unit 2 transition metals

oxidation

Radii

generally decreases and then increases across a row

• cations smaller

• anions bigger

elctron config and ox states

-1/2 filled always wanna be d5 of d10

-catiosn loose s e-s before D e-s

electron config transition metals D^n

*e- config of transition metal cations are sometimes simplified to d^N notation - N = number of e-s in the D orbittal

ionic and covalent

*Transition metals have both ionic and covalent charater.

• covalent bonds : usually coordinate covalent bonds - both e-s are donated by one group (ligand)

color

• any metal with partially filled d-subshells has color

• e- transition occurs upon absorption of light energy (electronic transitiosn between d - orbs)

• filled and unfilled d subshells colorless

Combination reaction

Decompisition reaction

single replacement reaction

Double replacemnt reaction

• Most transition metals R paramagnetic ( 1 unpaired e-)

• soem ferromagnetic - permanet domains of magnetism

catalysis

• multiple ox states and coordination numbers are possible

• ligands can easily bond and multiple bonding site s are avaliable

• transition metals are generall coordinatively unsaturated

Metallurgy

*ore → metal

*alloy - moxing two mentals together

1. Scandium

• d²

• Sc⁺³

• Common to Al, Y, La bc nonne got de-s

• colorless and dia

• high intensity lamps or alloys

2. Titanium

• Ti⁺⁴

• ^{hight strenght/weight ratio}

• ^{low corrosion}

• ^C,Si

• ^Colorless

3. Vanadium

• +2 … +5

• V₂O_{5 - catalyst}

• tough and strong steel

4. Chromium

• +2, +3, +6 common ox

• corrosion resistant

• color red

5. Tungsten

• W - woldfam

• lightbulb

• Hard substance used in drills

6. Maganese

• +2 … +7

• - MnO₂

• in a dry cell battery ()

7. Techntium

• smallest element w/ no stable isotopes

• very radioactive

8. Iron

• most important

• +2, +3

• steel, alloys, heme

• 4.7% of earths crust

• M-CO

9. Cobalt

• +2, +3

• cathode, Lion battery cell

• color difficutl to isolate (blue)

• in vitamin B12

10. Nickel

• Corrosion resistant

• +2 ox state

• M-CO

• Doubly magic - extreamly stable (#protons and # neutrons)

• *NiCad cath

• catalysit fo hydrogenation

11. Platinum

• +2, +4

• Not very reactive

12. copper

• coinage metals cuz corrosion resistant

• bronse Cu Sn

• brass CU + Zn

• very conductive

• s e-s dominate its chemistry

13. Gold

• dont oxidize in air or water

• consistant conainge metal

• malleable

14. Zinc

• +2, d^10

• colorless, Dia

• galvanizing

• dry cell anode

• corrosion resistant

15. Cadium

• +2

• cathode NiCad

• Tabacco

Mercury

• +1, +2

• toxic

• liquid at STP

Lanthahides

• inner transition metals

• +3

• highly reactive w/ halogens and chalcogens

• F shell

• e-s lost in S shell before f e-s

vesper

coordinate compounds

transition metal ions, in combo with ligands form these compunds and counter ions

complex ion

Transition metal iosn in combo with ligand from - transition metal species has nonzero charge

counter ions

aniosn or catiosn needed to produce a compund with no net charge

• added to make coordination compund neutral

ligand

group surrounding transition metal ion

coordination number

number of nearest neighors to transition metal ion

• neighbors, usually ligands

• How to find: count number of ligands aroudn transition metal ion,

• can vary from 2-12 , 6 most common, 2 or 4

Ligand will have a

• lone pair of e-s ready to form a coordinate covalent bond

• neutral or negative charge

vesper summary

removing D e-s

d^n notation

As oxidation increases….

it becomes more acidic bc the ox state of metal increases so it enhances the metal oxide’s ability to accept e- pairs or donate protons.

3 types of magnetism…

As you move down the table.. (transition metals)

• The stability of oxidation states increases - bc the V e-s are further form the nuc - affects removal E.

Stability…

• influnced by # of e-s

• increases as more e-s in d orb

• most stable: Cu, Fe, Ni, Zn

Max e-s held in each orb?

• p - 6

• f - 14

• d - 10

• s - 2

Hybridization

• s, p, d orbs together

counter ion

• ion present to balance charge of the complex ion but is not directly bonded to the central metal by donating e-s

how many bonds can a single EDTA forms

• 6

Monodentate ligand

• ligand with 1 pair of e-s to attatch

polydent

• 2 or more pair of e-s

• Chelating

Bidentate ligand

2

tridentate

3

tetradentate

4

pentadente

5

Hexadentate ligand

6 donor sites

Why does the chelate effect lead to increased stability?

The replacement of multiple monodentate ligands by a single polydentate ligand results in increased entropy

monodenate ligands

polydente ligand

nomeclature new

• 1.cations named 1st, then anions

• 2. ligands named using:

• -ide → -o

• -ite → -ito

• - ate → -ato

• 3. number of ligands is named by prefix (mono, bi, tri, tetra, penta, hexa)

• Composite ligands - contain prefixes in its name (complicated ligands) but not all polyd ligands r composite,. YOU WILL HAVE TO USE composted PREFIXES EN,OX, ACAC AND EDTA

• 4. When naming complex ion, ligands are named alphabetically in order 1st (not including prefix) AND THEN the metal with ox state is named last

• A. if complex ion is an anion, metal nust be named in latin (if possible) with the suffix - ate. latin stem in table below

• (Iron - ferrate, Copper - cuprate, Tin - stannate, Silver Argentate, lead - plumbate, Gold - Aurate)

• b. if complex ion is cation, metal is named english with no additional suffix

• 5. When writing a formula: list ligands in abc order

nomen new summary

• 1. identift coordination sphehre - central metal aion and ligands

• 2. ligand 1st - in abc order

• A. neutral -

• ammine - NH3

• aqua - H2O

• corbonyl - CO

• nitrosyl - NO

• B. Anionic - end with O

• Cl- - chloro

• OH- → hydroxo

• CN- > cyano

• O²- → oxo

• C. prefixes

• mono

• di

• tri

• tetra

• penta

• hexa

• D polydente ligands like EDTA

• Bis - 2

• Tris - 3

• Tetrakis - 4

• 3. metal name

• a.is neutral or cationic : use normal metal name

• b. Complex is anionic - at ate to the end

• 4 dtermien and add metal od state

• use form : ox state of metal - overall charge - sum of ligand charges

• 5. combo everything

If there are counter ions : name the cation 1st then anion - leave a space in between co

nomeclature old 1. Binary ionic compounds

• Metals give e-s - catiosn

• metals take e-s - anions

• state cation then anion

• 1. A name = of element

• 2. B Name = elemnt name end s with - ide

• complete charge shoudl = 0

Nomen old 2 - metals w/ more than 1 OX state

• metals with more than 1 oxidation state

• write name and then in () roman numeral of ox state given

Nonmen 2 - acids and anions - Cl

acid name dep on # of atoms attached to Cl

• parent - chloric acid

• 1 or more - perchloric acid

• 1 less is chlorous acid

• 2 less - hypo chloric acid

• no O - hydrochloric

End depends of ending of acid

• anions ate → ic acid

• anions ite → ous acid

• acid from only 2 e- (NO O) - anion

Nomen 3 oxianions

• ite → ate by removing 1 O

• Per - 1 more O than ate

• hypo 1 less O than ite

polyatomic ions

• ate - more O

• Ite - less o

• Per - ate is most O

• hypo -ite is least O

nomen binary covalent

• Nonmetals can bond with other nonmetals

*binary covalent comps always end with -ide

• mono - neber used for 1st e-

• di - 2

• tri - 3

• tetra - 4

• penta - 5

• hexa - 6

• hepta - 7

• octa - 8

• nona 9

• deca 10