The correct formula for Chromium (II) Carbide is Cr2C.
This is because Carbon (or Carbide) has a negative 4 charge because it wants to gain four electrons to have it's valence electrons to equal 8. So if it gains four electrons, and electrons are negatively charged, then it has a negative four charge. Chromium has a positive two charge because it has the roman numeral II next to it. Chromium is a metal and all metals are positively charged when they become ions, so it has a positive two charge. In order to be a stable compound, the charges must cancel each other out. So in order for that to happen, you must have two Chromium atoms, to make a positive four charge in total, and one Carbon, to make a total of negative four. And since positive four and negative four cancel each other out, then the formula is Cr2C (two Chromium and one Carbon atom).
Formula: CrN2
the chemical formula for chromim(II) fluoride is CrF2
Chromium(II) Iodide
Iron (II) Carbonate
CrNO3 ************2nd Opinion*********** To get the correct formula, you need to state the oxidation number of chromium in the compound, using a Roman numeral. It's likely to be chromium(III) nitrate, which is Cr(NO3)3
Chromium has four oxidation states: 2, 3, 4, and 6.Iodine has one, and it's -1.There will be a iodide for each oxidation state of chromium.CrI2 Chromium (II) iodideCrI3 Chromium (III) iodideCrI4 Chromium (IV) iodideCrI6 Chromium (VI) iodide
the chemical formula for chromim(II) fluoride is CrF2
Cr2O3 is the chemical formula for chromium (III) oxide
Chromium (II) chloride = CrCl2Chromium (III) chloride = CrCl3 Chromium (IV) chloride = CrCl4
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(II) Iodide
Chromium (II) Carbonate. Although I'm not sure Chromium (II) can form, there might be an overall charge on your formula there...
Iron (II) Carbonate
An example is the chromium chloride: CrCl2.
CrO is the formula for chromium(II) oxide. Cr is the elemental symbol for chrome, and O represents oxygen. The molecular weight of CrO is 68.00 grams/per mole using two significant figures. Variants of CrO include II, III and VI.
Chromium(II) nitrate: Cr(NO3)2Chromium(III) nitrate: Cr(NO3)3
CrNO3 ************2nd Opinion*********** To get the correct formula, you need to state the oxidation number of chromium in the compound, using a Roman numeral. It's likely to be chromium(III) nitrate, which is Cr(NO3)3
Chromium has four oxidation states: 2, 3, 4, and 6.Iodine has one, and it's -1.There will be a iodide for each oxidation state of chromium.CrI2 Chromium (II) iodideCrI3 Chromium (III) iodideCrI4 Chromium (IV) iodideCrI6 Chromium (VI) iodide