B + 3O-(-3)=0
B-6+3=0
B=+3
i hope this helps
The oxidation state of boron in the peroxoborate ion is +3. The peroxoborate ion has the formula BO3^3-, where the boron atom has three oxygen atoms bound to it in addition to the peroxide group, giving boron an oxidation state of +3.
There are many factors when it comes to Boron. If it were to form an Ion, then it would drop a total of three electrons.
+3 oxygen is always -2 and the complex total oxidation=0 -6+(3*2)=0
There are two Iron chlorides. Iron(II) chloride, in which iron is in +2 oxidation state, and Iron(III) chloride, in which iron is in +3 oxidation state.
The oxidation state of phosphate (PO4) is -3. This is because oxygen (O) typically has an oxidation state of -2, so there are 4 oxygen atoms in the phosphate molecule, contributing to a total charge of -8. This leaves the phosphorus atom with an oxidation state of +5 to balance the overall charge to -3.
The oxidation state of Boron in BO3^-3 is +3. This is because the overall charge of the ion is -3, and each oxygen atom has an oxidation state of -2. Hence, the Boron atom must have an oxidation state of +3 to balance the charges.
The oxidation state of boron in the peroxoborate ion is +3. The peroxoborate ion has the formula BO3^3-, where the boron atom has three oxygen atoms bound to it in addition to the peroxide group, giving boron an oxidation state of +3.
The oxidation state of boron in Na2B4O7 is +3. This is because boron typically exhibits an oxidation state of +3 in its compounds due to its electron configuration and bonding characteristics.
+3
The oxidation state of boron is either three electrons or one electron. Boron has an valence electron configuration of ns2np1.
The oxidation state of boron in B2O3 is +3. Boron typically forms compounds where it has a formal oxidation state of +3 due to its electron configuration and tendency to acquire three additional electrons to achieve a stable octet.
The 3+ oxidation state of boron is not stable because boron has a small atomic size and high electronegativity, making it difficult to lose three electrons. In the 3+ state, boron often acts as a Lewis acid by accepting a pair of electrons to achieve a stable electron configuration.
The oxidation state of boron in B4C is +3. Each boron atom in B4C contributes 3 electrons to form B4C, while the carbon atoms each contribute 4 electrons.
The oxidation state of boron (B) in B2Cl4 is +3, as each boron atom contributes three valence electrons. The chlorine (Cl) atoms have an oxidation state of -1 each.
Boron (B, atom number 5, the 1ST member of group 13) has an oxidation state of +3, it is rather a metaloid, even more than Al (2nd member), so it forms an acidic oxide B2O3.
Oxiborate is the ion with the chemical formula (BO3)3-. A compound without oxygen is the boron hydride, BH3.
The oxidation number for boron is typically +3. Boron is an element that tends to lose three electrons when forming compounds.