Hallo
I have a few questions to ask regarding ionization energies of
elements.
-In period 2 and 3, the ionization energy increases with
increasing atomic number. May I know why this is so?
I can't offer a detailed explanation but I will try my hand at
doing so and please correct where necessary.
Explanation: As we move along period 2 and 3, the properties of
the elements become more metallic. Thus the tendency to gain
electrons rather than to lose electrons increases. This as a result
contributes to the rise in ionization energies.
2. Compare the ionization energies of the Group 2 elements with
that of the noble gases. Give a possible reason for your
deduction.
Firstly, in both group 2 and 8, ionization energies of elements
decrease down the group. However i can't explain why.
3. Give a reason why the ionization energy for neon is higher
than that for Argon.
What I want to know is, is neon in anyway less reactive than
argon? I think yes... but then again, is there a scenario where
noble gases can be more reactive or less reactive than the
other?
Lots of thanks
Ionization energy decreases down a group as the atom gets larger
and the larger it is, the further the outermost electrons are from
the nucleus. This makes the 'attraction' force of the nucleus
weaker so that less energy is required to remove an electron.