What is the balanced net ionic equation for magnesium metal being placed in a solution of gold(3) chloride ?(with steps please)
Balanced molecular equation.
2AuCl3(aq) + 3Mg(s) ==> 3MgCl2(aq) + 2Au(s)
To convert to ionic.
1. gases remain as molecules
2. solids remain as molecules
3. strong electrolytes are displayed as ions.
4. weak electrolytes remain as molecules.
From above, AuCl3 will be split.
Mg remains as is
MgCl2 is split
etc.
2Au^2+(aq) + 6Cl^-(aq) + 3Mg(s) ==> 3Mg^2+(aq) + 6Cl^-(aq) + 2Au(s)
To convert from the full ionic equation to the net ionic equation, cancel anything common to both sides; i.e., the 6Cl- will cancel on each side but nothing else will. So you are left with this as the net ionic equation.
2Au^3+(aq) + 3Mg(s) ==> 3Mg^2+(aq) + 2Au(s)
To determine the balanced net ionic equation for magnesium metal being placed in a solution of gold(III) chloride, we need to follow a set of steps. Here's how you can find the answer:
Step 1: Write the chemical formula for the reactants.
The reactants in this case are magnesium metal (Mg) and gold(III) chloride (AuCl3).
Step 2: Determine the products of the reaction.
When magnesium reacts with gold(III) chloride, it will form magnesium chloride (MgCl2) and gold metal (Au).
Step 3: Write the complete ionic equation.
First, we need to identify the spectator ions, which are the ions that do not take part in the reaction. In this case, the chloride ion (Cl-) is a spectator ion because it appears on both sides of the equation.
The complete ionic equation is:
Mg(s) + 2AuCl3(aq) -> MgCl2(aq) + 2Au(s) + 6Cl-(aq)
Step 4: Write the net ionic equation.
The net ionic equation eliminates the spectator ions. In this case, the chloride ion is the spectator ion. Therefore, we remove it from the equation.
The net ionic equation is:
Mg(s) + 2AuCl3(aq) -> MgCl2(aq) + 2Au(s)
So, the balanced net ionic equation for magnesium metal being placed in a solution of gold(III) chloride is:
Mg(s) + 2AuCl3(aq) -> MgCl2(aq) + 2Au(s)