Transition metal general properties Flashcards
(30 cards)
where are they found
between group 2 and 3 in the d block
where are the outer electrons
in the d orbital
why do we fill the 4s orbital before the 3d
the 4s orbital is closer to the nucleas so it fills before the 3d orbital
what are the exception
chromium and copper
what I the structure like in chromium
3d and 4s both contain one elctron each whihcmake the complex more stable
what is the structure of copper like
the 3d orbital is and the 4d orbital contains one electron
how do we form ion
the 4d orbital are emptied first
what are the positions of the 3d and 4s like
they are very close together
what happens when energy is supplied
the energy supplied causes the energy level to shift around to expected order as a result of the bombardment of electrons
why is scandium/ zinc transition metal
when we remove an electron it has a completely empty d orbital
when we remove an electron it has a completely full d orbital
therefore a transition metal has
an incomplete d orbital and they cannot form ions with incomplete d orbitals
what are the main characteristics of transition metals
they form colored ions, they can act as catalyst they have variable oxidation states and form complexed
what is the most common oxidation state and why
oxidation STATE OF PLUS TWO AS USUALLY THE 4S ORBITAL EMPTIES FIRST WHICH has two electrons in oouter shell
why do they form variable oxidation state
as the orbitals are very close together in energy levels so electron can be removed easily
what is a complex ion
a central metal ion surrounded by coordinately bonded ligands
what is a ligand
a molecule or an ion with a lone pair of electrons which donates to form a coordinate bond
what is a monodentate ligand and example
have one atom that can donate a lone pair of electron to form one coordinate bond h20 cl
what is bidentate ligand
two atoms each donating a lone pair of electrons to form two coordinate bonds ehandioate ions
what are multidentate ligands
several atoms donating a lone pair of electrons to form many coordinate bonds EDTA
how to calculate the oxidation state of the metal ions
THE charge of the complex- the charge of the ligands
how NOT ict the shape of a complex ions
the electron repulsion cannot be used as there is too many electron in the d orbital to estimate angles
so what does the shape depend on
the size of the ligand attached and the number of coordinate bonds
what metal ions can form octahedral complexes
cu/fe/co
what are the structure of octahedral complexes
form 6 coordinate bonds with water/ammonia as they are small enough to surround central metal atom
