The nature of Sodium and Chloride

[Aerlinn]

Can someone please help me with these two questions?
In terms of bonding and properties, why does Sodium conduct electricity in both the solid state and in solution/ molten state?
In terms of bonding and properties, why doesn't Chlorine conduct electricity either in the solid state or in solution/ molten state?
I just wanted to confirm whether my answers to these were correct, so can anyone answer them? =)

Thanks!

[opuntia]

In NaCl, when it is in solid form as well as in molten state, the electrons are free to move and carry charge, hence conduct electricity.
But in Cl the electrons are not free to move even if they are in solid state or molten.


PS. You should have included your answer with the question.

[Aerlinn]

I think you were refering to Sodium Chloride. Those two were separate questions, about Sodium, and about Chlorine.
What I wrote was that Sodium is a metal, there has a metal lattice which conducts electricity in both solid and molten state, because in both states, the electrons experience a pull towards the positive end when an electric current is applied.
(But I'm not sure whether that's right or whether Sodium is a metal)

And for the other one, since Chlorine would be covalent molecular element... it would be non-metal, and unable to conduct electricity.
(I'm not sure, in terms of bonding, why!)

Help?

[opuntia]

:oops: I'm so sorry for the mistake.

Sodium is a metal and your answer is right as far as my knowledge about Na is concerned.

In chlorine no, free electrons are there to carry charge and that's why it cannot conduct electricity.

[RobJim]

Sodium is a metal and participates in metallic bonds. In this sort of bond, valence electrons can move throughout the entire mass of metal freely. Chlorine ties it's valence electrons in covelant bonds which are confined to the area between two atoms. There is no sharing of valence electrons throughout a large mass of chlorine, so electrons cannot move around (AKA conduct electricity).

[Neecze]

In terms of bonding and properties, why doesn't Chlorine conduct electricity either in the solid state or in solution/ molten state?

Well, chlorine in (for example) water solution can conduct electricity but that conductivity is poor.

In water solution chlorine undergo reaction:
Cl2 + 3H2O <=> ClO- + Cl- + 2H3O+

And because of presence of these ions - water solutions of chlorine can conduct electricity.

[mr.chemistry]

Originally Posted by Aerlinn

Can someone please help me with these two questions?
In terms of bonding and properties, why does Sodium conduct electricity in both the solid state and in solution/ molten state?
In terms of bonding and properties, why doesn't Chlorine conduct electricity either in the solid state or in solution/ molten state?
I just wanted to confirm whether my answers to these were correct, so can anyone answer them? =)

Thanks!

my dear
i hope that i can help u in the following:-
Sodium is a metal whic is located in group 1A in the periodic table, and it is characterized by its large atomic radius.
so the valence electron in the outer most level is free electron due to the weak attractive force of the nucleus.
as a result the free electrons allow the passage of electric current.
that's about the sodium in its elementary state, but in its compounds such as Na Cl.
at firist, just ionic compounds or the polar compounds that can conduct electricity but in the form of moltens or solution.( why??)
so that the ions will be free and allow the passage of current.
but about chlorine:-
it is a gaseous non metal which has a small atomic radius, so it has no free electrons.
but in its aquoeous solution it conducts electricity but the reason here is due to the presence of what is called hydronium ions H3O^+