# I Found Two Old Cans of Alkali Metal Amides ## Метаданные - **Канал:** ChemicalForce - **YouTube:** https://www.youtube.com/watch?v=Q2HuEeUsnsU - **Дата:** 03.04.2026 - **Длительность:** 8:42 - **Просмотры:** 49,621 ## Описание I found two old cans of chemical reagents that were decades old, opened them, and performed several experiments with what was inside. _________________ 0:00 Intro 0:34 Opening a can of sodium amide and its reactions 1:50 Opening a can of lithium amide 2:30 Lithium amide and water 2:40 Generating ammonia by mixing two solids 2:56 Lithium amide and hydrochloric acid 3:10 Lithium amide and nitric acid 3:48 Lithium amide and liquid nitrogen dioxide 4:33 Combustion of lithium in ammonia 4:46 A solution of lithium in liquid ammonia and concentrated nitric acid 6:00 Decolorization of a blue solution of lithium in liquid ammonia by passing carbon monoxide 6:41 Magnetic attraction of iron particles from iron pentacarbonyl decomposition _________________ ❤️‍🔥 https://www.patreon.com/ChemicalForce ❤️‍🔥 ## Содержание ### [0:00](https://www.youtube.com/watch?v=Q2HuEeUsnsU) Intro Hey guys, take a look at this old tin can of sodium amide that I managed to find. Sodium amide is an extremely reactive and hazardous substance that requires strict adherence to safety precautions. But what interested me the most is the following. On the Wikipedia page about sodium amide, it states that in the presence of peroxides may form. This is accompanied by yellowing or browning of a solid. As such, sodium amide is to be stored in a tightly closed container under an atmosphere of an inner gas. Sodium amide samples which are yellow or brown in color represent explosion risks. To be honest, I don't ### [0:34](https://www.youtube.com/watch?v=Q2HuEeUsnsU&t=34s) Opening a can of sodium amide and its reactions think we'll be able to find any traces of those yellow or brown denderos peroxides in such a tightly sealed can. I've broken the seal. Now, let's see what condition the sodium is in. Good. Sodium amide has a noticeable ammonia smell in air, but these caked chunks don't look like a reactive chemical at all. I'm sure it won't even react with water, but we still needed to check. There is absolutely no reaction and no ammonia smell, just barely noticeable bubbles. Even if I bring a piece of dumplitmos paper close to it, there is no color change. Nothing like what you'd see ammonia were present in the air. Write in the comments what you think sodium has turned into after such a long period of storage. But before you share your thoughts, take a look at its reaction with nitric acid. ### [1:50](https://www.youtube.com/watch?v=Q2HuEeUsnsU&t=110s) Opening a can of lithium amide The second older tin can turned out to contain lithium. Even though it's old, the packaging looks intact and reliable. Let's open this can. The lid of the can even shows instructions on how to do it properly. This reagent looks much more promising. It also has a slight ammonia smell. Overall, lithium is less reactive than sodium. So, if we add water to it, it reacts just like for sodium without the release of ammonia, but without ### [2:30](https://www.youtube.com/watch?v=Q2HuEeUsnsU&t=150s) Lithium amide and water ignition. Ammonia ### [2:40](https://www.youtube.com/watch?v=Q2HuEeUsnsU&t=160s) Generating ammonia by mixing two solids will also be released actively if we add dry ammonium chloride powder to lithium amide. The indicator paper quickly changes color to one characteristic of an alkaline reaction. If a lot of ammon is produced during hydraysis, then reacting it with hydrochloric acid will ### [2:56](https://www.youtube.com/watch?v=Q2HuEeUsnsU&t=176s) Lithium amide and hydrochloric acid generate a lot of white films of ammonium chloride. Nitric acid unlike hydrochloric acid can ### [3:10](https://www.youtube.com/watch?v=Q2HuEeUsnsU&t=190s) Lithium amide and nitric acid ignite lithium amide. Liquid nitrogen dioxide can do the same ### [3:48](https://www.youtube.com/watch?v=Q2HuEeUsnsU&t=228s) Lithium amide and liquid nitrogen dioxide thing. Lithium itself burns with a bright white ### [4:33](https://www.youtube.com/watch?v=Q2HuEeUsnsU&t=273s) Combustion of lithium in ammonia flame. But if you direct a stream of ammonia at it, it will start burning with a red orange flame forming lithium ammide. ### [4:46](https://www.youtube.com/watch?v=Q2HuEeUsnsU&t=286s) A solution of lithium in liquid ammonia and concentrated nitric acid Lithium like other alkali metals can be dissolved in liquid ammonia forming a so-called blue solution of salvated electrons. If after some time the ammon is evaporated. Of course, in the absence of moisture and under an inert atmosphere, you can obtain lithium amide. By the way, concentrated nitric acid can ignite a solution of lithium in liquid ammonia. ### [6:00](https://www.youtube.com/watch?v=Q2HuEeUsnsU&t=360s) Decolorization of a blue solution of lithium in liquid ammonia by passing carbon monoxide Now, let's drop another piece of lithium into liquid ammonia and wait until the test tube turns almost completely blue. Now, I'll insert a glass tube into this solution and start bubbling carbon monoxide through it. Pretty soon, the blue color of the solution disappears. This happens due to a formation of lithium acetylene dilate and lithium benzinhexate. These compounds were once mistakenly thought to be lithium carbonel. ### [6:41](https://www.youtube.com/watch?v=Q2HuEeUsnsU&t=401s) Magnetic attraction of iron particles from iron pentacarbonyl decomposition For our next experiment, I'll put a small amount of lithium amide into a test tube and heat it slightly. Then I'll place a magnet above a test tube. Next, we'll need iron pentacarbonel. We shall add drop by drop to the heated lithium amide. As a result of this reaction, very fine particles of metallic iron are formed which immediately get attracted to the magnet as they leave the test tube. However, due to the strontium hood, not all the iron particles managed to get attracted to the magnet. When I filmed this reaction in one take, I added quite a lot of iron pentacarbonel at once and before it could decompose, it evaporated from the test tube and its vapors ignited. So, I decided to include this shot. It seemed really interesting to me. So guys, I hope you enjoyed the video, an idea for which came to me as soon as I found a couple of old cans of sodium and lithium. I hope you learned something new and I'm really glad I was able to put them to good use. I'd also like to give a huge thank you to all my patronons. It's thanks to you that this channel lives and grows and that new videos keep coming out. Without you, this channel wouldn't exist and I wouldn't have the opportunity to create new content for all of you. So, if you have the opportunity, please consider becoming my patron. It's critically important. Thanks for watching. See you in the next video. --- *Источник: https://ekstraktznaniy.ru/video/49297*