Why do first ionisation energies decrease down a group?
This is an example of remembering the basic trends of ionisation energies of different elements across the periodic table and applying this knowledge in detailWe take the Bohr model of the atom where the energy levels of an atom are quantized and the electrons occupy a specific space in time.As we go down a group there are more shells, so more shielding ,so overall the attraction of outer electrons to the nucleus decreases.
BD
Related Chemistry A Level answers
All answers ▸For the equilibrium reaction PCl5(g) (equilibrium arrow)-> PCl3(g) + Cl2(g) explain the effect of increasing the concentration of Chlorine gas using the equilibrium constant.
Periodicity shows a fairly smooth increasing trend across a period for ionisation energy. However, between groups 2 & 3 and groups 5 & 6, the trend doesn't appear to be followed. Using your knowledge of chemistry, explain why the trend isn't followed here
Which compound has a higher boiling point and why: water (H2O) or methane (CH4)?
Why is 2-trichloroethanoic acid such a strong acid?