1.3 - Transition metals Flashcards
what is common between all transition metals?
they all have an incomplete d-subshell in at least one of their ions
which transition metals do not follow the aufbau principle when filling d-orbitals?
chromium and copper
why do chromium and copper atoms not fill the 4s subshell before the 3d subshell?
there is a special stability associated with half or fully filled subshells
which electrons are lost first during ionisation? in the FIRST ROW of the transition metals
the electrons of the 4s subshell/orbital rather than those of the 3d subshell/orbitals
what can determine the colour of a compound containing a transition metal?
different oxidation states
what is oxidation in terms of oxidation number
an increase in oxidation number
compounds containing metals in a (too) high oxidation state are often …………….. agents
oxidising agents
what are the 2 types of possible ligands
negative ions, molecules with non-bonding pairs of electrons
what does a complex contain?
a central metal atom/ion and a ligand
what does a ligand donate to the central metal?
pairs of electrons
what does a monodentate ligand do?
donate one pair of electrons
what is the coordination number?
the total number of bonds from the ligands to the central transition metal
what complexes must you be able to name? those which contain…
copper (cuprate) iron (ferrate)
ligands: water, ammonia, halogens, cyanide, hydroxide, oxalate
what are no longer degenerate in a transition metal, in a complex
the d-orbitals
which d-orbitals are split to higher energies?
those with lobes along the axes (dx2 -y2 and dz2)
