In this case you have a Salt that comes from a binarius acid (HCl) you have to remember in salts you are always using the oxidation number with H (Cl= -1) so Cr is using 3 :) as you have seen im not a English native speaker... sorry for mistakes :D
The oxidation number of chromium changes from +6 in Na2Cr2O7 to +3 in CrCl3. This represents a reduction in oxidation number by three units.
The correct formula for the ionic compound chromium chloride is CrCl3. This is because chromium (Cr) has a 3+ charge, and chloride (Cl) has a 1- charge, so three chloride ions are needed to balance the charge of one chromium ion.
Chromium undergoes oxidation in the given chemical equation. In this reaction, chromium changes from a +6 oxidation state to a +3 oxidation state, indicating that it has lost electrons and undergone oxidation.
Chromium (III) chloride
(NH3)5Cl3CrIt would be more descriptive to write it like this though [(NH3)5ClCr]2+ 2Cl-
The oxidation number of chromium changes from +6 in Na2Cr2O7 to +3 in CrCl3. This represents a reduction in oxidation number by three units.
The correct formula for the ionic compound chromium chloride is CrCl3. This is because chromium (Cr) has a 3+ charge, and chloride (Cl) has a 1- charge, so three chloride ions are needed to balance the charge of one chromium ion.
Chromium undergoes oxidation in the given chemical equation. In this reaction, chromium changes from a +6 oxidation state to a +3 oxidation state, indicating that it has lost electrons and undergone oxidation.
The correct formula for the ionic compound formed between chromium and chloride is CrCl3. This is because chromium has a 3+ charge and chloride has a 1- charge, so it takes three chloride ions to balance the charge of one chromium ion.
Chromium (III) chloride
CrCl3: A chloride ion has only a single negative charge; therefore, three of them are required to have the same magnitude of electric charge as a chromium (III) ion.
(NH3)5Cl3CrIt would be more descriptive to write it like this though [(NH3)5ClCr]2+ 2Cl-
Because the chromium ion is in its trivalent form.
Under still milder conditions, chromium metal reacts with the halogens fluorine, F2, chlorine, Cl2, bromine, Br2, and iodine, I2, to form the corresponding trihalideschromium(III) fluoride, CrF3, chromium(III) chloride, CrCl3, chromium(III) bromide, CrBr3, or chromium(III) iodide, CrI3.
The lattice energy of CrCl3, which is the energy released when one mole of solid CrCl3 is formed from its constituent ions in the gas phase, is approximately -707 kJ/mol. This value represents the strength of the ionic bonds between chromium and chlorine atoms in the crystal lattice of solid CrCl3.
The charge on CrCl3 is 0, since it is a neutral compound. Each Cl ion has a charge of -1, meaning that three Cl ions combine with one Cr ion with a charge of +3 to form the compound with an overall charge of 0.
There is no compound with the formula CrCI3 (uppercase i). You most likelt mean CrCl3, with a lowercase L. This is chromium III chloride.