Write the chemical reaction of lithium metal in a solution of silver nitrate. Indicate the charge of each species. Clearly indicate which metal is undergoing oxidation and which metal is undergoing reduction. State which ion is the spectator ion. Explain how you arrived at your answers.
The molecular equation is this.
Li(s) + AgNO3(aq) ==> LiNO3(aq) + Ag(s)
The complete ionic equation is this.
Li(s) + Ag^+(aq) + NO3^-(aq) ==> Li^+(aq) + NO3^-(aq) + Ag(s)
Cancel the ions common to both sides to leave the net ionic equation. The ion you cancel is the spectator ion.
Li(s) + Ag^+(aq) ==> Li^+(aq) + Ag(s)
Oxidation is the loss of electrons; reduction is the gain of electrons. Li metal goes from oxidation state of 0 to +1; Ag goes from +1 to 0. You take it from there.
Post your work if you have questions.
What type of reaction would this be tho? Synthesis, double displacement, single displacement, etc...
Well, it seems like the lithium and silver are having a little dance party in the silver nitrate solution! Let's see what's happening.
The chemical reaction is as follows:
2Li (s) + 2AgNO3 (aq) → 2LiNO3 (aq) + Ag (s)
In this reaction, the lithium metal (Li) is being oxidized because it loses electrons and increases its charge from 0 to +1. On the other hand, the silver ion (Ag+) from the silver nitrate (AgNO3) is being reduced because it gains electrons and decreases its charge from +1 to 0.
During the reaction, the nitrate ion (NO3-) acts as a spectator ion, meaning it doesn't take part in the actual redox reaction. It's just there to keep the charges balanced and party with the other ions.
So, in summary, lithium is getting a bit wild and losing electrons (oxidation), while silver is getting all dressed up and gaining electrons (reduction). And the nitrate ions are just politely spectating the whole show.
To determine the chemical reaction of lithium metal in a solution of silver nitrate, we need to consider the charges of each species involved.
First, let's take a look at the individual species:
Lithium metal (Li) has a charge of +1, as it tends to lose one electron to achieve a stable configuration.
Silver nitrate (AgNO3) dissociates into the following ions in solution:
- Silver ion (Ag+), which carries a charge of +1.
- Nitrate ion (NO3-), which carries a charge of -1.
Now, when lithium metal reacts with silver nitrate, the following chemical reaction occurs:
2Li(s) + 2AgNO3(aq) -> 2LiNO3(aq) + Ag(s)
In this reaction, lithium metal (Li) is undergoing oxidation because it loses an electron to form lithium ions (Li+). The silver ion (Ag+) in silver nitrate gains this electron to form solid silver (Ag), undergoing reduction.
The spectator ion in this reaction is the nitrate ion (NO3-). It remains unchanged throughout the reaction and does not participate in the oxidation or reduction processes.
To arrive at these answers, we need to apply the principles of redox reactions. Understanding the charges of individual species and balancing the electron transfer helps identify the oxidized and reduced species, as well as the spectator ion.