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?

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.

To show the complete ionic equation for the given reaction, you need to break down all the compounds into their respective ions. Here is the complete ionic equation for the reaction:

Na(s) + H2O(l) → Na+(aq) + OH-(aq) + H2(g)

Explanation:
1. Start with the balanced molecular equation: Na(s) + H2O(l) → NaOH(aq) + H2(g). This equation represents the overall reaction but does not show the individual ions involved.
2. Break down the soluble compounds (those that dissociate into ions in solution) into their constituent ions. In this case, NaOH(aq) dissociates into Na+ and OH- ions.
3. Keep any solid (s) or liquid (l) compounds unchanged since they do not dissociate into ions in the reaction.
4. Write the balanced complete ionic equation by showing all the individual ions involved in the reaction.

So, the complete ionic equation for the reaction Na(s) + H2O(l) → NaOH(aq) + H2(g) is:

Na(s) + H2O(l) → Na+(aq) + OH-(aq) + H2(g)

Note that the + and - symbols represent the charges on the ions. Na+ and OH- are positively and negatively charged ions, respectively, while H2(g) represents hydrogen gas formed during the reaction.