Transition Metals, Ions & Naming Conventions

Flashcards covering electronic configurations of transition metals and ions, common anions and polyatomic ions, transition metal ion nomenclature, metal occurrences and applications, and definitions of oxidation state vs. formal charge.

Transition Metal Ion Electron Loss (General Rule)

Transition metal ions lose 4s electrons before (n-1)d electrons.

Scandium (Sc) Electronic Configuration

[Ar] 3d1 4s2

Scandium ion (Sc2+) Electronic Configuration

[Ar] 3d1

Scandium ion (Sc3+) Electronic Configuration

[Ar]

Vanadium (V) Electronic Configuration

[Ar] 4s2 3d3

Vanadium (II) ion (V2+) Electronic Configuration

[Ar] 3d3

Vanadium (III) ion (V3+) Electronic Configuration

[Ar] 3d2

Vanadium (V) ion (V5+) Electronic Configuration

[Ar] 3d0

Iron (Fe) Electronic Configuration

[Ar] 4s2 3d6

Iron (II) ion (Fe2+) Electronic Configuration

[Ar] 3d6

Iron (III) ion (Fe3+) Electronic Configuration

[Ar] 3d5 (half-filled d-orbital)

Cobalt (Co) Electronic Configuration

[Ar] 4s2 3d7

Cobalt (II) ion (Co2+) Electronic Configuration

[Ar] 3d7

Cobalt (III) ion (Co3+) Electronic Configuration

[Ar] 3d6

Manganese (Mn) Electronic Configuration

[Ar] 4s2 3d5

Hydride

H- anion

Fluoride

F- anion

Chloride

Cl- anion

Bromide

Br- anion

Iodide

I- anion

Oxide

O2- anion

Sulfide

S2- anion

Nitride

N3- anion

Phosphide

P3- anion

Ammonium

NH4+ polyatomic ion

Nitrite

NO2- polyatomic ion

Nitrate

NO3- polyatomic ion

Sulfite

SO3 2- polyatomic ion

Sulfate

SO4 2- polyatomic ion

Hydrogen sulfate (Bisulfate)

HSO4- polyatomic ion

Hydroxide

OH- polyatomic ion

Cyanide

CN- polyatomic ion

Phosphate

PO4 3- polyatomic ion

Hydrogen phosphate

HPO4 2- polyatomic ion

Dihydrogen phosphate

H2PO4- polyatomic ion

Carbonate

CO3 2- polyatomic ion

Hydrogen carbonate (Bicarbonate)

HCO3- polyatomic ion

Hypochlorite

ClO- polyatomic ion

Chlorite

ClO2- polyatomic ion

Chlorate

ClO3- polyatomic ion

Perchlorate

ClO4- polyatomic ion

Acetate

C2H3O2- polyatomic ion

Permanganate

MnO4- polyatomic ion

Dichromate

Cr2O7 2- polyatomic ion

Chromate

CrO4 2- polyatomic ion

Peroxide

O2 2- polyatomic ion

Ferric ion

Iron (III) ion, Fe3+

Ferrous ion

Iron (II) ion, Fe2+

Cupric ion

Copper (II) ion, Cu2+

Cuprous ion

Copper (I) ion, Cu+

Cobaltic ion

Cobalt (III) ion, Co3+

Cobaltous ion

Cobalt (II) ion, Co2+

Stannic ion

Tin (IV) ion, Sn4+

Stannous ion

Tin (II) ion, Sn2+

Plumbic ion

Lead (IV) ion, Pb4+

Plumbous ion

Lead (II) ion, Pb2+

Mercuric ion

Mercury (II) ion, Hg2+

Mercurous ion

Mercury (I) ion, Hg2 2+

Native ores

Ores where metals like gold (Au), silver (Ag), platinum (Pt), and copper (Cu) are found in elemental form.

Oxide ores

Ores containing metals like iron, aluminum, manganese, and tin in oxide form.

Sulfide ores

Ores containing metals like zinc, cadmium, mercury, copper, lead, nickel, cobalt, and silver in sulfide form.

Halide ores

Ores containing metals like sodium, potassium, magnesium, calcium, and silver in halide form.

Hard water

Water containing excessive amounts of Ca2+ and Mg2+ ions, which form insoluble salts with soap and detergent.

Bronze

An alloy typically composed of 70-95% Cu, 1-25% Zn, and 1-18% Sn.

Sterling Silver

An alloy composed of 92.5% Ag and 7.5% Cu.

Stainless Steel

An alloy primarily of Fe with 14-18% Cr and 7-9% Ni, used for cutlery and instruments.

Iron (Catalyst)

Used as a catalyst in processes like ammonia manufacture and diamond manufacture.

Nickel (Catalyst)

Used as a catalyst in the steam-hydrocarbon reforming process and in H2 + O2 fuel cells.

Platinum (Catalyst)

Used in finely divided forms (Pt black or Pt sponge) as a catalyst in the oxidation of SO2 (contact process) and ammonia to NO.

Metal hydrides

Compounds like CaH2, used as chemical dehydrating and reducing agents.

Sodium Carbonate (Na2CO3)

Used for CO2 absorption.

Calcium Carbonate (CaCO3)

Used in lime production.

Zeolites

Porous aluminosilicate minerals (Mx/n[(AlO2)x(SiO2)y]•2H2O) with applications in various industrial processes.

Oxidation state

The hypothetical charge on an ion corresponding to the number of electrons it gains or loses, assigning electrons in a bond to the more electronegative atom.

Formal charge

A hypothetical charge assigned to an atom in a molecule by equally distributing electrons in a bond between atoms, calculated as (# valence shell electrons) - (# lone pair electrons) - (1/2 # bonding electrons).