D And F Flashcards
Transition metals have high mp
This is due to the Involvement of greater number of electrons from an minus one day, in addition to the NS electrons in the interatomic bonding.
Transition metals have high enthalpy of atomization
This is because of large number of unpaid electrons in the atoms that has stronger in it, interatomic interaction, and hence stronger bonding between atoms
In the first transition series of the enthalpy of zinc is the lowest
Zinc has completely Finity orbitals in the formation of metallic bonds in a number of electrons from the 3D Orbitals are involved in the case of Zn
The metals of the second and third series have a greater and then piece of atomization than the corresponding elements of the first series.
This is because of more frequent metal metal banding in them.
Manganese in the first translation series technician in the second transition series and rhenium in the third transition series have low melting point than expected this is due to
The exactly half of the day orbitals. The electronic configuration is stable and electrons are tightly held by the nucleus so that the D localization isles. And the metallic bonding is much weaker than the present than that of preceeding elements.
The atomic and ionic size decrease with increasing atomic number
D orbital are being filled up
The effective nuclear charge increases
Why is there a slight increase in atomic radius towards the end?
This is due to electron electron repulsion between the added electrons in the same orbital
The second and third transition series had the almost same size
The second and third transition series had the almost same size due to lanthanoid contraction.
Why is there an increase in ionization enthalpy along the series from left to right?
Due to an increase in the nuclear charge of unaccompanied, the filling of inner d orbitals
Transition metals show variable oxidation states
- small difference in the energies of ns (n-1)d orbitals
They can use 1 to 5 electrons from (n-1)d orbitals in addition to ns electrons.
The highest oxidation state of a metal is exhibited in. It’s a oxide or fluoride only.
Due to the small size and a high electronegativity of oxygen and the flouride , they can oxidize metals to their higher oxidation state
Cu + compounds are unstable in aq solution and undergo disproportionation
The stability of Cu2+ aq rather than Cu+ in aq is due to the much more Negative hydration enthalpy of CU, 2+ aqueous than CU + which more than compensates the second ionization enthalpy, and the 2nd ionization of Copper
