For those who haven't seen my previous post; I request you to go and search for it, it says Lab part 1 on it. You will not know what I'm asking about, if you don't read it it. Overall nothing will make sense. Thank you very much for all your help.
These are my observations in the data table: The object is in the first column and the properties that I recorded for that object are in the second.
Object |Properties
Copper (II)
Chloride = blue powder,
sparkly
CuCl2(soln) = almost clear blue,
green at bottom
Aluminum = shiny, metallic
silver
Reaction
Observation = aluminum piece is
going brown, the
water is going
darker from the top
Bubbles r arising
by the aluminum
Filter Residue = It is dark brown
in colour and looks
crusty
Can you please help me add more for the last one = Filter Residue.
Questions:
1.What ions r present in a solutions of copper(iI) chloride? What colour do you think the copper(II) ions are? Explain.
I don't really get the first part. When it says "What ions" does it refer to the size, shape of those ions, meaning how they kind of look like? For the 2nd part I got blue in colour, but I'm not sure if it's supposed to be bluish green.
2.What r the properties of aluminum that confirm it is a metal?
I just wrote that it is silver and shiny like one. - Do I need to add more?
3.What observations convinced u that a chemical reaction was occuring between the aluminum foil & the copper(II) chloride solution?
I wrote: Observations which convinced me that a chemical reaction was occuring beteen the aluminum foil and the copper(II) chloride solution was that the aluminum piece was changing its colour and bubbles were starting to arise. - is this good?
4.What happened to the aluminum atoms in the foil? Explain.
?????????????????????
5.What happened to the copper(II) ions in the solutions? Explain
I just wrote that they began to dissolve.-How would I explain this?
6.What happened to the chloride ions in the solution?
I don't think anything happened to them.
I'll appreciate all the help you could give me, thank you very, very much:-)
1.What ions r present in a solutions of copper(iI) chloride? What colour do you think the copper(II) ions are? Explain.
I didn't search for the first part because that's too laborious; however, I think I can HELP answer these questions.
I don't really get the first part. When it says "What ions" does it refer to the size, shape of those ions, meaning how they kind of look like? For the 2nd part I got blue in colour, but I'm not sure if it's supposed to be bluish green.
It's referring to the ions in the CuCl2 solution. You have Cu+2 ions and Cl^-. Cu ions are blue or blue green in almost all of their compounds (some exceptions)
2.What r the properties of aluminum that confirm it is a metal?
I just wrote that it is silver and shiny like one. - Do I need to add more?
I would have said it looked metallic. It is a solid (most metals are solid? right?
3.What observations convinced u that a chemical reaction was occuring between the aluminum foil & the copper(II) chloride solution?
I wrote: Observations which convinced me that a chemical reaction was occuring beteen the aluminum foil and the copper(II) chloride solution was that the aluminum piece was changing its colour and bubbles were starting to arise. - is this good? Yes
4.What happened to the aluminum atoms in the foil? Explain.
?????????????????????
The aluminum metal was dissolving and forming Al^+3 ions in the solution.
5.What happened to the copper(II) ions in the solutions? Explain
The copper(II) ions are coming out of solution (each ion adds two electrons) and forming metallic copper on the aluminum foil.
Cu^+2 + 2e ==> Cu(s)
Al(s) ==> Al^+3 + 3e
I just wrote that they began to dissolve.-How would I explain this?
The copper is not dissolving. The copper ions are already in solution.
6.What happened to the chloride ions in the solution?
I don't think anything happened to them
You are right. The chloride ions started in solution and they stay in solution. They are not part of the reaction. Ions that don't enter the equation are called spectator ions. The net ionic equation is
2Al + 3Cu^+2 ==> 2Al^+3 + 3Cu
Thank you very much DrBob222:-)
oh my god i love this.
i don't get the answer at number 5 though. becaude if the aluminum is a +3 ion charged. i don't know where the ions added the two electrons. ?:|.
1. To determine the ions present in a solution of copper(II) chloride, we need to understand what ions are and how they relate to copper(II) chloride. In chemistry, ions are atoms or molecules that have gained or lost electrons, resulting in a net positive or negative charge. In the case of copper(II) chloride, it dissociates in water to form copper(II) ions (Cu2+) and chloride ions (Cl-). So, when we refer to "ions" in this context, we are asking about the copper(II) ions and chloride ions present in the solution.
Regarding the color of copper(II) ions, copper(II) ions are typically blue in color. However, in the case of copper(II) chloride, the color may appear more bluish-green due to the combination of the copper(II) ions and chloride ions interacting with each other.
2. The properties of aluminum that confirm it is a metal include its shiny, metallic silver appearance. Additionally, metals are generally good conductors of heat and electricity, so if you had observed those properties, you could mention them as well.
3. Your observation that the aluminum foil was changing its color and that bubbles were arising indicates a chemical reaction between the aluminum foil and the copper(II) chloride solution. These observations suggest that a chemical transformation was occurring, which is characteristic of a chemical reaction.
4. When aluminum foil reacts with copper(II) chloride solution, the aluminum atoms lose electrons to form aluminum ions. This electron transfer is known as oxidation. The aluminum atoms are oxidized into aluminum ions with a positive charge (Al3+). These aluminum ions contribute to the overall chemical changes taking place in the reaction.
5. The copper(II) ions in the solution initially present as copper(II) chloride (CuCl2) dissolved in water. During the reaction with aluminum foil, the copper(II) ions undergo reduction, meaning they gain electrons from the aluminum atoms. This reduction reaction leads to the formation of metallic copper (Cu) as a solid product, which might appear as a layer on the aluminum foil.
6. In the solution, the chloride ions may not undergo any significant change or reaction. They can remain in the solution as chloride ions (Cl-) unless there are specific reaction conditions or other reactants that interact with them.
I hope this explanation helps! Let me know if you have any further questions.