About Metallic bonding...........

[albertlee]

Siple as the title......... WHY ONLY PURE METALS USE THIS KIND OF BONDING?

 

What is so special about the characteristics of pure Metals due to this kind of bonding? since why the non-Metals cannot use this type of bonding.....?

 

thx for the responds

[Sayonara]

Aren't they pure metals because they use that bonding?

[albertlee]

So........ What is so special about metallic bonding? since why only pure metals apply to use that bonding?

 

Any help?

[Skye]

It's basically because metal atoms pack in close together in solids, so close they are contact with maybe a dozen other metal atoms. They don't have enough valence electrons to form bonds with all these other atoms, so their electrons flit between the surrounding atoms, and you get your cliched 'sea of electrons'.

[aommaster]

It's basically because metal atoms pack in close together in solids, so close they are contact with maybe a dozen other metal atoms. They don't have enough valence electrons to form bonds with all these other atoms, so their electrons flit between the surrounding atoms, and you get your cliched 'sea of electrons'.

 

and so, they conduct electricity and heat very well

[wolfson]

correct aommaster, and the metalic bonding in transition elements is due to involving the 3d electrons in the delocalisation as well as the 4s. The more electrons you can involve, the stronger the attractions tend to be.

[aommaster]

thank you! I didn;t know about that transition metals bit!

[wolfson]

yw MD

[albertlee]

So...... why does pure metal almost always stay in solid? if other non-metals also stays in solid, and dont have valence electrons, either..Wont the non-metals also apply to metallic bonding?

 

Any help?

 

Cheers

[Crash]

ah......semi-metals.

This i guessing is like ceramics,graphite?(with metallic bonding) thats how they are making room temp superconductors

 

The 3d orbital is also responsible for their lustre

[albertlee]

Thx to Crash........but....... Any more complete answers to my previous message?

[albertlee]

Can any body pease help to my last question?

[albertlee]

Any body?

[aommaster]

Well, some non metlas have different types of bonding. The metallic bonding is ESPECALLY for metals. Other non metals may have bonding like molecular etc.

Hope that helps

[albertlee]

aommaster, I know, the metallic bonding is only for metals, but i am just asking why pure metals can stay in solid, which means have such high melting anf boiling point? I think it is not the matter of bonding anymore, metals just have high melting and boiling points themselves......... I think that is also another best way to identify metals, having high melting point,using not covalent bonding................

 

Any help?

[aommaster]

well, that is to do with the strength of the bonds. Molecular covalent bonds are weak, that is why the substances that have them have low melting and boiling points. The metallic bonds are strong bonds, causing high melting and boiling points

[albertlee]

Ok, AOM, As i have said, it is not a matter of bonding anymore here about metal, but is about the elements themselves, which means if, the metals "apply" to covalent bonding, then therefore, they get low melting point..............

 

Say it more clearly, what cause the metals "apply" to metallic bonding, but not covalent bonding?

 

Any help?

[aommaster]

covalent bonding requries electrons to be 'shared' between atoms. In this case, they cannot share electrons between atoms because the numbers just do not match to make a full outer shell. They could in one way, but, it would take too much energy, and the atoms are too 'lazy' to do so.

 

Ionic bonding has the same story, they have to give too many electrons or take too many electrons. It just doessn't work

 

That is where the metallic bonding kicks in

 

Does that help?

[albertlee]

Thanks, AOM, but that only answers 50% of my question!

The other 50% is why dont metals just become single atoms, but bond it together using so-called metallic bond?

 

Any help?

[Crash]

Ask one damn question properly, Metals dont become just single atoms due to a partially filled octet and need bonding(metallic) to complete a full shell.

 

As for the original question; this is due to the metal atoms not having enough electrons so they are delocalized. the "d" orbital is semi responsible for these properties due to the weird things the "d" orbital can do....

Awnser your question now?

[aommaster]

the simple answer is that ALL atoms are looking for FULL outer shells (the interior ones are laready filled up). And THAT is why they form metallic bonds.

[Crash]

not nessecarily full, like Cu 4s2,3d9 -> Cu 3d10 4s1 the main stable formations are full shells, Full orbitals or half filled e.g 3d5 or 3d10

[aommaster]

welll.... yeah!

That's the problem with metals like the transition metals...unpredictable!

[albertlee]

Ok............

So why dont the non-metals apply to "metallic bonding" if they can do so, since if it takes less energy?

 

Can any one answer to that?

 

Cheers

[aommaster]

well, since non-metals have more than 4 electrons in their outer shell, they do covalent bonding and share the electrons. Its easier for them to do that!