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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!
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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^+