FORMULAS

QUANTITATIVE

$particles = (moles)(N_A)$

$N_A = 6.02 × 10^{23} \frac{particles}{mol}$

$mass = (moles)(molar\ mass)$

$\% \ composition = \dfrac{M_{element}}{M_{molecule}} × 100\%$

$\% \ yield = \dfrac{actual\ yield}{theoretical\ yield} × 100\%$

SOLUTIONS

$\text{Molarity} = \dfrac{mol\ solute}{volume\ solution\ (L)}$

$\text{Mole Fraction} = \dfrac{mol}{mol\ system}$

$\text{Molality} = \dfrac{mol\ solute}{mass\ solvent\ (kg)}$

$\text{Normality} = \dfrac{mass\ solute\ (g)}{volume solution\ (L)}$

Dilutions

$C_1V_1 = C_2V_2 \quad\quad\quad\quad\quad C = \dfrac{n_{total}}{V_{total}}$

Solubility

$aA + bB ⇌ cC + dD$

$K_{sp}, K_{eq}, Q = \dfrac{[C]^c [D]^d}{[A]^a [B]^b}$

only aqueous or gas included in K_sp
(Not liquid or solid)

K_c same as K_eq
K_p for gases K_eq << 1 ... [products] < [reactants]
K_eq ≈ 1 ... [products] ≈ [reactants]
K_eq >> 1 ... [products] > [reactants] K_sp < Q ... precipitate
K_sp ≈ Q ... starts
K_sp > Q ... no precipitate

GAS

Constants:

$\begin{align} R & = 8.314 \frac{L\,kPa}{mol\,K} \\ \\ & = 8.314 \frac{J}{mol\,K} \\ \\ & = 0.082 \frac{L\,atm}{mol\,K} \end{align}$

Molar Volume

$\begin{align} & = 22.4\ \tfrac{L}{mol}\ at\ \text{STP} \\ \\ & = 24.8\ \tfrac{L}{mol}\ at\ \text{SATP} \\ \\ \end{align}$

Conditions:

$STP = 0˚C, 100\ kPa$

$SATP = 25˚C, 100\ kPa$

Pressure Units:

$\begin{align} 1.0\ atm & = 101.3\ kPa \\ \\ & = 760\ mmHg \\ \\ & = 760\ torr \end{align}$

Boyle's

$P_1V_1 = P_2V_2$

Charles'

$\dfrac{V_1}{T_1} = \dfrac{V_2}{V_2}$

Temperature always
in Kelvin Avogadro's

$\dfrac{n_1}{V_1} = \dfrac{n_2}{V_2}$

Gay-Lussac's

$\dfrac{P_1}{T_1} = \dfrac{P_2}{T_2}$

Combined Gas Law

$\dfrac{P_1\,V_1}{T_1} = \dfrac{P_2\,V_2}{T_2}$

Ideal Gas Law

$P\,V = n\,R\,T$

Partial Pressures

$P_T = P_1 + P_2 + P_3 + \, ...$

$P_x = \dfrac{n_x}{n_T}P_T$

THERMODYNAMICS

Specific Heat

$C = m × c$

c = specific heat = specific heat capacity
C = heat capacity
Q = heat energy

$Q = m × c × \Delta t$

$Q = m × L$

(for phase changes)
L = latent heat

$\begin{align} \text{molar heat capacity} & = c × molar\ mass \\ & = \dfrac{Q}{n × \Delta t} \end{align}$

1^st Law Thermodynamics

$\Delta U = Q - W$

+Q = heat added to system
-Q = removed from system
+W = work done by system (out)
-W = work done on system (in)

$W = Q_{in} - Q_{out}$

Changes

$Isothermal: \Delta T = 0 \\ Isobaric: \Delta P = 0 \\ Adiabatic: Q = 0 \$

Enthalpy (H)

$\Delta H_{rxn} = n\,\Delta H_{products} - n\,\Delta H_{reactants}$

diatomic gases not included

$\Delta H_{rxn} = n\, BE_{reactants} - n\, BE_{products}$

BE = bond energy Entropy (S)

$\Delta S_{reaction} = n\,\Delta S_{products} - n\,\Delta S_{reactants}$

2^ndLaw Thermodynamics

$\Delta S_{universe} = \Delta S_{system} + \Delta S_{surroundings}$

Gibbs (G)

$\Delta G_{reaction} = n\,\Delta G_{products} - n\,\Delta G_{reactants}$

+∆G = Non-spontaneous (Endergonic)
-∆G = Spontaneous (Exergonic)
∆G = 0 = @ Equilibrium

$\Delta G = \Delta H - T \, \Delta S$

-∆H & +∆S = Spontaneous
+∆H & -∆S = Non-spontaneous
+∆H & +∆S = Spontaneous at High T
-∆H & -∆S = Spontaneous at Low T Units

$\Delta H_f = \frac{kJ}{mol} \\ \Delta H_{rxn} = kJ \\ \Delta S = \frac{J}{mol\,K} \\ \Delta S_{rxn} = \frac{J}{K} \\ \Delta G = \frac{kJ}{mol} \\ \Delta G_{rxn} = kJ \$

KINETICS

Experimental Rate Law

$Rate = k\,[A]^x × [B]^y$

k, x, y are determined experimentally

$Rate\ units = \frac{mol}{L\,s}$

Reaction Order

$0^{th}\ order: [C] ∝ t \\ 1^{st}\ order: \ln[C] ∝ t \\ 2^{nd}\ order: \frac{1}{[C]} ∝ t \$

Integrated Rate Law, 1^st Order

$\ln [A]_t = -k\,t + \ln [A]_0$

[A]₀ = initial reactant concentration
[A]_t = final reactant concentration
k = rate constant Integrated Rate Law, 2^nd Order

$\dfrac{1}{[A]_t} = k\,t + \dfrac{1}{[A]_0}$

ACID-BASE

$acid + base → salt + water$

$H_2O ⇌ H^+ + OH^-$

$pH = -\log[H^+] = \log\left(\frac{1}{[H^+]}\right)$

$pOH = -\log[OH^-] = \log\left(\frac{1}{[OH^-]}\right)$

Henderson-Hasselbalch

$pH = pK_a + \log\left( \dfrac{[conjugate\ base]}{[weak\ acid]} \right)$

$pOH = pK_b + \log\left( \dfrac{[conjugate\ acid]}{[weak\ base]} \right)$

Subheader

$14 = pH + pOH$

$\begin{align} K_w & = 10^{-14} \\ & = [H^+] × [OH^-] \end{align}$

Weak Acid, Base

$K_a = \dfrac{[H^+][A^-]}{[HA]}$

$K_b = \dfrac{[B^+][OH^-]}{[BOH]}$

ELECTROCHEMISTRY

Pseudonyms

$An. Ox. , Red. Cat.$

$O.I.L. \ R.I.G. \\ (L.E.O. \ G.E.R.)$

Cell Potential

$E˚_{cell} = E˚_{red} - E˚_{ox}$

+E˚_cell = spontaneous

$E˚_{red} = higher\ number \\ E˚_{ox} = lower\ number$

Nernst

$E˚_{cell} = E˚ + \left(\dfrac{R\,T}{n\,F}\right)\ln\,Q$

E˚ = standard cell potential
F = Faraday 96,485 sA/mol
T = temp in K
n = mol e^- transferred in redox Gibbs

$\Delta G˚_{cell} = - \Delta \,n\,F\,E˚_{cell}$

$\Delta G˚_{cell} = -R\,T\,\ln K_{eq}$

COLLIGATIVE (AP)

Boiling Elevation & Freezing Depression

$\Delta T_{freeze} = n\,k_f \dfrac{n_{solute}}{m_{solvent}}$

n = moles solute (1 for non-electrolytes)
m_solvent in kg
k_{f water} = 1.86 ˚Ckg/mol
k_{b water} = 0.52 ˚Ckg/mol

$\Delta T_{boil} = n\,k_b \dfrac{n_{solute}}{m_{solvent}}$

Osmotic Pressure

$π = M\,R\,T$

π = osmotic pressure
M = Molarity
R = universal gas constant
T = temperature in Kelvin

$\begin{align} R & = 8.314 \frac{L\,kPa}{mol\,K} \\ \\ & = 8.314 \frac{J}{mol\,K} \\ \\ & = 0.082 \frac{L\,atm}{mol\,K} \end{align}$

ORGANIC

Priority:

$\begin{align} Highest & = \text{Carboxylic Acid} \\ & = \text{Ester} \\ & = \text{Amide} \\ & = \text{Nitrile} \\ & = \text{Aldehyde} \\ & = \text{Ketone} \\ & = \text{Alcohol} \\ & = \text{Amine} \\ & = \text{Ether} \\ & = \text{Benzene} \\ & = \text{Alkene} \\ & = \text{Alkyne} \\ & = \text{Alkane} \\ Lowest & = \text{Alkyl, Halogen} \\ \end{align}$

Hydrogenation (Addition)

$Alkene \xrightarrow{H_2,\ Pd} Alkane$

Halogenation (Addition)

$Alkene \xrightarrow{X_2} Alkyl\ Halide$

Hydrohalogenation (Markovnikov, Addition)

$Alkene \xrightarrow{HX,\ UV} Alkyl\ Halide$

Markovnikov:
OH or X adds to more highly substituted carbon Hydration (Markovnikov, Addition)

$Alkene \xrightarrow{H_2O,\ H^+} Alcohol$

Substitution (Mixed results)

$Alkane \xrightarrow{X_2,\ UV} Alkyl\ Halide + \ ...$

Dehydration (Elimination)

$Alcohol \xrightarrow{H_2SO_4} Alkene$

Dehydration

$Alcohol + Alcohol \xrightarrow{H_2SO_4} Ether$

Oxidation, Ketones

$Internal\ Alcohol \xrightarrow{KMnO_4,\ H^+} Ketone$

Oxidation, Aldehyde

$Terminal\ Alcohol \xrightarrow{PCC} Aldehyde$

Oxidation, Carboxylic Acid

$Terminal\ Alcohol \xrightarrow{KMnO_4,\ H^+} Carboxylic\ Acid$

Esterification (Dehydration)

$Alcohol + Carboxylic\ Acid \xrightarrow{H_2SO_4} Ester$

Benzene Hydrogenation

$Benzene \xrightarrow{H_2,\ heat,\ catalyst} Cyclohexane$

Benzene Halogenation

$Benzene \xrightarrow{X_2} Monosubstituted\ Benzene$

Benzene Alkylation

$Benzene \xrightarrow{R-Cl,\ AlCl_3} Alkyl\ Benzene$

Cyclohexene Halogenation

$Cyclohexene \xrightarrow{X_2,\ CCl_4} Disubstituted-1,2\ Cyclohexane$

Cyclohexene Hydration

$Cyclohexene \xrightarrow{KMnO_4} Cyclohexane-1,2-diol$

Cyclohexanol Dehydration

$Cyclohexanol \xrightarrow{H_2SO_4} Cyclohexene$

REACTIONS

Oxidation Numbers of Polyatomic Oxide Ions

( # non-oxides )( oxidation state of non-oxide ) + ( # oxides )( oxidation state of oxide ) = polyatomic charge

E.g.) SO₄^2-, Sulfate(VI), [aka Sulphate(VI)]

$\begin{align} (1)(s) + (4)(-2) & = -2 \\ \\ s & = +6 \end{align}$

Synthesis from Elemental Molecules

$2H_{2 (g)} + O_{2 (g)} \xrightarrow{} 2H_2O_{(l)}$

Decomposition of a Single Compound

$2H_2O_{2 (l)} + \xrightarrow{} 2H_2O_{(l)} + O_{2 (g)}$

Neutralization Strong Acid + Strong Base → Salt + Water

$NaOH_{(aq)} + HCl_{(aq)} \xrightarrow{} NaCl_{(aq)} + H_2O_{(l)}$

Single Displacement with Hydrogen → Salt + Hydrogen Gas

$Ca_{(s)} + H_2O_{(l)} \xrightarrow{} CaO_{(s)} + H_{2 (g)}$

Single Displacement of Anions → Salt + Some Gas

$F_{2 (g)} + 2NaCl_{(aq)} \xrightarrow{} 2NaF_{(aq)} + Cl_{2 (g)}$

Complete Combustion Organic Compound + Oxygen → Carbon Dioxide + Water

$C_2H_6O_{(g)} + 3O_{2 (g)} \xrightarrow{} 2CO_{2 (g)} + 3H_2O_{(l)}$

Incomplete Combustion Organic Compound + Oxygen → Carbon Monoxide + Water

$2C_4H_{10 (g)} + 9O_{2 (g)} \xrightarrow{} 8CO_{(g)} + 10H_2O_{(l)}$

Metal Oxide + Carbon Dioxide → Metal Carbonate

$CaO_{(s)} + CO_{2 (g)} \xrightarrow{} CaCO_{3 (s)}$

Metal Oxide + Sulfur Dioxide → Metal Sulfite/Sulphite

$CaO_{(s)} + SO_{2 (g)} \xrightarrow{} CaSO_{3 (s)}$

(Metal or Metal Oxide) + Water → Base + Hydrogen Gas

$2Li_{(s)} + 2H_2O_{(l)} \xrightarrow{} 2LiOH_{(aq)} + H_{2 (g)}$

Metal Oxide + Hydrogen Gas → Metal + Water

$FeO_{(s)} + H_{2 (g)} \xrightarrow{} Fe_{(s)} + H_2O_{(l)}$

Metal + Oxygen → Metal Oxide

$2Fe_{(s)} + 2O_{2 (g)} \xrightarrow{} 2Fe_2O_{3 (s)}$

Nonmetal Oxide + Water → Acid

$N_2O_{5 (s)} + H_2O_{(l)} \xrightarrow{} 2HNO_{3 (aq)}$

Single Displacement, RedOx, Synthesis, Dehydration

$Cu_{(s)} + 4HNO_{3 (aq)} \xrightarrow{} {\color{DeepSkyBlue} Cu(NO_3)_{2 (aq)} } + 2NO_{2 (g)} + 2H_2O_{(l)}$

Double Displacement

${\color{DeepSkyBlue} Cu(NO_3)_{2 (aq)} } + NaOH_{(aq)} \xrightarrow{} {\color{Green} Cu(OH)_{2 (s)} } + 2Na(NO_3)_{(aq)}$

Decomposition, Dehydration

${\color{Green} Cu(OH)_{2 (s)} } \xrightarrow{\Delta} {\color{DarkOrchid} CuO_{(s)} } + H_2O{(l)}$

Double Displacement

${\color{DarkOrchid} CuO_{(s)} } + H_2SO_{4 (aq)} \xrightarrow{} {\color{OrangeRed} Cu(SO_4)_{(aq)} } + H_2O_{(l)}$

Single Displacement Ionic compound + Metal

${\color{OrangeRed} 2Cu(SO_4)_{(aq)} } + Zn_{(s)} \xrightarrow{} Zn(SO_4)_{(aq)} + 2Cu_{(s)}$

$H_2SO_{4 (aq)} + Zn_{(s)} \xrightarrow{} H_{2 (g)} + Zn(SO_4)_{(aq)}$

POLYATOMIC

Group Trends:

[FO₃^– ≈ ClO₃^– ≈ BrO₃^– ≈ IO₃^–]

[CO₃^2– ≈ SiO₃^2-]

Formula	Name	IUPAC Oxyanion/Oxoanion Name
CATIONS
NH₄⁺	ammonium
ANIONS
OH^–	hydroxide
BO₃^3–	borate	borate(III)
HCO₂^–	formate
C₂H₃O₂^– or CH₃COO^–	acetate, ethanoate
C₂O₄^2–	oxalate, oxylate	oxalate(III)
CO₃^2–	carbonate	carbonate(IV)
CN^–	cyanide
OCN^–	cyanate
CNO^–	fulminate
SCN^–	thiocyanate
HCO₃^–	bicarbonate (or hydrogen carbonate)
SiO₃^2–	silicate	silicate(IV)
NO₃^–	nitrate	nitrate(V)
NO₂^–	nitrite	nitrate(III)
N₂O₂^2–	hyponitrite	nitrate(I)
N₃^–	azide
O₂^–	superoxide
O₂^2–	peroxide
PO₄^3–	phosphate	phosphate(V)
PO₃^3–	phosphite	phosphate(III)
PO₂^3–	hypophosphite	phosphate(I)
HPO₄^2–	hydrogen phosphate
H₂PO₄^–	dihydrogen phosphate
HPO₃^2–	hydrogen phosphite
H₂PO₃^–	dihydrogen phosphite
PO₂^3–	hypophosphite
AsO₄^3–	arsenate	arsenate(V)
SbO₄^3–	antimonate	antimonate(V)
SO₅^2–	persulfate, aka persulphate	sulfate(VIII), aka sulphate(VIII)
SO₄^2–	sulfate, aka sulphate	sulfate(VI), aka sulphate(VI)
SO₃^2–	sulfite, aka sulphite	sulfate(IV), aka sulphate(IV)
SO₂^2–	hyposulfite, aka hyposulphite	sulfate(II), aka sulphate(IV)
HSO₄^–	hydrogen sulfate or bisulfate
HSO₃^–	hydrogen sulfite or bisulfite
S₂O₃^2–	thiosulfate	thiosulfate(II)
SeO₄^2–	selenate	selenate(VI)
FO₄^–	perfluorate	fluorate(VII)
FO₃^–	fluorate	fluorate(V)
FO₂^–	fluorite	fluorate(III)
FO^–	hypofluorite	fluorate(I)
ClO₄^–	perchlorate	chlorate(VII)
ClO₃^–	chlorate	chlorate(V)
ClO₂^–	chlorite	chlorate(III)
ClO^–	hypochlorite	chlorate(I)
BrO₄^–	perbromate	bromate(VII)
BrO₃^–	bromate	bromate(V)
BrO₂^–	bromite	bromate(III)
BrO^–	hypobromite	bromate(I)
IO₄^–	periodiate	iodate(VII)
IO₃^–	iodate	iodate(V)
IO₂^–	iodite	iodate(III)
IO^–	hypoiodite	iodate(I)
I₃^–	triiodide
VO₃^–	vanadate	vanadate(V)
CrO₄^2–	chromate	chromate(VI)
Cr₂O₇^2–	dichromate	chromate(VI)
CrO₃^2–	?	chromate(IV)
CrO₂^1– , Cr₂O₄^2-	chromite	chromate(III)
FeO₄^2–	ferrate	ferrate(VI)
MnO₄^–	permanganate	manganate(VII)
SnO₃^2–	stannate	stannate(IV)
PbO₃^2–	plumbate	plumbate(IV)

Modern IUPAC Oxyanion/Oxoanion Oxidation Numbers

Oxyanion/Oxoanion	Oxidation Number on 'X'
XO^1-	+1
XO₂^1-	+3
XO₂^2-	+2
XO₃^1-	+5
XO₃^2-	+4
XO₃^3-	+3
XO₄^1-	+7
XO₄^2-	+6
XO₄^3-	+5
XO₅^2-	+8

REACTIVITY

Reactivity Ranking	Cation Element
1 (Most Reactive)	Lithium, Li
2	Potassium, K
3	Barium, Ba
4	Calcium, Ca
5	Sodium, Na
6	Magnesium, Mg
7	Aluminum, Al
8	Zinc, Zn
9	Chromium, Cr
10	Iron, Fe
11	Cadmium, Cd
12	Cobalt, Co
13	Nickel, Ni
14	Tin, Sn
15	Lead, Pb
16	Hydrogen, H
17	Copper, Cu
18	Mercury, Hg
19	Silver, Ag
20	Platinum, Pt
21 (Least Reactive)	Gold, Au

Reactivity Ranking	Anion Element
1 (Most Reactive)	Fluoride, F^-
2	Sulfate, SO₄^2-
3	Nitrate, NO₃^-
4	Chloride, Cl^-
5	Bromide, Br^-
6	Iodide, I^-
7 (Least Reactive)	Hydroxide, OH^-

SOLUBILITY

[] < 0.01 M = INSOLUBLE

[] > 0.1 M = SOLUBLE

Order (Ranking)	Cation	Anion	Solubility	Exceptions
1 (Highest)	Li⁺, Na⁺, K⁺, NH₄⁺	NO₃^-, ClO₃^-, CH₃COO^-	Soluble	Insoluble: Ca(ClO₃)₂
2	Ag⁺, Hg²⁺, Pb⁺	OH^-, PO₄^3-, CO₃^2-, O₂^-, S^2-,	*Insoluble*	Soluble: BaO, Ba(OH)₂, and Group 2 Sulfides
3		Cl^-, Br^-, I^-	Soluble
4	Ca²⁺, Sr²⁺, Ba²⁺		*Insoluble*
5 (Lowest)	Mg²⁺, Al³⁺, Fe²⁺, Fe³⁺, Cu²⁺, Zn²⁺	SO₄^2-	Soluble

K CONSTANTS

Compound	Formula	K_sp (25 °C, 298 K)
Aluminium hydroxide	Al(OH)₃	3×10^-34
Aluminium phosphate	AlPO₄	9.84×10^-21
Barium bromate	Ba(BrO₃)₂	2.43×10^-4
Barium carbonate	BaCO₃	2.58×10^-9
Barium chromate	BaCrO₄	1.17×10^-10
Barium fluoride	BaF₂	1.84×10^-7
Barium hydroxide octahydrate	Ba(OH)₂×8H₂O	2.55×10^-4
Barium iodate	Ba(IO₃)₂	4.01×10^-9
Barium iodate monohydrate	Ba(IO₃)₂×H₂O	1.67×10^-9
Barium molybdate	BaMoO₄	3.54×10^-8
Barium nitrate	Ba(NO₃)₂	4.64×10^-3
Barium selenate	BaSeO₄	3.40×10^-8
Barium sulfate/sulphate	BaSO₄	1.08×10^-10
Barium sulfite/sulphite	BaSO₃	5.0×10^-10
Beryllium hydroxide	Be(OH)₂	6.92×10^-22
Bismuth arsenate	BiAsO₄	4.43×10^-10
Bismuth iodide	BiI	7.71×10^-19
Cadmium arsenate	Cd₃(AsO₄)₂	2.2×10^-33
Cadmium carbonate	CdCO₃	1.0×10^-12
Cadmium fluoride	CdF₂	6.44×10^-3
Cadmium hydroxide	Cd(OH)₂	7.2×10^-15
Cadmium iodate	Cd(IO₃)₂	2.5×10^-8
Cadmium oxalate trihydrate	CdC₂O₄×3H₂O	1.42×10^-8
Cadmium phosphate	Cd₃(PO₄)₂	2.53×10^-33
Cadmium sulfide	CdS	1×10^-27
Caesium perchlorate	CsClO₄	3.95×10^-3
Caesium periodate	CsIO₄	5.16×10^-6
Calcium carbonate (calcite)	CaCO₃	3.36×10^-9
Calcium carbonate (aragonite)	CaCO₃	6.0×10^-9
Calcium fluoride	CaF₂	3.45×10^-11
Calcium hydroxide	Ca(OH)₂	5.02×10^-6
Calcium iodate	Ca(IO₃)₂	6.47×10^-6
Calcium iodate hexahydrate	Ca(IO₃)₂×6H₂O	7.10×10^-7
Calcium molybdate	CaMoO	1.46×10^-8
Calcium oxalate monohydrate	CaC₂O₄×H₂O	2.32×10^-9
Calcium phosphate	Ca₃(PO₄)₂	2.07×10^-33
Calcium sulfate/sulphate	CaSO₄	4.93×10^-5
Calcium sulfate/sulphate dihydrate	CaSO₄×2H₂O	3.14×10^-5
Calcium sulfate/sulphate hemihydrate	CaSO₄×0.5H₂O	3.1×10^-7
Cobalt(II) arsenate	Co₃(AsO₄)₂	6.80×10^-29
Cobalt(II) carbonate	CoCO₃	1.0×10^-10
Cobalt(II) hydroxide (blue)	Co(OH)₂	5.92×10^-15
Cobalt(II) iodate dihydrate	Co(IO₃)₂×2H₂O	1.21×10^-2
Cobalt(II) phosphate	Co₃(PO₄)₂	2.05×10^-35
Cobalt(II) sulfide (alpha)	CoS	5×10^-22
Cobalt(II) sulfide (beta)	CoS	3×10^-26
Copper(I) bromide	CuBr	6.27×10^-9
Copper(I) chloride	CuCl	1.72×10^-7
Copper(I) cyanide	CuCN	3.47×10^-20
Copper(I) hydroxide	Cu₂O	2×10^-15
Copper(I) iodide	CuI	1.27×10^-12
Copper(I) thiocyanate	CuSCN	1.77×10^-13
Copper(II) arsenate	Cu₃(AsO₄)₂	7.95×10^-36
Copper(II) hydroxide	Cu(OH)₂	4.8×10^-20
Copper(II) iodate monohydrate	Cu(IO₃)₂×H₂O	6.94×10^-8
Copper(II) oxalate	CuC₂O₄	4.43×10^-10
Copper(II) phosphate	Cu₃(PO₄)₂	1.40×10^-37
Copper(II) sulfide	CuS	8×10^-37
Europium(III) hydroxide	Eu(OH)₃	9.38×10^-27
Gallium(III) hydroxide	Ga(OH)₃	7.28×10^-36
Iron(II) carbonate	FeCO₃	3.13×10^-11
Iron(II) fluoride	FeF₂	2.36×10^-6
Iron(II) hydroxide	Fe(OH)₂	4.87×10^-17
Iron(II) sulfide	FeS	8×10^-19
Iron(III) hydroxide	Fe(OH)₃	2.79×10^-39
Iron(III) phosphate dihydrate	FePO₄×2H₂O	9.91×10^-16
Lanthanum iodate	La(IO₃)₃	7.50×10^-12
Lead(II) bromide	PbBr₂	6.60×10^-6
Lead(II) carbonate	PbCO₃	7.40×10^-14
Lead(II) chloride	PbCl₂	1.70×10^-5
Lead(II) chromate	PbCrO₄	3×10^-13
Lead(II) fluoride	PbF₂	3.3×10^-8
Lead(II) hydroxide	Pb(OH)₂	1.43×10^-20
Lead(II) iodate	Pb(IO₃)₂	3.69×10^-13
Lead(II) iodide	PbI₂	9.8×10^-9
Lead(II) oxalate	PbC₂O₄	8.5×10^-9
Lead(II) selenate	PbSeO₄	1.37×10^-7
Lead(II) sulfate/sulphate	PbSO₄	2.53×10^-8
Lead(II) sulfide	PbS	3×10^-28
Lithium carbonate	Li₂CO₃	8.15×10^-4
Lithium fluoride	LiF	1.84×10^-3
Lithium phosphate	Li₃PO₄	2.37×10^-4
Magnesium ammonium phosphate	MgNH₄PO₄	3×10^-13
Magnesium carbonate	MgCO₃	6.82×10^-6
Magnesium carbonate trihydrate	MgCO₃×3H₂O	2.38×10^-6
Magnesium carbonate pentahydrate	MgCO₃×5H₂O	3.79×10^-6
Magnesium fluoride	MgF₂	5.16×10^-11
Magnesium hydroxide	Mg(OH)₂	5.61×10^-12
Magnesium oxalate dihydrate	MgC₂O₄×2H₂O	4.83×10^-6
Magnesium phosphate	Mg₃(PO₄)₂	1.04×10^-24
Manganese(II) carbonate	MnCO₃	2.24×10^-11
Manganese(II) iodate	Mn(IO₃)₂	4.37×10^-7
Manganese(II) hydroxide	Mn(OH)₂	2×10^-13
Manganese(II) oxalate dihydrate	MnC₂O₄×2H₂O	1.70×10^-7
Manganese(II) sulfide (pink)	MnS	3×10^-11
Manganese(II) sulfide (green)	MnS	3×10^-14
Mercury(I) bromide	Hg₂Br₂	6.40×10^-23
Mercury(I) carbonate	Hg₂CO₃	3.6×10^-17
Mercury(I) chloride	Hg₂Cl₂	1.43×10^-18
Mercury(I) fluoride	Hg₂F₂	3.10×10^-6
Mercury(I) iodide	Hg₂I₂	5.2×10^-29
Mercury(I) oxalate	Hg₂C₂O₄	1.75×10^-13
Mercury(I) sulfate/sulphate	Hg₂SO₄	6.5×10^-7
Mercury(I) thiocyanate	Hg₂(SCN)₂	3.2×10^-20
Mercury(II) bromide	HgBr₂	6.2×10^-20
Mercury(II) hydroxide	HgO	3.6×10^-26
Mercury(II) iodide	HgI₂	2.9×10^-29
Mercury(II) sulfide (black)	HgS	2×10^-53
Mercury(II) sulfide (red)	HgS	2×10^-54
Neodymium carbonate	Nd₂(CO₃)₃	1.08×10^-33
Nickel(II) carbonate	NiCO₃	1.42×10^-7
Nickel(II) hydroxide	Ni(OH)₂	5.48×10^-16
Nickel(II) iodate	Ni(IO₃)₂	4.71×10^-5
Nickel(II) phosphate	Ni₃(PO₄)₂	4.74×10^-32
Nickel(II) sulfide (alpha)	NiS	4×10^-20
Nickel(II) sulfide (beta)	NiS	1.3×10^-25
Palladium(II) thiocyanate	Pd(SCN)₂	4.39×10^-23
Potassium hexachloroplatinate	K₂PtCl₆	7.48×10^-6
Potassium perchlorate	KClO₄	1.05×10^-2
Potassium periodate	KIO₄	3.71×10^-4
Praseodymium hydroxide	Pr(OH)₃	3.39×10^-24
Radium iodate	Ra(IO₃)₂	1.16×10^-9
Radium sulfate/sulphate	RaSO₄	3.66×10^-11
Rubidium perchlorate	RuClO₄	3.00×10^-3
Scandium fluoride	ScF₃	5.81×10^-24
Scandium hydroxide	Sc(OH)₃	2.22×10^-31
Silver(I) acetate	AgCH₃COO	1.94×10^-3
Silver(I) arsenate	Ag₃AsO₄	1.03×10^-22
Silver(I) bromate	AgBrO₃	5.38×10^-5
Silver(I) bromide	AgBr	5.35×10^-13
Silver(I) carbonate	Ag₂CO₃	8.46×10^-12
Silver(I) chloride	AgCl	1.77×10^-10
Silver(I) chromate	Ag₂CrO₄	1.12×10^-12
Silver(I) cyanide	AgCN	5.97×10^-17
Silver(I) iodate	AgIO₃	3.17×10^-8
Silver(I) iodide	AgI	8.52×10^-17
Silver(I) oxalate	Ag₂C₂O₄	5.40×10^-12
Silver(I) phosphate	Ag₃PO₄	8.89×10^-17
Silver(I) sulfate/sulphate	Ag₂SO₄	1.20×10^-5
Silver(I) sulfite/sulphite	Ag₂SO₃	1.50×10^-14
Silver(I) sulfide	Ag₂S	8×10^-51
Silver(I) thiocyanate	AgSCN	1.03×10^-12
Strontium arsenate	Sr₃(AsO₄)₂	4.29×10^-19
Strontium carbonate	SrCO₃	5.60×10^-10
Strontium fluoride	SrF₂	4.33×10^-9
Strontium iodate	Sr(IO₃)₂	1.14×10^-7
Strontium iodate monohydrate	Sr(IO₃)₂×H₂O	3.77×10^-7
Strontium iodate hexahydrate	Sr(IO₃)₂×6H₂O	4.55×10^-7
Strontium oxalate	SrC₂O₄	5×10^-8
Strontium sulfate/sulphate	SrSO₄	3.44×10^-7
Thallium(I) bromate	TlBrO₃	1.10×10^-4
Thallium(I) bromide	TlBr	3.71×10^-6
Thallium(I) chloride	TlCl	1.86×10^-4
Thallium(I) chromate	Tl₂CrO₄	8.67×10^-13
Thallium(I) hydroxide	Tl(OH)₃	1.68×10^-44
Thallium(I) iodate	TlIO₃	3.12×10^-6
Thallium(I) iodide	TlI	5.54×10^-8
Thallium(I) thiocyanate	TlSCN	1.57×10^-4
Thallium(I) sulfide	Tl₂S	6×10^-22
Tin(II) hydroxide	Sn(OH)₂	5.45×10^-27
Yttrium carbonate	Y₂(CO₃)₃	1.03×10^-31
Yttrium fluoride	YF₃	8.62×10^-21
Yttrium hydroxide	Y(OH)₃	1.00×10^-22
Yttrium iodate	Y(IO₃)₃	1.12×10^-10
Zinc arsenate	Zn₃(AsO₄)₂	2.8×10^-28
Zinc carbonate	ZnCO₃	1.46×10^-10
Zinc carbonate monohydrate	ZnCO₃×H₂O	5.42×10^-11
Zinc fluoride	ZnF	3.04×10^-2
Zinc hydroxide	Zn(OH)₂	3×10^-17
Zinc iodate dihydrate	Zn(IO₃)₂×2H₂O	4.1×10^-6
Zinc oxalate dihydrate	ZnC₂O₄×2H₂O	1.38×10^-9
Zinc selenide	ZnSe	3.6×10^-26
Zinc selenite monohydrate	ZnSe×H₂O	1.59×10^-7
Zinc sulfide (alpha)	ZnS	2×10^-25
Zinc sulfide (beta)	ZnS	3×10^-23

ACIDS/BASES

6 Most Common Strong Acids

HCl

HBr

HNO₃

H₂SO₄

HClO₄

7 Most Common Strong Bases

LiOH

NaOH

KOH

RbOH

Ca(OH)₂

Sr(OH)₂

Ba(OH)₂

HALF-REACTIONS

Largest (positive) number gets reduced

Reduction Half-Reaction	Standard Potential E_red° (V)
F₂_(g) + 2e ^– → 2F^–_(aq)	+2.87
O₃_(g) + 2H₃O⁺_(aq) + 2e^– → O₂_(g) + 3H₂O_(l)	+2.076
Co³⁺_(aq) + e^– → Co²⁺_(aq)	+1.92
H₂O₂_(aq) + 2H₃O⁺_(aq) + 2e^– → 2H₂O_(l)	+1.776
N₂O_(g) + 2H₃O⁺_(aq) + 2e^– → N₂_(g) + 3H₂O_(l)	+1.766
Ce⁴⁺_(aq) + e^– → Ce³⁺_(aq)	+1.72
PbO₂_(s) + SO₄^2–_(aq) + 4H₃O⁺_(aq) + 2e^– → PbSO₄_(s) + 6H₂O_(l)	+1.6913
MnO₄^–_(aq) + 4H₃O⁺_(aq) + 3e^– → MnO₂_(s) + 6H₂O_(l)	+1.679
NiO₂_(s) + 4H₃O⁺_(aq) + 2e^– → Ni²⁺_(aq) + 6H₂O_(l)	+1.678
2HClO_(aq) + 2H₃O⁺_(aq) + 2e^– → Cl₂_(g) +2H₂O_(l)	+1.611
H₅IO₆_(s) + H₃O⁺_(aq) + 2e^– → IO₃^–_(aq) + 4H₂O_(l)	+1.601
2NO_(g) + 2H₃O⁺_(aq) + 2e^– → N₂O_(g) + 3H₂O_(l)	+1.591
MnO₄^–_(aq) + 8H₃O⁺_(aq) + 5e^– → Mn²⁺_(aq) + 12H₂O_(l)	+1.507
Au³⁺_(aq) + 3e^– → Au_(s)	+1.498
PbO₂_(s) + 4H₃O⁺_(aq)+ 2e^– → Pb²⁺_(aq) + 6H₂O_(l)	+1.455
ClO₃^–_(aq) + 6H₃O⁺_(aq) + 6e^– → Cl^–_(aq) + 9H₂O_(l)	+1.451
BrO₃^–_(aq) + 6H₃O⁺_(aq) + 5e– → 1/2Br₂_(l) + 9H₂O_(l)	+1.482
2ClO₄^–_(aq) + 16H₃O⁺_(aq) + 14e^– → Cl₂_(g) + 24H₂O_(l)	+1.39
ClO₄^–_(aq) + 8H₃O⁺_(aq) + 8e^– → Cl^–_(aq) + 12H₂O_(l)	+1.389
Cl₂_(g) + 2e^– → 2Cl^–_(aq)	+1.36
ClO₄^–_(aq) + 6H₃O⁺_(aq) + 6e^– → ClO^–_(aq) + 9H₂O_(l)	+1.36
HBrO_(aq) + H₃O⁺_(aq) + 2e^– → Br^– + 2H₂O_(l)	+1.331
Cr₂O₇^2–_(aq) + 14H₃O⁺_(aq) + 6e^– → 2Cr³⁺_(aq) + 21H₂O_(l)	+1.232
O₂_(g) + 4H⁺_(aq) + 4e^– → 2H₂O_(l)	+1.23
MnO₂_(s) + 4H₃O⁺_(aq) + 2e^– → Mn²⁺_(aq) + 6H₂O_(l)	+1.224
2IO₃^–_(aq) + 12H₃O⁺_(aq) + 10e^– → I₂_(s) + 18H₂O_(l)	+1.195
ClO₄^–_(aq) + 2H₃O+_(aq) + 2e^– → ClO₃^–_(aq) + 3H₂O_(l)	+1.189
Pt²⁺_(aq) + 2e^– → Pt_(s)	+1.18
Br₂_(aq) + 2e^– → 2Br^–_(aq)	+1.0873
Br₂_(l) + 2e^– → 2Br^–_(aq)	+1.07
NO₂_(g) + 2H₃O⁺_(aq) + 2e^– → NO_(g) + 3H₂O_(l)	+1.03
NO₃^–_(aq) + 4H₃O⁺_(aq) +3e^– → NO_(g) + 6H₂O_(l)	+0.957
2Hg²⁺_(aq) + 2e^– → Hg₂²⁺_(aq)	+0.920
Pd²⁺_(aq) + 2e^– → Pd_(s)	+0.915
Hg²⁺_(aq) + 2e^– → Hg_(l)	+0.851
ClO^–_(aq) + H₂O_(l) + 2e^– → Cl^–_(aq) + 2OH^–_(aq)	+0.81
Ag⁺_(aq) + e^– → Ag_(s)	+0.80
Hg₂²⁺_(aq) + 2e^– → 2Hg_(l)	+0.7973
Fe³⁺_(aq) + e^– → Fe²⁺_(aq)	+0.771
Ni(OH)₂_(s) + 2e^– → Ni_(s) + 2OH^–_(aq)	+0.72
p-benzoquinone + H₃O⁺_(aq) + 2e^– → hydroquinone + H₂O_(l)	+0.6992
O₂_(g) + 2H₃O⁺_(aq) + 2e^– → H₂O₂_(l) + 2H₂O_(l)	+0.695
MnO₄^–_(aq) + 2H₂O_(l) + 3e^– → MnO₂_(s) + 4OH^–_(aq)	+0.595
I₂_(s) + 2e^– → 2I^–_(aq)	+0.54
I₃–_(aq) + 2e^– → 3I^–_(aq)	+0.536
Cu⁺_(aq) + e^– → Cu_(s)	+0.52
O₂_(g) + 2H₂O + 4e^– → 4OH^–_(aq)	+0.401
Fe(CN)₆^3–_(aq) + e^– → Fe(CN)₆^4–_(aq)	+0.358
Cu²⁺_(aq) + 2e^– → Cu_(s)	+0.34
Hg₂Cl₂_(s) + 2e^– → 2Hg_(l) + 2Cl^–_(aq)	+0.26808
HAsO₂_(s) + 3H₃O⁺_(aq) + 3e^– → As_(s) + 5H₂O	+0.248
AgCl_(s) + e^– → Ag_(s) + Cl^-_(aq)	+0.22233
Cu²⁺_(aq) + e^– → Cu⁺_(aq)	+0.153
Sn⁴⁺_(aq) +2e^– → Sn²⁺_(aq)	+0.151
S_(s) + 2H₃O⁺_(aq) + 2e^– → H₂S_(s) + 2H₂O_(l)	+0.14
NO₃^–_(aq) +2H₂O_(l) + 3e^– → NO_(g) + 4OH^–_(aq)	+0.109
N₂_(g) + 8H₃O⁺_(aq) + 6e^– → 2NH₄⁺_(aq) +8H₂O_(l)	+0.092
S₄O₆^2–_(aq) + 2e^– → 2S₃O₃^2–_(aq)	+0.08
AgBr_(s) + e^– → Ag_(s) + Br^–_(aq)	+0.07133
2H⁺_(aq) + 2e^– → H₂_(g)	0.000
Fe³⁺_(aq) + 3e^– → Fe_(s)	-0.04
[Co(NH₃)₆]³⁺_(aq) + e^– → [Co(NH₃)₆]²⁺_(aq)	-0.108
Pb²⁺_(aq) + 2e^– → Pb_(s)	–0.13
Sn²⁺_(aq) + 2e^– → Sn_(s)	–0.14
O₂_(g) + 2H₂O_(l) + 2e^– → H₂O₂_(l) + 2OH^–_(aq)	–0.146
AgI_(s) + e^– → Ag_(s) + I^– _(aq)	–0.15224
CO₂_(g) + 2H₃O+_(aq) + 2e^– → HCO₂H_(s) + 2H₂O_(l)	–0.199
Cu(OH)₂_(s) + 2e^– → Cu_(s) + 2OH^–_(aq)	–0.222
Ni²⁺_(aq) + 2e^– → Ni_(s)	–0.26
Co²⁺_(aq) + 2e^– → Co_(s)	–0.28
PbSO₄_(s) + 2e^– → Pb_(s) + SO₄^2–_(aq)	–0.3588
SeO₃^2–_(aq) + 3H₂O_(l) + 4e^– → Se + 6OH^–_(aq)	–0.366
Cd²⁺_(aq) + 2e– → Cd_(s)	–0.403
Cr³⁺_(aq) + e– → Cr²⁺_(aq)	–0.407
Fe²⁺_(aq) + 2e^– → Fe_(s)	–0.44
NO₂^–_(g) + H₂O_(l) + 3e^– → NO_(g) + 2OH^–_(aq)	–0.46
S_(s) + 2e^– → S^2–_(aq)	–0.48
2CO₂_(g) + 2H₃O⁺_(aq) + 2e^– → H₂C₂O₄_(s) + H₂O_(l)	–0.49
TiO₂_(s) + 4H₃O⁺ + 2e^– → Ti²⁺_(aq) + 6H₂O_(l)	–0.502
Au(CN)₂^–_(aq) + e^– → Au_(s) + 2CN^–_(aq)	–0.60
Cr³⁺_(aq) + 3e^– → Cr_(s)	–0.74
Zn²⁺_(aq) + 2e^– → Zn_(s)	–0.76
Cd(OH)₂_(s) + 2e– → Cd_(s) + 2OH–_(aq)	–0.809
2H₂O_(l) + 2e^– → H₂_(g) + 2OH^–_(aq)	–0.83
Ti³⁺_(aq) + e^– → Ti²⁺_(aq)	–0.85
H₃BO₃_(s) + 3H₃O⁺ + 3e^– → B_(s) + 6H₂O_(l)	–0.8698
Cr²⁺_(aq) + 2e^– → Cr_(s)	–0.91
CNO^–_(aq) + H₂O_(l) + 2e^– → CN^–_(aq) + 2OH^–_(aq)	–0.970
[Zn(NH₃)₄]²⁺_(aq) + 2e^– → Zn_(s) + 4NH₃_(aq)	–1.04
Mn²⁺_(aq) + 2e^– → Mn_(s)	–1.185
Cr(OH)₃_(s) + 3e^– → Cr_(s) + 3OH^–_(aq)	–1.48
Ti²⁺_(aq) + 2e^– → Ti_(s)	–1.630
Al³⁺_(aq) + 3e^– → Al_(s)	–1.66
Al(OH)₃_(s) + 3e^– → Al_(s) + 3OH^–_(aq)	–2.31
Mg²⁺_(aq) + 2e^– → Mg_(s)	–2.38
Mg(OH)₂_(s) + 2e^– → Mg_(s) + 2OH^–_(aq)	–2.69
Na⁺_(aq) + e^– → Na_(s)	–2.71
Ca²⁺_(aq) + 2e^– → Ca_(s)	–2.87
Ba²⁺_(aq) + 2e^– → Ba_(s)	–2.912
K⁺_(aq) + e^– → K_(s)	–2.931
Ba(OH)₂_(s) + 2e^– → Ba_(s) + 2OH^–_(aq)	–2.99
Ca(OH)₂_(s) + 2e^– → Ca_(s) + 2OH^–_(aq)	–3.02
Cs⁺_(aq) + e^– → Cs_(s)	–3.026
Li⁺_(aq) + e^– → Li_(s)	–3.04

FORMATION

Substance	∆H_f˚ (kJ/mol)	∆G_f˚ (kJ/mol)	S˚ (J/mol K)
Ag_(s)	0	0	42.6
Ag⁺_(aq)	105.8	77.107	73.4
Ag₂O_(s)	–31.1	–11.2	121.3
Ag₂S_(s)	–32.6	–40.7	144.0
AgBr_(s)	–100.4	–96.9	107.1
AgCl_(s)	–127.0	–109.8	96.3
AgI_(s)	–61.8	–66.2	115.5
AgNO₃_(s)	–124.4	–33.4	140.9
Al_(s)	0	0	28.3
Al₂O₃_(s)	–1675.7	–1582.3	50.9
AlCl₃_(s)	–704.2	–628.8	109.3
Ar_(g)	0	0	154.843
As_(s)	0	0	35.1
As₂O₅_(s)	–924.9	–782.3	105.4
AsCl₃_(l)	–305.0	–259.4	216.3
Au_(s)	0	0	47.4
Ba_(s)	0	0	62.5
BaCl₂_(s)	–855.0	–806.7	123.7
BaCO₃_(s)	–1213.0	–1134.4	112.1
BaO_(s)	–548.0	–520.3	72.1
BaSO₄_(s)	–1473.2	–1362.2	132.2
B_(s)	0	0	5.9
B₂O₃_(s)	–1273.5	–1194.3	54.0
H₃BO₃_(s)	–1094.3	–968.9	90.0
BCl₃_(g)	–403.8	–388.7	290.1
BCl₃_(l)	–427.2	–387.4	206.3
BCl₃_(s)	–403.8	–388.7	290.1
Be(OH)₂_(s)	–902.5	–815.0	45.5
Be_(s)	0	0	9.5
BeO_(s)	0	-580.1	13.8
Br_(g)	111.9	82.4	175.0
Br₂_(g)	30.9	3.1	245.5
Br₂_(l)	0	0	152.2
Br^–_(aq)	–121.4	–104.0	82.4
BrO^–_(aq)	–94.1	–33.4	42
BrF₃_(g)	–255.6	–229.4	292.5
C(diamond)	1.9	2.9	2.4
C_(g)	716.7	671.3	158.1
C(graphite)	0	0	5.7
CCl₄_(l)	–139	–68.6	214.4
CH₄_(g)	–74.6	–50.5	186.3
C₂H₂_(g)	227.4	209.9	200.9
C₂H₄_(g)	52.4	68.4	219.3
C₂H₅OH_(g)	–234.8	–167.9	281.6
C₂H₅OH_(l)	–277.6	–174.8	160.7
C₂H₆_(g)	–84.0	–32.0	229.2
C₃H₆_(g)	20.0	74.62	226.9
C₃H₈_(g)	–103.8	–23.4	270.3
C₆H₆_(l)	49.1	124.5	173.4
Ca_(g)	177.8	144	154.9
Ca(OH)₂_(s)	–985.2	–897.5	83.4
Ca_(s)	0	0	41.6
Ca²⁺_(aq)	–543.0	–553.6	–56.2
Ca₃(PO₄)₂_(s)	-4120.8	–3884.7	236.0
CaC₂_(s)	–59.8	–64.9	70.0
CaCl₂_(s)	–795.4	–748.8	108.4
CaCO₃_(s)	–1207.6	–1129.1	91.7
CaF₂_(s)	–1228.0	–1175.6	68.5
CaH₂_(s)	–181.5	–142.5	41.4
CaO_(s)	–634.9	–603.3	38.1
CaS_(s)	–482.4	–477.4	56.5
CaSO₄_(s)	–1434.5	–1322.0	106.5
CH₃OH_(g)	–201.0	–162.3	239.9
CH₃OH_(l)	–239.2	–166.6	126.8
CH₄_(g)	–74.6	–50.5	186.3
CH₃CHO_(g)	–166.2	–127.6	263.8
CH₃CO₂H_(l)	–484.3	–389.9	159.8
CH₃CH₂OH_(l)	–277.6	–174.8	160.7
CH₃CN_(l)	40.6	86.5	149.6
CHCl₃_(g)	–102.7	6.0	295.7
CHCl₃_(l)	–134.1	–73.7	201.7
Cd_(s)	0	0	51.8
CdO_(s)	–258.4	–228.7	54.8
CdCl_(s)	–391.5	–343.9	115.3
Cl₂_(g)	0	0	223.1
Cl_(g)	121.3	105.3	165.2
Cl^–_(aq)	–167.1	–131.0	165.2
ClO^–_(aq)	–107.1	–36.8	42
ClO₂^–_(aq)	–67	17	101
ClO₃^–_(aq)	–104	–3	162
ClO₄^–_(aq)	–128.1	–8.52	184.0
ClO_(g)	101.8	98.1	226.6
ClO₂_(g)	102.5	120.5	256.8
CO_(g)	–110.5	–137.2	197.7
CO₂_(g)	–393.5	–394.4	213.8
COCl₂_(g)	–219.1	–204.9	283.5
Cr_(s)	0	0	23.8
Cr₂O₃_(s)	–1139.7	–1058.1	81.2
CrCl₃_(s)	–556.5	–486.1	123.1
Co_(s)	0	0	30.0
CoO_(s)	–237.9	–214.2	53.0
CoCl₂_(s)	–312.5	–269.8	109.2
Cs_(s)	0	0	85.2
CS₂_(g)	116.7	67.1	237.8
CS₂_(l)	89.0	64.6	151.3
CsCl_(s)	–443.0	–414.5	101.2
Cu_(s)	0	0	33.2
CuO_(s)	–157.3	–129.7	42.6
CuS_(s)	–53.1	–53.6	66.5
CuCl₂_(s)	–220.1	–175.7	108.1
CuCl_(s)	–137.2	–119.9	86.2
CuBr_(s)	–104.6	–100.8	96.1
CuI_(s)	–67.8	–69.5	96.7
CuSO₄_(s)	–771.4	–662.2	109.2
F_(g)	79.4	62.3	158.8
F₂_(g)	0	0	202.8
F^–_(g)	–335.4	–278.79	–13.8
Fe_(s)	0	0	27.3
Fe₂O₃_(s)	–824.2	–742.2	87.4
FeO_(s)	–272.0	–251.4	60.8
Fe₃O₄_(s)	–1118.4	–1015.4	146.4
Fe(OH)₃_(s)	–823.0	–696.5	106.7
FeCl₂_(s)	–341.8	–302.3	118.0
FeCl₃_(s)	–399.5	–334.0	142
FeSO₄_(s)	–928.4	–820.8	107.5
FeS_(s)	–100.0	–100.4	60.3
FeS₂_(s)	–178.2	–166.9	52.9
Ga_(s)	0	0	40.8
Ga₂O₃_(s)	–1089.1	–998.3	85.0
Ge_(s)	0	0	31.1
GeO_(s)	–261.9	–237.2	50.0
GeCl₄_(g)	–495.8	–457.3	347.7
GeO₂_(s)	–580.0	–521.4	39.7
H⁺_(aq)	0	0	0
H₂_(g)	0	0	130.7
H₂O_(g)	–241.8	–228.6	188.8
H₂O_(l)	–285.8	–237.1	70.0
H₃O⁺_(aq)	–285.83	–237.1	69.95
H₂O₂_(l)	–187.8	–120.4	109.6
H₂S_(g)	–20.6	–33.4	205.8
H₂SO₄_(l)	–814	–690.0	156.9
H₃PO₄	–1271.7	–1123.6	150.8
HBr_(g)	–36.3	–53.4	198.7
HCl_(g)	–92.3	–95.3	186.9
HCN_(g)	135.1	124.7	201.8
HF_(g)	–273.3	–275.4	173.8
HNO₃_(l)	-174.1	-80.7	155.6
HNO₃_(g)	–133.9	–73.5	266.9
H₂Se_(g)	29.7	15.9	219.0
Hg_(l)	0	0	75.9
Hg_(g)	61.4	31.8	175.0
HgO_(s)	–90.8	–58.5	70.3
HgS_(s)	–58.2	–50.6	82.4
HgCl₂_(s)	–224.3	–178.6	146.0
Hg₂Cl₂_(s)	–265.4	–210.7	191.6
HI_(g)	26.5	1.7	206.6
He_(g)	0	0	126.153
I₂_(g)	62.4	19.3	260.7
I₂_(s)	0	0	116.1
I^–_(aq)	–56.78	–51.57	106.5
K_(s)	0	0	64.7
K⁺_(aq)	–252.1	–283.7	101.2
KO₂_(aq)	–284.9	–239.4	116.7
KOH_(s)	–424.6	–378.9	78.9
KBr_(s)	–393.8	–380.7	95.9
KCl_(s)	–436.5	–408.5	82.6
KClO₃_(s)	–397.7	–296.3	143.1
KF_(s)	–567.3	–537.8	66.6
KI_(s)	–327.9	–324.9	106.3
Kr_(g)	0	0	164.085
Li_(s)	0	0	29.1
Li⁺_(aq)	–278.47	–293.31	12.2
Li₂O_(s)	–597.9	–561.2	37.6
LiOH_(s)	–484.9	–439.0	42.8
LiCl_(s)	–408.6	–384.4	59.3
Mg_(s)	0	0	32.7
Mg²⁺_(aq)	–467.0	–454.8	–137
Mg(OH)₂_(s)	–924.5	–833.5	63.2
MgCl₂_(s)	–641.3	–591.8	89.6
MgF₂_(s)	–1124.2	–1071.1	57.2
MgCO₃_(s)	–1095.8	–1012.1	65.7
MgO_(s)	–601.6	–569.3	27.0
MgSO₄_(s)	–1284.9	–1170.6	91.6
Mn_(s)	0	0	32.0
MnO_(s)	–385.2	–362.9	59.7
MnO₂_(s)	–520.0	–465.1	53.1
MnCl₂_(s)	–481.3	–440.5	118.2
MnCO₃_(s)	–894.1	–816.7	85.8
MnSO₄_(s)	–1065.25	–957.36	112.1
N₂_(g)	0	0	191.6
N₂H₄_(l)	50.6	149.3	121.2
N₂O_(g)	81.6	103.7	220.0
N₂O₄_(g)	11.1	99.8	304.4
N₂O₅_(g)	13.3	117.1	355.7
NH₃_(g)	–45.9	–16.4	192.8
NH₃_(aq)	–80.29	–26.50	111.3
NH₄⁺_(aq)	–133.3	–79.31	111.2
NH₄Cl_(s)	–314.4	–202.9	94.6
NH₄NO₃_(s)	–365.6	–183.9	151.1
(NH₂)₂CO_(s)	–333.1	–198	105
Na_(s)	0	0	51.3
Na⁺_(aq)	–240.3	–261.905	58.5
Na₂CO₃_(s)	–1130.7	–1044.4	135.0
NaCl_(s)	–411.2	–384.1	72.1
NaF_(s)	–576.6	–546.3	51.1
NaBr_(s)	–361.1	–349.0	86.8
NaI_(s)	–287.8	–286.1	98.5
NaNO₃_(s)	–467.9	–367.0	116.5
NaOH_(s)	–425.8	–379.7	64.4
Na₂O_(s)	-414.2	-375.5	75.1
Ne_(g)	0	0	146.328
Ni_(s)	0	0	29.9
NiO_(s)	–239.7	–211.7	37.99
NiCl₂_(s)	–305.3	–259.0	97.7
NO_(g)	91.3	87.6	210.8
NO₂_(g)	33.2	51.3	240.1
O_(g)	249.2	231.7	161.1
O₂_(g)	0	0	205.2
O₃_(g)	142.7	163.2	238.9
OH^–_(aq)	–230.0	–157.244	–10.9
OPb_(s) (massicot)	-217.3	-187.9	68.7
O₂Te_(s)	-322.6	-270.3	79.5
OTl₂_(s)	-178.7	-147.3	126.0
P(s, white)	0	0	41.1
P(s, red)	–17.6	–12.1	22.8
P₄_(g)	58.9	24.4	280.0
PH₃_(g)	5.4	13.4	210.2
P₄O₁₀_(s)	–2984.0	–2697.7	228.86
PCl₃_(g)	–287.0	–267.8	311.8
PCl₅_(g)	–374.9	–305.0	364.6
Pb_(s)	0	0	64.8
PbCl₂_(s)	–359.4	–314.1	136.0
PbO_(s)	–217.3	–187.9	68.7
PbO₂_(s)	–277.4	–217.3	68.6
PbS_(s)	–100.4	–98.7	91.2
Sb_(s)	0	0	45.7
Sb₄O₆_(s)	–1417.1	–1253.0	246.0
Se_(s)	0	0	42.7
Si_(s)	0	0	18.8
SiH₄_(g)	34.3	56.9	204.6
SiO₂_(s)	–910.7	–856.3	41.5
SiCl₄_(l)	–687.0	–619.8	239.7
SiC_(s)	–65.3	–62.8	16.6
Sn(s, white)	0	0	51.2
Sn(s, gray)	–2.1	0.13	44.1
SnO_(s)	–280.7	–251.9	57.2
SnO₂_(s)	–577.6	–515.8	49.0
SnCl₄_(s)	–511.3	–440.1	258.6
Sr_(s)	0	0	55.0
SrO_(s)	–592.0	–561.9	54.4
SrCl₂_(s)	–828.9	–781.1	114.9
S₈_(s)	0	0	31.80
S₈_(g)	102.30	49.63	430.23
SO₂_(g)	–296.8	–300.1	248.2
SO₃_(g)	–395.7	–371.1	256.8
SO₄^2–_(aq)	–909.3	–774.53	18.5
SF₆_(g)	–1220.5	–1116.5	291.5
Te_(s)	0	0	49.7
TeO₂_(s)	–322.6	–270.3	79.5
Ti_(s)	0	0	30.7
TiCl₄_(l)	–804.2	–737.2	252.3
TiCl₄_(g)	–763.2	–726.3	353.2
TiO₂_(s)	–944.0	–888.8	50.6
Tl_(s)	0	0	64.2
U_(s)	0	0	50.2
UO₂_(s)	–1085.0	–1031.8	77.0
UF₆_(g)	–2147.4	–2063.7	377.9
Xe_(g)	0	0	169.685
XeF4_(s)	–261.5	–138	316
Zn_(s)	0	0	41.63
ZnO_(s)	–350.5	–320.5	43.7
ZnCl₂_(s)	–415.1	–369.4	111.5
ZnS_(s)	–206.0	–201.3	57.7

instil

math science

tutoring

FORMULAS

QUANTITATIVE

SOLUTIONS

GAS

THERMODYNAMICS

KINETICS

ACID-BASE

ELECTROCHEMISTRY

COLLIGATIVE (AP)

ORGANIC

REACTIONS

POLYATOMIC

Group Trends:

[FO₃^– ≈ ClO₃^– ≈ BrO₃^– ≈ IO₃^–]

[CO₃^2– ≈ SiO₃^2-]

Modern IUPAC Oxyanion/Oxoanion Oxidation Numbers

REACTIVITY

SOLUBILITY

[] < 0.01 M = INSOLUBLE

[] > 0.1 M = SOLUBLE

K CONSTANTS

ACIDS/BASES

HALF-REACTIONS

Largest (positive) number gets reduced

FORMATION

CLASS PAGE SETTINGS

Streamlined Question View

Level of Difficulty

KEYBOARD SHORTCUTS

LINK

FAVORITES

OPTIONS

CLASS OPTIONS

FORMULAS

QUANTITATIVE

SOLUTIONS

GAS

THERMODYNAMICS

KINETICS

ACID-BASE

ELECTROCHEMISTRY

COLLIGATIVE (AP)

ORGANIC

REACTIONS

POLYATOMIC

Group Trends:

[FO3– ≈ ClO3– ≈ BrO3– ≈ IO3–]

[CO32– ≈ SiO32-]

Modern IUPAC Oxyanion/Oxoanion Oxidation Numbers

REACTIVITY

SOLUBILITY

[] < 0.01 M = INSOLUBLE

[] > 0.1 M = SOLUBLE

K CONSTANTS

ACIDS/BASES

HALF-REACTIONS

Largest (positive) number gets reduced

FORMATION

CLASS PAGE SETTINGS

Streamlined Question View

Level of Difficulty

KEYBOARD SHORTCUTS

LINK

[FO₃^– ≈ ClO₃^– ≈ BrO₃^– ≈ IO₃^–]

[CO₃^2– ≈ SiO₃^2-]