Inorganic Chemistry

Lithium and Chlorine both have valencies of one but they form positive one and negative one charged ions respectively during chemical reactions. Explain why. Pls reply ASAP!!!

wat could i use as an inert "oil" or watever for my lithium that i could obtain pretty easily without having to buy online?

hey i read somewhere that lithium can cause some really weird reactions that can purify metal oxides chlorides nitrates ... and so on. theres this reaction thats very strange its KNO3 + Li ---> LiNO3 + K is this possible? I heard its how some scientists purify a few unamed actinides. can anyone shed some light on this?

I dont know if this realy goes here but I want to know what the coldest substance known to man is... I know that liquid helium is the coldest on earth but whats the hottest?

Hi there! I'm just wondering why my nice lil equation isn't working in reality: 2Al+3H2SO4=>Al2(SO4)3+3H2 excess sulphuric is always used. The Sulphuric acid is battery grade, so I'm guessing it must be contaminated, but isn't it usually just some Pb? Even when I concentrated the acid, still nothing appeared to happen a d no effervence was noted. I know the Al has an oxide coating, but it should still go to completion.even if i do get a drop of water, shouldn't it still continue on with evolving H2. Al2O3+3H2SO4=>2Al2(SO4)3+3H20 What am i doing wrong here? It seems pretty simple, but hmmm (I haven't done formal chem for some months now so maybe i'm…

Hi, I am new to chemistry and been keeping up with my summer school work on chemistry. There is one problem I am stuck on..... Is NaNO3 a ionic, covalent, or both? Thanks.

With copper and zinc electrode, copper(II) sulphate as electrolyte, what will be the product? My exercise book said that there will be a gas from the positive electrode (copper electrode). I checked the standard reduction potential and found that the oxidizing power of sulphate ion is smaller than that of copper (II) ion. so is my book wrong? And which anion has a smaller oxidizing power than copper (II) ion as well?

I'm having trouble igniting my thermite. I'm using magnesium ribbon as fuse, which is what most people use, so I'm guessing that it has to do with the ratio of aluminum powder to rust. I don't have a scale of any sort so I used the densities to calculate the approximate volumetric ratios which came out to be (I may have miscalculated) about two parts of rust to one of aluminum. What am I doing wrong?

By the Arrhenius definition, acids and bases must be in aqeous solution. Is it possible to have acidic/basic compounds outside of solution? I know that HCl is a gas and NaOH is a crystalline solid outside of solution, but is it possible to have compounds like hydrogen sulfate or hydrogen nitrate OUTSIDE of solution?

theres a big rust stain on my carpet, is there a chemical that could oxidize the iron oxide to a colorless form or something?- without hurting the the color of the structure of the carpet itself

1, How do you test a substance whether it is or not water, chemically? 2, When Water and Phosphorus Tribromide are reacted, what reagent is water here? above are the questions that apear in my exam, and I have already done, but just want to see how you other will solve it. Albert

Ok, i hooked it up to some electricity and it didnt work maybe the salt bridge is too small? what do you guys think.. it was just suposed to be a "prototype" improvised from some old pipe and a PET bottle. The power supply was 5V at 13A and i used carbon electrodes from a lantern battery.

Im familiar with magnesum burning very bright, and i can obtain that at a local chemical sellign store, but im wondering what other materials that i have access to (not being in a university etc not even being 18) burn extreamily bright, as bright or brighter then magnesum.

Ive always wondered this, would it be possible for us humans to recreate the ozone layer we destroyed? i mean, i know its not this simple, but if we produced massive amounts of ozone, would it make its way back up into the stratoshpere (or werever the ozone layer is)"? I mean, could you just imagine a bunch of international ozone plants that use UV light or X-rays or something to create ozone thwn just get a clever way to pipe it to a desolate place and realease it? Ok, so this is a crazy idea, but it might just work.

Why ethanedioic acid is present?According to my book, ethanioate ions have a higher reducing power than H+? so ethanioate ion will be oxidized and H+ will be reduced. One more question: Why Aqua regia does not last very long?

Is potassium nitrate reactive with any liquids i.e. alcohol or water ? Well, thx for the info

ive heard froma few sources that lithium will absorb the oxides chlorides adn other "ides" from other transition and alkali metals and leave the existing metal in its semi pure state. i have a buttload of lithium culled from a huge amount of battery picking... i want sodium and soem of the other alkali metals whats the process can anyone help?

I was wondering whether there are any chemists who can help me find an alloy which will decompose water into hydrogen and oxygen at a rapid rate. I have very limited chemistry knowledge and any assistance or knowledge you can provide me with will be greatly appreciated. I have been told Zinc would work. But is this inexpensive and what rate of hydrogen production is expected. I was told that there is an inexpensive alloy which can act as a catalyst and rapidly split water (no one wants to divulge the name!). Anyone have any ideas?

Given this equation: PH2O2-(aq) + OH-(aq) --> PHO32-(aq) + H2(g) How do I determine whether the OH- is acting as an acid or base? Any explanations will be greatly appreciated. Thanks in advance.

so i was reading about energetic mixtures of acids and bases, enthalpy change, flash boiling and the like when i decided to think about the anhydrides of such acids and bases. so if we want to consider the most energetic acid/base mixture, our acid will be conc H2SO4. perchloric acid cannot get up to as high concentrations and the fact that it is an oxidizing acid and can also decompose at elevated temperatures is irrelevant, because we are considering just the acid/base reaction. now as for a base, cesium hydroxide would be beastly, and is soluble in 0.25 parts water. thus, 4g CsOH/1g H2O. 4(132.9+16+1)/(4(132.9+16+1)+(18))=0.97 so we can get CsOH to 97% conc.…

Is NH4NO3 ammoniume nitrate ? and is this a resonable price for it ? http://advance-scientific.net/Properties.asp?CODE=A1217

Is 35% H202 lab garde stuff ? I bough some and i was wondering if there where some cool exerements with it? Thx for the info.

i decided that since my personal lab is severely underfunded i may as well use it to produce some kind of income. first, i wish to electroplate silver onto various items. of course, AgNO3 and AgClO4 are two of the very few Ag salts are reasonably soluble at any reasonable temperature. AgNO3 would be a beast to try to make AgClO4 would as well, but i have an idea; tell me if you think this is possible and/or sane mix clorox with ammonia, recover gas evolved. burn the gas. problem is attempting to add the Ag. if i bubble it into a solution i'll get plenty of HClO4... beyond electroplating, there is electrolysis. hey, it's cheap, no? anybody know…

Once I have performed electrolysis in a container, I have both O2 and H2 dormant in the electrolysis container. I'm trying to find a way of both separating the two gasses (no longer ions) and presurizing them out of the chamber later to be forced into the intake of a vehicle. Anyone have any ideas for doing the two described processes (separating and pressurizing the gasses). If I put them into a vacuum line, then air is sucked into the electrolysis chamber (due to the negative pressure created by sucking the H2 and O2 gasses out). The air sucked in dilutes my pure mixture of Hydrogen and Oxygen, further complicating matters. Ideally, I would like to speparate both the hy…

Does anybody know how to oxidise ammonia? I need nitric acid very badly. Thanks!