What is the formula for manganese(VI) chloride?

Answer 1

MnCl2

Manganese is two electrons away from becoming a noble gas, in fact it has two too many. Chlorine is one away from becoming a noble gas and needs one electron. So two chlorine atoms would have to come to take (steal) manganese's two electrons.

So

Mn2+ (has two electrons to give) Cl22- (wants to take two electrons)

Answer 2

Previous contributor's answer: Mn3Cl

New answer: Manganese has a +4 charge in this case and chloride has a -1 charge.

Metal -- non-metal, so you criss-cross applesauce to give you MnCl4. However, I don't think this compound is really produced, as the only one I've heard of with this combo is MnCl2 (Manganese II chloride).

Answer 3

Charges of each ion: manganese(III) = Mn3+ chlorine = Cl1- Solution: The charges of each ion deviate to the other ion. In this case, the ionic charge of manganese(III) is a positive three (3+) and becomes the subscript of chlorine and the ionic charge of chlorine is negative one (1-) and becomes the "invisible" subscript of manganese. (Mn1-)(Cl3+) = MnCl3

Answer 4

Mn+5 Cl-1 ---> these are the ions and their charges. You know Mn's charge because of the (V).

Mn+5 Cl-1 Cl-1 Cl-1 Cl-1 Cl-1 -----> the charges have to add up to zero, so four negative Cl ions are added to cancel out the +5 Mn ion (5+ -1 + -1 + -1+ -1+ -1 = 0)

MnCl5 -----> simplify (one Mn ion and five Cl ions)

Although, I'm not sure if Mn and Cl forms a Manganese (V) chloride compound, if it does then the formula is as above. But I do know it forms a Manganese (II) chloride compound.

Answer 5

MnCl2 - make sure the '2' is small, subscript (ie slightly below the line)

Answer 6

Two manganese chlorides are known: MnCl2 and MnCl3.

Manganese(IV) chloride doesn't exist.

Answer 7

MnCl2. This molecular formula was deduced by equalling the oxidation states of both elements.

Answer 8

Very probable this compound doesn't exist.
I suppose that you think to MnCl2 or MnCl3.

Answer 9

Mn(ClO3)2