Transition Metals and Complexes Nomenclature

H2O

aqua

NH3

ammine

CO

carbonyl

CH3NH2

methylamine

NO

nitrosyl

C5H5N

pyridine

F-

fluoro

Cl-

chloro

Br-

bromo

I-

iodo

O(2-)

oxo

OH-

hydroxo

CN-

cyano

SO4(2-)

sulfato

S2O3(2-)

thiosulfato

NO2-

nitrito-N-

ONO-

nitrito-O-

SCN-

thiocyanato-S-

NCS-

thiocyanato-N-

NH2CH2CH2NH2 (bidentate)

ethylenediamine (en)

C2O4(2-) (bidentate)

oxalato (ox)

C4H13N3 (tridentate)

diethylenetriamine

C10H16N2O8(4-) (hexadentate)

ethylenediaminetetraacetic acid (EDTA)

Scandium (Sc)

Common O.S. = 0, +3

no d-electrons in ions (colorless and diamagnetic)

Titanium (Ti)

Common O.S. = 0, +4

similar chemistry to C, Si

strong, light-weight metal

used in paint as brightener

Vanadium (V)

Common O.S. = 0, +5

used in alloys to strengthen material

toxic

Nobium (Nb) & Tantalum (Ta)

Common O.S. = 0, +5

named after Greek mythology

Nobium is a material for superconductors

Chromium (Cr)

Common O.S. = 0, +3, +4, +6

first family with multiple oxidation states found in nature

name derived from greek word for color

toxic

Molybdenum (Mo) & Tungsten (W)

Common O.S. = 0, +3, +4, +6

biologically important for enzymes/pigments

W has a high melting point (used for light bulb filaments)

Manganese (Mn)

most O.S. of first row transition metals +2, +3, +4, +6, +7

only found as an ore in nature (not as a pure metal)

used as a catalyst

used in alkaline batteries

used as a strengthening component in steel

used as a cofactor to many enzymes

permanganates are very strong oxidizing agents

Technetium (Tc)

lightest radioactive element

man made

Iron (Fe)

Possible O.S. = +2 to +6, Common O.S. = +2, +3

major component in steel

most common element by mass

oxygen transport, redox enzymes

Cobalt (Co)

O.S.= +2, +3

D to D transitions

very rare to find pure

blue

Rhodium (Rh)

hard, corrosion resistant, chemically inert

very rare

excellent metal for plating jewelry

Iridium (Ir)

rare, comes from outer space

Nickel (Ni) & Palladium (Pd) & Platinum (Pt)

O.S. = +2

stable, less reactive metals

all are good catalysts

Nickel: coins, batteries

Platinum: rare, unreactive

Copper (Cu)

O.S. = +1, +2

excellent conductor, durable

Silver (Ag)

O.S. = +1

highest thermal/electrical conductivity and reflectivity

Gold (Au)

O.S. = +1, +3

unreactive, malleable

Zinc (Zn)

O.S. = +2

corrosion resistant, toxic

Cadmium (Cd)

Common O.S. = +2

toxic, used in batteries

Mercury (Hg)

toxic, liquid at room temperature

Alkali Metals (Li, Na, K, Rb, Cs, Fr)

Common O.S. = +1

react vigorously with water to form H2 gas

highly reactive

react with oxygen to form oxides, peroxides, and superoxides

Lithium: important for batteries

Hydrogen (H)

lightest element

small, low intermolecular forces

non-metal

Alkaline Earth Metals (Be, Mg, Ca, Sr, Ba, Ra)

Common O.S. = +2

low densities, low melting/boiling points, low solubility

Beryllium: smaller, harder, higher melting point/ionization energy, less reactive

Radium: radioactive

Magnesium/Calcium: lower solubility (hard water)

Barium: toxic, absorbs X-rays, used in gastromedicine

Group 13 (B, Al, Gam In, Tl)

Common O.S. = +1, +3

metals are soft, relatively reactive

Aluminium: +3, aluminum oxide is the basis for many gems

Boron: not a metal, supports 6 electrons in valence, can form dimers

Gallium: higher density liquid, low melting point

Group 14 (C, Si, Ge, Sn, Pb)

common OS: +2, +4

carbon and silcon can be -4

Carbon: can form pi bonds, basis for life

Silicon: Si-O bonds are stronger than Si-Si bonds, basis for biological world

Germanium: rare, semiconductors

Tin: soft metal, silvery color

Lead: soft, toxic, low melting point

Group 15 (N, P, As, Sb, Bi)

Common O.S. = multiple

Nitrogen: stable or highly reactive, can form pi bonds, DNA, nitrogen fixation, atmosphere

Phosphorus: larger, d-orbitals available for electrons, ATP/ADP, fertilizer

Arsenic: toxic, semi-metal

Bismuth: heavy, not toxic, substitute for lead

Group 16 (O, S, Se, Te, Po)

Common O.S. = 0, -1, -2

Oxygen: found as O2 and O3 (toxic)

Sulfur: unpleasant smell, many uses, 30 allotropes

Polonium: radioactive, lethal, present in tobacco

Halogens (F, Cl, Br, I, At)

Common O.S. = -1

atomic form not found in nature (diatomic molecules)

high electronegativity, polar covalent bonds

oxyacids: HClO, HClO2, HClO3

Fluorine: small, high electronegativity, used in dental care, gives stability to CFCs and PFAs

Astatine: radioactive, short half life

Noble Gases (He, Ne, Ar, Kr, Xe, Rn)

Common O.S. = 0

low reactivity, colorless, odorless, neutral

Helium: forms no compounds, escapes atmosphere

Neon: no compounds

Argon: major component of air

Krypton/Xenon: many stable compounds possible with expanded octet

Radon: radioactive

oxides

O^(2-)

peroxides

O2^(2-)

superoxides

O2^(1-)