Atomic and Nuclear Physics Answers

to find the ionisation energy of atoms in a period,if we move from left to right to the periodic table,the ionisation energy generally increases.because with the increase of atomic number,there is an increase of nuclear charge and so the nucleus of an atom has more attaraction to the electron and thus the ionisation energy increases.i know ionisation energy of Be is greater than B.i know the reason too.for this case Be has stable 2s2 thats why.i found another reason.the last electron of Be is removed from s orbital and the last electron of B from p orbital.and s is closer to the nucleus than p orbital.so to remove electron from s orbital is harder than to remove from p orbital as the attraction of the nucleus and s orbital is more than p.now my question is why in a period to find ionisation energy we dont say that with the increase of atomic number the last electron is in s,p,d.and s is too close to nucleus and the others are not closer like s orbital.why not the left sided atoms have more ionisation energy

The wavelength of radiation emmitted,when in He+ electron falls from infinity to stationary state would be
(1)2.2*10^-8m
(2)22*10^-9m
(3)120m
(4)22*10^7m

In which of the following ions do you expect angular momentum quenching and why:
Ti3+, Gd3+, Ni2+

Is the following statement true for vibrations of a chain of two different types of atoms:
“At the centre of the Brillouin zone, the frequency of the optical branch is less than the
frequency of the acoustic branch”? Explain.

The electronic and lattice heat capacities for copper at 0.01 K are 5.04 x 10^-6 J /(kmole K) and
4.60 x 10^-11 J /(kmole K) respectively. What do you
conclude from these magnitudes?