Transition metals Flashcards
What is a d block transition metals
A metal which for at least one of its ions has an incomplete d sub shell.
Difference in orbital filling rules for transition metals
For copper and chromium (number 4 and 9) having a half filled or filled 3d sub shell is more stable than a 4s sub shell, so the last electron goes into the 3d sub shell.
Difference in ions formed in transition metals
In transition metals the 4s electrons are lost before the 3d electrons .
Oxidation number rules
Uncombined elements have ON =0
Ions of single atoms have ON equal to charge
Oxygen has ON = -2 in compounds
In its compounds hydrogen has ON=+1
Compounds ON =0
Polyatomic ions ON= charge
Oxidation state
The oxidation number in Roman numerals
Oxidation number or state of individual ion in compound
Calculate oxidation number of other ion,
make it equal to the individual ion
Take away or add charge.
Oxidation effect on oxidation number
Increase
Reduction effect on oxidation number
Decrease
Transition metals oxidation states
Have variable oxidation states with different stability
High oxidation states
Oxidising agents
Low oxidation states
Reducing agents.
Transition metal complex definition
A central metal atom or ion surrounded by ligands which have formed dative covalent bonds with the metal.
Ligand’s definition
Molecules or negative ions with non bonding electrons which they donate to the unfilled d sub shell
Common ligands ( negative ions)
Cl-
CN-
OH-
Common ligands (molecules)
H2O, NH3
Process of ligand forming covalent bond
The ligands non bonded electron pair will donate both electrons to the metal ions orbital and form a dative covalent bond.
Dative covalent bond
A covalent bond formed by a ligand donating a non bonded electron pair.
Dative bond properties
Identical to other covalent bonds after formed.