Not quite.
Some of the rules are as follows:
Show solids, liquids, gases as the molecule. Show aqueous solution as ions IF they are strong electrolytes.
Here is the way I would write it.
Na(s) + H2O(l) ==> Na^+(aq) + OH^-(aq) + H2(g)
H2O is a weak electrolyte so it isn't shown as ions. Even when it does ionize (slightly), it is written as
H2O ==> H^ + OH^- I show the Na^+ and OH^- as hydrated ions which they will be in solution. By the way, the original equation isn't balanced.
The molecular formula is:
Na(s)+ H2O(l)---->NaOH(aq)+H2(g)
This is showing a single displacement reaction.I am not sure how to show the complete ionic equation, this is what I have so far:
Na+(s)+ H+ H+O2-(l)---->Na+OH-(aq)+H2+(g)
Is this how you show it?
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