Balance the following half-reactions. (b) (basic) Ni(OH) 2 (s) → Ni 2 O 3 (s)

Hi everyone. So you're asking about the balance have reactions under basic conditions and identify whether it is an oxidation or reduction reaction. We need to first write this out. We have video two plus years. It's gonna give us B. O two plus one. Now we need to balance the non hydrogen and non oxygen elements first. And as you can see this is already balanced. So the next thing we need to do is balance the oxygen by adding H20 liquid. To decide that needs oxygen. You have to auction on the reaction side. Put one on the product side so we can add one H 20 liquid. And then we have two options on the product side. Now I need to balance our hydrogen by adding H plus the side that needs hydrogen. We have no hydrogen on the right hand side we have two on the product side. We can add two h plus on the reacting side, dynamic imbalance are charges by adding the electrons to the more positive side. If you look at our charges plus two here plus one here plus two and zero we're gonna have overall charge of plus three Over here Plus two over here we need to add electrons to the reacting side. We're gonna add one electron. So now we're gonna balance any remaining H plus by adding an equal amount of O. H minus ions to both sides. You have to age plus on the right hand side but none on the private side. We need to add 20 H minus to both sides. We're gonna get the L two plus equals Plus two H plus plus one electron plus two O H minus. It's going to be L two plus. Like what Plus H 2 0. Liquid. That's 20. H minus. Hey chris. And so now that H plus and the O H minus will combine to form H +20 liquid. You're gonna get bl two plus a quiz plus two H +20 liquid plus one electron, Michelle's VL two plus Quinn plus H +20 liquid plus two O H minus. So now we can cancel our common species. We have two H two over on the raft inside. But one on the product side we're gonna be left at one H on the inside. So far. Our balanced reaction. V O two plus Plus H 20. Quinn Plus one electron. And it shows v. O. In class Plus 20. H. Finance for our oxidation reaction. This means we're losing electrons that the electrons gonna be on the product side. And for the reduction reaction we're gaining electrons to the electron is going to be on the wrapped inside. But in this case this is a reduction reaction. You have electrons on the left side. We're gaining electrons. Thanks for watching my video and I hope it was helpful

Ch.19 - Electrochemistry

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McMurry 8th Edition

Ch.19 - Electrochemistry

Problem 49b

Chapter 19, Problem 49b

Balance the following half-reactions. (b) (basic) Ni(OH)₂(s) → Ni₂O₃(s)

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Identify the elements that are changing oxidation states. Here, nickel (Ni) is the element undergoing a change.

Write the oxidation half-reaction for nickel. Determine the change in oxidation state for Ni from Ni(OH)_2 to Ni_2O_3.

Balance the number of Ni atoms on both sides of the equation. Since there are two Ni atoms in Ni_2O_3, you need two Ni(OH)_2 on the reactant side.

Balance the oxygen atoms by adding water (H_2O) molecules to the side that needs more oxygen. In this case, add water to the reactant side to balance the oxygen atoms.

Balance the hydrogen atoms by adding hydroxide ions (OH^-) to the side that needs more hydrogen. This will also help to balance the charge in a basic solution.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Half-Reaction Method

The half-reaction method involves separating oxidation and reduction processes to balance redox reactions. Each half-reaction is balanced for mass and charge, allowing for a clearer understanding of electron transfer. This method is particularly useful in complex reactions, such as those occurring in basic or acidic solutions.

Balancing in Basic Solutions

When balancing reactions in basic solutions, hydroxide ions (OH⁻) are used to neutralize any hydrogen ions (H⁺) that appear during the balancing process. This often involves adding water molecules to balance oxygen atoms and then adding OH⁻ to balance any resulting H⁺ ions, ensuring that the final equation reflects the basic conditions.

Oxidation States

Oxidation states are a way to keep track of electron transfer in redox reactions. Each element in a compound is assigned an oxidation state based on its electron configuration and bonding. Understanding oxidation states is crucial for identifying which species are oxidized and reduced, thus aiding in the balancing of half-reactions.