c. Answer (g) :- Fe2(SO3)3 species contain SO3(2-) ion. S + - 6 = -2 . Oxygen has an oxidation number of 2-. Favorite Answer. 2 Answers. So, in SO3, in order to create a net neutral, or zero charge, the S must have an oxidation number 6+ to cancel out the 3*(-2)= -6 of the oxygen in the compound. S = 4 The oxid'n number of sulphur. Explanation: let oxidation number of S be x. oxidation number of O is -2 . Then there are 3 oxygens hence 3 x -2 = -6 . However in SO3^2- (aq) the Oxidation states are: Sulfur (+4) & Oxygen (-2). The sum of the oxidation numbers of all of the atoms in a neutral compound is zero. (Recall that O has an oxidation number of -2.) The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion. That would be the oxidation number. S = -2 + 6 . hydrogen. PLEASE HELp In the redox conversion of SO3 to SO−, S is ? Add . S is reduced and its oxidation number goes from 6+ … Electrons are transferred. + indicates +1 charge, sum of charges of compounds always equals zero. Because the sulfite ion (SO3) has a -2 charge (and you'd have to consult a list of polyatomic ions to know that) and the zinc ion MUST be +2 in order to balance that out. Consider the following reaction. Since the zinc ion's charge is +2, so is its oxidation number (rule 2). Lv 7. For HSO3- it is the negative sign, indicating a -1 charge for the bisulfite ion. x= +4 and its oxidation number goes from ? Mg + Cl2 mc005-1.jpg Mg2+ + 2Clmc005-2.jpg. Don't get the two confused, they may both be written with out the charge, but if SO3 is (aq) it has a charge of -2. The oxidation number (ON) of an element details the number of electrons lost or gained by the element in order to achieve its current state. Since the anion has an oerall charge of '-2 ' , then we create a sum . c. Given the reaction below, which is the oxidized substance? Answer Save. Oxidation State of Sulfur + (3 Oxidation state of Oxygen) = -2 Oxidation state of sulfur + (3 (-2 view the full answer Previous question Next question Commonly, sulfur (s) forms 2- oxidation state, but in bisulfite it forms 4+. The sulphite anion is SO3^2- Using '-2' for oxygen as the yardstick . The oxidation number of a Group 17 element in a binary compound is -1. to ? Fluorine in compounds is always assigned an oxidation number of -1. What is the oxidation number for S in the compound SO3? Sum of charges in this case, for these polyatomic ions, equals the charge on the ion. The alkali metals (group I) always have an oxidation number … The easiest way is to remember certain common numbers: O (in most cases): -II, H: +I For oxidation numbers we use Roman numerals! The oxidation number of a free element is always 0. Roger the Mole. Rules for assigning oxidation numbers. The oxidation number for SULFUR is +4, and the oxidation number for oxygen is -2. so, x+3(-2)= -2. x-6=-2. The oxidation number of a monatomic ion equals the charge of the ion. The given compound is, Let the oxidation state of S be, 'x' Hence, the oxidation state of S is, (+4) It can be determined using the following rules: 1. 4 years ago. Hydrogen has an oxidation number of 1+. To answer this question, let's first look at the atoms in the compounds for which we know the oxidation number. Which best identifies why the rusting of an iron nail in the presence of water and oxygen is an oxidation-reduction reaction? Relevance. What is the oxidation number for S in the compound SO3? d. Which identifies an oxidation-reduction reaction? Answer: oxidation number of S in SO3-2 is +4. ... Why? (Recall that O has an oxidation number of -2.) The Oxidation states in in SO3(g) are: Sulfur (+6) & Oxygen (-2), b/c SO3(g) has no charge.