Many element collectors like to display their samples in a wall-mounted glass case. Well, I was thinking that the same could be done with salts, coordination complexes and organometallic compounds of transition (d block) metals to exhibit the diversity of colours.
I'm pretty sure that it is possible to get a nice rainbow, which could fill up quite a lot of space, even with samples which are only a few grams. Nevertheless, it would for sure look awesome!
GREAT VIDEO.....I swear there are a lot of ammonia/transition metal complexes that have such great colors. Yeah no camera picks up color the way it is in real life. I record something orange it looks red. I record something red and it looks orange...lol.
Hi😎 How to make Hexamine Nickel II Perchlorate ? Can I prepare with Perchloric Acid 70%, Like Nickel II Perchlorate prepared ❤️ Please Reply... Make a video ❤️ Thanks...
The ice bath is needed to cool the reaction, as it becomes quite hot. And it decreases the solubility of the product afterwards. The washing is to remove ammonium chloride.
I think I'm about to do something like this tomorrow. Two questions, ... 1. Why wouldn't the aqueous solution of NiCl₂ turn into the hexaaqua ion [Ni(H₂O)₆]Cl₂? 2. Why add the saturated NH₄Cl solution before the concentrated ammonia? Is this a buffer solution because just ammonia would deprotonate the [Ni(H₂O)₆]²⁺ to [Ni(H₂O)₄(OH)₂]?
Actually, it turns into the aqua complex in solution, but this is often neglected in chemical equations. The NH4Cl helps to lower the solubility of the amine complex, due to the same anion as far as I know.
Usually it is made by students to practice the synthesis of an inorganic complex. I had to prepare it myself, when I studied chemistry :) The only use I found when doing my research, was that the ligands are substituted by cyclopentadiene and it is used as a precursor to other more sophisticated complexes.
Random Experiments Int. - Experiments and syntheses Thank you. Mine is labeled 28%-30%. I'll make the adjustment. (Or would you say, in this case it, would not mater?)
You can adjust it, but a higher concentration doesn't have any negative effects. It would be just about cost and efficiency. To be honest, I would be lazy and simply use the higher concentration. :)
It's highly likely that the ammine complex hasn't formed. Green is very likely nickel(II) hydroxide. Possibly not enough ammonia solution or the concentration of the ammonia is too low.
I would mix a solution of nickel sulfate with a solution of calcium or barium nitrate. This would cause calcium or barium sulfate to precipitate out. Then I'd filter off or decant the solution, let the filtrate evaporate (boiling would be pretty toxic) and do a few recrystallizations, slightly below boiling on the resulting nickel nitrate.
The precipitation of the complex was I guess due to common ion effect of chloride ions. So i guess sodium chloride could be used instead of ammonium chloride. Again why mix nickel chloride with ammonium chloride at first? It would decrease solubility of nickel chloride isn't it? It should have been added after complexation.
The [Ni(NH3)6]Cl2 is somewhat well soluble in water. The NH4Cl is highly soluble and increases the concentration of chloride ions lowering the solubility of the complex. You can watch my videos about the solubility product, if you want to know more.
Lucas Wang we need to make this bigger, I mean she was a prominent channel, in fact I got sub to Random Experiments bc I saw him in the comments of ChemPlayer :(
I myself have a sort of backup of Chem Player videos. I have 186 videos in my Chem Player download folder; all MP4's in 720p resolution. I'm perfectly willing to share them about, however I hesitate to do so without having his/her/their permission beforehand. My downloads aren't max-res and also don't include the text accompaniments so I regard them an incomplete record.
You are guilty of two unforgiveable sins: Twice you added liquid to chemcals - the chemical should always be added to the liquid - best practice. Your project and end result however was fabulous!
This video was very well made and very informative. Thank you!
Interesting and well presented. I've just discovered your channel, and well worth a sub. Keep them coming.
Interesting, thank you! But what is the use for this compound, except that it has a nice color?
Thanks, that will make nice flowering!
Many element collectors like to display their samples in a wall-mounted glass case. Well, I was thinking that the same could be done with salts, coordination complexes and organometallic compounds of transition (d block) metals to exhibit the diversity of colours.
I'm pretty sure that it is possible to get a nice rainbow, which could fill up quite a lot of space, even with samples which are only a few grams. Nevertheless, it would for sure look awesome!
@@RaExpIn please make video on NiCo2O4 synthesis by hydrothermal method
GREAT VIDEO.....I swear there are a lot of ammonia/transition metal complexes that have such great colors. Yeah no camera picks up color the way it is in real life. I record something orange it looks red. I record something red and it looks orange...lol.
Nice sir very helpful
What are you going to use this chemical for?
What can it be used for?
Nice work! Other than being interesting and pretty does it have any known uses or other features an amateur would find interesting?
Wikipedia says it can be used as a source of highly pure cobalt-free nickel ¯\_(ツ)_/¯
The chloride version not so much.
The nitrate (TACN) and the perchlorate (TACP) versions are explosives.
Reference?
Very useful to me teaching my students during COVID-19 pandemy. Thks
Glad I could help :)
Hi😎 How to make Hexamine Nickel II Perchlorate ? Can I prepare with Perchloric Acid 70%, Like Nickel II Perchlorate prepared ❤️ Please Reply... Make a video ❤️ Thanks...
Awesome ❤️
will have a lab test very soon. wish me luck!
Superb
Thank you
what is the role of the ice bath and the washing?
The ice bath is needed to cool the reaction, as it becomes quite hot. And it decreases the solubility of the product afterwards. The washing is to remove ammonium chloride.
Thankyou sir
just asking, where did you get that hotplate/stirrer combo?
The ones I have are all from the trash at a school or university. And I got one from ebay.
Why haven't you used ethanol to crush the product out of solution in the first place?
Very pretty and informative. But why was the ammonium chloride needed for the reaction?
I'm pretty sure that it is added to increase the concentration of the chloride ions. This decreases the solubility of the complex.
I think I'm about to do something like this tomorrow. Two questions, ...
1. Why wouldn't the aqueous solution of NiCl₂ turn into the hexaaqua ion [Ni(H₂O)₆]Cl₂?
2. Why add the saturated NH₄Cl solution before the concentrated ammonia? Is this a buffer solution because just ammonia would deprotonate the [Ni(H₂O)₆]²⁺ to [Ni(H₂O)₄(OH)₂]?
Actually, it turns into the aqua complex in solution, but this is often neglected in chemical equations. The NH4Cl helps to lower the solubility of the amine complex, due to the same anion as far as I know.
GOOD JOB!
Thx :)
Great synthesis. what are the properties of this compound?
Usually it is made by students to practice the synthesis of an inorganic complex. I had to prepare it myself, when I studied chemistry :) The only use I found when doing my research, was that the ligands are substituted by cyclopentadiene and it is used as a precursor to other more sophisticated complexes.
Would be interesting to see this made during the separation of nickel from cobalt in a mixed ore.
Is it a viable way to separate the metals because cobalt forms dozens of ammonia complexes
What is the role of saturated ammonium chloride in this experiment??
I'm guessing it increases the concentration of chloride ions and decreases the solubility of the complex, which leads to a better yield.
What is the strength of the concentrated aqueous ammonia?
Michael Aichlmayr 25%
Random Experiments Int. - Experiments and syntheses Thank you. Mine is labeled 28%-30%. I'll make the adjustment. (Or would you say, in this case it, would not mater?)
You can adjust it, but a higher concentration doesn't have any negative effects. It would be just about cost and efficiency. To be honest, I would be lazy and simply use the higher concentration. :)
what is the possible reason if my complex turns green instead of violet :'(
It's highly likely that the ammine complex hasn't formed. Green is very likely nickel(II) hydroxide. Possibly not enough ammonia solution or the concentration of the ammonia is too low.
How would you change nickle sulfate to nickle nitrate?
I would mix a solution of nickel sulfate with a solution of calcium or barium nitrate. This would cause calcium or barium sulfate to precipitate out. Then I'd filter off or decant the solution, let the filtrate evaporate (boiling would be pretty toxic) and do a few recrystallizations, slightly below boiling on the resulting nickel nitrate.
@@RaExpIn Awesome, thanks, i have some barium nitrate so i will try that out.
The precipitation of the complex was I guess due to common ion effect of chloride ions. So i guess sodium chloride could be used instead of ammonium chloride. Again why mix nickel chloride with ammonium chloride at first? It would decrease solubility of nickel chloride isn't it? It should have been added after complexation.
nh3 a strong field ligand, then why the electrons are not pairing ?! in hexaamminenickel(ii) chloride
It's a moderate ligand not strong field
مادور الامونيا في هذا التجربه
What was that capsule
Do you mean the glass ampoule?
it looks yummy i wanna eat it.
Why do you use NH4Cl?
To lower the solubility of the complex.
@@RaExpIn why??? I don t understand....
The [Ni(NH3)6]Cl2 is somewhat well soluble in water. The NH4Cl is highly soluble and increases the concentration of chloride ions lowering the solubility of the complex. You can watch my videos about the solubility product, if you want to know more.
Looks like candy. Mmmm. ;-)
ChemPlayer got shut down!
Oh no! I loved that channel :(
Seriously?! What can be done to help him out?
JamesG I dont know but yt is bookburning good channels with no reason or stupid fear mongering justifications, hope she got a backup
Lucas Wang we need to make this bigger, I mean she was a prominent channel, in fact I got sub to Random Experiments bc I saw him in the comments of ChemPlayer :(
I myself have a sort of backup of Chem Player videos. I have 186 videos in my Chem Player download folder; all MP4's in 720p resolution. I'm perfectly willing to share them about, however I hesitate to do so without having his/her/their permission beforehand. My downloads aren't max-res and also don't include the text accompaniments so I regard them an incomplete record.
You are guilty of two unforgiveable sins: Twice you added liquid to chemcals - the chemical should always be added to the liquid - best practice. Your project and end result however was fabulous!
0:01 *color was edited. Yeah no. Don't. This isn't your sister's instagram sunset photoshoot.