splitting of ionic compounds into ions?
139481
What I think you want is how do you split ionic compounds into ions.  Solutions!\n\nWhen you have an ionic compound, like salt (NaCl) you can split the compound into its ions by dissolving it in water.\n\n     (H2O)\nNaCl(s) ----->  Na+(aq) + Cl-(aq)\n\nThe (s) means solid, cause salt is a solid.  When you put it in water, it changes from (s) to (aq) which means aqueous.  Aqueos basically means that the substance is an ion in a water solution.\n\nHope this helps.
960373
In chemistry, an ionic compound is a chemical compound in which ions are held together in a lattice structure by ionic bonds. The positively charged ion is usually a metal ion and the negatively charged ion is non-metallic element or molecule.\n\nIons can be single atoms, as in common table salt sodium chloride, or more complex groups such as calcium carbonate. But to be considered ions, they must carry a positive or negative charge.\n\nThus, in an ionic bond, one 'bonder' must have a positive charge and the other a negative one. By sticking to each other, they resolve, or partially resolve, their separate charge imbalances. Positive to positive and negative to negative ionic bonds do not occur. (For a real world analogy, experiment with a pair of bar magnets.)
1139103
There is a LIST of them in the link below:\nhttp://www.alltheinternet.com/texis/open/all?q=lewis+structure+of+ions
218524
In Ionic bond, elements looses or gains electron(s) and become ions and the electrostatic potential of these ions bind them\n\nIn covalent, the participating elements are bound by sharing electrons between them.
883690
The compounds have a high lattice enthalpy, thus much energy is required to break to ions up in solution. The also have very low solubility products, that is the product of the compounds ions in a saturated solution.
65580
1) covalent\n2) ionic
835169
molecules are turned into ions....by an electron beam...\nions are separated according to their mass...by a magnet, deflection....\n\nmass spectroscopy can be used to study or analyse mixture of compounds....
764101
In all reactions one uses that 2 OH -> H2O + O, the split of oxygen goes to create the ion. Finally balance the equation:\n \nSO3 + 2 NaOH -> Na2SO4 + H2O\n\nCO2 + 2 KOH -> K2CO3 + H2O \n\nSO2 + Ba(OH)2 -> BaSO3 + H2O
742326
positive ions (a positively charged element in this case since you specified 'atoms')  To be compounds, different types of atoms must combine.
386269
-molecular:it is a double replacement reaction.  i.e.:ab+cd=ad+bc.  \n-net ionic: you find the one that becomes the solid, and you remove all the other spectator ions.\n\nno way, i have to do the same exact thing for homework tonight.  writing net ionic, gross ionic, and molecular formulas. damn.  are you doing molarity too?  are you a sophomore?  damn science.  i hate science.
874983
1. Molarity = concentration and it expressed as mol per dm^3\n    Change the mass to mole and the 851 ml to dm^3. Then find   \n    the ratio of the number of moles to volume in dm^3\n\n2. Soluble ionic compounds breaks up the water molecules in H^+ ions and OH^- ions. Sodium carbonate give Na^+ ions and CO3^2- ions......Other ions that are present are HCO3^- ions called hydrogen carbonate ions. I have found that a solution of sodium carbonate is alkaline: implying that there are more OH^- ions to H^+ ions, due to the formation of HCO^- ions.\n3. OH^- (aq) + H^+(aq) ----> H2O (l)\n4. H^+ ions (ie. hydrogen ions), OH^- ions (ie. hydroxyl ions),\n   Ca^2+ calcium ions and Cl^- chloride ions\n5. Hydrogen ions, hydroxyl ions. ammonium ions and sulphate ions.\n6. Actually the calcium metal reacts with water to give hydrogen gas and calcium hydroxide. At the same time, calcium reacts with nitric acid to give calcium nitrate, water and brown nitrogen dioxide gas.\nHence there is no simple ionic equation for your question\nYou may want to consider this one:\nCa^0  +  2H^+   + 2OH^-  -----> H2(g)  + Ca^2+  + 2OH^-\n7. Hydrogen ions, hydroxyl ions, iron (III) ions Fe^3+  and sulphate ion SO4^2-
706819
this is double replacement, group a cation wit ha different anion. Then, using solubility rules, find the precipitate, this is your solid. Write the rest as ions.
968063
Substances in a mixture just need to be separated, which might happen naturally over time, or could be done by filtration, distillation or a centrifuge (which spins fast to take heavier items out of the mixture).  \n\nElements in a compound are chemically bonded, so you have to reverse the bonding process, which is different depending on the elements in the compound.  If it is a salt, it is as simple as adding water and using electricity to pull the ions you want out.  Once you do, those ions are not all going to be elements--further manipulation will be needed.  Other chemicals are much more complicated though.
783799
wait a minute.....i know this one.........calcium doesn't have multiple ionic charges so there's only Calcium (I) or just plain calcium.\nCaCl \nUnlike iron and copper and others calcium only has one ionic charge\n\nYou don't use prefixes with ionic compounds, however you do\n with molecular compunds\nGO COWBOYS!!!!!!!!!!!!!!!!! in your face indy 9-1
382235
Ionic precipitation is when two ions say Ba+2 and a S-2 get together and precipitate into BaS2 (ppt) which in insoluble. Which is different if two organic molecules react to form an insoluble substance.
1028869
For some values of difficult to test.\n\nTypically, inorganic compounds are ionic in nature, so you're more likely to get chlori*d*e than chlorine (you do appreciate the difference, right?) so you can do things like addition of silver nitrate to get a ppt.\n\nHowever, you can also run mass specs and things - chlorine has a typical splitting pattern here based on isotopic ratios and so in this instance it's probably just as easy to detect it in organic (if not more so) than in inorganic compounds
424592
H2SO4 + 2NaOH ----> 2H2O + Na2SO4\n\nYOU MUST SEPARATE AND CANCEL THE COMMON IONS (AQUEOUS ONES)