1.4 Transition Metals Flashcards
transition metal
metals with an incomplete d subshell in at least one of their ions
metals with an incomplete d subshell in at least one of their ions
transition metal
when are TM ions formed
TMs losing electrons from the 4s orbital
properties of TMs
- have atoms or ions with an incomplete d subshell (except Zn 2+)
- can form complexes
- have variable oxidation states (numbers)
- form coloured ions
- show catalytic ability
transition metal complex
a central metal ion surrounded by ligands
oxidation number
the charge on the ion if the element was isolated
rules for finding oxidation numbers
- oxidation number of an uncombined element is 0
- for monatomic ions, the oxidation number is the same as the charge on the ion
- oxygens oxidation number is -2
- hydrogens oxidation number is +1, however in metallic hydrides it is -1
- the sum of all the oxidation numbers of all the atoms in a molecule or neutral compound must add up to 0
- the sum of all the oxidation numbers of all the atoms in a polyatomic ion is equal to the charge on the ion
oxidation
increase in oxidation number
increase in oxidation number
oxidation
reduction
decrease in oxidation number
decrease in oxidation number
reduction
what happens to oxidising agents
they are reduced
what happens to reducing agents
they are oxidised
oxidation agents value
oxidation number >3
ligand
a molecule or negatively charged ion with electron pairs available for dative covalent bonding
monodente
donates 1 electron pair to a metal ion
bidente
donates 2 pairs of electrons to a metal ion
quadridente
donates 4 pairs of electrons to a metal ion
hexadente
donates 6 pairs of electrons to a metal ion
what can ligands be
- negative ions (OH-)
- molecules with non-bonding electrons (NH3)
coordination number
the total number of bonds from the ligands to the metal ion
the total number of bonds from the ligands to the metal ion
coordination number
coordination number 2 shape
linear
coordination number 4 shape
square planar
or
tetrahedral