[hsp]

 have two simple questions that I'm not too sure about.

The first is can carbon form the C4+ Ion?

I know that it can't occur naturally.. but radioactively and in things like single-walled carbon nanotube paper?

Secondly..

Is the reaction of magnesium metal with dilute hydrochloric acid a redox reaction?

I'm leaning towards no as I can't see any transfer of electrons and i see no transfer of oxygens etc?

Mg(s) + 2HCl(aq) => Mg^2+(aq) + 2Cl^-(aq) + H2(g)

Magnesium has a 2+ to begin with etc? Frustratingly simple I know but I'm only just starting out on redox reactions etc.

Any help asap would be great! Cheers.

[UG]

Is the reaction of magnesium metal with dilute hydrochloric acid a redox reaction?

I'm leaning towards no as I can't see any transfer of electrons and I see no transfer of oxygens etc?

Mg(s) + 2HCl(aq) => Mg²⁺(aq) + 2Cl^-(aq) + H₂(g)

Magnesium has a 2+ to begin with etc? Frustratingly simple I know but I'm only just starting out on redox reactions etc.

Any help asap would be great! Cheers.

Redox reactions can also involve the transfer of electrons (in this case) as well as hydrogen.
Magnesium metal has lost 2 electrons (it has been oxidised) and the 2 hydrogen ions (H⁺) have gained 1 electron each to form hydrogen gas (H₂), they've been reduced. So this is a redox equation. 

[hsp]

Is the reaction of magnesium metal with dilute hydrochloric acid a redox reaction?

I'm leaning towards no as I can't see any transfer of electrons and I see no transfer of oxygens etc?

Mg(s) + 2HCl(aq) => Mg²⁺(aq) + 2Cl^-(aq) + H₂(g)

Magnesium has a 2+ to begin with etc? Frustratingly simple I know but I'm only just starting out on redox reactions etc.

Any help asap would be great! Cheers.

Redox reactions can also involve the transfer of electrons (in this case) as well as hydrogen.
Magnesium metal has lost 2 electrons (it has been oxidised) and the 2 hydrogen ions (H⁺) have gained 1 electron each to form hydrogen gas (H₂), they've been reduced. So this is a redox equation. 

Thanks a million for the reply!

So I'm just trying to grasp the concept, if you don't have time to reply it's all good..
So is Mg to begin with 2+ or not? If not then I understand how it has been oxidised, i just thought Mg was 2+ to begin with but I suppose that's pretty stupid ha.

Cheers... and if anyone has help with the C4+ Ion i'd appreciate it a lot.
It seems pretty obvious, I just want to make sure I'm correct.

Thanks.

[UG]

So is Mg to begin with 2+ or not? If not then I understand how it has been oxidised

The oxidation number of magnesium to start off with is 0, the oxidation number of a monoatomic ion is the same as the charge on the ion so the O.N becomes +2. Are you familiar with oxidation numbers?

[hsp]

I didn't do chemistry in high-school, i'm currently doing introductory chem at uni before going onto harder stuff.

I understand about electron transfer, reduction, oxidation & which get what (generally)...
but i don't know about half equations as of yet.

Still basic knowledge.. i know that oxidated compounds/atoms come first in the equation etc.

Thanks for the help. I'm sure it'll catch on more as I progress further.

[UG]

No problem hsp 
Any time.

[hsp]

If anyone has a suggestion or some help about my C4+ ion question then feel free!

I'm pretty sure im right in saying no but any help is help.

[Borek]

C4+

C₄⁺ or C⁴⁺?

Not that I will know the answer

More seriously - I think there is no problem with creating isolated C⁴⁺ in gaseous phase. Well, perhaps "no problem" is an exagerration, but for sure it is doable. However, I doubt it is possible in the presence of other atoms.

[hsp]

yea i meant C⁴⁺...

Well from what I've been able to read is that Carbon in theory can form C⁴⁺ but in reality it's not likely because once those electrons are gone, the carbon almost instantly tries to find/be attracted to other atoms etc?

Hopefully that makes sense..

It's just annoying because I don't know if the question is referring to naturally or in some other lame form.

Thanks though.