Question

1.define ionization energy(IE)?explain the factors effect on ionization energy
2.explain why ionization energy 2(IE2) is greater than ionization energy 1 (IE1).
3.arrange the following elements in ascending order of ionization energy
N,P, O,Ne.
4.explain how metallic and non metallic properties change in groups and periods.

Plz ans total or any Qs
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Answer 1

heya !!

here are your answers:-

1.) IONISATION POTENTIAL:- the amount of energy required to remove a loosely bound electron from the outermost shell of an isolated(seperated) gaseous atom.

FACTORS WHICH AFFECT I.P.:-

◆atomic size- as atomic size increase, i.p. decrease.
reason:- when atomic size increases the nuclear attraction on the outer electrons decreases.
hence, the outer electron's are loosely held. so, I.P. increases.

◆nuclear charge:-as nuclear charge increases, i.p. increases.
reason:- when the nuclear charge increases, the nuclear attraction on the outer electrons increases.
hence, the outer electrons are more firmly held.so, I.P. increases.


2.) WHY 2ND IONISATION POTENTIAL IS GREATER THAN FIRST IONISATION POTENTIAL :-

first of all , what is 1st I.P. and 2nd I.P .? the first i.p. will be the energy required to remove the 1st electron and 2nd i.p. will be the energy required to remove the 2nd electron of an isolated gaseous atom.

so, once you will remove the first electron, the attraction force in the atom will increase due to decrease in size ... so when this force of attraction increases , obviously it will take more energy to remove the second atom from the valence shell of that atom.hence, second i.p. is more than 1st i.p.


3.)since ionisation potential increases across a period from left to right, the elements will be arranged in the way they appear in periodic table :-
N<O<Ne<P.


4.)the fourth answer I've given in the attached pic above. please see from there.


◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆


i hope it helps u !!!☺

Answer 2

1.) IONISATION POTENTIAL:- the amount of energy required to remove a loosely bound electron from the outermost shell of an isolated(seperated) gaseous atom.

FACTORS WHICH AFFECT I.P.:-

◆atomic size- as atomic size increase, i.p. decrease.

reason:- when atomic size increases the nuclear attraction on the outer electrons decreases.

hence, the outer electron's are loosely held. so, I.P. increases.

◆nuclear charge:-as nuclear charge increases, i.p. increases.

reason:- when the nuclear charge increases, the nuclear attraction on the outer electrons increases.

hence, the outer electrons are more firmly held.so, I.P. increases.

2.) first of all , what is 1st I.P. and 2nd I.P .? the first i.p. will be the energy required to remove the 1st electron and 2nd i.p. will be the energy required to remove the 2nd electron of an isolated gaseous atom.

so, once you will remove the first electron, the attraction force in the atom will increase due to decrease in size ... so when this force of attraction increases , obviously it will take more energy to remove the second atom from the valence shell of that atom.hence, second i.p. is more than 1st i.p.

3.)since ionisation potential increases across a period from left to right, the elements will be arranged in the way they appear in periodic table :-

N<O<Ne<P.

4.)the fourth answer I've given in the attached pic above. please see from there.