How do you know if a solution consists of anions or cations (positive/negative charge)?
551430
You cannot have one without the other.  If there are cations present, there will be an equally charged pile of anions there with it.  The charge on any system is always neutral (or very close - it may have some electrical potential but relatively speaking, it's very low).
342877
the group 1, 2, and 3 anions are the ions that have a negative charge of 1, 2, or 3.
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.
499916
An ionic compound is dissolved with an appropriate solvent, or otherwise melted by heat, so that its ions are available in the liquid. An electrical current is applied between a pair of inert electrodes immersed in the liquid. The negatively charged electrode is called the cathode, and the positively charged one the anode. Each electrode attracts ions which are of the opposite charge. Therefore, positively charged ions (called cations) move towards the cathode, while negatively charged ions (termed anions) move toward the anode. The energy required to separate the ions, and cause them to gather at the respective electrodes, is provided by an electrical power supply. At the probes, electrons are absorbed or released by the ions, forming a collection of the desired element or compound.
446923
A\n\nAcid changes litmus to red. I am not sure what reacts with bases to produce salts. I am also not sure what becomes negative when exposed to other elements. You should review your chemistry properties.
488144
In chemistry, a salt is any ionic compound composed of positively charged cations and negatively charged anions so that the product is neutral and without a net charge. These ions can be inorganic (Cl−) as well as organic (CH3COO−) and monoatomic (F−) as well as polyatomic ions (SO42−).\n\nSalts are formed when acids and bases react.\n\nSolutions of salts in water are called electrolytes. Electrolytes as well as molten salts conduct electricity.\n\nZwitterions are salts that contain an anionic center and a cationic center in the same molecule; examples include amino acids, many metabolites, peptides and proteins.\n\nMixtures of many different ions in solution like in the cytoplasm of cells, in blood, urine, plant saps and mineral waters usually do not form defined salts after evaporation of the water. Therefore, their salt content is given for the respective ions.
819578
1)  At the centre, you have the nucleus (positively charged) and, around that, there are the electronic orbitals (negatively charged).\n2)  By losing one or more electrons, to produce a cation (positively charged), e.g. Na+, Ca++, Al+++\nOr by gaining one or more electrons, to produce an anion (negatively charged), e.g. Cl-, O--, N---\n3)  An ion.
858790
Ionic compound\n\n The crystal structure of NaCl, a typical ionic compoundIn 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.)\n\nIonic compounds have strong bonds between particles and thus generally have high melting and boiling points. They have good electrical conductivity when molten or in aqueous solution. While ionic inorganic compounds are solids at room temperature and will usually form crystals, organic ionic liquids are increasingly of interest.\n\nIonic compounds also dissolve in polarised liquids, of which water is an example, while they do not dissolve in organic liquids, such as Petrol. This is the opposite of covalent compounds.\n\nWhen an ionic compound is named, the cation is named first and then the anion. When an elemental anion is named, the suffix, -ide, is added to the name of the element. There are two common types of cations: Type I and Type II. Type I cations have only one charge and their name is simply listed when the compound is named. Type II cations have more than one charge and when the ionic compound is named, a Roman numeral is used to denote the charge of the cation. In addition, there are common polyatomic anions which do not have suffixes in their name such as hypochlorite (ClO–).\n\nRetrieved from "http://en.wikipedia.org/wiki/Ionic_compound"
98382
You will not find ions along by themselves, they are paired with other ions, forming ionic compounds.\nSome ionic compounds are soluble, some are.  The ones that are can range in solubility based on the solvent, temperature, and other ions in solution.\n\nFor instance, NaCl is very soluble in water at room temperature, where as under the same conditions, Silver Chloride is considered insoluble.\n\nTherre are actually a set of solubility rules to determine whether an ionic compound is or is not soluble in water based on the ions that make it up.\nhttp://www.csudh.edu/oliver/chemdata/solrules.htm
709959
No, the zinc ion has a positive charge because it is transition metal (+2 charge) but the sulfide ion has a negative charge (-2 charge). If you wanted, there could be a compound of Zinc Sulfide, since zinc is a metal and sulfide is a nonmetal.
1179756
Always remember that salts are formed by ions:\n\nCommon salt-forming cations include:\n\nammonium NH4+ \ncalcium Ca2+ \niron Fe2+ and Fe 3+ \nmagnesium Mg2+ \npotassium K+ \npyridinium C5H5NH+ \nquaternary ammonium NR4+ \nsodium Na+\n\nCommon salt-forming anions (and the name of the parent acids in parentheses) include:\n\nacetate CH3COO− (acetic acid) \ncarbonate CO32− (carbonic acid) \nchloride Cl− (hydrochloric acid) \ncitrate HOC(COO−)(CH2COO−)2 (citric acid) \ncyanide C≡N− (hydrogen cyanide) \nhydroxide OH− (water) \nnitrate NO3− (nitric acid) \nnitrite NO2− (nitrous acid) \noxide O2− (water) \nphosphate PO43− (phosphoric acid) \nsulfate SO42− (sulfuric acid)
811889
No concrete way to work it out. Groups one and two take positive charges equal to their group number (Mg2+, Li1+ etc). Groups 3, 4, 5, 6 and 7 ionise to a negative charge of 8 minus their group number (Cl1-, O2- etc), though 3, 4, and 5 tend to resist ionisation and are much more commonly found bonded covalently. The Transition elements ion charges are virtually impossible to predict without an extensive knowledge of d orbitals etc..
967315
say u are going to perform a test for anion A in some sample. but you know that this test may also have a positive result with other anions B and C. \n\nyou then have to take into consideration that B and C might give you false positives as u test for A. if the background of the sample suggests it may contain B and C then find a way to remove these without affecting A.\n\nthen test for A using your originally proposed method.\n\n\nnow for the example:\nyou are to test for chloride ions. the reagent that comes to mind is aq silver nitrate which will result in white ppt of AgCl. then you realise that a ppt will form with any halide ion such as Br- and I-. you also know that AgBr and AgI solids will dissolve in ammonia while AgCl will not. so you first add ammonia to the sample, then test with silver nitrate. voila, now if a ppt forms, you will know it is AgCl only, and of course the conclusion that Cl- was present.
875639
you look at the charge of the overall equation.  if As2O3 has a charge of 0 then you know that As has a charge of +3.  If the charge is say -2 than As has a charge of +2.
279857
I have no idea what you are asking, would you like to rephrase the question?\n\nNitrate is an ion....a poly atomic ion with chemical formula NO3 with a super script -1, indicating it has a negative 1 charge over the entire ion.  Nitrate is an anion, meaning it has a negative charge, it will combine with cations (+) to form ionic compounds.\nCations and anions combine so form an overall neutral compound.\n\nFor example, in the case that Nitrate combines with a Potassium Ion to make Potassium Nitrate, the formula is,\nK+ + NO3- --> KNO3\nSince Potassium has a +1 charge, only 1 Nitrate is needed to make an overall neutral compound, however, in the case of a Calcium ion combining with Nitrate,\nCa+2 + NO3- --? Ca(NO3)2\n2 Nitrates are needed to balance the +2 charge on Calcium.
955815
In this compound (potassium chlorate),  the net charge is zero. The potassium ion has a charge of +1, and the chlorate ion (ClO3-) has a charge of -1.\nSo, the total negative charge is -1.
217978
Barium +2 is a positive ion.  It belongs to the alkaline earth metals group together with Beryllium, Magnesium, Cesium and Francium.