In any neutral compound, this number must be zero.
The sum of the oxidation numbers of all of the atoms in a polyatomic ion must equal the charge on the polyatomic ion. Example: phoshpate ion, PO4^3- has a negative 3 charge. Oxidation number for P is 5+, and that for each oxygen is 2-. Summing them, you get +5 + (-8) = -3.
In a polyatomic ion, the overall charge is equal to the sum of he oxidation numbers of all atoms. Let's take sulfate as example. There is -8 for oxygen (four atoms with -2) and +6 for central sulfur atom. Their sum is (-8) + (+6) = -2 which is also equal to its overall charge.
Zero.. it always has to be zero otherwise the compound will be unstable
In any neutral compound, this number must be zero.
Zero to maintain charge neutrality
The sum will be 0.
zero
the charge on that ion
the charge on that ion
The oxidation numbers of the elements in a chemical formula, some of which will be positive and others of which will be negative, when multiplied by the numbers of atoms with each oxidation number, must produce products that add to a net result of zero.
-3. The sum of oxidation numbers of the atoms in all polyatomic ion is the net charge - its part of the definition of oxidation number.
the charge on a mono-atomic ion is the same as the oxidation number, for a polyatomic ion the charge is the sum of the oxidation numbers of its constituent elements.
the charge on that ion
the charge on that ion
The oxidation numbers of the elements in a chemical formula, some of which will be positive and others of which will be negative, when multiplied by the numbers of atoms with each oxidation number, must produce products that add to a net result of zero.
-3. The sum of oxidation numbers of the atoms in all polyatomic ion is the net charge - its part of the definition of oxidation number.
the charge on a mono-atomic ion is the same as the oxidation number, for a polyatomic ion the charge is the sum of the oxidation numbers of its constituent elements.
For a neutral molecule it is zero, for polyatomic ions the sum is the same as the ionic charge.
In principle, only by comparing the chemical formula for the compound with the formulas of ions known to be polyatomic to determine whether the sequence of letters and subscript numbers (if any) in any part of the chemical formula corresponds to the sequence of letters and subscript numbers in the formula of a know polyatomic ion.
I assume you mean the oxidation number of Mn in the permanganate ion , MnO4- The sum of the oxidation numbers is the charge on a polyatomic ion so Mn has an oxidation number of +7 as each O is assigned -2.
The oxidation number of phosphorous as an element by itself is 0. The oxidation number of P in a compound or polyatomic ion will depend on the other atoms it is bonded with. A commonly used period table lists -3, +3, and +5 as the most common oxidation numbers for P in compounds.
The known oxidation numbers of chromium are +2, +3, and +6, while the known oxidation numbers of selenium are -2, +4, and +6. Within this constraint, the only oxidation numbers that can match the formula given are -2 for selenium and +2 for chromium.
AlI3 The algebraic sum of the oxidation numbers of the combining atoms must equal zero. The oxidation state of Al3+ is balanced by three ions of iodine (I-).
It can mean that the element has lost 2 electrons to form a pos. 2 ion. Or it can mean that in a particular compound (or polyatomic ion) that atom is combined with more electronegative elements in a particular combination that the rules used to assign oxidation numbers gives this atom a +2 oxidation number.