Eli5: Why are Group 1 Metals the most Reactive
In: Chemistry
They aren’t most reactive because they’re in Group 1, they’re in Group 1 because they have one free electron in their outer atomic shell, and that electron “wants” more than anything to be in a complete outer shell, and it gloms onto any “hole” in an outer shell that belongs to some other kind of atom. A reaction is essentially what happens when atoms with incomplete outer shells share elctrons.
The most reactive atoms have just one outer shell electron, and the least reactive atoms have just one “space” left over for an additional electron, and NON-reactive atoms like helium, argon, etc. have completely full outer shells. Group 1 metals (and hydrogen is also in group 1) are reactive because they readily lose this outer electron.
EDIT: I have been rightly corrected. Elements with one “space” left over are also highly reactive for a similar reason. Those with a partly-full outer shell are not as reactive.
Group one metals are used in many biological processes! They help control an electrical gradient and carry on many processes in cells. Many life forms naturally adapt to utilize these metal regularly in the body, so they are reactive because everything is reactive in the right environment.
Why, because they carry a plus one or two charge usually and it allows the body to closely regulate the electrical gradient in systems.
They are super awesome metals.
Now check how they bond with =dem noble gasses, the group 1 that is.
The Group 1 metals have an outermost electron shell that has only a single electron in it, and they *REALLY* do not like that. They want to dump that electron anywhere they can so that the next shell in, which is full on Group 1, becomes the outermost shell. Full electron shells are like shields, and are VERY difficult to interactand react with.
Its like covering a Jawbreaker in a layer of powdered candy. That outer layer with its single electron will come off quite easily (and make a mess in doing so) but the jawbreaker (and its complete next shell) is much much harder to get into.
Conversely, the Group 17 elements (Fluorine, Chlorine, etc) have all space except for 1 electron in their outer shell filled, and they ***really REALLY*** want that outer shell filled. They do not care where they get it, they just want it. Its why Fluorine is so reactive; under the right conditions it can set just about anything on fire.
It is because they have a single electron in their outermost shell. This makes them eager to lose it and achieve stability, reacting vigorously with water and air.
So every atom has electrons that encompass the nucleus like a shell. And this shell has layers, like an onion. The first layer holds two electrons, the next two layers hold eight, and every layer after that holds eighteen each.
Atoms want to have a clean outermost layer to be complete, either by gaining some electrons, or losing some electrons, or sharing them. The closer they are on either side to gaining that complete layer, the more reactive they tend to be. That’s why Group 1 metals and Hydrogen are so highly reactive, they have only one electron floating around in their outermost layer and REALLY want to ditch that electron. Meanwhile Group 17 elements like Chlorine or Fluorine are also highly reactive, because they only need to gain one more electron for a complete layer. And Group 18, the noble gases, have a complete outer layer so they almost never react with any other element under normal circumstances.
Latest Answers