Write molecular, ionic, and net ionic equations.

AgNO3(aq) + KBr(aq) -->

The molecular equation.

AgNO3(aq) + KBr(aq) ==> AgBr(s) + KNO3(aQ)
The net ionic equation is
Ag^+(aq) + Br^-(aq) = AgBr(s)
I will leave the total ionic equation to you. Post your work if you need further help.

Molecular equation:

AgNO3(aq) + KBr(aq) --> AgBr(s) + KNO3(aq)

Ionic equation:

Ag+(aq) + NO3-(aq) + K+(aq) + Br-(aq) --> AgBr(s) + K+(aq) + NO3-(aq)

Net ionic equation:

Ag+(aq) + Br-(aq) --> AgBr(s)

To write molecular, ionic, and net ionic equations, you need to know the solubility rules for compounds and the phase of each species involved. Let's break down the given chemical equation and write the equations step by step.

The given chemical equation is:

AgNO3(aq) + KBr(aq) -->

Step 1: Write the molecular equation.
In the molecular equation, you represent all the reactants and products as if they were intact, undissociated compounds.

AgNO3(aq) + KBr(aq) → AgBr(s) + KNO3(aq)

Step 2: Write the complete ionic equation.
In the complete ionic equation, you represent all of the soluble ionic compounds as dissociated ions. You represent insoluble compounds and those that are weak electrolytes as undissociated compounds.

Ag+(aq) + NO3-(aq) + K+(aq) + Br-(aq) → AgBr(s) + K+(aq) + NO3-(aq)

Step 3: Write the net ionic equation.
In the net ionic equation, you eliminate the spectator ions (ions that appear on both sides of the equation) since they do not participate in the actual chemical reaction.

Net ionic equation: Ag+(aq) + Br-(aq) → AgBr(s)

In this case, both K+ and NO3- ions are spectator ions and do not participate in the actual reaction.

This really helped me with figuring out the equations.