why-are-metals-that-are-more-active-also-considered-less-stable-2

Name: why are metals that are more active also considered less stable 2
Uploaded: 2020-10-28
Duration: 1 min 52 s
Channel: Numerade
Description: Why are metals that are more active also considered less stable?

Question

Why are metals that are more active also considered less stable?

Madi Sousa · Accepted Answer

in this problem, we have to understand and talk about the the reactivity of metals. And specifically we see that metals are reactive but not very stable. And this is extremely important to understand, because this is what a chemist really wants to know. How are elements or how are compounds going to react? So what we see is that metals react extremely easily and extremely compared to other elements on the periodic table, and they form metal oxides, which are impure metals. Now you should already know about oxidation and how that deals with the charge of the compound in the number of electrons. And that&#x27;s at the heart of this conversation around metal reactivity. And here are some of the reasons why we see metals can react easily but are not very stable. And one of them is that the react violently with chemicals. So an example of this would be the reaction of potassium and water. You could look up a video of this and you&#x27;ll see that it explodes basically because it produces hydrogen gas and makes the reaction very violent. Another thing is that metals, remember we&#x27;re talking about oxidation is that they easily give up electrons because of their oxidation state. They can give up electrons to whatever they&#x27;re reacting with and react quite easily. The other thing is that they can corrode easily. So think about the rust on pipes, things like that. That is an oxidation reduction reaction and that also deals with the reactivity of medals. So I hope that this helped you understand or maybe even introduced you to, um the reactivity of metals and understanding how it impacts things like stability and oxidation.

Zachary Papazian · Answer

But an element belongs to tell you a lot about how the specially due to the amount of valence electrons. So in group One you have the, um, alkali metals, which have one valence electrons. So it makes sense for them to want to sort of get rid of that elect wrong in a reaction to they can be more stable, uh, so that that is what they tend to do. Now if you move over one group to the right to group to here at the alkaline Earth Metals, which to violent electron, no, they&#x27;d have to get rid of those two to get to that, um, point of stability, which is possible. And they do do that. However, it&#x27;s obvious that it&#x27;s harder to use two electrons, and it is one. That&#x27;s why they&#x27;re a little bit less reactive than the alkali metal

Catherine Lemar · Answer

alkali metals like sodium, are very reactive because they have one valence electron in their outer energy level, so that one electron wants to form a bond with another Adam to become more stable. And so because of this, the element will give that electron away, and it does so very easily, making it very unstable.

Cameron Oden · Answer

as we&#x27;re talking about. Transition metals were talking about D electrons mostly. And so because of that, when we look at the nucleus as we go out will encounter s electrons, p electrons. And lastly, the D electrons are gonna be further out from the nucleus. Then the SRP electrons. So for alkaline earth metals, for instance, you get calcium two plus, and that&#x27;s the only oxidation state you&#x27;re going to see. But for iron, you might see neutral iron two plus iron in three plus iron and all of these air stable. So why is that? Well, because thes d electrons air further from the nucleus, the for instance, with iron. The second ionization energy is pretty similar about equal to the third ionization energy been for a lot of these metals, depending on what their ground state is. The&#x27;s ionization energies may not be very different in magnitude. So the difference between removing 123 or four electrons, or even mawr sometimes may not be that different. So you can find several oxidation states that are all state

Keenan Mintz · Answer

and let&#x27;s talk about problem six from Chapter 22. This problem were asked about transition metals and why they have several oxidation states, while other elements typically only have one or maybe two that are stable. And so the reason for this is due to, um, the energy of their valence electrons. So these valence electrons and the D and the three D and four s orbital&#x27;s air or any comparable DNS orbital&#x27;s are going to have the, uh, pretty similar energies similar ionization energies. So depending on the environment, different amounts could be removed. Could be in. The Adam can be stable after they are. If you look about if you think about ionization energies for sodium or calcium than if you remove one or two, respectively, the ionization energies jumps to a huge level. But for transition metals, there&#x27;s many D electrons to play with. And so, um, there&#x27;s multiple states which could be stable

Bryan Wang · Answer

alright. In this question, we&#x27;re talking about why models are often found as yours or compounds as opposed to in their pure form. So if we look at the pure out in table Group one, a group to say, These are your alkali and alkaline earth metals and then we have the transition metals over here now why dio if he&#x27;s not exist in the normal state? Well, look at the number of valence electrons and these metals, So lithium, for example, has just one billion electron. That means it&#x27;s looking to get rid of that electron, and it will be very reactive with other elements and compounds so that it could get rid of its electron. It becomes stable. Okay, our atmosphere is full of oxygen and nitrogen, but we&#x27;re going to use Oxford because it&#x27;s more reactive, so place and we have something like magnesium. Magnesium really wants to form a two plus ion because it would become stable if I got rid of its two electrons. Oxygen conveniently is looking to gain two electrons, so when magnesium in its native form, if it exists in that&#x27;s needed form, would have re out very strongly with oxygen and it would send its two electrons over, and all the metals are going to behave in a similar manner. Some medals will be much more reactive than others. But this is why something like Iron, for example, look, this is iron or because it&#x27;s not going to be in its native iron form when the moment at contacts with anything in our atmosphere it will react to form iron oxide, for example. Okay, that&#x27;s a

Problem

If zinc nitrate, $Z \mathrm{n}\left(\mathrm{NO}_{…

Problem 2 Easy Difficulty

Why are metals that are more active also considered less stable?

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