my laptop sucks, otherwise I would have answered to this question.
Use Avogadro's number. 2 mole Fe(3+) ( 6.022 X 10^23/1 mole Fe(3+) ) = 1.20 X 10^24 ions of Fe(3+)
Iron (Fe)
Yes
combination
CuSO4 (aq) + Fe (s) -> FeSO4 (aq) + Cu (s)
Fe 2+ is Ferrous Fe 3+ is Ferric
O does not exist by itself. The balanced equation would be 4Fe + 3O2 --> 2Fe2O3
Use Avogadro's number. 2 mole Fe(3+) ( 6.022 X 10^23/1 mole Fe(3+) ) = 1.20 X 10^24 ions of Fe(3+)
Fe + 3AgNO3 ==> Fe(NO3)3 plus 3Ag The oxidation number of Ag in AgNO3 (on the left side) is 1+ and in Ag (on the right side), it is zero. Thus, in this reaction, silver (Ag) has been reduced.
H3PO4 is added to Mohr's salt (ammonium iron(II) sulfate) to prevent oxidation of Fe²⁺ ions to Fe³⁺ ions during permanganate titrations. This reaction interferes with the accurate determination of oxidizable substances and is minimized by the presence of H3PO4, which stabilizes Fe²⁺ ions.
Cr and Fe have four unpaired electrons in their 2 plus ions.
two elements with ions with a 2 plus charge are Sulfurand Oxygen
When iron is immersed in an acidic solution, it can react with the hydrogen ions from the acid to form ferrous ions (Fe2+). These ferrous ions can then react with hydroxide ions (OH-) in the solution to form iron(II) hydroxide (Fe(OH)2), which is a metallic hydroxide compound.
The oxidation half-reaction for the given equation is: Fe → Fe2+ + 2e-. This represents the loss of electrons from iron (Fe) to form iron ions (Fe2+).
No, it forms positive ions.
There are several simple tests for identifying Iron(II) ions, which can be carried out even in an elementary chemistry laboratory.Add some ammonia solution to the testing solution, if Fe2+ present, there will be a green precipitate; Fe(OH)2.Add some ammonium sulphide to the testing solution, if Fe2+ present, FeS would be observed as a black precipitate.To the given solution, add a few milliliters from a K4[Fe(CN)6] solution, a Prussian blue solution or precipitate indicates that there is Fe2+ present.To the given solution, add a few milliliters from a K3[Fe(CN)6] solution, a white precipitate indicates that there is Fe2+ present. (If the Prussian blue solution or precipitate is observed in this instance, there is Fe3+ present in the solution).To the given solution, add a solution of ammonium thiocyanate. There will be no chemical change in this instance. Now add few drops of concentrated nitric acid and warm the solution. A deep red colour, (actually the colour intensity depends on the quantity of ammonium thiocyanate added) depicts that there is Fe2+ in the solution.The related link below is posted to observe the contrasts between identifying Iron (II) ions and Iron (III) ions.
fe+3=..............* .9 =fe+2