What would happen if you add water to the alkali metals and alkali earth metals?
813459
Alkaline metals like lithium, sodium and potassium etc in  pure form would float in water is added to them. But that would be only part of the reaction because simultaneously  they are reacting with the water, producing hydrogen bubbles which buoy them up. Potassium producing enough that it bursts into flame normally and sodium sometimes depending on the size of chunk. The remaining alkali metals all have explosive reactions with water.
207266
Alkali metals and alkali earth metals tend to form ionic bonds.  They have a +1 or +2 charge.\n\nThe halogens normally form ionic bonds when "joined" with a IA or IIA metal.\n\nTransition metals normally are ionic.\n\nNow for the trick part:  Carbon and nitrogen generally form covalent bonds.  When joined with other elements, they can produce a neutral molecule (CO, CO2).  But they also form polyatomic ions (C03- (carbonate); NO3- (nitrate) ).  \n\nGeneral rule of thumb - IA, IIA, and VIIA atoms will make ionic bonds.  \n\nHope this helps!
254971
I am assuming you mean by adding a base to water, you mean something along the lines of a floor not a chemical.\n\n The floor would reflect any heat generated by the sun of other heating devices back up through the water thereby working as a secondary heater to the water.
1156112
You will probably have to mix the water with another substance, or use an entirely different substance for it.\n\nThe fusion of a substance can never change - it can only be maintaned. By mixing water with a substance with a better fusion point, it will keep the water frozen for a longer period.
868490
assuming you know basic chemistry:\nall metals are cations, right? that means they have + electrons and will bond with non metals easily to form salts. NaCl for example, sodium being the metal, chlorine being the nonmetal.\n\nwell what happens with metal solids and aloys is this: all those extra "valence" electrons floating around their full largest P full shell (you know, 1s2, 2s2, 3p6 and so on..) create a system of delocalized electrons which allow the metals to bond together. since this free system of electrons exists all around the metals that explains why electrons are able to pass through solid metals so easily. (conductivity). the system also give various metals and alloys the ability to be very strong, or rust proof, etc.
856024
Alkali earths are the elements of group 2.\nAlkali metals are the elements of group 1.\n\nHere are the properties of group 2\nhttp://en.wikipedia.org/wiki/Alkaline_earth_metal\n\nHere are the properties of group 1\nhttp://en.wikipedia.org/wiki/Alkali_metal\n\nYou can compare them.\n\nHere is the water reaction with elements of group 1 (example K)\n\n2K (s) + 2H2O (l) → 2KOH (aq) + H2 (g)\n\nHere is the water reaction with elements of group 2 (example Mg)\n\nMg + 2H2O → Mg(OH)2 + H2\n\nAs you go to the extremes of the table and down the table the reactivity is higher because the electronegativiy is lower so they have a greater tendency to lose the electron and react.
769428
Sodium, Potassium, Barium\n\n As long as the metal is more reactive than magnesium, it will be able to displace magnesium ion.
59648
You'll probably want to know typical values for drinking water and sea water.\n\nNormally, water contains dissolved salts with Na, K, Ca, Mg and depending on quality Fe and Mn as main kations and carbonate (and hydrogen carbonate), chloride, sulfate and to (hopefully) lesser extent nitrate and phosphate ions. There are numerous possibilities to combine these ions into solid salts, making the exercise fairly pointless.\n\nIf your teacher insists, Na and K for all the anions except HCO3(1-) and CO3(2-) which usually are written as Mg and Ca salts.\n\nCommon trace elements/compunds include Al, Si, NO2(1-), Li.\n\nMore or less routinely monitored heavy metal traces include As, Cd, Cr, Co, Cu, Ni, Hg, Pb, Sb, Tl, Zn
713783
The alkali metals and the alkali earth metals are the the first columns appearing the periodic table.  Each of the elements found in these groups has the ability to lose electrons, thus making them cations (they become positively charged by losing a negative charge).\n\nHowever, all elements need to have a complete valence shell, which means that their outermost electron shell must be full.  Any deficiency or excess of electrons in their outermost ring will make the elements either lose the excess electrons or gain more in order to completely fill their outermost electron shell.\n\nHydrogen, which is the first element in the periodic table, has only 1 electron.  If Hydgrogen donates this electron, it becomes known as a proton, usually denoted as H+.  If you are writing out equations, H+ will work fine.  Remember, with only one electron, a Hydrogen atom is only composed of one electron and one proton.  \n\nOther than Hydrogen, almost no element will completely lose all of its electrons.
925364
Definitely not water, as those three metals will burn on contact with water (and potassium will explode.) Liquid CO2 might do, as it would cool the burning material extensively, possibly below the ignition point. The sand (SiO2) would be a smothering agent. I'm not sure about the carbon tet.\n\n5 NOV 06, 1522 hrs, GMT.
728017
This is essentially correct as far as you have gotten.  The answer to the second part of the question is no.  Reduction of a water solution of CaCl2 will result in H2 being produced at the cathode because the reduction potential is much lower than that of the Ca+2 ion.
375562
I assume you mean alkaline earth metals and they are all metals in the second column of the periodic table and include beryllium, magnesium, calcium, strontium, barium, and radium.  They oxidize easily in air so most often pure samples are stored in oil.
30770
Excellent question.  Food for thought for both of us.  Let's see- changing the pH of water could allow for greater or less solubility of minerals.  With more minerals in solution, the rate of evaporation increases while the boiling/freezing point lowers, as intermolecular attraction is decreased.  The opposite would then be true with less minerals in solution.
50562
adding water to potassium already causes it to explode.  you are correct - the reaction releases hydrogen and forms an oxide of potassium, and the considerably exothermic nature of the reaction generates enough heat to ignite the hydrogen gas.  so, mixing water and potassium solid typically causes a big-time explosion - just like mixing water and sodium.\n\nas for the powdered magnesium in there - i suspect that the explosion would scatter it, and it might ignite - the ignition temperature for magnesium metal is 450 C - so you'd probably end up with white-hot burning magnesium shrapnel flying everywhere!\n\nso, if you're ever thinking about making a nasty bomb, sounds like a good way to do it.
778216
the alkali earth metals are Be,Mg,Ca,---etc. there valance electrone is +2\nso there hydroxides are\nBe(OH)2\nMg(OH)2\nCa(OH)2\n---\n--etc
888412
Technically, yes.  You can have the oxygen react with something that is more eager to get in a molecule than carbon is, like any alkali metal such as lithium or sodium or potassium; but that would require very tight laboratory conditions, and measure to ensure the metal would not oxidize in the air.\n\nPlants do that "for a living", they get the carbon out and use it to synthesize sugars, rejecting the oxygen in the atmosphere.  Which approach is best would depend on why you'd want to take the carbon out: to have the pure carbon, or to remove it from the molecule and release pure oxygen.
680279
Technically a process can require the addition or extraction/removal of heat ENERGY.\n\nI cannot off the top of my head recognize a chem formula any longer, but adding oxygen to any system is oxidation and generates its own heat.  Tehcnically even iron rusting generates heat, just a very small amount, since any metal "rusting" is just it oxidizing.  \n\nAs far as the ice cubes, simply the removal of heat will not cause water molecule to become ice crystals,  I apologize, but I forget why.  I remember an experiment I saw and tried.  In a very clean container, pour distilled water. Now cover that container with another container that does not touch the first.  (Like putting a big bowl over a smaller bowl with the distilled water.  The water stays liquid all the way down to around -20 C.  But if you damage the stablility of the bowl by say gently tapping the side, the water will then turn to a solid.\n\nSnow in clouds form when the water molucle has a dust mote or other item to cling to and begin forming the ice crystal which eventually gets heavy enough to possibly fall all the way to the ground.