budullewraagh

KClO3+sugar isnt good to start with a hammer. it isnt as likely to start reacting as if you use a drop of sulfuric acid. in fact, it's best to add a drop of H2SO4, creating very unstable chloric acid, which oxidizes the sugar. that way you can, you know, get out of there before you have moles of CO2 in your lungs

From: http://www.foxnews.com/printer_friendly_story/0,3566,159348,00.html now why on earth would 20 people not be proud to sign their respective names on a piece of paper condemning lynching in this land of the free? what is so frightening is that these 20 people decided that supporting such legislation was very likely a bad choice, as it would lose them support more than it would gain them support. i, for one, am disgusted. discuss as you wish

with wood? friction? sparks? bam

whats up with kids and potassium nitrate? don't they know that chlorates are significantly more fun?

carbocations can be prepared in a laboratory, but in order to remain stable over a span of time, require the presence of superacids (HSbF6, H2FSO3, etc)

no, i honestly don't know the enthalpy of formation. it won't be easy to find anything on this. it's unlikely that you will find much information on cesium auride. so...make some and test it

yes, in the overall reaction, there is an extra hydrogen atom in the product. in the product, the carbon on the left should be bonded to two hydrogen. the third joins the hydroxyl radical

yes.

KNO3 will react with bases that have more active cations. thing is, the only one is LiOH...unless the reduction potential of Rb+ is slightly more negative than -2.924. im sure fused KNO3 will react with ethanol and zinc. just won't at room temperature

nope. it's a methyl group singly bonded to a carbon. 3+1=4

there is absolutely no comparison. flash powder is exponentially faster than gunpowder. gunpowder is exponentially faster than any thermite

any radioactivity is negligible in a bismuth crystal

"Just plain aqueous. No fusing at all..." thats very, very surprising. Fe(OH)3 is almost completely insoluble in water and i've NEVER seen KOH used as an oxidizing agent in any state except fused

i searched online and found almost nothing of the iridium anion. it seems to be incredibly rare and generally unheard of. the concept of reducing iridium in such a way is too intriguing to just overlook, but i'm coming up with nothing. i'll check out harvard libraries in two weeks and i'll ask my associates.

heavy water is deuterium oxide

flash powder reacts FAR more rapidly than thermite. use a strip of magnesium as a fuse; ignite it, run away, and then watch the reaction

the iron is oxidized to +3 and is the hydroxide. ferric hydroxide is completely insoluble in water.

the idea iwth collecting hydrogen isn't particularly practical, as there will be other gases mixed with the hydrogen when it is collected. try a titration.

oh they look the same. AHAHAAHAHAH. but organic is soooo weird like that. these are enantiomers. while they appear to be the same, they are different. they rotate plane polarized light in opposite directions. it should be noted that they rotate light in equal amounts. in a given solution, if you have equal parts of an isomer that is optically active and its isomer, the solution is considered "racemic" and will not rotate the light. if you have unequal parts of chiral enantiomers of a compound, the solution is "scalemic."

that was a typographical error; forgot to add in the fact that it is an anionic complex. changed to: "Ir-1: [ir(CO)3(PPh3)]-" btw, the complex with Ir in the +1 state is called Vaska's Complex, formed from an iridium salt (usually IrCl3 hydrates or H2IrCl6) and triphenylphosphine, dimethylforamide and aniline under nitrogen. a quote from wikipedia: "Vaska's complex, with 16 valence electrons, is therefore unsaturated and can bind to one two-electron or two-electron ligand before it becomes electronically saturated. Vaska's complex is most famous because it undergoes oxidative addition. The iridium in Vaska's complex has an assigned oxidation state of Ir(I). During oxidative addition the Ir(I) center inserts into the σ-bond of the reactant. In this process, the oxidation state of the iridium increases to Ir(III). The four-coordinated square planar arrangement in the starting complex converts to an octahedral, six-coordinate product. Vaska's complex undergoes oxidative addition with conventional oxidants such as halogens, strong acids such as HCl, and other molecules known to react as electrophiles, such as CH3I. An interesting characteristic of Vaska's complex is that it binds O2 reversibly. IrCl(CO)[P(C6H5)3]2 + O2 <—> IrCl(CO)[P(C6H5)3]2O2. This reaction is simply carried out by bubbling O2 through a solution of Vaska's complex in toluene."

woelen, on your site the reaction: 2Fe(OH)3 + 3ClO– + 4OH– → 2FeO42- + 3Cl– + 5H2O is a bit unclear to me. surely the hydroxide must be fused, not aqueous, right?

i was looking through a book on the elements today when i came across iridium. interestingly enough, it mentioned the Ir- oxidation state, as well as the Ir+, which, apparently, are very rare. In addition, it mentioned a clathrate where iridium is at a neutral state. Ir-1: [ir(CO)3(PPh3)]- Ir(O): [ir4(CO)12] Ir+1: [ir(CO)Cl(PPh3)2] has anyone ever tried making any these? is anyone familiar with any of these? the concept of reducing elemental iridium to an anion is most intriguing.

"oxidation is the loss of electrons. reduction is the gain of electrons." <--what you'll hear in high school chem. that is true, although it's not exclusive for electrostatic ionic bonds. it works for polar covalent bonds as well. consider LiF; the Li is at +1 and the F is at -1. The lithium cation has an electron configuration equivalent to that of helium and fluoride anion has an electron configuration equivalent to that of neon. now consider ClO4-. the O all needs to "reduce" to "-2" (even though the Cl-O bond is polar covalent and far from "ionic.") 2*4=8. ClO4- is -7, so Cl must be at +7. in other news, i knew NaOCl was a powerful oxidizer and that the anhydrous form is very explosive, but i never knew it could oxidize iron to form ferrates. i've heard of the fused KOH+KNO3+Fe and BaO2+Fe2O3, and the electrolytic methods, but recently i've been impressed by the oxidizing abilities of NaOCl. interesting, that

really toxic and carcinogenic. good idea though; sounds like an interesting compound. i'm half tempted to make some, but the gas is so dense and such a strong oxidizing agent that any inhalation would probably prove fatal

hardly, but whatev. if you really want to, you can, and it's not particularly expensive