Oxidation Numbers

The oxidation number of the IF4+ ion is +5, because iodine typically has an oxidation number of -1 in compounds and there are 4 fluorine atoms with an oxidation number of -1 each.

The formal charge of the IF4+ ion is 0, because iodine has 7 valence electrons and each fluorine contributes 1 electron to the bonding, resulting in a total of 10 electrons (4 from fluorine atoms and 6 from iodine).

It is customary to assign oxygen an oxidation number of -2, except in peroxides and superoxides. Using this convention, phosphorus must have an oxidation number of +3 to balance the charges in P4O6. (6 X 2 = 4 X 3)

The oxidation number of sodium (Na) is +1 since it is an alkali metal. The oxidation number of oxygen is typically -2. Since the compound NaIO3 is neutral overall, the oxidation numbers must add up to zero. Therefore, the oxidation number of iodine in NaIO3 is +5.

If an element gains electrons, it has a negative oxidation number. The oxidation number is determined based on the number of electrons gained or lost by an atom in a compound. The rule is that in ionic compounds, the oxidation number of an element is equal to the charge it would have if it were an ion.

In AlOH^1-, oxygen typically has an oxidation number of -2. Since the overall charge of AlOH^1- is -1, the oxidation number of Al can be calculated as follows: (oxidation number of Al) + (oxidation number of O) + (oxidation number of H) = -1. Solving for Al gives an oxidation number of +3.

The most likely elements are iron, ruthenium, osmium, chromium, cobalt, nickel, molybdenum

The oxidation number of chromium (Cr) in Cr2O7^2- is +6. This can be determined by assigning oxygen an oxidation number of -2 and setting up an equation based on the overall charge of the ion.

The oxidation number of iodide is -1. Iodine is in Group 17 of the periodic table, commonly known as the halogens, which typically have an oxidation number of -1 when in ionic compounds.

The oxidation number of P in P2O5 is +5. This is because oxygen typically has an oxidation number of -2, and there are 5 oxygen atoms in P2O5. The sum of the oxidation numbers in a neutral compound must equal zero, so the oxidation number of P is calculated as +5.

The oxidation number of chlorine in ClO4 is +7. Each oxygen atom has an oxidation number of -2 and the overall charge of the ion is -1, which means the oxidation number of chlorine must be +7 to balance the charge.

In NaMoO3, sodium (Na) has an oxidation number of +1, oxygen (O) has an oxidation number of -2, and the overall charge of the compound is 0. Since there is only one Mo atom in the compound, the oxidation number of molybdenum (Mo) can be calculated to be +6 using the formula: (+1) + x + 3(-2) = 0 where x is the oxidation number of Mo.

To establish oxidation numbers, follow these rules:

1. In a compound, the most electronegative element typically has a negative oxidation number (except in compounds with themselves).
2. The sum of all oxidation numbers in a neutral compound is zero, and in a polyatomic ion, it equals the charge of the ion.
3. Fluorine always has an oxidation number of -1 in compounds.
4. Hydrogen usually has an oxidation number of +1, and oxygen is usually -2.

The oxidation number for Pb in PbO2 is +4. Oxygen in compounds is typically -2, so with two oxygens, the total oxidation number contributed by oxygen is -4. This means that the oxidation number of Pb must be +4 to balance the charges.

1. Iron: Iron can oxidize in the presence of oxygen to form iron oxide (rust).
2. Hydrogen: Hydrogen gas can undergo oxidation reactions to form water when combined with oxygen.
3. Copper: Copper can undergo oxidation reactions to form copper oxide.
4. Ethanol: Ethanol can undergo oxidation reactions to produce acetic acid.
5. Sulfur: Sulfur can undergo oxidation reactions to form sulfur dioxide or sulfur trioxide.

+1 for hydrogen

-1 for fluorine

It never has -2 oxidation number.

Nitrogen oxidation numbers are possible: -3 (nitrides), 0 (elemental), +3 (nitrites), +5 (nitrates).

Also +1, +2 and maybe +4 are possible (in Nitro-oxides only).

Chlorine, bromine, and iodine can have both 1+ and 1- oxidation states.

They most often occur in the 1- oxidation state, often in tho form , especially as the ions Cl-, Br-, and I- but can also achieve as 1+ oxidation state, particularly in the oxyanions ClO-, BrO-, IO- and the corresponding acids.

In TiCl4, the oxidation number of titanium (Ti) is +4 since each chlorine atom (Cl) has an oxidation number of -1. Overall, the sum of the oxidation numbers in TiCl4 equals zero, indicating a neutral compound.

The oxidation number is the same as the charge that the atom has. If the atom usually loses an electron, then it is losing a negative charge and having more positive making it a + 1. If the atom loses two electrons, then the oxidation number would be +2. The same thing with gaining electrons, then there would be more negative charges then positive. If the atom gains one electron, then the oxidation number would be - 1. If the atom gains two electrons, then the oxidation number would be - 2.

I hope that this was helpful.

If the question is Ga2, then it is equivalent to Ga and the oxidation number for any element is zero.
If the question is Ga2+, then the oxidation number is +2.

A pure element consists of atoms that are electrically neutral, with an equal number of protons and electrons. Since the oxidation number reflects the charge an atom would have in a compound, a pure element is considered to have an oxidation number of 0 because there is no exchange or sharing of electrons with other atoms.

The oxidation number of rhodium in a coordination compound can vary, but it is commonly found in the +2 or +3 oxidation state. The coordination number of rhodium in a coordination compound is typically 6, as it can coordinate with up to six ligands.

The oxidation number for oxygen in most compounds is -2.

The oxidation number of carbonate ion (CO3) is -2. Each oxygen atom has an oxidation number of -2, and the sum of the oxidation numbers in the ion must equal the charge of the ion, which is -2.