Ionization Energy

[Erik Buetow 1F]

Why is it that in general elements with low ionization energy tend to form actions and conduct electricity in their solid state? Does it have to do with placement in the periodic table?

[TheresaDsilva4A]

Elements with low ionization energy tend to form cations because it is easier (requires less energy) to remove electrons from their orbitals. Thus, the formation of a positively charged ion (cation) is favored. The characteristic of having low ionization energy also enables these elements (metals) to be good conductors of electricity. This is because their electrons are delocalized/able to flow more freely.

To answer your second question, yes, it does have to do with placement in the periodic table. These elements are typically s/d block elements with a lower effective nuclear charge than p block elements, thereby requiring less energy to remove electrons. I hope this helps!

[Megan Jung 3A]

Elements with low ionization energy means that they require very little energy to remove an electron from their outermost valence shell. Thus, they tend to form cations and loose electrons because this would bring them to a stable octet or outer shell which is favored. Most of these elements are metals and a property of metal is the ability to conduct electricity.

The periodic table also places elements in a way so that going down a group, ionization energy decreases and across a period (left to right) ionization energy increases.

[005384106]

Why is there more energy the farther an atom is from a nucleus?

[lilymayek_1E]

Why is there more energy the farther an atom is from a nucleus?

I'm going to assume you mean electron, but as an electron is further away from the nucleus, it's n value (representing energy and size of the shell) increases. additionally, an electron farther away from the nucleus is said to have higher energy because there is a lower value of energy required to take that electron away (less ionization energy). this comes with the assumption that there's a certain threshold of energy that an electron must exceed to be taken away from an atom, and having lower ionization energy required means that the electron has greater energy initially.