Cr2+ is a divalent cation of chromium; ex.: chromium in chromium diiodide, CrI2.
It is a chromium III
Cr^+2 is the symbol for the Chromium(II) ion
Chromium has several valence states, only one of which is Chromium III. States 2, 3, and 6 are most common but 1, 4, and 5 are possible. Total chromium means the amount of chromium in all valence states.
Chromium (iii) Phosphite
it is a chromium 2 as a good point of reference, and if you don't know the specific charge of an atom, check the ion to which it is bound: the phosphide ion is most commonly charged as a 3- ion because its period is has 3 electrons more than it needs to form a complete octet 2 phosphide ions (per your empirical formula) would have a total ionic charge of 6- if you distribute the (6-) charge evenly through the 3 chromium ions in your empirical formula, then each chromium ion would have to have a charge of 2+ in order for the ionic salt to be neutrally charged. therefore the chromium is chromium (II)
It is a chromium III
Chromium has three valences: 2, 3, and 6.
chromium(II) nitrite
Cr^+2 is the symbol for the Chromium(II) ion
CrO2this is the incorrect formula. For Chromium II oxide the formula is actually CrO without the 2. The reason for this is simple. the II after chromium indicates that it has a charge of +2, and the oxygen, we know is in group 16, has a charge of -2. The formula CrO2 is actually the formula for chromium IV oxide>
Chromium has several valence states, only one of which is Chromium III. States 2, 3, and 6 are most common but 1, 4, and 5 are possible. Total chromium means the amount of chromium in all valence states.
Chromium (iii) Phosphite
Chromium has 25 known isotopes, 2 isomers, 3 of which are non-radioactive.
it is a chromium 2 as a good point of reference, and if you don't know the specific charge of an atom, check the ion to which it is bound: the phosphide ion is most commonly charged as a 3- ion because its period is has 3 electrons more than it needs to form a complete octet 2 phosphide ions (per your empirical formula) would have a total ionic charge of 6- if you distribute the (6-) charge evenly through the 3 chromium ions in your empirical formula, then each chromium ion would have to have a charge of 2+ in order for the ionic salt to be neutrally charged. therefore the chromium is chromium (II)
Chromium Phosphide... Cr is the element Chromium and P is the element Phosphorus (It's a binary ionic compound -2 elements- so the second element ends in -ide)
Cr(HCO3)2
The compound is Chromium(III) Oxide. Chromium is 3+, since the compound has to have a charge equal to 0. Since there is 2 chromium atoms each chromium atom must have a charge of 3+ to balance out the 3(2-) charges of each oxygen atom; 2x+3(-2)=0, transpose for x(chromium), (in case you need the working out).