transition metals and inorganic chem

week 11, question 4

d-block elements

outer most electrons in d-subshell

4s fills

BEFORE 3d

transition metal

d-block element with at least ONE STABLE ION with an INCOMPLETE D-SUBSHELL of electrons

why are physical properties of transition elements in the same period similar

• small changes in first IE across period

• increase in nuclear charge BUT 3-d e-s are shielded

• very small increase in nuclear attraction

properties of transition elements

• good conductors

• strong + hard

• high mp and bp

why are transition metals good conductors

delocalised e-s free to move through structure

transition metals and oxidation

show variable oxi numbers in their ions and compounds and participate in redox reactions

highest possible oxidation state =

group number

transition metals and colour

colour changes according to oxidation state

transition metals and catalysts

frequently used as catalysts because of PARTLY FILLED D-ORBITALS and VARIABLE OXIDATION number

what type of catalyst a t-metals used as

heterogenous

transition metals can form

complex ions

complex ion =

t-metal ion surrounded by ions/ligands bonded to it by coordinate bonds

ligand =

ion/molecule with a LONE PAIR of electrons that forms a COORDINATE BOND with a TRASNITION METAL ION

coordination number =

number of coordinate bonds to ligands

coord number 2=

linear, 180

coord number 6=

octahedral, 90

monodentate ligands

donate ONE LONE PAIR of e-s to metal ion to form ONE coordinate bond

bidentate ligands

donate TWO lone pairs of e-s to metal ion to form coordinate bonds

multidentate ligands

donate 2+ lone pairs of e-s to metal ion to form 2+ coordinate bonds to a metal ion

scandium and zinc

NOT t-metals = only ONE oxidation state

E_cell

E_cathode - E_anode

subshell configuration

[Ar] 3d^x

comparing lattice energy

CSA: charge, size, attraction

cathode

positive

anode

negative

lewis base

H2O

coord numer 4=

square planar, 90 / tetrahedral, 109.5