Скачать или смотреть Periodic Trends (Part 3 of 7) - Ionization Energy (IE)

In this video, I define Ionization Energy, discuss the trend up, down, and across the periodic table, and discuss particularly important aspects of Ionization Energy.

Ionization Energy is defined as the amount of energy (often in kJ) required to completely remove one mole of electrons from one mole of gaseous atoms (or ions). The definition in a sort of reaction form is provided in the video. Ionization Energy is always a positive value, indicating that energy is required to remove an electron from an atom. Why is this? It’s because electron’s, with their negative charges, are attracted to positively-charged atomic nuclei by an electrostatic force that must be overcome by the input of energy.

Ionization Energy increases up and to the right on the periodic table. It’s worth noting that this trend is opposite that of Atomic Size / Atomic Radius. This makes sense, as it basically implies that the smaller an atom is, the harder it is to pull an electron away from it. When electrons are closer to the nucleus, the electrostatic force between them is stronger, and it requires more energy to pull an electron away from the positively-charged nucleus.

It must be kept in mind that the trend is just that – a trend, and that it’s not sure-fire. I discuss a trend break in the periodic table between nitrogen (N) and oxygen (O). The trend says that oxygen’s ionization energy should be higher than nitrogen’s, but the opposite is true. The reason for this involves the fact that a nitrogen atom has a very stable half-filled electron orbital configuration that requires a particularly large amount of energy to disrupt. Oxygen, on the other hand, can lose an electron to yield a very stable half-filled electron orbital configuration.

I finish by discussing the idea that successive ionization energies are always higher than their preceding ionization energies. I provide an example problem discussing “jumps” in successive ionization energies and how to solve and explain them.

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