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# anion cation list

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anion

anion , atom or group of atoms carrying a negative charge. The charge results because there are more electrons than protons in the anion. Anions can be formed from nonmetals by reduction (see oxidation and reduction ) or from neutral acids (see acids and bases ) or polar compounds by ionization. Anionic species include Cl - , SO 4-- , and CH 3 COO - . Highly colored intermediates in organic reactions are often radical anions (anions containing an unpaired electron). Salts are made up of anions and cations . See ion .

cation

cation , atom or group of atoms carrying a positive charge. The charge results because there are more protons than electrons in the cation. Cations can be formed from a metal by oxidation (see oxidation and reduction ), from a neutral base (see acids and bases ) by protonation, or from a polar compound by ionization. Cationic species include Na + , Mg ++ , and NH 4+ . The cations of the transition elements have characteristic colors in water solution. Salts are made up of cations and anions . See ion .

Question:An unknown solution possibly containing alkali metal ions, alkaline earth metal ions, and halide ions gave a violet color when placed in a flame. The solution gave no precipitate when an ammonium carbonate solution was added. Addition of chlorine water, hexane and nitric acid produced two layers with a deep violet color in the upper layer. Identify the cations and anions present in the mixture.

Answers:cations= + NH4^+ anions= - CO3^2- Cl^- NO3^-

Question:I don't recall how to do it. Is there where you use the "criss cross method"? I have a list of over 50 of them and this is the first one on the list, but before I start doing it I want to make sure I do it right. Thanks. SORRY, with anion I-1

Answers:Remember this: The sum of the oxidation numbers of the cations and anions must equal zero Take iron (III) oxide for example. The formula is Fe2O3 The Roman numeral III tells us that Fe is +3 and we know that oxygen is -2 Fe2O3 = Fe Fe O O O +3 +3 +(-2) + (-2) + (-2) = 0 Or you can "crisscross" the oxidation numbers: +3 -2 Fe O +3 -2 Fe2O +3 -2 Fe2O3 The danger in using the "crisscross method" is that sometimes the subscripts will need to be reduced. Consider lead (IV) oxide +4 -2 Pb O Pb2O4 Notice that 2 and 4 are both divisible by 2; therefore reduce PbO2 In your example, it's even easier. Since the cobalt is +3, the anions must add up to -3, so if the anion is -1, then you need three of them. Or you can crisscross. +3 -1 Co X CoX3 =========== Follow up =========== Aluminum iodide = AlI3. Yes it does look odd doesn't it.

Question:Here are your options: sodium chloride, sodium carbonate, sodium sulfate, sodium acetate, sodium chromate, sodium nitrite, sodium iodide, sodium nitrate 1. When sodiumXXX was mixed with 12 M sulfuric acid a slight vinegar smell occured, without gases. SodiumXXX desolved in water. 2. When sodiumXXX was mixed with mercury nitrate, a light yellow color showed up, with a light vinigar smell. 3. When sodiumXXX was mixed with 3M aquenous hydroxide, nothing happend and a light vinegar smell occured. 4. When sodiumXXX was mixed with .1 M barium chlordie, a mirky colored water occured with a strong vinegar smell. 5. When sodiumXXX was mixed with 6 M sodium hydroxide acid, no smell occured. 6. When sodiumXXX was mixed with 6 M ammonium hydroxide, nothing happend. after more 6 M ammonium hydroxide was added, a light vinegar smell occured. 7. When sodiumXXX was put under fire, the sodiumXXX was bright orange. IF YOU ARE CONVINCED THE SOLUTION IS NOT _____, THAN SAY SO. IF YOU THINK THE SOLUTION MIGHT BE ____, THAN SAY SO. IF YOU THINK THE SOLUTION IS PROBABLY ___, THAN SAY SO. BASICALLY, LIST EVERYTHING YOU THINK OF. EVERYTHING WILL HELP

Answers:sodium acetate. Why - because vinegar is ~ 3 - 5% aqueous acetic acid which contains the anion acetate. What gave it away was the vinegar smell with most of the reactions. Also, Acetic acid which is the acid that would be produced from the reaction of sodium acetate and another salt, would be stronger if the acid was more concentrated. Depending on what sodium acetate reacts with, a vinegar smell may not appear (due to no reaction) or it might be slight (due to little reaction).