akcapr

ummm...... 3212445. i dunno. h2so4 said he found one.

ya there is

oh well with a wood stick, maybe, but still unlikely

theres some infor here: http://www.cs.rochester.edu/users/faculty/nelson/cesium/cesium_compounds.html uve probly already seen tho

kno3 wont just blow up from u grinding it

the oxygen bonded to the hydrogen is negative wehn seperated, its o -2. so it travels to the positive anode, where it is oxidzed?/reduced? to normal O nutral. same for hydrogen except its positive so it goes to the negative cathode. why the gas is reduced.oxidized im not sure, but i belive it has to do with electrons from electrisity fulfilling the charge.

the cl- ion(anion) is attracted to the positive anode, the Na+ ion (cation) goes to the cathode.

ya however thermite can react really fast, but generally flash powder is alot faster.

a positive ion is called a cathode, while a positive electrodes is called the anide.

iron reacts quite slowly with acids, unlike zinc for example wich reacts fast(relitively).

if someone told me that seriously it would have explained like 80% of wat i wanted to know about oxidation. thx

is oxidation state in alot of cases just the ionic charge?

isnt it part of the iron hydroxide?

oh u will, its not an explosion- ull be able to to get away. Like look at my avatar- im lghting that flash powder with the equivalent of a blow torch, and i got away easily and i got it on film and wasnt hurt at all, and flash powder is a bit more violent than thermite, however thermite can fling hot fragments.

yes large ones would help to an extent. but the bigger you make it, the less and less it will help produce gas.

interesting. i may try it in the future. im really interested in producing fruit-smelling compounds. thats out of my reach for the while however.

ah that helps some. but im confused about this quote from woelens site: On heating, the hypochlorite is capable of oxidizing the ferric hydroxide and hydrous manganese (IV) oxide further: 2Fe(OH)3 + 3ClO– + 4OH– → 2FeO42- + 3Cl– + 5H2O 2MnO2 + 3ClO– + 2OH– → MnO4– + 3Cl– + H2O can someone explain why heating causes "further oxidation" (???) and what exactly is happenning there. thx for putting up with my dumbnesseness.

i never said its not reactive or wont btw you can collect the rust that forms and save that for thermite and other things.

copper isnt too reactive so you wont have as much crud coming off that. to "bend: the carbon, (which you cant) take a wire and wrapp it around the bottom of the carbon stick, froming a 90 degree angle. Hot glue all over the copper wire so none of it is exposed. you can then stick the carbon into the mouth of the bottle with the wires still being able to come out and hook up to your power source.

oh those, i make those everyday.....not

try it with magnesium again, or a blowtorch. and if u can get some picture of ur thermite.

the orange "crap" are a mixture of compounds produced when the anode is oxidized. It all depends on your electrodes. if ur using iron (nails, steel, etc.) you have mixture of iron chloride, iron oxide, iron hydroxide, and many more. if you use graphite (carbon) for you electrodes you will not have any residue in your water.

Oxidation sattes, they confuse me. What exactly are they? i was lookin at this part of woelens site V and the manganese and iron oxidation states.. - (http://81.207.88.128/science/chem/exps/bleach/index.html) confused me. could someone explain the oxidation states and how it haopens, and wat the products are. thx

in teresting, ill try that. do u know what the reaction is for the first part?

ya thats why i havent used it much