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
>>> the properties of the elements become more metallic. <<<
You should focus on increasing nuclear charge (due to increasing proton number) across a period.
>>> What I want to know is, is neon in anyway less reactive than argon? <<<
That's true, but you're required to focus on the concept of greater shielding/screening effect (experienced by the ionizing electron of Ar compared to Ne, due to an additional electron shell between the positively charged nucleus and ionizing electron in the valence shell).
Originally posted by Audi: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.