Periodic Trend: Ionization Energy (Simplified) - Video Tutorials & Practice Problems

Periodic Trend: Ionization Energy (Simplified) Concept 1

now, ionization energy, which is abbreviated as E represents the energy required to remove an electron from a gashes atom or ion based on position in units of killer jewels. Now, for example, let's take a look here. We have nitrogen in its gaseous state. So we're dealing with a gashes atom ionization energy will be a reactant because we have to input energy into the gas gas atom in order to extract an electron. So the energy I just put in in terms of ionization energy helps me to remove an electron removing an electron from nitrogen, nitrogen are negatively charged, losing one means not nitrogen will be plus one still in its gaseous state. And the electron that I just removed will be a product next to it. So they've been separated from one another. So again when it comes to ionization energy, it's important to realize that ionization energy will be written as it reacted because we're inputting energy and the electron we remove will be a product. Now, what else can we say? What we can say here that the basic periodic trend is ionization energy will increase as removing from left to right across a period and going up a group. And it's important to realize that what type of ionization energy means that the electron is easily lost. Well, ionization energy is the energy to remove the electron. So the energy required is very small. That means going to be pretty easy to remove that electron. So we're gonna stay here. That low ionization energies means the electron can be removed very easily on the flip side of that. If our ionization energy is very high, that means a lot of energy is required to remove an electron. That means that the electron will not be easily removed or easily lost. Now realize here that noble gases are perfect because they have the great electron arrangement or configuration um in their outer shells, so it would require a lot of energy to remove their electron. Because of this, noble gases will possess very high ionization energies. Right? So just remember these fundamental principles when it comes to the idea of ion on ionization energy.

Periodic Trend: Ionization Energy (Simplified) Concept 2

So remember the general trend is as we move from left to write of a period and as we go up a group, your organization energy will increase. This means that helium would possess the highest ionization energy at 2000, 372 killer jewels, whereas francie um which is on the exact opposite end, would have one of the lowest at 3 93 killer jewels. Remember, the higher ionization energy is, the harder it is to remove that electron. We can see that here and we're going to see here that the small organization energy is, the easier it is to remove an electron. So francine would be much easier to remove an electron than helium. Now, of course, there are exceptions. In terms of this trend. In terms of those exceptions, you don't have to delve too much into it. We won't talk about for the most part, those exceptions just realize that the general trend is as we're heading towards the top right corner of the periodic table, we expect our ionization energy to increase. Now, you'll also see that some of these boxes are great out. That's because those are our heavy elements. Their atomic masses are so large, their atomic numbers are so large that they're pretty unstable. A vast majority of them have been synthesized within laps and the only last mere moments in terms of existing. And because of that, we really don't talk about their ionization energies. So again, just remember, the general trend is as we head towards the top right corner, are ionization energy should be increasing.

Periodic Trend: Ionization Energy (Simplified) Example 1

here, it says. Which of the following Adams has the smallest ionization energy. Remember, the general trend is as we're heading towards the top right corner, your ionization energy should be increasing. So if we take a look, we have phosphorus. We have flooring, potassium, chromium and bro me. We want the smallest ionization energy, so we're looking for something that's closer to the left side and lower down for the periodic table. Out of the choices presented, the one that fits that definition the best is potassium. It's the one most to the left and lowest down in terms of the periodic table and therefore to have the smallest ionization energy.

Rank the following elements in order of increasing ionization energy:Br, F, Ga, K and Se.

• A. Ga < K < Br < Se < F
• B. Ga < Br < K < Se < F
• C. K < Se < Ga < Br < F
• D. K < Ga < Se < Br < F
• E. K < Ga < Se < F <  Br

Which of the following elements would lose an electron the easiest?

• A. Ar
• B. Li
• C. Zn
• D. Br
• E. B

Which element from Group 7A has lowest ionization energy.

• A. I
• B. Br
• C. Cl
• D. F
• E. Ne

Which of the following has the highest ionization energy? 

• A. Ar
• B. Na⁺
• C. Na
• D. Mg
• E. Kr