When nickel combines with flourine to form nickel [3] floride, the charge of the nickel ion is
All of my references list NiF2 as the formula. Therefore, Ni would have a charge of +2.
To determine the charge of the nickel ion in nickel fluoride, we need to consider the oxidation states of both nickel and fluorine.
First, let's look at the chemical formula: nickel [3] fluoride usually written as NiF2. Here, Ni represents nickel, and F represents fluorine.
Since the formula states that there are two fluorine atoms (F2), we know that the total charge of the two fluorine ions combined must be -2 (since each fluorine ion has a charge of -1).
Now, since the overall compound doesn't have any net charge (it is neutral), the positive charge of the nickel ion must balance out the negative charge of the fluorine ions.
Based on the charge of the fluorine ions, we can conclude that the nickel ion (Ni) in nickel fluoride (NiF2) must have a charge of +2. This is because two negatively charged fluoride ions (-1 each) combine with one positively charged nickel ion (+2) to achieve a net charge of zero.
Therefore, the charge of the nickel ion in nickel [3] fluoride is +2.