Ionization Energy - Basic Introduction

Lower ones, like the 2s level versus the 3s level, those electrons tend to be closer to the nucleus. Electrons that exist at higher

energy

levels tend to be further from the nucleus, so the fact that it is less stable means it has more

energy

and on average means it will be further from the nucleus, which means that it is easier to remove. Paired electrons are easier to remove than unpaired electrons since everything else is equal, which is why this value is lower because you are moving a paired electron instead of an unpaired electron, so I think that is enough to lectures, let's work on some examples. which atom or ion has the highest

ionization

energy so let's compare magnesium and calcium which one will win now if we place these elements in a respective position in the periodic table magnesium is above calcium these are alkaline earth metals and we know that the energy Ionization increases as you go up, so magnesium should have a higher

ionization

energy than calcium and if you want to find the values ​​of the ionization energies of the elements, just go to Google Images and type in the periodic table of ionization energy and You should find a few things there: magnesium has an ionization energy according to my textbook of 735 and calcium is 590.

So clearly magnesium wins, it has a higher ionization energy, it is much harder to remove one electron from magnesium than from calcium in the gaseous state, so now let's move on to part b then which one has the greater ionization energy silicon or phosphorus now in the periodic table phosphorus is to the right of silicon so which one is going to win well we know that As you travel to the right the ionization energy increases, therefore we should expect phosphorus to have a higher ionization energy than silicon, in fact the ionization energy of silicon, the former, is 780 and the first ionization energy of phosphorus is 1060.

So, when going from 3p2 to 3p3, the ionization energy increases towards the now let's move on to part c, which has a higher ionization energy: beryllium or boron. Now beryllium and boron are in the second row of the periodic table and borons are to the right of beryllium, so naturally we should expect the ionization energy to increase. However, as we go to the right, this is one of those exceptions because beryllium is in the 2s sublevel and boron is in a two piece level and every time you go from s to p as you cross to the right, it doesn't always , but for the most part, for most elements, the ionization energy will decrease;

Typically, the elements at the top of the periodic table tend to show this, but the heavy elements at the bottom may not show the trend for Beryllium has a first ionization energy of 899. and for Boron is 800. So 2p has much more energy than 2s, since the difference is significant, so it is easier to remove an electron from the 2p sublevel than from the 2s sublevel, so the answer is beryllium, it has a first energy of higher ionization. And now what happens? phosphorus and selenium actually I mean I jumped ahead let's go to the part d nitrogen or oxygen oxygen is to the right of nitrogen now nitrogen ends in 2p3 oxygen ends in 2p4 now although we are going to the right side oxygen it is not going to have the highest ionization energy it is one of those exceptions every time you go from p3 to p4 you are comparing an unpaired electron with a paired electron nitrogen has that unpaired electron this is the 2p electron an oxygen has a pit electron the 2p4 and so it will be.

It is easier to eliminate the 2p4 electron than the 2p3 electron due to the repulsions of the electrons, so in the case of nitrogen it takes 1402 kilojoules per mole of energy to eliminate that electron, for oxygen it is less than 1314 , so nitrogen has the highest ionization energy. Now let's move on to part e, let's compare arsenic and sulfur, now these two elements are not in the same row, so arsenic is in the fourth row and selenium, I mean sulfur is in the third row, so what the sulfur is one row above the arsenic and is to the right, so which one is going to gain arsenic or sulfur above the arsenic, it has phosphorus below the sulfur, it has selenium.

Now keep in mind that the ionization energy increases as you go up and to the right, so the ionization energy increases this way towards helium, so based on that trend, it should be clear to us that sulfur should have the highest ionization energy. The ionization energy of arsenic is 947 and for sulfur it is one thousand five, so sulfur has the highest ionization energy. Follow this trend. Now what about part f? What if we compare phosphorus and? selenium which has the highest first ionization energy now which has more priority is going up or going to the left or rather I meant going to the right because selenium is to the right of phosphorus it turns out that sometimes it varies going Up has more priority It has to go clockwise and sometimes it's the other way around, so whenever you have two elements in this position, the best way to find the answer is to look up the values.

Phosphorus has an ionization value of 1060 and selenium is 941, so in this case phosphorus wins against selenium in other examples it will not be like that, for example if you compare sulfur and bromine, bromine should be right here on the periodic table. Sulfur is 1005, but the first ionization energy of bromine is 1143, so this time. the element in this position wins and that's why it varies every time you have two elements arranged this way, you just have to compare the numbers. Now let's move on to part g. Which has a higher first ionization energy? Is it aluminum plus two ions or the?

Aluminum plus three ions In the previous part of this video, when we went over the different ionization energies of silicon, we saw that as the charge on the silicon ion increased, the ionization energy increased, so aluminum has the positive charge higher, so we should expect that to be we're going to have the highest ionization energy now, what if we're dealing with negatively charged ions which one is going to win for these two ions? This trend still holds, so which ion has the highest charge or the highest positive charge negative 2 is more positive than negative three minus two is less negative than negative three so this one is going to win on a number line minus two is greater than negative three so let's make a number line here is the charge of aluminum plus three this is the aluminum plus two charge this is zero this is the negative charge two of the first phosphorus ion and here is the negative charge three of the second, for which as you travel this way in terms of charge, the ionization energy will increase, so the aluminum plus three ion has a higher charge than the aluminum plus two ions and p minus two will be greater than p minus three, so which you can look at it that way if it helps, but the one with the most positive charge or the least negative charge will be the one with the highest ionization energy, so positively charged ions have a higher ionization energy than ions with negative charge.

Now let's move on to this one. Rank the following elements in order of increasing first ionization energy. Now the best thing you can do is to place these elements in their respective positions according to the periodicity. table, so barium is somewhere down here, it's a transition metal that's around this area and then silicon is somewhere around here and then here's oxygen and then here's helium, the ionization energy increases as you go up and to the right so

basic

ally it increases as you travel towards helium so we should expect helium to have the highest ionization energy and barium to have the lowest so to write it in Increasing order, we will first start with the lowest ionization energy and then to the right with the highest one, so that the iron metal has a higher ionization energy. the ionization energy that the carrier metal and then the silicon is even greater than the iron and then we have oxygen and then helium now if you want the values ​​here they are so for b a is 503 for iron metal is uh for silicon is 780 for oxygen is 1314 and helium is 2377.

So as you can see, generally speaking, the ionization energy increases as you travel towards helium number three. The ionization energies of an unknown element are listed below based on its data. Which of the following elements could be the unknown element? Is it potassium, aluminum, sulfur? krypton or silicon now what you need to focus on is the jump that happens from the third to the fourth ionization energy, it jumps almost by 9000 so the jump is huge which means that since the jump happens in the fourth ionization energy, the first three are valence electrons the fourth ionization energy represents the removal of an electron from the nucleus, so if the jump occurs at the fourth ionization energy that means this element has three valence electrons, then Your task is to identify which element has three valence electrons.

Silicon is in group four. it has four valence electrons krypton is a noble gas it has eight valence electrons sulfur has six aluminum has three potassium has one so this element would correspond to aluminum which is the unknown element aluminum has three valence electrons and that is why it is You might see a question like this on the test, let's say if the jump happens from the sixth to the seventh ionization energy, then the seventh ionization energy is very, very large, that means the element would have six valence electrons and that element will be sulfur and this is how you can answer the questions. which looks like this if you see it in the test, but for this particular problem the answer is b due to the fact that we have three valence electrons.