Three atoms (I, II, and III) are indicated in the molecule shown below. What is the oxidation state of atom I? Enter your answer as an integer number. What is the oxidation state of atom II? Enter your answer as an integer number. What is the oxidation state of atom III? Enter your answer as an integer number.
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- Calculate the increase or decrease in the oxidation state for each element listed as it changes from a reactant to a product. Use a negative sign to show a decrease in oxidation state. sulfur, beginning in the reactant ZnS nitrogen, beginning in the reactant NH, chlorine, beginning in the reactant Cl-Write True if the statement is correct and False if it is wrong. Write your answer on the space provided after each number. 4. Reducing agents undergo reduction reaction. 5. Oxidizing agents undergo oxidation. 6. Free and uncombined elements have zero charges. 7. Oxygen and Hydrogen have varying oxidation states.Part I. Write True if the statement is correct and False if it is wrong. Write your answer on the space provided after each number. Oxidation occurs when a specie gains electron. ________ Reduction occurs when a specie loses electron. ________ Oxidation and reduction reactions occur simultaneously. ________ Reducing agents undergo reduction reaction. ________ Oxidizing agents undergo oxidation. ________ Free and uncombined elements have zero charges. ________ Oxygen and Hydrogen have varying oxidation states. ________ The oxidation number of a neutral compound is equal to zero. ________ Protons are gained and lost during redox reactions. ________ The algebraic sum of the positive and negative oxidation states is always zero. ________
- Whenever a substance is oxidized, some other substance must be reduced. O it is called the oxidizing agent. O it gains electrons. O hydronium ions are produced.Identify whether or not each of the following reactions is a redox reaction. To determine whether or not a reaction is a redox reaction, figure out the oxidation number of each atom. If the oxidation numbers do not change from one side to another, then it is not a redox reaction. Write the oxidation number of each atom above it on both the reactant and product side. Write the oxidation number for only one atom. For example, the oxidation number of each Br in Br2 is zero, so write a zero above Br2. H2O + H2O → H3O+ + OH- Cu + S → CuS 2 NOBr → N2 + O2 + Br2 CH3CH2CH3 + 5 O2 → 3 CO2 + 4 H2O Ca(NO3)2 + Na2SO4 → 2 NaNO3 + CaSO4 Provide a definition for each of the four types of redox reactions. Indicate the type of redox reaction each redox reaction is in the section above. Single Displacement Combustion Synthesis DecompositionAccording to the chemical reaction below. Answer the following questions: 1/402 + 1/6NH,* → 1/6NO2¯ + 1/3H* + 1/6H,O 1. What the oxidation state of N atom is NH4" molecule? 2. What the oxidation state of N atom is NO? molecule? 3. What the oxidation state of O atom is O2 molecule? 4. What the oxidation state of O atom is NO2" molecule? 5. What the oxidation state of H atom is NH* molecule? 6. What the oxidation state of H atom is H2O molecule? 7. What is the substance that reduced? 8. What is the substances that oxidized? 9. What is the reductant in the above reaction? 10. What is the oxidizer in the above reaction?
- In redox reactions, what ALWAYS happens to oxidizing agents? They always get reduced. They always get oxidized. They always reduce another compound.If you add all the oxidation numbers in a polyatomic ion, what should the sum be? A The sum should equal 0. B The sum should equal -1. с The sum should equal -2. D The sum should equal the charge on the ion.E O Home - AP Student.. 6 Elk Grové Unifled Constants | Peniodic Table Oxidation states are important for keeping track of electrons in oxidation-reduction reactions. Here are some general rules to remember: Neutral compounds • Atoms of a free element have an oxidation number of 0. • Monoatomic ions have an oxidation state equal to their charge. Polyatomic ions and neutral molecules have a charge equal to the In a neutral compound, the sum of the oxidation states is zero. Note that the sign of the oxidation states and the number of atoms associated with each oxidation state must be considered. In H2O, for example, each hydrogen atom has an oxidation state of +1 and each oxygen atom has an oxidation state of -2 for a total of 2(+1) + (-2) = 0. %3D charge on the species. • Metals in compounds have positive oxidation states. Group 1A and 2A metals have oxidations states of +1 and +2 respectively. • Nonmetals in compounds have oxidation states with the priority listed Part A What is the…
- First, assign oxidation numbers for each atom in the balanced chemical equation below. You'll find it easiest to fill the blanks in left to right since once there is an oxidation number typed in the blank it will be much closer to appearing over the appropriate elemental symbol. Blank 1 Blank 2Blank 3 12Blank 13 Blank 4Blank 5Blank 6 Blank 14Blank 15Blank 16 KMnO4(aq) + KCIO₂(aq) + H₂O(l) → 4 MnO₂(s) + 3 KCIO4(aq) + 4 KOH(aq) Now, identify each of the following What underwent reduction? Blank 17 Blank 7Blank 8 What gained electrons? Blank 18 • What got oxidized? Blank 19 What is the oxidizing agent? Blank 20 • What is the reducer? Blank 21 What lost electrons? Blank 22 Blank 9Blank 10 Blank 11 BlankCalcium, barium, and magnesium are three elements in group 2 of the periodic table. Calcium is in period 4, barium is in period 6, and magnesium is in period 3. Choose the correct statements: 1. Calcium can replace barium in its solution. 2. Both barium and calcium can replace magnesium in its solution. 3. Calcium can oxidize magnesium in its solution. 4. Only Barium can replace calcium but magnesium can't replace calcium in its solution. 5. Magnesium can replace both calcium and Barium in their solutions. O 2 and 4 are true O 1 and 2 only are true 1,2,3,4,5 are true 1 only is true 2 and 3 are true 2 only is true Hockey O 2, 3 and 5 are true sageFor each chemical reaction listed in the table below, decide whether the highlighted atom is being oxidized or reduced. highlighted atom is being... reaction neither oxidized nor reduced oxidized reduced CH(9)+H,O(g) → CO(g)+3 H,(g) CO(g)+H,O(9) → CO,(9)+H,(9) N(9)+3 H,(9) → 2 NH3(9) 4 HF(g)+ SiO,(s) → SiF,(9)+2 H,O(9)
