d-orbitals And TM Trends Flashcards
What’s the shape of the dxy orbital?
What’s the shape of the dxz orbital?
What’s the shape of the dyz orbital?
What’s the shape of the dz^2 orbital?
What’s the shape of the dx^2-y^2
Does the 4s orbital penetrate the nucleus effectively?
Yes, very effectively
Why do the s orbitals effectively penetrate the [Ar] core?
Due to the s orbitals having a peak of radial distribution of electrons at small r.
4s does not shield 3d from the nucleus
What must a transition metal have?
A TM must have a partially filled d-shell
When is 4s lower in energy than 3d?
4s is lower in energy than 3d for K and Ca, hence 4s fills first
What’s the significance of Cr and Cu?
Both lose an electron from the 4s shell to the 3d shell giving [Ar] 4s1 3d5 and [Ar] 4s1 3d10 respectively.
This is due to additional stability of the half and fully filled 3d shell
What electrons are lost first, 4s or 3d for transition metals?
4s as they are of higher energy
Why is Zinc not a TM?
Because it has a full d shell at ground state and when ionised
It is included in discussion however as it shows similarities to transition metals
What is the effective nuclear charge?
It is the amount of the nuclear charge seen by an electron in that orbital
What does effective nuclear charge depend on?
How good electrons in inner shells are at shielding outer electrons from nuclear charge
How good outer electrons are at penetrating underlying shells
What are the properties of smaller ions?
They have higher charge densities and so are expected to favour harder ligands
