Inorganic Chemistry

Hi, I'm having hard time convincing myself to two answers from my inorganic chemistry course's last year's exam. 1. Which of the following statements are valid concerning ideal gas mixtures: (there are three choices, two of which make sense to me, but this is the one I disagree) * Each gas present in the mixture behaves independently of the others. The solution says that it is valid, but I do not agree. Like, in the textbook, it mentioned how oxygen gas would not react with water, but NH3 would readily dissolve in the water - which clearly show that gases like NH3's behaviors are dependent on other molecules. Or, am I reading something into the question? 2…

In the lecture I have just attended the professor talked about molecular orbital (MO) theory. He said a bond orbital, even for an individual orbital contribute so little that the contribution tends to none, should have an energy lower than all the contributing constituent orbitals. I have been thinking about this statement, and got some confusion in the following circumstance. If, now, we consider oxygen molecule, each oxygen has its 2s and three 2p considered. 1) The two 2s would form a bonding and an anti-bonding orbitals (1sigma and 2sigma*). 2) The two 2px would form a bonding and an anti-bonding orbitals (3sigma and 4sigma*). 3) The 2py and 2pz in each oxygen…

I had some black powder containing charcoal, sulfur, and sodium nitrate, which I added some magnesium powder to. After mixing, I started to compress some in preparation for ignition, but as soon as I started to press it together, it became suddenly warm. Yikes! What is the magnesium reacting with that is causing this to happen? BTW, the amound of powder was very small so don't worry about me blowing myself up. When you experiment with explosives, ALWAYS START SMALL!

The compounds KMnO4, KBrO3, NaBrO3, NaIO3, KIO3 are oxygen liberators. They become explosives if they are dealt with organic alcohol,aldeheyde and ketones. They form explosive mixtures. People should learn the chemistry and chemical reactions of these compounds before handling them with any small lab experiments.

I'm trying to collect all the (non highly-radioactive) elements of the periodic table, in pure form. I already have about 65, and I just received 50g of iodine, and will soon receive 5ml of bromine. I'm having problems with storage of iodine though, and I suppose bromine will be even worse... The iodine arrived in a glass container with a plastic/rubbery seal, and it was already slightly corroded. I put it in a borosilicate glass vial with a screw-cap with silicone seal, but it turned yellow pretty soon. Iodine smell didn't come out but I guess it was just a matter of time. Then somebody told me to store it in a glass vial with glass cap (the ones with a "ground" glass …

i have no idea what i made i was doing electrolysis an and a saltwater solution. light blue green color started forming in the solution what is this. i also noticed both electrodes were bubbeling the one bubbeling more im guessing is hydrogen and the one bubbeling less is chlorine i also notice the one bubbeling less is dissolveing so whats in the solution please tell me thanks. i also did this with one electrode copper and the other an aluminum pop tab the aluminum dissolved and the solution was grey and thick please tell me what happend.

I was just wondering about the reaction of soft-acids and soft bases. Like generic acid/base reaction give a salt and water/neutral species, does soft acid and soft bases give a salt or they would give an adduct/complex? Lets say that the soft base is NMe3 and soft acid is a diradical oxgen molecule. Is this similar to the reaction between ammonia and diradical oxygen which goes like this 4NH3 + 5O2 -------> 4NO + 6H2O? Second question is more of a thought really. Why do we want to look for electrons when we look at an atom. I am asking this question as a quantum mechanics student. Does position or state of an electron give us all the information about a wh…

2H3PO4_Aq_ + 3CA(OH)2 --------> 6H20_liq_ + Ca3(PO4)2_Solid_ complete ionic: 2H3PO4 + 3Ca + 6OH---->6H20+ Ca3(PO4)2 Why doesn't phospohoric acid break down. I understand that it is a strong acid, but could someone give me a better explanation than that?

hey everyone, I was reading the inorganic book today and i have got a question. say we have an amine-borane adduct lets take (CH3)3CH2N:BH3, can it undergo redox or acid-base reactions? I mean the adduct doesnt act as a base because the empty 2p orbital on B is filled when Nitrogen in (CH3)3CNH2 datively forms a bond with BH3 so I am thinking that it cant have undergo any acid-base reaction. Can anyone tell me if I am thinking rightly here. I will be grateful for any direction.

It is a question arose while I was dealing with MO of sulfuric acid manually. I adopted the ligand orbital approach, that is, to interact the four oxygen 'ligand' first. I interact the four s- ligand orbitals of the four oxygen, and get four MO (don't know if the word MO is appropriate or not, as it has not yet been a molecule) that would form four sigma bonds with sulfur atom. I followed the coordinate of 'xy coordinate on this plane (so the axis out from the computer screen is the z axis)'. Then I interact the four pz orbitals to form one orbital (a), two orbitals and one orbital (a*) which is the anti-bonding orbital for (a). Besides there are 8 non-bonding orbitals (N…

i know this must be a dumb question, but can metal exist in the gas state? if not then what forces exist that restrict metals from being a gas, i would think it would be the electro-magnetic weak force or universal gravitation.

How many mol of NaHCO3 are needed to completely neutralize 1 mol of H2SO4? answer is 2 mol but why? How many mol of Na2CO3 are needed to completely neutralize 1 mol of H2SO4? answer is 1 mol Na2CO3 (accepts 2 H+) These are notes I wrote in class but i'm not understanding what the question is or why this happens.

Which of the follwoing is not a property of water? A) Water readily dissolves many ionic salts. B) Water boils at 100 degrees celcius. C) Water has a relatively high surface tension. D) Water is colourless and odourless.

Over the last few days, I had an AP (armour-piercing) bullet in a ferric chloride etchant bath to remove the copper jacket. Which it did, but to my surprise some of the underlying penetrator was attacked as well. AFAIK, these are hardened steel, so I wouldn't have expected the iron(III) chloride to have affected it. Was my expectation incorrect? Will ferric chloride attack iron and steel items as well? Thanks! Merged post follows: Consecutive posts mergedWas this a stupid question?

What Chemical(s) In "NEGATIVE-X" Makes It Ignite On Contact With Water And Can You Change The Zinc With Sulfur.

Today I burned an alloy of magnesium and zinc I had made, and to my surprise, little blobs of oxide grew on it as it burned, and started floating away in the wind. It burned much less violently than pure magnesium metal, just glowing bright red-orange and making the blobs (opposed to making the standard powder and wispy fumes seen when burning pure magnesium). I saved some of the white oxide material, and when I look at it, it shows slightly bluish through the white, just like aerogel does. When I held it up so that it was illuminated by the ceiling light from behind, it appeared to glow orange. It is very light, and has such a weak structure that it can be compressed by …

I was synthesizing magnesium nitride in a small clay crucible. I lit a small chunk of magnesium with a blowtorch (causing it to have a lot of carbon on it as it reduced the carbon in the carbon dioxide from the blowtorch flame). After it was burning bright, I dropped it into the crucible and put the lid on. The limited oxygen supply inside the crucible is supposed to cause the magnesium to start burning in the nitrogen, creating magnesium nitride. After a while, thinking the magnesium was spent, I took the lid off the crucible only to hear a pop and have a fireball spit out of it. This indicates that it may have been filled with a flammable gas which could not ignite with…

In this Astronomy Now article, "Should Mars really be black?", scientists claim to have produced red hematite from black magnetite without the presence of water through a purely mechanical process. http://www.astronomynow.com/news/n0909/18mars/ “Subsequent analysis of the flask material and dust has shown that the magnetite was transformed into the red mineral hematite, through a completely mechanical process without the presence of water at any stage of this process.” My question is: Can magnetite Fe3O4 really be transformed into hematite Fe2O3 through a purely mechanical process? Magnetite consists of a mixture of iron(II) and iron(III), and hematite is just…

Hello. I do not get it; can anyone explain on layman terms ? This reaction on a Mg - C cell uses the dissolved oxygen : http://www-odp.tamu.edu/publications/191_IR/chap_03/c3_5.htm From the galvanic series table Mg and C are at the extremes (I assume to yield maximum potential difference): http://www.corrosion-doctors.org/Definitions/galvanic-series.htm ---> Why are the most abundant Cl and Na ions not considered better to be used for the reaction ?

Does anyone know an easy way to make cristal grow, by dilution of a chemical compound in a liquid ? And maybe too, if there is a list to which form of the cristal corresponds to which powder ?

I have a new post that I could use some help with. I need to determine whether I have potassium hydroxide or sodium hydroxide. (I have a 50lb barrel of half-round pellets that is not labeled that was left by the previous chemist...) It is used for degrease and/or paint stripping... Is there a simple reaction experiment the can determine the chemical?

OK so today I tried a new demo and i'm very excited. Before I start I should remind everyone that this cannot be attempted outside of a proper chemistry laboratory. Bromine is extremely hazardous and hard to safely dispose of and handle and the same is true of potassium. Anyway, what I did was this: I took a long piece of metal (steel, i think), and bent the end downwards by 90°, so that the end part was just long enough to reach the bottom of a large beaker. To the end I attached a piece of copper wire. Into the large beaker I placed a small beaker with enough bromine in it to cover the bottom. To the top of the bent part of the metal stick I attached a D…

Hello, I have currently, after doing a variety of theoretical work have begun to venture into the world of the chemical, only to find my first impediment. Obtaining chemicals. To my dissappointment, canada, seems not to be a principal nation in the amateur chemistry department, and as such am at a loss to obtain various key chemicals. My primary concern, as of now, is the obtaining of strong acid or base, such as hydrochloric acid, sulfuric acid, sodium hydroxide, etc. I have currently been able to attain magnesium, copper, iron, iron (III) oxide, Copper sulfate, Calcium Hydroxide, ammonium chloride, potassium hexacyanoferrate, sodium hydrogen sulfate, ammonium iron (III)…

What is the difference between VB theory and Molecular orbital theory? Tutorials on valence bond theory state that the orbitals of the individual atoms overlap when a bond forms. Doesn't that also form a molecular orbital? if so what is molecular orbital theory?

what other type of thermites are there except the iron oxide and aluminium one and what ratio are they mixed in