is sodium reactivity?
544737
Sodium in it's metallic form is extremely reactive with water.  Setting out some sodium can cause spontaneous combustion if the humidity is high or its sits long enough in moderate humidity.  Pure sodium is extremely reactive.  Sodium salts (like table salt) are much less reactive than pure sodium.  Their reactivities are dependant on the anion... (carbonates, Chlorine, nitrates...)
389448
Na+ and OH- you are dissolving a salt\n\nby the way, i am getting a phd in chem, so trust me. also, there are tons of answers in there that are totally bullshit.
334010
The only way I've heard of to obtain pure sodium metal is by electrolysis of NaCl.  Basically, place the salt solution between two electrodes (Na+ attracted to anode, Cl- attracted to cathode).\n\nPure Na is extremely reactive, though.  It is very difficult to store, as any exposure to air will cause almost instant oxidation of the surface (formation of Na2O).  There is also very little commercial use for pure Na.  There are many, many commercially viable sodium compounds, but pure sodium is rarely useful.
570619
no this is incorrect\n\nsodium hydroxide will ionise in water to produce sodium+ ions and Hydroyl (-ve) ions\nso\n\nthewater is not truely a reagent in this reaction,  it is simply the solvent\n\nNaOH + H2O -> Na(+)aq + OH(-)aq\n\nthe aq after an ion indicates it is in aqueous solution (ie in water\nions charges should be written in superscript after the ion (ie above and after) - not in brackets
212381
What are you asking about these reactions?
979402
reactant(s)\nSynthetic
899611
Ba(NO3)2 and sodium phosphate\n\n1.  Ba(NO3)2 + Na3PO4 --> NaNO3 + Ba3(PO4)2\n\n2.  Ba(+2) + NO3(-1) + Na(+1) + PO4(-3) --> Na(+1) + NO3(-1) + Ba(+2) + PO4(-3)\n\n3.  No reaction (All spectator ions cancel out)\n\nBa(NO3)2 and sodium carbonate\n\n1.  Ba(NO3)2 + Na2CO3 --> BaCO3 + NaNO3\n\n2.  Ba(+2) + NO3(-1) + Na(+1) + CO3(-2) --> BaCO3 + Na(+1) + NO3(-1)\n\n3.  Forms BaCO3 (Barium Carbonate)\n\n\nBa(NO3)2 and pottasium iodide\n\n1.  Ba(NO3)2 + KI --> BaI2 + KNO3 \n\n2.  Ba(+2) + NO3(-1) + K(+1) + I(-1) --> Ba(+2) + I(-1) + K(+1) + NO3(-1)\n\n3.  No reaction (All spectator ions cancel out)\n\nBa(NO3)2 and sodium sulfate\n\n1.  Ba(NO3)2 + Na2SO4 --> NaNO3 + BaSO4\n\n2.  Ba(+2) + NO3(-1) + Na(+1) + SO4(-2) --> Na(+1) + NO3(-1) + BaSO4\n\n3.  Forms BaSO4 (Barium Sulfate)\n\nHopes this helps you!
813427
The size of the metal would be dependant on many factors such as plane design and location of the explosion to name a few.\n\nthe problem with elemental rare earth metals is they are very reactive with water, making handling them in such a manner virtually impossible.\n\nAs far as the realative reactivity, the ammount of energy released can be calculated from the Gibbs free energy for each reaction.\n\nFor the reaction of sodium with water at room tempreture\n\nSodium with enough water would release 9260 KJ per pound of sodium while Potassium would release 2350 KJ per pound.\n\nI would suspect that at least 10 pounds of sodium to do any significant damage to a plane and 50 pounds of potassium.\n\nThis is a very unreasonable amount, although the cost would be less than 1000 dollars for this ammount of sodium, there are very few places that a large quantity could be obtained.\n\nAdditionally, sodium is so reactive, that I do not think that anyone could ever get it onto a plane before it blew. Lastly, that large of an ammount of sodium would fill a carry on bag, and would never get thru even the worst of TSA screeners.
659372
It does apply loosely to other halides, but Cl and Fl are considerably more reactive.  Br and especially I have more significant steric hindrances to overcome.\n\nSee the link below to see where Markownikoff gort his idea.
238675
If the reactants are in aqueous solution, in high enough concentrations, then solid silver chloride (AgCl) will precipitate. Sodium nitrate wiill remain in solution as sodium and nitrate ions. No chloride ions should remain - they will all have reacted with the silver ions.\n\ni.e.   AgNO3 + NaCl  + NaNO3   ->    AgCl  +   NaNO3\n\nDon't forget to balance the equation.
972593
Flame tests are "OK" when you are dealing with a reasonably pure solution.  If there are more than one cation present, such as sodium and potassium, then the resultant color in the flame will not be so determinant.  Also, if you are color blind flame tests suck.
38065
There are innumerable soluble salts of organic and inorganic compounds. For some soluble salts, there will be no precipitate when sodium hydroxide is added. You can consider sodium acetate as one example of this but there are many many others. \nFor some soluble salts, there will be a precipitate when sodium hydroxide is added to solution. The appearance of the precipitate depends on the nature of the salt. For some soluble salts, such as ammonium hydroxide, the addition of sodium hydroxide will evolve ammonia as a gas. That reaction is part of the classical determination of protein in nutritional laboratories.
240126
Tommy was right as far as Mg & Ca are concerned.  Na is a Group 1 metal and is more reactive than either because it's 3s1 structure is an incomplete atomic orbital, whereas Mg (3s2) and Ca (4s2) have a certain stability from being a complete electron pair.
881903
These elements are too reactive to be found free in nature. Sodium occurs mainly as NaCI (salt) in sea-water and dried-up sea beds. Potassium is more widely distributed in minerals such as sylvite, KCI, but is also extracted from sea-water. The alkali metals are so reactive they cannot be displaced by another element, so are isolated by electrolysis of their molten salts.\n\nEarth Crust Occurrence\n\nLithium 65 ppm\nSodium 2.6%\nPotassium 2.4%\nRubidium 90 ppm\nCesium 7 ppm\nFrancium Artificial\n\nSea Water Occurrance\n\nLithium 0.178 ppm\nSodium 10800 ppm\nPotassium 399 ppm\nRubidium 0.124 ppm\nCesium 2.9x10^-4 ppm\nFrancium Artificial
464975
If you mean NaCl (letter L at the end instead of number one), then, yes, sodium chloride is an ionic compound. In solid form it is NaCl(s), commonly known as table salt.\n\nIn case you're wondering, the formula NaCl is actually considered a "formula unit" rather than a "molecule." In solid form, ionic compounds are 3-D matrices of ions. But when dissolved or solvated in water, the ions become free floating Na+ and Cl- ions rather than individual NaCl units. A formula unit simply shows the lowest whole-number ratio of cations (positively charged ions) to anions (negatively charged ions) given by the formula. Sodium chloride's cation to anion ratio is one sodium cation Na+ per chloride anion Cl-, or 1 to 1.\n\nBy way of contrast, the formula H2O (for water) represents a molecule, because each molecule of water is a distinct unit.
63545
use sodium hydrolic solution
170895
Sodion Hypochlorite and Sodium Thiosulfate?  Ive never heard of Na2(s2o3)2?!  Anyways heres the balanced equation:\n\n2NaOCl + Na2S2O3 ---> Na2S2O3 + 2NaOCl\n\nPretty straight forward I guess.  Double Replacement reaction.