Final answer:
The products of the reaction shown above are Ca2+ and 2NO3-.
Step-by-step explanation:
Since this is a compound (there is no charge indicated on the molecule), the net charge on the molecule is zero (rule 6). So we have:
This particular example is important because all of the reactants and the products are aqueous, meaning they cancel out of the net ionic equation. There is no solid precipitate formed; therefore, no precipitation reaction occurs.
Examining this equation shows that two chemical species are present in identical form on both sides of the arrow, Ca2+(aq) and NO3(aq). These spectator ions-ions whose presence is required to maintain charge neutrality-are neither chemically nor physically changed by the process, and so they may be eliminated from the equation to yield a more succinct representation called a net ionic equation:
Ca2+ (aq) + 2NO3- (aq) → Ca(NO3)2 (aq)