Fe3+

Fe2+iron (III)

iron (II)

26atomicnumberionchargeionname

symbol (IUPAC)

KEY

58 59 60 61 62 63 64 65 66 67 68 69 70 71

90 91 92 93 94 95 96 97 98 99 100 101 102 103

Ce3+cerium

Pr3+praseodymium

Nd3+neodymium

Pm3+promethium

Sm3+samarium(III)

samarium(II)

Eu3+

Eu2+europium (III)

europium (II)

Th4+thorium

Pa5+

Pa4+protactinium(V)

protactinium(IV)

U6+

U4+uranium (VI)

uranium (IV)

Gd3+gadolinium

Tb3+terbium

Dy3+dysprosium

Ho3+holmium

Er3+erbium

Tm3+thulium

Yb3+

Yb3+ytterbium(III)

ytterbium(II)Sm2+

Lu3+lutetium

Np5+Pu4+

Pu6+plutonium(IV)

Am3+

Am4+americium(IV)

americium(III)neptunium

Bk3+

Bk4+berkelium(IV)

berkelium(III)Cm3+curium

Cf3+californium

Es3+einsteinium

Fm3+fermium

Md2+

Md3+mendelevium (II)

mendelevium (III)

Lr3+lawrencium

No2+

No3+nobelium(II)

nobelium(III)plutonium(VI)

PERIODIC TABLE OF IONSacetatearsenatearsenitebenzoateboratebromatecarbonatechloratechloridechloritechromatecyanatecyanidedichromate

CH3COO–AsO43–AsO33–C6H5COO–BO33–BrO3 –CO32–ClO3 –Cl–ClO2 –CrO42–CNO–CN–Cr2O72–

oxalateperchlorateperiodatepermanganateperoxidephosphatepyrophosphatesulfatesulfitethiocyanatethiosulfate

ammoniumhydronium

C2O42–ClO4 –IO4 –MnO4 –O22–PO43–P2O74–SO42–SO32–SCN–S2O32–

NH4+H3O+

POSITIVE POLYATOMIC IONS

TABLE OF POLYATOMIC IONS

H2PO4 –HCO3 –HC2O4 –

HSO4 –HS–HSO3 –OH–ClO–IO3 –HPO42–NO3 –NO2 –SiO44–

hydrogen carbonatehydrogen oxalatehydrogen sulfatehydrogen sulfidehydrogen sulfitehydroxidehypochloriteiodate

nitratenitriteorthosilicate

monohydrogen phosphate

dihydrogen phosphate

1 2

3 4 5 6 7 8 9 10

13 14 15 16 17 1811 12

19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36Ti4+titanium (IV)

Ti3+titanium (III)

V3+vanadium(III)

V5+vanadium (V)

Cr3+

Cr2+chromium (III)

chromium (II)

Mn2+

Mn4+manganese(II)

manganese(IV)

Fe3+

Fe2+iron (III)

iron (II)

Co2+

Co3+cobalt (II)

cobalt (III)

Ni2+

Ni3+nickel (II)

nickel (III)

Cu2+

Cu+copper (II)

copper (I)

Ga3+gallium

Sc3+scandium

Y3+yttrium

La3+lanthanum

Ac3+actinium

Zr4+zirconium

Hf4+hafnium

Nb5+

Nb3+niobium (V)

niobium(III)

37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54

Mo6+molybdenum

Rh3+rhodium

Ru3+

Ru4+ruthenium(III)

ruthenium(IV)

Pd2+

Pd4+paladium(II)

paladium(IV)

Ag+silver

Cd2+cadmium

Pt4+

Pt2+platinum(IV)

platinum(II)

55 56 57 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86Au3+

Au+gold (III)

gold (I)

Hg2+

Hg+mercury (II)

mercury (I)

Tl+

Tl3+thallium (I)

thallium(III)

Pb2+

Pb4+lead (II)

lead (IV)

Bi3+

Bi5+bismuth(III)

bismuth(V)

Sn4+

Sn2+tin (IV)

tin (II)

Sb3+

Sb5+antimony(III)

antimony(V)

Tc7+

Ta5+tantalum

W6+tungsten

Re7+rhenium

Os4+osmium

Ir4+iridium

87 88 89

H+hydrogen

Li+lithium

Be2+beryllium

Na+sodium

Mg2+magnesium

K+potassium

Ca2+

Rb+rubidium

Sr2+strontium

Cs+cesium

Ba2+

calcium

barium

Fr+francium

Ra2+radium

Bboron

Ccarbon nitride

N3-oxideO2-

fluorideF-

neonNe

Al3+aluminum

Sisilicon phosphide

P3-sulfiide

S2-chloride

Cl-argonAr

heliumHe

Zn2+zinc

In3+indium

Ge4+germanium

As3-arsenide selenide

Se2-bromide

Br-krypton

Kr

tellurideTe2-

Po2+polonium(II)

polonium(IV)Po4+

iodideI-

xenonXe

astatideAt-

radonRn

hydrideH-

1

1

2

3 4 5 6 7 8 9 10 11 12

13 14 15 16

17 18

technetium

List of Common Multivalent Ions

The following elements form multivalent ions, and therefore require a

Roman numeral charge when writing the name of the compound. Rare and

synthetic elements are not included in this list.

Element Sym. Possible Charges

Element Sym. Possible Charges

Titanium Ti +2, +3, +4 Tin Sn +2, +4 Vanadium V +2, +3, +4, +5 Rhenium Re +4, +6, +7 Chromium Cr +2, +3, +6 Osmium Os +3, +4 Manganese Mn +2, +3, +4, +7 Iridium Ir +3, +4

Iron Fe +2, +3 Platinum Pt +2, +4 Cobalt Co +2, +3 Gold Au +1, +3 Nickel Ni +2, +3 Mercury Hg +1, +2 Copper Cu +1, +2 Thallium Tl +1, +3

Niobium Nb +2, +5 Lead Pb +2, +4 Molybdenum Mo +3, +6 Bismuth Bi +3, +5

Palladium Pd +2, +4 Polonium Po +2, +4

Steps to Determine Charge from the Chemical Formula

1. Find total negative charge on all anions.

2. Divide value by number of cations to give charge on one multivalent

cation.

Electron Configuration

Copyright 1999, Washington University, All Rights Reserved.

E XX

180°

VSEPR GeometriesStericNo.

Basic Geometry0 lone pair

1 lone pair 2 lone pairs 3 lone pairs 4 lone pairs

2

Linear

3

Trigonal Planar Bent or Angular

4

Tetrahedral Trigonal Pyramid Bent or Angular

5

Trigonal Bipyramid Sawhorse or Seesaw T-shape Linear

6

Octahedral Square Pyramid Square Planar T-shape Linear

EX

X

X

120° EXX

< 120°

X

E

XX

X< 90°

< 120°

X

EXX

X 109° EXX

X

< 109°

E

Solubility Product Constant (Ksp) Values at 25 oC Salt Ksp Salt Ksp Salt Ksp Salt Ksp

Bromides Carbonates Oxalates Sulfides PbBr2 6.610-6 MgCO3 6.810-6 MgC2O4 4.810-6 CoS 2.010-25

CuBr 6.310-9 NiCO3 1.310-7 FeC2O4 210-7 CuS 6.310-36 AgBr 5.410-13 CaCO3 5.010-9 NiC2O4 110-7 FeS 6.310-18

Hg2Br2 6.410-23 SrCO3 5.610-10 SrC2O4 510-8 HgS 1.610-52

Chlorides MnCO3 2.210-11 CuC2O4 310-8 PbS 8.010-28

PbCl2 1.210-5 CuCO3 2.510-10 BaC2O4 1.610-7 CdS 810-27

CuCl 1.710-7 CoCO3 1.010-10 CdC2O4 1.410-8 MnS 2.510-10

AgCl 1.810-10 FeCO3 2.110-11 ZnC2O4 1.410-9 NiS 310-19

Hg2Cl2 1.410-18 ZnCO3 1.210-10 CaC2O4 2.310-9 AgS 610-50

Fluorides Ag2CO3 8.110-12 Ag2C2O4 3.510-11 ZnS 1.110-21

BaF2 1.810-7 CdCO3 6.210-12 PbC2O4 4.810-12 Hydroxides MgF2 7.410-11 PbCO3 7.410-14 Hg2C2O4 1.810-13 Ba(OH)2 5.010-3 SrF2 2.510-9 Chromates MnC2O4 110-15 Sr(OH)2 6.410-3 CaF2 1.510-10 CaCrO4 7.110-4 Phosphates Ca(OH)2 4.710-6

Iodides SrCrO4 2.210-5 Ag3PO4 8.910-17 Mg(OH)2 5.610-12 PbI2 8.510-9 Hg2CrO4 2.010-9 AlPO4 9.810-21 Mn(OH)2 2.110-13 CuI 1.110-12 BaCrO4 1.210-10 Mn3(PO4)2 110-22 Cd(OH)2 5.310-15 AgI 8.510-17 Ag2CrO4 2.010-12 Ba3(PO4)2 310-23 Pb(OH)2 1.210-15

Hg2I2 4.510-29 PbCrO4 2.810-13 BiPO4 1.310-23 Fe(OH)2 4.910-17 Sulfates Acetates Sr3(PO4)2 410-28 Ni(OH)2 5.510-16

CaSO4 7.110-5 AgCH3COO 4.410-3 Pb3(PO4)2 7.910-43 Co(OH)2 1.110-15 Hg2SO4 6.810-7 Hg2(CH3COO)2 410-10 Ca3(PO4)2 110-26 Zn(OH)2 4.110-17 Ag2SO4 1.210-5 Arsenates Cu(OH)2 1.610-19 SrSO4 3.510-7 Pb3(AsO4)2 410-36 Hg(OH)2 3.110-26 PbSO4 1.810-8 Mg3(AsO4)2 210-20 Sn(OH)2 5.410-27 BaSO4 1.110-10 Cr(OH)3 6.710-31

Fe(OH)3 2.610-39 Al(OH)3 1.910-33

EQUILIBRIUM CONSTANTSAcid-Ionization Constants, Ka, at 25°C.

Substance Formula KaAcetic acid HC2H302 1.7 10-5

Benzoic acid HC7H502 6.3 10-5

Boric acid H3B03 5.9 10-10

Carbonic acid H2C03 4.3 10-7

HC03 4.8 10-11

Chlorous acid HClO2 1.1 x 10-2

Cyanic acid HOCN 3.5 10-4

Formic acid HCH02 1.7 10-4

Hydrocyanic acid HCN 4.9 10-10

Hydrofluoric acid HF 6.8 10-4

Hydrogen sulfate ion HS04 1.1 10-2

Hydrosulfuric acid H2S 8.9 10-8

HS 1.2 10-13

Hypobromous acid HBrO 2.1 x 10-9

Hypochlorous acid HClO 3.5 10-8

Nitrous acid HN02 4.5 10-4

Oxalic acid H2C204 5.6 10-2

HC204 5.1 10-5

Phosphoric acid H3P04 6.9 10-3

H2P04 6.2 10-8

HPO42 4.8 10-13

Phosphorous acid H3P03 1.6 10-2

H2P03 7 10-7

Propionic acid HC3H502 1.3 10-5

Pyruvic acid HC3H303 1.4 10-4

Sulfuric acid H2SO4 strongHSO4 1.3 x 10-2

Sulfurous acid H2S03 1.3 10-2

HS03 6.3 10-8

Base Ionization Constants, Kb, at 25°C.

Substance Formula KbAmmonia NH3 1.8 10-5

Aniline C6H5NH2 4.2 10-10

Dimethylamine (CH3)2NH 5.1 10-4

Ethylamine C2H5NH2 4.7 10-4

Hydrazine N2H4 1.7 10-6

Hydroxylamine NH20H 1.1 10-8

Methylamine CH3NH2 4.4 10-4

Pyridine C5H5N 1.4 10-9

Urea NH2CONH2 1.5 10-14

Rules for Assigning Oxidation Numbers

Oxidation numbers are real or hypothetical charges onatoms, assigned by the following rules:

1. Atoms in elements are assigned 0.

2. All simple monatomic ions have oxidation numbersequal to their charges. (e.g., all Group IA ions are +1;all group IIA ions are +2; all the following ions haveoxidation numbers given by their charges - Fe2+, Al3+,S2-, N3-)

3. Fluorine is always -1 in its compounds.

4. Halogens are usually -1, except when a central atom orwhen combined with a more electronegative element (e.g., assign I as -1 in NI3, but +3 in ICl3).

5. Oxygen is -2 in most of its compounds, except in caseslike peroxides (H2O2, Na2O2) where it is -1.

6. Hydrogen is usually +1, except in hydrides withelectropositive elements, particularly with metalcations, where it is -1 (e.g., NaH, CaH2, BH4

-).

7. The sum of all oxidation numbers for a neutralcompound is zero; the sum is the charge on the speciesfor a complex ion.

Standard Reduction Potentials (at 25ْC, 101.325 kPa, 1M)

Half-Reaction Eْ (Volts) Li+ + e- → Li -3.040 K

+ + e

- → K -2.942

Rb

+ + e

-→ Rb -2.942

Cs+ + e

-→ Cs -2.923

Ba2+

+ 2e-→ Ba -2.92

Sr2+

+ 2e- → Sr -2.89

Ca2+

+ 2e- → Ca -2.84

Na+ + e

- → Na -2.713

La3+

+ 3e- → La -2.37

Mg2+

+ 2e- → Mg -2.356

Ce3+

+ 3e- → Ce -2.34

Nd3+

+ 3e- → Nd -2.32

H2 + 2e- → 2H

- -2.25

Sc3+

+ 3e- → Sc -2.03

Be2+

+ 2e- → Be -1.97

Al3+

+ 3e- → Al -1.676

U3+

+ 3e- → U -1.66

Ti2+

+ 2e- → Ti -1.63

Hf4+

+ 4e-→ Hf -1.56

No3+

+ 3e- → No -1.2

Mn2+

+ 2e- → Mn -1.18

Cr2+

+ 2e- → Cr -0.90

2H2O + 2e- → H2 + 2OH

- -0.828

Zn2+

+ 2e- → Zn -0.7626

Cr3+

+ 3e- → Cr -0.74

Ga3+

+ 3e- → Ga -0.529

U4+

+ e- → U

3+ -0.52

2CO2 + 2H+ + 2e

- → H2C2O4 -0.475

S + 2e- → S

2- -0.447

Fe2+

+ 2e- → Fe -0.44

Cr3+

+ e- → Cr

2+ -0.424

2H2O + 2e- → H2 + 2OH

-(10

-7M) -0.414

Cd2+

+ 2e- → Cd -0.4025

Ti3+

+ e- → Ti

2+ -0.37

PbI2 + 2e- → Pb + 2I

- -0.365

PbSO4 + 2e- → Pb + SO4 -0.3505

In3+

+ 3e- → In -0.3382

Tl+ + e

- → Tl -0.3363

Co2+

+ 2e- → Co -0.277

H3PO4 + 2H+ + 2e

- → H3PO3 + H2O -0.276

Ni2+

+ 2e- → Ni -0.257

Sn2+

+ 2e- → Sn -0.136

Pb2+

+ 2e- → Pb -0.1251

Hg2I2 + 2e- → 2Hg + 2I

- -0.0405

Fe3+

+ 3e- → Fe -0.04

2H+ + 2e

- → H2 0.0000

Sn4+

+ 2e- → Sn

2+ 0.154

Half-Reaction EْVolts SO4

2- + 4H

+ + 2e

- → H2SO3 + H2O 0.158

Cu2+

+ e- → Cu

+ 0.159

HAsO2 + 3H+ + 3e

- → As + 2H2O 0.248

UO22+

+ 4H+ + 2e

- → U

4+ + 2H2O 0.27

Bi3+

+ 3e- → Bi 0.3172

Cu2+

+ 2e- → Cu 0.340

O2 + 2H2O + 4e- → 4OH

- 0.401

Cu+ + e

- → Cu 0.520

I2 + 2e- → 2I

- 0.5355

H3AsO4 + 2H+ + 2e

- → HAsO2 + 2H2O 0.560

O2 + 2H+ + 2e

- → H2O2 0.695

Rh3+

+ 3e- → Rh 0.7

Tl3+

+ 3e- → Tl 0.72

Fe3+

+ e- → Fe

2+ 0.771

NO3- + 2H

+ + e

- → NO2 + H2O 0.775

Hg22+

+ 2e- → Hg 0.7960

Ag+ + e

- → Ag 0.7991

O2 + 4H+(10

-7M) + 4e

- → 2H2O 0.815

AmO2+ + 4H

+ + e

- → Am

4+ + 2H2O 0.82

NO3- + 2H

+ + 2e

- → NO2

- + H2O 0.835

OsO4 + 8H+ 8e

- → Os + 4H2O 0.84

Hg2+

+ 2e- → Hg 0.8535

2Hg2+

+ 2e- → Hg2

2+ 0.9110

Pd2+

+ 2e- → Pd 0.915

NO3- + 4H

+ + 3e

- → NO(g) + 2H2O 0.957

Br2 + 2e- → 2Br

- 1.0652

SeO42-

+ 4H+ + 2e

- → H2SeO3 + H2O 1.151

Ir3+

+ 3e- → Ir 1.156

Pt2+

+ 2e- → Pt 1.188

O2 + 4H+ + 4e

- → 2H2O 1.229

Tl3+

+ 2e- → Tl

+ 1.25

Pd4+

+ 2e- → Pd

2+ 1.263

Cl2 + 2e- → 2Cl

- 1.35828

Au3+

+ 2e- → Au

+ 1.36

Cr2O72-

+ 14H+ + 6e

- → 2Cr

3+ + 7H2O 1.36

MnO4- + 8H

+ 5e

- → Mn

2+ + 4H2O 1.51

Au3+

+ 3e- → Au 1.52

H5IO6 + H+ + 2e

- → IO3

- + 3H2O 1.603

2HBrO + 2H+ + 2e

- → Br2 + 2H2O 1.604

PbO2 + SO42-

+ 4H+ + 2e

- → PbSO4 + 2H2O 1.698

H2O2 + 2H+ + 2e

- → 2H2O 1.763

Au+ + e

- → Au 1.83

Co3+

+ e- → Co

2+ 1.92

S2O82-

+ 2e- → 2SO4

2- 1.96

O3 + 2H+ + 2e

- → O2 + H2O 2.075

F2 + 2e- → 2F

- 2.87

F2 + 2H+ +2e

- → 2HF 3.053