It can be determined using the following rules: 1. to ? 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. Since the zinc ion's charge is +2, so is its oxidation number (rule 2). Oxidation State of Sulfur + (3 Oxidation state of Oxygen) = -2 Oxidation state of sulfur + (3 (-2 view the full answer Previous question Next question The alkali metals (group I) always have an oxidation number ⦠The sum of the oxidation numbers of all of the atoms in a neutral compound is zero. Explanation: let oxidation number of S be x. oxidation number of O is -2 . x= +4 Commonly, sulfur (s) forms 2- oxidation state, but in bisulfite it forms 4+. hydrogen. The oxidation number for SULFUR is +4, and the oxidation number for oxygen is -2. Hydrogen has an oxidation number of 1+. Since the anion has an oerall charge of '-2 ' , then we create a sum . What is the oxidation number for S in the compound SO3? c. Given the reaction below, which is the oxidized substance? Which best identifies why the rusting of an iron nail in the presence of water and oxygen is an oxidation-reduction reaction? The given compound is, Let the oxidation state of S be, 'x' Hence, the oxidation state of S is, (+4) 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. The oxidation number of a Group 17 element in a binary compound is -1. However in SO3^2- (aq) the Oxidation states are: Sulfur (+4) & Oxygen (-2). Oxygen has an oxidation number of 2-. The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion. Answer Save. S + - 6 = -2 . 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. Answer: oxidation number of S in SO3-2 is +4. so, x+3(-2)= -2. x-6=-2. Fluorine in compounds is always assigned an oxidation number of -1. Roger the Mole. (Recall that O has an oxidation number of -2.) The oxidation number of a monatomic ion equals the charge of the ion. 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. The sulphite anion is SO3^2- Using '-2' for oxygen as the yardstick . For HSO3- it is the negative sign, indicating a -1 charge for the bisulfite ion. c. What is the oxidation number for S in the compound SO3? Relevance. 4 years ago. S is reduced and its oxidation number goes from 6+ ⦠Lv 7. ... Why? Add . and its oxidation number goes from ? Consider the following reaction. Sum of charges in this case, for these polyatomic ions, equals the charge on the ion. S = -2 + 6 . To answer this question, let's first look at the atoms in the compounds for which we know the oxidation number. Favorite Answer. Electrons are transferred. Answer (g) :- Fe2(SO3)3 species contain SO3(2-) ion. 2 Answers. S = 4 The oxid'n number of sulphur. The Oxidation states in in SO3(g) are: Sulfur (+6) & Oxygen (-2), b/c SO3(g) has no charge. + indicates +1 charge, sum of charges of compounds always equals zero. (Recall that O has an oxidation number of -2.) PLEASE HELp In the redox conversion of SO3 to SOâ, S is ? That would be the 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! d. Which identifies an oxidation-reduction reaction? The oxidation number of a free element is always 0. Mg + Cl2 mc005-1.jpg Mg2+ + 2Clmc005-2.jpg. Then there are 3 oxygens hence 3 x -2 = -6 . Rules for assigning oxidation numbers. Fluorine in compounds is always assigned an oxidation number ⦠What is the oxidized substance of an nail. Ions, equals the charge of '-2 ' for oxygen is -2., for these polyatomic,... 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