[croatianboii]

I have a chemistry assignment and need help with a few questions.

1. Why does Ne have a larger IE then Li.
2. Why does Na have a larger IE then K.

[macman104]

Show some effort first.

[croatianboii]

Show some effort first.

Yea, well im sorry i missed the note on this cause i was sick today, and every one in my class finished it during class, so no one brought it home. There were 12 questions and these were the two i had trouble with. I attempted to research it a bit but i have a feeling my answer is off.

Thanks though, im sorry chemistry isn't my strongest subject and my parents pretty much forced me into it, and im trying my best but still doing awful. You're an awesome person.

[macman104]

It's ok, we can work through it.

What does Ionization Energy describe?  What does it measure?

[croatianboii]

It's ok, we can work through it.

What does Ionization Energy describe?  What does it measure?

Its alright, i waited a little bit for a reply but decided to go to bed before you replied (it was past 11 and i was tired). I think i did the questions right, but the wording of them is awkward and my explanation is kind of basic.

[Astrokel]

do you mind posting your explanations?

as long as you mention about nuclear attraction and shielding effect and conclude with effective nuclear charge correctly, i think it should be fine!

[croatianboii]

do you mind posting your explanations?

as long as you mention about nuclear attraction and shielding effect and conclude with effective nuclear charge correctly, i think it should be fine!

1.    Ne has a larger IE then Li because Li has 1 electron in its valence shell, while Ne has many more. Li only requires 1 electron to be lost to become stable, so its IE is low since it is easy for it to become stable by loosing electrons, while Ne wants electrons so it can become stable.  Many electrons would have to be lost for Ne to become stable, so therefore it has a larger IE the Li.

2.   Na has a larger IE then K because K’s outermost valence electrons are farther from the nucleus than Na’s.  K has more energy levels then Na, so the electrons are weakly held for K and  easily removable. Therefore Na has a larger IE then K.

[Astrokel]

Hi, just to improve your answer bit...

1. Li: 1s2 2s1   Ne: 1s2 2s2 2p6

Since both Ne and Li are in the same period, their screening effect is approximate the same. As Ne has more protons than Li, the nuclear charge of Ne is more than Li. Hence electrons are more strongly attracted by the positive nucleus in Ne and therefore more energy is required to remove an electron in Ne than in Li.

2. Na: 1s2 2s2 2p6 3s1  K: 1s2 2s2 2p6 3s2 3p6 4s1

K has more protons than Na resulting in K has higher nuclear charge. However, K has more inner electron shells than Na resulting in its shielding effect is higher, therefore it outweighs the effective nuclear charge, resulting in Na higher IE than K.

hope it helps some..

[macman104]

I would base my explanations on the fact that Ne has a valence of eight and satisfies the octet rule, so it is reluctant to lose/gain electrons because it sacrifices stability.  For Li, it has one electron to have an "octet", so it is eager to lose one electron.

For the Na or K, then you do need to use other rationale for explaining this.

[Borek]

Many electrons would have to be lost for Ne to become stable

It already is stable. It can't get more stability neither by loosing nor getting electrons.