =
𝑉
−𝑏 ± √𝑏 2 − 4𝑎𝑐 𝑃𝑉 𝑃2 𝑉2
Quadratic Formula 𝑥= Combined Gas Law =
2𝑎 𝑇 𝑇2
∆𝑐
Calorimetry 𝑞𝑐𝑎𝑙 = 𝑚𝑐∆𝑇 Rate 𝑟=
∆𝑡

Hess’ Law ∆𝐻𝑡𝑎𝑟𝑔𝑒𝑡 = ∑ ∆𝐻𝑓𝑜 𝑝𝑟𝑜𝑑𝑢𝑐𝑡𝑠 − ∑ ∆𝐻𝑓𝑜 𝑟𝑒𝑎𝑔𝑒𝑛𝑡𝑠

POTENTIALLY USEFUL CONSTANTS & CONVERSIONS:

Avogadro’s Number 6.02 x 1023 particles/mol Faraday’s Constant 9.65 x 104 C/mol

𝑘𝑃𝑎𝐿
Temperature 𝐾 = ℃ + 273 Universal Gas Law 8.314
𝑚𝑜𝑙𝐾

Pressure 1 atm = 760 mmHg = 760 torr = 101.3 kPa = 1.01325 bar

STP 101.325 kPa & 273 K SATP 100 kPa & 298 K

Molar Volume @STP 22.4 L/mol @SATP 24.8 L/mol

SCH POLYATOMIC IONS & OXY-ACIDS

Common Polyatomic Ions:

ammonium 𝑁𝐻41+ cyanide 𝐶𝑁 1− chromate 𝐶𝑟𝑂42−

hydroxide 𝑂𝐻1− cyanate 𝑂𝐶𝑁1− dichromate 𝐶𝑟2 𝑂72−

permanganate 𝑀𝑛𝑂41− thiocyanate 𝑆𝐶𝑁 1− thiosulphate 𝑆2 𝑂32−

Main & Lesser Oxy-Acids & their Variant’s:

pernitric acid 𝐻𝑁𝑂4 pernitrate 𝑁𝑂41− Add one oxygen
nitric acid 𝑯𝑵𝑶𝟑 nitrate 𝑵𝑶𝟏−
𝟑

nitrous acid 𝐻𝑁𝑂2 nitrite 𝑁𝑂21− Remove one oxygen

1−
hyponitrous acid 𝐻𝑁𝑂 hyponitrite 𝑁𝑂 Remove two oxygen

carbonic acid 𝑯𝟐 𝑪𝑶𝟑 carbonate 𝑪𝑶𝟐−

𝟑 silicic acid 𝐻2 𝑆𝑖𝑂3 silicate 𝑆𝑖𝑂32−

chloric acid 𝑯𝑪𝒍𝑶𝟑 chlorate 𝑪𝒍𝑶𝟏−

𝟑 bromic acid 𝐻𝐵𝑟𝑂3 bromate 𝐵𝑟𝑂31−
iodic acid 𝐻𝐼𝑂3 iodate 𝐼𝑂31−
sulphuric acid 𝑯𝟐 𝑺𝑶𝟒 sulphate 𝑺𝑶𝟐−
𝟒

phosphoric acid 𝑯𝟑 𝑷𝑶𝟒 phosphate 𝑷𝑶𝟑−𝟒

*Note each main oxy-acid and lesser oxy-acid will form each of the variants.

Acid Salts & Organics:

dihydrogen phosphate 𝐻2 𝑃𝑂41− hydrogen sulphate 𝐻𝑆𝑂41−
hydrogen phosphate 𝐻𝑃𝑂42− hydrogen carbonate 𝐻𝐶𝑂31−

ethanoic acid (acetic acid) 𝐻𝐶2 𝐻3 𝑂2 or 𝐶𝐻3 𝐶𝑂𝑂𝐻 acetate 𝐶2 𝐻3 𝑂21− or 𝐶𝐻3 𝐶𝑂𝑂1−
*Note: the acid salts may contain any of the variants of the polyprotic oxy-acids.
SCH ORGANIC FUNCTIONAL GROUPS & PRIORITY

FUNCTIONAL GROUP
PRIORITY SUFFIX or PREFIX SIDE GROUP
NAME GENERAL FORMULA
Highest O
carboxylic acid C - oic acid
R OH

O
ester C - oate
1
R O R
O

amide C 1 - amide
R N R
2
R
O
aldehyde C - al
R H

O
ketone C - one
1
R R

alcohol R OH - ol hydroxy –
2
R
1
amine N R - amine amino –
R
O
ether R R
1
- oxy -

aromatic - benzene phenyl –

alkene C C - ene

alkyne C C - yne

alkane C C - ane alkyl –

X fluoro –
chloro –
Lowest haloalkane X is any halogen
C C bromo –
iodo –
 SOLUBILTY OF COMMON IONS IN WATER
ANION CATION *SOLUBILTIY
Alkali metals
1. Most hydrogen Soluble
ammonium
nitrate Most Soluble
2. Ag+ Insoluble
acetate
Most others Soluble
chloride Ag+, Pb2+, Hg2+, Cu+ Tl+ Insoluble
3. bromide
iodide All others Soluble
Mg2+, Ca2+, Ba2+, Pb2+ Insoluble
4. fluoride
Most others Soluble
Ca2+, Sr2+, Ba2+, Pb2+ Insoluble
5. sulphate
All others Soluble
Alkali metals, H+, NH4+, Be2+, Mg2+, Ca2+, Sr2+, Ba2+ Soluble
6. sulphide
All others Insoluble

Alkali metals, H+, NH4+, Sr2+, Ba2+, Tl+ Soluble

7. hydroxide
All others Insoluble

phosphate Alkali metals, H+, NH4+ Soluble

8. carbonate
sulphite All others Insoluble

Alkali metals, NH4+, Mg2+, Ca2+ Soluble

9. chromate
All others Insoluble
*Compounds listed as soluble have solubilities of at least 1 g / 100 mL of water at SATP.

COMMON EXPERIMENTAL ION COLOURATION

AQUEOUS COLOUR
ION CATION FLAME COLOUR
1.0 M 0.010 M
chromate yellow pale yellow boron(II) green
chromium(III) blue-green green calcium red
chromium(II) dark blue pale blue cesium violet
cobalt(II) red pink copper(II) bluish-green
copper(II) blue pale blue lithium red
copper(I) blue-green pale blue-green magnesium bright white
dichromate orange pale orange potassium violet
iron(III) orange-yellow pale yellow sodium yellow
iron(II) lime green colourless strontium red
manganese(II) pale pink colourless
permanganate deep purple purple-pink
 ACTIVITY SERIES FOR METALS

METAL DISPLACES HYDROGEN FROM… REACTIVITY

lithium most reactive
potassium
barium
calcium
sodium cold water
magnesium
aluminum
zinc
chromium
iron
cadmium
cobalt
nickel
lead acids
hydrogen
copper
mercury
silver
platinum
gold least reactive

ACTIVITY SERIES FOR HALOGENS

HALOGEN REACTIVITY

fluorine most reactive

chlorine

bromine

iodine least reactive

 STANDARD MOLAR ENTHALPIES OF FORMATION
CHEMICAL NAME FORMULA 𝛥𝐻𝑓𝑜 (𝑘𝐽⁄𝑚𝑜𝑙 ) CHEMICAL NAME FORMULA 𝛥𝐻𝑓𝑜 (𝑘𝐽⁄𝑚𝑜𝑙 )
1,2-dichloroethane C2H4Cl2(l) - 126.9 hexane C6H14(l) - 198.7
1,2-ethanediol C2H4(OH)2(l) - 454.8 N2H4(l) + 50.6
hydrazine
2,2,4-trimethylpentane C8H18(l) - 259.2 N2H4(g) + 95.4
acetone (CH3)2CO(l) – 248.1 hydrogen bromide HBr(g) - 36.3
aluminum oxide Al2O3(s) - 1675.7 hydrogen chloride HCl(g) - 92.3
ammonia NH3(g) - 45.9 hydrogen cyanide HCN(g) + 135.1
NH4Cl(s) - 314.4 hydrogen fluoride HF(g) - 273.2
ammonium chloride
NH4Cl(aq) - 299.7 hydrogen iodide HI(g) + 26.5
ammonium nitrate NH4NO3(s) - 365.6 hydrogen peroxide H2O2(l) - 187.8
barium carbonate BaCO3(s) - 1216.3 hydrogen sulfide H2S(g) - 20.6
barium hydroxide Ba(OH)2(s) - 944.7 iodine (vapour) I2(g) + 62.4
barium oxide BaO(s) - 553.5 iron(II) oxide FeO(s) - 272.0
barium sulfate BaSO4(s) - 1473.2 iron(II, III) oxide Fe3O4(s) - 1118.4
benzene C6H6(l) + 49.0 iron(III) oxide Fe2O3(s) - 824.2
bromine (vapour) Br2(g) + 30.9 iron(IV) sulfide FeS2(s) - 178.2
butane C4H10(g) - 125.6 lead(II) chloride PbCl2(s) - 359.4
calcium carbonate CaCO3(s) - 1206.9 lead(II) oxide PbO(s) - 219.0
calcium chloride CaCl2(s) - 795.8 lead(IV) oxide PbO2(s) - 277.4
calcium hydroxide Ca(OH)2(s) - 986.1 magnesium carbonate MgCO3(s) - 1095.8
calcium oxide CaO(s) - 634.9 magnesium chloride MgCl2(s) - 641.3
calcium sulfate CaSO4(s) - 1434.1 magnesium hydroxide Mg(OH)2(s) -924.5
carbon dioxide CO2(g) - 393.5 magnesium oxide MgO(s) - 601.6
carbon(IV) sulfide CS2(l) + 89.0 manganese(II) oxide MnO(s) - 385.2
carbon monoxide CO(g) - 110.5 manganese(IV) oxide MnO2(s) - 520.0
CCl4(l) - 128.2 mercury (vapour) Hg(g) + 61.4
carbon(IV) chloride
CCl4(g) - 95.7 mercury(II) oxide HgO(s) - 90.8
carbon(IV) sulfide CS2(g) + 116.7 mercury(II) sulfide HgS(s) - 58.2
chloroethene C2H3Cl(g) + 37.3 methanal (formaldehyde) CH2O(g) - 108.6
chromium(III) chloride CrCl3(g) - 556.5 methane CH4(g) - 74.4
chromium(III) oxide Cr2O3(s) - 1139.7 methanoic (formic) acid HCOOH(l) - 425.1
copper(I) chloride CuCl(s) - 137.2 methanol CH3OH(l) - 239.1
copper(I) oxide Cu2O(s) - 168.6 methoxymethane CH3OCH3(l) - 184.0
copper(I) sulfide Cu2S(s) - 79.5 methylpropane C4H10(g) - 134.2
copper(II) chloride CuCl2(s) - 220.1 nickel(II) oxide NiO(s) - 239.7
copper(II) nitrate Cu(NO3)2(s) - 302.9 nitric acid HNO3(l) - 174.1
copper(II) oxide CuO(s) - 157.3 nitrogen dioxide NO2(g) + 33.2
copper(II) sulfide CuS(s) - 53.1 nitrogen monoxide NO(g) + 90.2
cyclopropane C3H6(g) + 17.8 nitrogen(I) oxide N2O(g) + 81.6
dinitrogen tetroxide N2O4(g) + 11.1 nitromethane CH3NO2(l) - 113.1
ethane C2H6(g) - 83.8 octane C8H18(l) - 250.1
ethanoic (acetic) acid CH3COOH(l) - 432.8 ozone O3(g) + 142.7
C2H5OH(l) - 235.2 pentane C5H12(l) - 173.5
ethanol
C2H5OH(g) - 235.2 phenylethene (styrene) C6H5CHCH2(l) + 103.8
ethene (ethylene) C2H4(g) + 52.5 phosgene COCl2(g) - 219.1
ethyne (acetylene) C2H2(g) + 228.2 phosphoric acid H3PO4(s) - 1284.4
glucose C6H12O6(s) - 1273.1 phosphorous pentoxide P4O10(s) - 2984.0
 STANDARD MOLAR ENTHALPIES OF FORMATION
CHEMICAL NAME FORMULA 𝛥𝐻𝑓𝑜 (𝑘𝐽⁄𝑚𝑜𝑙 ) CHEMICAL NAME FORMULA 𝛥𝐻𝑓𝑜 (𝑘𝐽⁄𝑚𝑜𝑙 )
phosphorus(V) chloride PCl5(g) – 443.5 sodium hydroxide NaOH(s) - 425.6
PCl3(l) - 319.7 sodium iodide NaI(s) - 287.8
phosphorus(III) chloride
PCl3(g) - 287.0 sucrose C12H22O11(s) - 2225.5
phosphorus(III) hydride PH3(g) + 5.4 sulfur(IV) oxide SO2(g) - 296.8
potassium (liquid) K(l) + 2.3 SO3(l) - 441.0
sulfur(III) oxide
potassium bromide KBr(s) - 393.8 SO3(g) - 395.7
potassium chlorate KClO3(s) - 397.7 sulfuric acid H2SO4(l) - 814.0
potassium chloride KCl(s) - 436.7 sulfur(VI) fluoride SF6(g) - 1220.5
potassium hydroxide KOH(s) - 424.8 tetraphosphorous hexoxide P4O6(s) - 2144.3
propane C3H8(g) - 104.7 tin(II) chloride SnCl2(s) - 325.1
silicon dioxide SiO2(s) - 910.7 tin(II) oxide SnO(s) - 280.7
silver bromide AgBr(s) - 100.4 tin(IV) chloride SnCl4(l) - 511.3
silver carbonate Ag2CO3(s) - 505.8 tin(IV) oxide SnO2(s) - 577.6
silver chloride AgCl(s) - 127.0 trichloroethane CH3CHCl3(l) - 134.1
silver iodide AgI(s) - 61.8 trichloromethane CHCl3(l) - 134.1
silver nitrate AgNO3(s) - 124.8 urea CO(NH2)2(s) - 333.5
silver sulphide Ag2S(s) - 32.6 H2O(l) - 285.8
water
sodium bromide NaBr(s) - 361.1 H2O(g) - 241.8
sodium carbonate Na2CO3(s) - 1130.7 zinc oxide ZnO(s) - 350.5
sodium chloride NaCl(s) - 411.2 zinc sulfide ZnS(s) - 206.0

Specific Heat Capacities at SATP

ELEMENTS c (𝑘𝐽⁄𝑘𝑔℃) ELEMENTS c (𝑘𝐽⁄𝑘𝑔℃) COMPOUNDS c (𝑘𝐽⁄𝑘𝑔℃) MIXTURES c (𝑘𝐽⁄𝑘𝑔℃)
aluminum 0.897 magnesium 1.017 ammonia (liquid) 4.70 air 1.01

carbon (graphite) 0.709 mercury 0.138 ammonia (vapour) 2.06 concrete 0.88

calcium 0.653 nickel 0.444 ethanol 2.44 glass 0.84

copper 0.385 potassium 0.753 ice, H2O(s) 2.01 granite 0.79

gold 0.129 silver 0.237 water, H2O(l) 4.184 wood 1.26

hydrogen 14.267 sodium 1.226 steam, H2O(g) 2.01

iron 0.444 sulfur 0.732

lead 0.159 tin 0.213

lithium 3.556 zinc 0.388 Note: 1.0 kJ/kgoC = 1.0 J/goC

 SOLUBILITY PRODUCT CONSTANTS (Ksp @ SATP)

NAME FORMULA Ksp NAME FORMULA Ksp

aluminum phosphate AlPO4 9.84 x 10-21 lead(II) chloride PbCl2 1.2 x 10-5
barium carbonate BaCO3 2.58 x 10-9 lead(II) chromate PbCrO4 2.3 x 10-13
barium chromate BaCrO4 1.12 x 10-10 lead(II) hydroxide Pb(OH)2 1.43 x 10-12
barium fluoride BaF2 1.84 x 10-7 lead(II) iodate Pb(IO3)2 3.7 x 10-13
barium iodate Ba(IO3)2 4.01 x 10-9 lead(II) iodide PbI2 9.8 x 10-9
barium sulphate BaSO4 1.08 x 10-10 lead(II) sulphate PbSO4 1.8 x 10-8
beryllium hydroxide Be(OH)2 6.92 x 10-22 lead(II) thiocyanate Pb(SCN)2 4.39 x 10-23
cadmium fluoride CdF2 6.44 x 10-3 magnesium carbonate MgCO3 6.82 x 10-6
cadmium hydroxide Cd(OH)2 7.2 x 10-15 magnesium fluoride MgF2 6.4 x 10-9
calcium carbonate CaCO3 3.36 x 10-9 magnesium hydroxide Mg(OH)2 5.61 x 10-12
calcium fluoride CaF2 3.45 x 10-11 mercury(I) chloride HgCl 1.5 x 10-18
calcium hydroxide Ca(OH)2 5.02 x 10-6 mercury(I) sulphate Hg2SO4 6.5 x 10-7
calcium iodate Ca(IO3)2 6.47 x 10-6 nickel(II) hydroxide Ni(OH)2 5.48 x 10-16
calcium oxalate CaC2O4 2.3 x 10-9 nickel(II) phosphate Ni3(PO4)2 4.74 x 10-32
calcium phosphate Ca3(PO4)2 2.07 x 10-33 silver acetate AgC2H3O2 1.94 x 10-3
calcium sulphate CaSO4 4.93 x 10-5 silver bromate AgBrO3 5.38 x 10-5
cobalt(II) hydroxide Co(OH)2 5.92 x 10-15 silver bromide AgBr 5.35 x 10-13
cobalt(II) phosphate Co3(PO4)2 2.05 x 10-35 silver carbonate Ag2CO3 8.46 x 10-12
copper(I) bromide CuBr 6.27 x 10-9 silver chloride AgCl 1.77 x 10-10
copper(I) chloride CuCl 1.72 x 10-9 silver chromate Ag2CrO4 1.12 x 10-12
copper(I) cyanide CuCN 3.47 x 10-20 silver cyanide AgCN 5.97 x 10-17
copper(I) iodide CuI 1.27 x 10-12 silver iodate AgIO3 3.2 x 10-8
copper(I) thiocyanate CuSCN 1.08 x 10-13 silver iodide AgI 8.52 x 10-17
copper(II) iodate Cu(IO3)2 6.9 x 10-8 strontium carbonate SrCO3 5.6 x 10-10
copper(II) phosphate Cu3(PO4)2 1.40 x 10-37 strontium fluoride SrF2 4.3 x 10-9
copper(II) sulphide CuSO4 6.0 x 10-37 strontium iodate Sr(IO3)2 1.14 x 10-7
europium(III) hydroxide Eu(OH)3 9.38 x 10-27 strontium sulphate SrSO4 3.4 x 10-7
iron(II) fluoride FeF2 2.36 x 10-6 thallium(I) bromate TlBrO3 1.10 x 10-4
iron(II) hydroxide Fe(OH)2 4.87 x 10-17 tin(II) hydroxide Sn(OH)2 5.45 x 10-27
iron(II) sulphide FeSO4 6.0 x 10-19 yttrium iodate Y(IO3)3 1.12 x 10-10
iron(III) hydroxide Fe(OH)3 2.79 x 10-39 zinc hydroxide Zn(OH)2 3 x 10-17
lead(II) bromide PbBr2 6.60 x 10-6 zinc sulphide ZnSO4 2.0 x 10-25
lead(II) carbonate PbCO3 7.40 x 10-14
 ACID & BASE IONIZATION CONSTANTS (Ka & Kb @ SATP)
MONOPROTIC ACIDS WEAK BASES
FORMULA
NAME Ka NAME BASE FORMULA Kb
ACID CONJUGATE BASE
perchloric acid HClO4 𝐶𝑙𝑂41− very large N-methylmethanamine)
(CH3)2NH 5.4 x 10-4
aqueous hydrogen iodide HI(aq) I1- very large (dimethylamine)
aqueous hydrogen bromide HBr(aq) Br1- very large methanamine CH3NH2 4.6 x 10-4
aqueous hydrogen chloride HCl(aq) Cl1- very large ethanamine CH3CH2NH2 4.5 x 10-4
nitric acid HNO3 𝑁𝑂31− very large 1,2-diaminoethane
NH2(CH2)2NH2 8.4 x 10-5
hydronium ion H3O1+ H2O(l) 1 (ethylenediamine)
hydrofluoric acid HF(aq) F1- 6.3 x 10-4 N,N-dimethylmethanamine
(CH3)3N 6.4 x 10-5
nitrous acid HNO2 𝑁𝑂21− 5.6 x 10-4 (trimethyl amine)
hydrogen cyanate HOCN OCN1- 3.5 x 10-4 ammonia NH3 1.8 x 10-5
methanoic acid HCHO2 𝐶𝐻𝑂21− 1.8 x 10-4 hydrazine N2H4 1.3 x 10-6
methyl orange HMo Mo1- ~ 10-4 hydroxylamine NH2OH 8.8 x 10-9
benzoic acid C6H5COOH C6H5COO1- 6.3 x 10-5 pyridine C5H5N 1.7 x 10-9
ethanoic acid HC2H3O2 𝐶2 𝐻3 𝑂21− 1.8 x 10-5 aniline C6H5NH2 7.5 x 10-10
bromothymol blue HBb Bb1- ~ 10-7 urea NH2CONH2 1.3 x 10-14
hypochlorous acid HClO ClO1- 4.0 x 10-8
phenolphthalein HPh Ph1- ~ 10-10
Note: All bases gain one hydrogen to become (1+) cation.
hydrocyanic acid HCN(aq) CN1- 6.2 x 10-10
ammonium ion 𝑁𝐻41+ NH3 5.6 x 10-10
boric acid H3BO3 𝐻2 𝐵𝑂31− 5.8 x 10-10
phenol C6H5OH C6H5O1- 1.0 x 10-10
hydrogen peroxide H2O2 H2O1- 2.2 x 10-12
water H2O OH1- 1.0 x 10-14
hydroxide ion OH1- O2- very small
POLYPROTIC ACIDS
FORMULA EQUILIBRIUM CONSTANT
NAME
ACID CONJUGATE BASE Ka1 Ka2 Ka3
sulphuric acid H2SO4 𝐻𝑆𝑂41− very large 1.0 x10-2
oxalic acid H2C2O4 𝐻𝐶2 𝑂41− 5.6 x 10-2 7.2 x 10-5
sulphurous acid (SO2 + H2O) H2SO3 𝐻𝑆𝑂31− 1.4 x 10-2 very small
phosphoric acid H3PO4 𝐻2 𝑃𝑂41− 6.9 x 10-3 6.2 x 10-8 4.8 x 10-13
citric acid H3C6H5O7 𝐻2 𝐶6 𝐻5 𝑂71− 7.4 x 10-4 1.7 x 10-5 4.0 x 10-7
ascorbic acid C6H8O6 𝐶6 𝐻7 𝑂61− 9.1 x 10-5 2.0 x 10-12
carbonic acid (CO2 + H2O) H2CO3 𝐻𝐶𝑂31− 4.5 x 10-7 4.7 x 10-11
aqueous hydrogen sulphide H2S(aq) HS1- 8.9 x 10-8 6.3 x 10-8
 STANDARD REDUCTION POTENTIALS @ SATP

Reducing Reducing
Oxidizing Agents 𝑬𝒐𝒓 (𝑽) Oxidizing Agents 𝑬𝒐𝒓 (𝑽)
Agents Agents
𝐹2 + 2𝑒 −  2𝐹1− + 2.87 2𝐻1+ + 2𝑒 −  𝐻2 0.000
𝐶𝑜 3+
+ 1𝑒 −  𝐶𝑜 2+
+ 1.92 𝐹𝑒 3+
+ 3𝑒 −  𝐹𝑒 - 0.04
𝐻2 𝑂2 + 2𝐻 1+
+ 2𝑒 −
 2𝐻2 𝑂 + 1.78 𝑃𝑏 2+
+ 2𝑒 −  𝑃𝑏 - 0.13
𝐶𝑒 4+
+ 1𝑒 −  𝐶𝑒 3+
+ 1.72 𝑆𝑛 2+
+ 2𝑒 −  𝑆𝑛 - 0.14
𝑃𝑏𝑂2 + 𝑆𝑂42− + 4𝐻1+ + 2𝑒 −  𝑃𝑏𝑆𝑂4 + 2𝐻2 𝑂 + 1.69 𝐴𝑔𝐼 + 1𝑒 −  𝐴𝑔 + 𝐼1− - 0.15
𝑀𝑛𝑂41− + 8𝐻1+ + 5𝑒 −  𝑀𝑛2+ + 4𝐻2 𝑂 + 1.51 𝑁𝑖 2+ + 2𝑒 −  𝑁𝑖 - 0.26
𝐴𝑢 3+
+ 3𝑒 −  𝐴𝑢 + 1.50 𝐶𝑜 2+
+ 2𝑒 −  𝐶𝑜 - 0.28
𝑃𝑏𝑂2 + 4𝐻 1+
+ 2𝑒 −
 𝑃𝑏 2+
+ 2𝐻2 𝑂 + 1.46 𝐻3 𝑃𝑂4 + 2𝐻 1+
+ 2𝑒 −
 𝐻3 𝑃𝑂3 + 𝐻2 𝑂 - 0.28
𝐶𝑙𝑂41− + 8𝐻 1+
+ 8𝑒 −  𝐶𝑙 1−
+ 4𝐻2 𝑂 + 1.39 𝑃𝑏𝑆𝑂4 + 2𝑒 −  𝑃𝑏 + 𝑆𝑂42− - 0.36
𝐶𝑙2 + 2𝑒 −  2𝐶𝑙 1−
+1.36 𝑆𝑒 + 2𝐻 1+
+ 2𝑒 −  𝐻2 𝑆𝑒 - 0.40
𝐻𝑁𝑂2 + 4𝐻1+ + 4𝑒 −  𝑁2 𝑂 + 3𝐻2 𝑂 + 1.30 𝐶𝑑 2+ + 2𝑒 −  𝐶𝑑 - 0.40
𝐶𝑟2 𝑂72− + 14𝐻 1+
+ 6𝑒 −  2𝐶𝑟 3+
+ 7𝐻2 𝑂 + 1.23 𝐶𝑟 3+
+ 1𝑒 −  𝐶𝑟 2+
- 0.41
𝑂2 + 4𝐻 1+
+ 4𝑒 −  2𝐻2 𝑂 + 1.23 𝐹𝑒 2+
+ 2𝑒 −  𝐹𝑒 - 0.45
𝑀𝑛𝑂2 + 4𝐻 1+
+ 2𝑒 −  𝑀𝑛 2+
+ 2𝐻2 𝑂 + 1.22 𝐴𝑔2 𝑆 + 2𝑒 −  2𝐴𝑔 + 𝑆 2−
- 0.69
2𝐼𝑂31− + 12𝐻 1+
+ 10𝑒 −  𝐼2 + 6𝐻2 𝑂 + 1.20 𝑍𝑛 2+
+ 2𝑒 −  𝑍𝑛 - 0.76
2𝐼𝑂31− + 6𝐻1+ + 6𝑒 −  𝐼1− + 3𝐻2 𝑂 + 1.08 𝑇𝑒 + 2𝐻1+ + 2𝑒 −  𝐻2 𝑇𝑒 - 0.79
𝐵𝑟2 + 2𝑒 −  2𝐵𝑟 1−
+ 1.07 2𝐻2 𝑂 + 2𝑒 −  𝐻2 + 2𝑂𝐻 1−
- 0.83
𝐴𝑢𝐶𝑙41− + 3𝑒 −  𝐴𝑢 + 4𝐶𝑙 1−
+ 1.00 𝐶𝑟 2+
+ 2𝑒 −  𝐶𝑟 - 0.91
𝑁𝑂31− + 4𝐻 1+
+ 3𝑒 −  𝑁𝑂 + 2𝐻2 𝑂 + 0.96 𝑆𝑂42− + 𝐻2 𝑂 + 2𝑒 −  𝑆𝑂32− + 2𝑂𝐻 1−
- 0.93
2𝐻𝑔 2+
+ 2𝑒 −  𝐻𝑔22+ + 0.92 𝐴𝑙 3+
+ 3𝑒 −  𝐴𝑙 - 1.66
𝐻𝑔2+ + 2𝑒 −  𝐻𝑔 + 0.85 𝑀𝑔2+ + 2𝑒 −  𝑀𝑔 - 2.37
𝐶𝑙𝑂1− + 𝐻2 𝑂 + 2𝑒 −  𝐶𝑙1− + 2𝑂𝐻1− + 0.84 𝐿𝑎3+ + 3𝑒 −  𝐿𝑎 - 2.38
𝐴𝑔 1+
+ 1𝑒 −  𝐴𝑔 + 0.80 𝑁𝑎 1+
+ 1𝑒 −  𝑁𝑎 - 2.71
𝐻𝑔22+ + 2𝑒 −  2𝐻𝑔 + 0.80 𝐶𝑎 2+
+ 2𝑒 −  𝐶𝑎 - 2.87
𝑁𝑂31− + 2𝐻 1+
+ 1𝑒 −  𝑁𝑂2 + 𝐻2 𝑂 + 0.80 𝐵𝑎 2+
+ 2𝑒 −  𝐵𝑎 - 2.91
𝐹𝑒 3+
+ 1𝑒 −  𝐹𝑒 2+
+ 0.77 𝐾 1+
+ 1𝑒 −  𝐾 - 2.93
𝑂2 + 2𝐻1+ + 2𝑒 −  𝐻2 𝑂2 + 0.70 𝐿𝑖 1+ + 1𝑒 −  𝐿𝑖 - 3.04
𝑀𝑛𝑂41− + 2𝐻2 𝑂 + 3𝑒 −  𝑀𝑛𝑂2 + 4𝑂𝐻 1−
+ 0.60
𝐼2 + 2𝑒 −  2𝐼 1−
+ 0.54
𝐶𝑢 1+
+ 1𝑒 −  𝐶𝑢 + 0.52
𝑂2 + 2𝐻2 𝑂 + 4𝑒 −  4𝑂𝐻 1−
+ 0.40
𝐶𝑢 2+
+ 2𝑒 −  𝐶𝑢 + 0.34
𝐴𝑔𝐶𝑙 + 1𝑒 −  𝐴𝑔 + 𝐶𝑙1− + 0.22 Note: You can consider this to be
one continuous redox table,
𝑆𝑂42− + 4𝐻1+ + 2𝑒 −  𝐻2 𝑆𝑂3 + 𝐻2 𝑂 + 0.17
split into two columns at the reference
𝑆𝑛 4+
+ 2𝑒 −  𝑆𝑛 2+
+ 0.15 half-cell in order to fit on a single page.
𝐶𝑢 2+
+ 1𝑒 −  𝐶𝑢 1+
+ 0.15
𝑆 + 2𝐻 1+
+ 2𝑒 −
 𝐻2 𝑆 + 0.14
𝐴𝑔𝐵𝑟 + 1𝑒 −  𝐴𝑔 + 𝐵𝑟 1− + 0.07
2𝐻 1+
+ 2𝑒 −
 𝐻2 0.000
MAIN REACTIONS OF ORGANIC MOLECULES
SCH VSEPR CODES & MOLECULAR GEOMETRY
SCH MEASUREMENT & THE METRIC SYSTEM

COMMON METRIC PREFIXES

PREFIX SYMBOL RELATIONSHIP TO BASE UNIT
tera - T 1012 = 1 000 000 000 000
giga - G 109 = 1 000 000 000
mega - M 106 = 1 000 000
kilo - k 103 = 1 000
hector - h 102 = 100
deca - da 101 = 10
-- base unit 100 = 1
deci - d 10-1 = 0.1
centi - c 10-2 = 0.01
milli - m 10-3 = 0.001
micro -  10-6 = 0.000 001
nano - n 10-9 = 0.000 000 001
pico - p 10-12 = 0.000 000 000 001

COMMONLY USED METRIC QUANTITIES, UNITS & SYMBOLS

QUANTITY UNIT SYMBOL
Length metre m
gram g
Mass
tonne t (1 000 kg)
square metre m2
Area
hectare ha (10 000 m2)
litre L
Volume
cubic centimetre cm3 = 1 mL
second s
Time minute min = 60 s
hour h = 60 min = 3600 s
degree Celsius oC
Temperature
Kelvin K (oC + 273.15)
Energy Joule J

Pressure pascal Pa

Electric Current ampere A (C/s)

Quantity of Electric Charge coulomb C

Frequency hertz Hz