Hello po! Oxidation and reduction in batteries and fuel cells involve transferring electrons, with oxidation releasing electrons and reduction accepting them. This electron movement creates an electric current, which stores or releases energy depending on the process. Oxidation and reduction help batteries and fuel cells work by moving electrons. When electrons flow, energy is either stored like nagchacharge po or released during use as electricity.
yo julz! oxidation and reduction help store and release energy in batteries and fuel cells by moving electrons. In batteries, electrons flow from one material (oxidation) to another (reduction), creating electricity to power devices. In fuel cells, fuel like hydrogen is oxidized, and oxygen is reduced, producing energy as electricity and heat. This movement of electrons is what powers many technologies we use every day.
Yes, the lecture outlines the steps for assigning oxidation states and identifying changes, I’m just wondering, what happens if we can't clearly identify the oxidation state changes in following these steps?
baks, if we cannot easily determine the oxidation state changes following these steps, it could be that the compound is complex, has mixed oxidation states, or involves a redox reaction that is not straightforward, and requires further analysis or more advanced methods to determine the oxidation states correctly.
If we can't clearly identify the oxidation state changes in a chemical reaction, we may struggle to understand the electron transfer process, which is essential for determining whether a reaction is a redox reaction, predicting reaction products, or balancing the equation correctly. It can lead to errors in analysis and calculations.
Hello sir good evening!!! My question is, In redox reactions, how do you determine the oxidation state of an element when it can have multiple possible oxidation states within a compound?
To find the oxidation states in a redox reaction, you can use either the oxidation number method (where some elements have predetermined oxidation states) or the ion-electron method (where oxidation states are determined by ion charges). Understanding both methods simplifies the process.
To determine the oxidation state of an element with multiple possible oxidation states in a compound, follow these steps: Use known oxidation states: Start with elements that have well-known oxidation states, such as alkali metals (+1), alkaline earth metals (+2), and halogens (-1). Sum of oxidation states: The sum of oxidation states in a neutral compound must be zero, and in a polyatomic ion, it must equal the ion's charge. Assign based on rules: Apply general rules (e.g., oxygen is usually -2, hydrogen is +1) to find the unknown oxidation state of the element in question. By considering these factors, you can deduce the oxidation state of the element within the compound.
The ion-electron method balances redox reactions by ensuring that the number of electrons lost during oxidation equals the number of electrons gained during reduction. This principle of equal electron transfer maintains charge neutrality and ensures the conservation of mass in the overall reaction.
Sir miles defines oxidation as addition of oxygen/loss of electrons and reduction as addition of hydrogen/gain of electrons. Now my question is, why can oxidation and reduction be defined in two different ways (oxygen/hydrogen vs. electrons)?
Sir miles what is the difference between redox and oxidation in terms of electron transfer? Can a reaction be considered redox without oxidation occurring?
The reduced element in the redox reaction examples provided by Sir Miles and those available online is typically the element or molecule containing oxygen. Do you believe that's how it always works?
That's a nice observation. If we go by definition, when we say reduction reaction, it is the adding of hydrogen and the removal of oxygen. And if an element undergoes the reduction reaction, it is the reduced element. And since reduction is the removal of oxygen, we could say that Oxygen is always the reduced element.
Hello po, the answer is yes po because from the term itself oxidation-reduction reaction (redox reaction) and if we'll go back to sir's definition of oxidation, it involves adding oxygen while the reduction, it involves removal of oxygen. Therefore, we can conclude po na oxygen will always be present in the equation.
Good Evening! How does the presence of different solvents or conditions ( for example like temperature and pressure) affect a redox reaction? Do these factors always alter the way the reaction proceeds?
(1) What is the difference between complete and incomplete combustion? (2) Can you also provide concrete in real life examples of complete and incomplete combustion with their by-products?
Answer for Question #1) We say can that it is complete combustion when the product in a reaction is CO2 and H20, while we can say it is incomplete combustion is when the products in a reaction consist of other element or compound (products could still react with oxygen; where carbon or carbon monoxide are produced) Answer for question #2) example of complete combustion is С3Н8+ 5O2 → 3CO2+ 4H20 example of incomplete combustion CH4 + 02 → C + 2H20
Redox reactions are essential because they involve the transfer of electrons, which drives many natural and industrial processes, such as energy production, metabolism, corrosion, and chemical synthesis. In chemistry, redox reactions are fundamental as they explain how substances gain or lose electrons, leading to changes in their chemical properties. This relationship helps us understand processes like combustion, electrochemistry, and the behavior of elements in the periodic table.
For a given redox reaction with unknown coefficients, what will be the step-by-step process of balancing it using the oxidation number method when the compounds are polyatomic ions
Given a complex redox reaction involving multiple elements, how would you systematically assign oxidation states to each atom and determine the electron flow?
What are the key rules for assigning oxidation states to elements in a chemical equation, and how do these rules apply to compounds such as water (H₂O) and sulfate ions (SO₄²⁻)?
The first rule states that an individual atom has an oxidation state of zero. Secondly, the total oxidation of all atoms in a neutral species is zero which is the case for the water molecule. However, for the sulfate ion, if we look at the periodic table, sulfur has numerous oxidation state so we need to solve for the sulfur's oxidation state.
What are the three most significant challenges facing the development of sustainable energy sources, and what innovative solutions are being explored to overcome them?
And my last question sir In balancing redox reactions in acidic media, why is it necessary to add H+ ions, and how do they contribute to maintaining charge neutrality?
Well in balancing redox reaction, to balance the oxygen, we need to add water molecule, the same goes to the hydrogen. In order to balance hydrogen atoms, we need to add H+ ions.
How are oxidation-reduction reactions connected to electron transfer? Can we show this with simple examples like the reaction between zinc and copper sulfate?
In a redox reaction involving transition metals, how can you determine the exact oxidation states of metals in various oxidation states, considering coordination complexes that might alter expected values?
Hello po! Transition metals can often exhibit multiple oxidation states po and the specific oxidation state in a complex depends on the ligands, their bonding to the metal, and other factors. And based on what I have searched po, the formation of a coordination complex can significantly alter the oxidation state of the central metal atom.While, Ligands are atoms, ions, or molecules that bond to the central metal atom in a coordination complex.
Sa redox reaction, ang oxidizing agent ay nag-aaccept ng electrons, kaya nag-o-oxidize ang iba. Ang reducing agent naman ay nagbibigay ng electrons, kaya nag-rereduce ang iba.Oxidizing agent, "kumukuha"; reducing agent, "nagbibigay".
Hello! In a redox reaction po, the oxidizing agent is the substance that gains electrons and gets reduced. Siya yung nagpa-push sa ibang substance para mag-lose ng electrons (oxidize). The reducing agent, on the other hand, loses electrons and gets oxidized. Siya naman yung nagpa-push sa ibang substance para mag-gain ng electrons (reduce). So, nag-iinteract sila kasi yung reducing agent nagbibigay ng electrons, at yung oxidizing agent naman tumatanggap.
Hello! In redox reactions, electrons are handled as reactants in reduction reactions, where a species gains electrons, and as products in oxidation reactions, where a species loses electrons. For example, in reduction, electrons are added to the left side of the half-reaction, such as when  gains electrons to form . In oxidation, electrons are placed on the right side, as seen when zinc metal () loses electrons to form . To ensure charge balance in the overall redox reaction, the number of electrons lost in the oxidation half-reaction must equal the number of electrons gained in the reduction half-reaction. This may require multiplying the half-reactions by appropriate factors, allowing the electrons to cancel out when the half-reactions are combined.
I consider oxygen to be a powerful oxidizing agent because it easily accepts electrons from other substances in redox reactions. This allows it to help other molecules lose electrons and become oxidized.
Hii! Oxygen is a powerful agent and is essential in cellular production as the final electron acceptor. Its high electronegativity and tendency to gain electrons make it effective in oxidizing other substances, and to achieve stable electron configuration, thereby facilitating the efficient production of cellular energy production or ATP.
The second rule of redox reactions, as sir. Miles mentioned, is that when determining the oxidation state of each element, we need to represent it as (x). I am just wondering, if the given compound has two elements with multiple possible oxidation states, how do you determine the oxidation state of each element?
There are two ways for you to balance oxidation redox reaction and to know the oxidation state of a compound. That is the oxidation number method and ion electron method. In oxidation redox reaction, some elements in a certain compound has already a fix oxidation states. While in ion electron method, the oxidation state of an element depends on its ion charges. It will be easier for you to identify oxidation states of an element if you know the rules of these two methods po.
As I’ve watched the video lecture in applying the rules of ion electron method in the given problem, why did the element iron was increased by 6 molecules?
Another question sir miles In redox reactions, if the standard steps for assigning oxidation states don't clearly identify the oxidation state changes, what alternative methods or considerations can be used?
hello pooo so like, noble gas compounds are important kasi they show na even super stable elements like noble gases can form bonds and undergo redox reactions. This helps scientists understand more about extreme oxidation states and bond formations, making them super useful sa advanced chemistry studies and applications.
To identify an atom if it belongs from the neutral species, you must first solve for it’s overall oxidation state. If the overall oxidation state result or answer is 0(zero) then it is a Neutral Species of atoms
If the overall oxidation state of the compound is O then it is a nuetral species. For example, H2O. Oxygen = -2 (oxidation state) × 1 (number of O atom in the compound) = -2 Hydrogen = +1 (oxidation state) × 2 (number of H atom in the compound) = 2 So -2 + (+2) = 0. Therefore, H2O is a neutral species.
Yes po, there are compounds and elements na…, where the general rules for oxidation states have exceptions or are not strictly followed. Nangyayari siya due to unique electronic structures, bonding scenarios, or resonance effects Ex: Peroxide ung oxygen nya has an oxidation state of -1 instead of the usual -2 (H2O2 basically) so in here po, each hydrogen is +1, and each oxygen may -1
Hello po as you can see dun po sa given natin natin which is 2C8O2 - 25O2 ang naging reactants po natin which is yung nasa left side naging 16CO2 + 18H2O yung 25 po naging constant po siya sa value ng nasa right side.
Sir miles my question is when a compound contains two elements with multiple possible oxidation states, how can we determine the oxidation state of each element in a redox reaction, following the second rule of representing each element's oxidation state as (x)?
You can identify a redox reaction by checking if there is a change in the oxidation states of elements in the reactants and products. First, Assign oxidation states to each atom in the reactants. Then, Compare oxidation states before and after the reaction. If an element’s oxidation state increases, it’s oxidized (loses electrons). If an element’s oxidation state decreases, it’s reduced (gains electrons). If both oxidation and reduction occur in the reaction, it’s a redox reaction.
We can identify redox reactions using oxidation numbers, which are assigned to atoms in molecules by assuming that all bonds to the atoms are ionic. An increase in oxidation number during a reaction corresponds to oxidation, while a decreases corresponds to reduction.
Helloo! I think po for simpler redox reactions, the oxidation number method, which focuses on assigning oxidation numbers to elements and balancing them, is mas okay na gamitin when balancing. However, for more complex example of redox reactions involving multiple electron transfers, the ion-electron method is generally preferred. This method involves breaking down the overall reaction into half-reactions, balancing each half-reaction independently, and then combining them to obtain the balanced overall equation. And it is a matter of preference na rin.
The ion-electron method is more suitable for complex redox reactions, especially in aqueous solutions, as it systematically balances electrons, atoms, and charges while accommodating acidic or basic conditions.
Hi! The ion-electron method focuses on understanding the transfer of electrons during chemical reactions. It uses these charges to balance the number of electrons lost and gained in redox reactions, ensuring the overall charge remains neutral.
If you’re solving for the oxidation state of an element, and the answer you got is not in the periodic table, is it required to follow the oxidation state of each element in the periodic table, or proceed with the answer you got?
Hello po. It is not necessarily na sundin 'yung oxidation state na nasa periodic table of elements because there will be instances talaga na 'yung oxidation state e nakadepende sa given compound
Good eve, sir!!! Can a redox reaction occur spontaneously in a completely closed system with no external energy or catalysts? If the answer is yes, kindly provide examples to deepen our understanding.
Good eve! Yes, a redox reaction can occur spontaneously in a closed system without external energy or catalysts, as long as the reaction is energetically favorable. A common example is the rusting of iron. When iron reacts with oxygen and moisture, a redox reaction happens naturally, forming iron oxide (rust). Another example is when zinc reacts with copper sulfate in a solution, causing the zinc to oxidize and copper to reduce, forming solid copper. These reactions happen because the materials involved naturally transfer electrons to reach a more stable state.
21:20 sa step two poser of assigning oxidation states for the products, if the equation was already 2x+3(-2)=0 naging 2x-6=0 then paano naging 2x=6 diretso na po ba?
iipag hihiwalay po kasi yung literal coefficient and numerical coefficient. kaya po from 2x-6=0 to 2x=6. kasi 2x is the literal coefficient so remain sa left part of equation, then yung six (numerical coefficient) ililipat mo to the right so from -6 magiging +6 na siya kasi inilipat mo. kaya po ganun :)) moreover, 2x=6 is hindi pa pwede na ma determine yung oxidation state. so idivide mo both sides by 2 para macancel yung numerical sa literal coefficient. so ang magiging sagot (yung oxidation state) is x=+3
On the ion electron method, step 3 states that if the oxidation number increases by 1, then add one e, then what if it increases by more than just 1? Are you going to still add ONE e? Or more than that?
If the oxidation number increases by more than just 1 in the ion-electron method, you will need to add the corresponding number of electrons to balance the change.
In the ion-electron method, balancing electrons for both half-reactions is necessary because the total number of electrons lost in the oxidation half-reaction must exactly equal the number of electrons gained in the reduction half-reaction . This means that the total number of electrons in the reaction stays the same ,they are not lost or gained.
The physical state of a substance-solid, liquid, gas, or aqueous solution-significantly influences redox (reduction-oxidation) reactions by affecting the rate, mechanism, and efficiency of electron transfer. In solids, surface area and the ability to donate or accept electrons play a key role, while in liquids, the solvent’s ability to dissociate ions impacts the reaction. Gases, due to their high kinetic energy and diffusion, facilitate fast reactions, and aqueous solutions, particularly water, support ion exchange and electron transfer.
The fundamental principle of balancing redox reactions using the ion-electron method is that the number of electrons lost during oxidation must equal the number of electrons gained during reduction.
Oxidation Number Method This method involves tracking changes in oxidation states to balance redox equations.Ion-Electron Method (Half-Reaction Method) This method separates the oxidation and reduction processes into two half-reactions, balances them individually, and then combines them.
Hello po. For me, lanthanides and actinides elements po does not make the equation complicated in redox reaction kasi like any other elements, they have normal oxidation state naman if we will base it on the periodic element, unlike sa noble gases na talagang walang given oxidation state except kay Og element
Sa Lanthanides and actinides meron po silang different oxidation states, which makes their chemistry tricky. Sa Lanthanides mostly meron po silang +3 charge, but some can have +2. Actinides naman po can range from +3 to +6.Dahil po sa special electron setup and radioactivity, their reactions are harder to predict, making their redox behavior more complicated.
In a simple redox reaction, electrons are transferred between two species, with one being oxidized (losing electrons) and the other reduced (gaining electrons). The changes in oxidation states are straightforward and typically involve individual atoms or simple ions.
To find oxidation state changes in a redox reaction, start by balancing the chemical equation. Then, assign oxidation numbers to each atom, following rules like alkali metals (+1), alkaline earth metals (+2), halogens (-1), oxygen (-2), and hydrogen (+1). Next, compare oxidation numbers before and after the reaction to identify which atoms are oxidized (increased number) and reduced (decreased number).
In living things, oxidation and reduction are vital for processes like breathing and making food. In "cellular respiration", cells break down glucose (sugar) to get energy. During this, glucose "loses electrons" (oxidized), and oxygen "gains electrons"(reduced) to form water, releasing energy the cell uses. In "photosynthesis", plants use sunlight to convert carbon dioxide and water into glucose (food) and oxygen. Here, water "loses electrons"(oxidized) to produce oxygen, and carbon dioxide "gains electrons" (reduced) to form glucose. These processes, powered by oxidation and reduction, help cells breathe and plants create food.
Sir, why is it necessary to add ions when balancing this redox reaction in an acidic medium, and what role do they play in maintaining charge neutrality?
In an acidic medium, adding ions, particularly H⁺ (hydrogen ions), is essential for balancing redox reactions. These ions help maintain charge neutrality and ensure that the reaction is mass-balanced. When electrons are transferred in redox reactions, H⁺ ions are often required to balance the charge, particularly when elements are reduced (gain electrons) or oxidized (lose electrons). Additionally, in an acidic medium, H⁺ ions combine with oxygen atoms to form water (H₂O), which helps balance the number of atoms in the reaction. The inclusion of electrons ensures that the number of electrons lost in oxidation equals the number gained in reduction, further preserving charge balance. Overall, these ions are crucial for achieving both mass and charge balance in the redox equation.
You need to follow the step. If changes in oxidation states and electron transfer are observed, the reaction is a redox reaction. For exmple Na 0 to +1 ( mean oxidizing ) Na +1 to 0 ( reduced
to check if a reaction is a redox reaction, look for electron transfer. If one substance loses electrons (oxidized) and another gains electrons (reduced), then it's a redox reaction.
Hello po. It is important po because if we go back to the definition of redox reaction, it involves transfer of electrons from a chemical substance to another. Meaning, substances cannot undergo redox reaction without transferring and accepting electrons in the process kasi we won't know which substance undergoes oxidation or reduction kung hindi natin malalaman kung ano 'yung nag bawas and nag accept ng electrons.
To determine a metal's oxidation state in a complex ion we calculate the total charge contributed by the ligands. Then assign an oxidation state to the metal that when combined with the ligand charges equals the overall charge of the complex ion
In redox reactions, electron transfer is the key process where one substance loses electrons (oxidation) and another gains electrons (reduction). In other types of chemical reactions, such as acid-base or precipitation reactions, no electrons are transferred; instead, other processes like proton transfer or ion exchange occur.
In redox reactions, electron transfer is the key process where one substance loses electrons (oxidation) and another gains electrons (reduction). In other types of chemical reactions, such as acid-base or precipitation reactions, no electrons are transferred; instead, other processes like proton transfer or ion exchange occur.
If in a redox reaction, the oxidation state of an element increases, what does this imply about the element's role, and how does it affect the reaction as a whole?
Hello po! When an element's oxidation state goes up in a redox reaction, it’s being oxidized-basically, it’s losing electrons. This element is the reducing agent because it gives away electrons to help another element get reduced. Redox reactions are all about this teamwork: one loses, one gains, and together they make the reaction happen.
Redox reactions involve electron transfer, where oxidation is the loss of electrons and reduction is the gain of electrons. To balance these reactions we ensure equal electron transfer between oxidizing and reducing agents, by using methods like the oxidation number or ion-electron methods.
Hello po. In the Ion-Electron Method, elements appear to have charges because we focus on oxidation states and electron transfers, not their elemental form. Sa ion electron method po kasi it tacks the electrons transferred during the reaction and assigns charges to elements or ions to reflect their new states after gaining or losing electrons.
Hi! Good eve! Hydrogen peroxide can act as both an oxidizing and reducing agent due to the presence of oxygen and because it can gain and lose electron. It can act as an oxidizing agent by gaining electrons and being reduced to water or H20 in a single process. It can operate as a reducing agent in another reaction by losing electrons and oxidizing to oxygen gas (02). Because of its dual function, hydrogen peroxide is a substance that can be used for a variety of purposes, including disinfection.
The most oxidation-prone elements are alkali metals (like sodium and potassium) and alkaline earth metals (like calcium and magnesium). They lose electrons easily, making them super reactive, especially with oxygen!
The half-reaction method is a vital technique for balancing redox equations, as it breaks the reaction into two parts: one for oxidation and one for reduction. This approach simplifies the process by clearly separating the electron loss (oxidation) and gain (reduction), ensuring that both mass and charge are conserved. By balancing the half-reactions individually, it guarantees that the number of electrons lost during oxidation equals the number of electrons gained during reduction. Additionally, the method is adaptable to both acidic and basic solutions, making it versatile for various reactions. Overall, the half-reaction method provides a systematic and effective way to balance complex redox equations, illustrating the electron transfer process and ensuring the accuracy of the final equation.
The primary rules for assigning oxidation states to elements in a compound ensure consistency in understanding electron transfer during chemical reactions. Elements in their pure form always have an oxidation state of 0, and monoatomic ions equal their charge. Oxygen usually has an oxidation state of -2, except in peroxides and with fluorine. Hydrogen is typically +1, except when bonded with metals in hydrides, where it is -1. The sum of oxidation states in a neutral compound is 0, and in a polyatomic ion, it equals the ion’s charge. Fluorine always has an oxidation state of -1, while other halogens typically have an oxidation state of -1, unless bonded to oxygen or fluorine, which can give them positive oxidation states. These rules help assign oxidation states systematically, enabling the understanding and balancing of redox reactions.
Hello! Based from what I learned from the internet, analyzing the presence of H+ or OH- ions in the balanced equation can determine the medium of the reaction.
Assign an oxidation number for each element. Oxidatio numbers are a way of keeping track of how many electrons an atom has gained or lost during a reaction. -Telan, Ma. Rielle
When an element changes during a redox reaction, how does its oxidation state change? Can we figure out if something is getting oxidized or reduced by looking at this?
We can say that an element is being oxidized if there is a loss of electron and an element is being reduced if it gains an electron. We can observe this by identifying the changes in the oxidation state between the reactant and the product
How can you determine that the equation will use Oxidation number method in Balancing its redox reaction instead of Ion electron method and vice versa?
Use the Oxidation Number Method for simpler reactions involving changes in oxidation states. Use the Ion-Electron Method for more complex reactions, especially in acidic or basic solutions, where balancing electrons and charges is critical.
Rusting is a redox reaction where iron reacts with oxygen and water. so to prevent rusting we must isolate iron from water and oxygen by applying protective coatings
We balance chemical reactions to adhere with the law of conservation of mass, which states that matter can not be created or destroyed in a chemical reaction.
Hello po! it's important to balance the reactants and products in order to follow po yung rules of mass and charge conservation (based on what I learned online). This means po that the number of atoms and the total charge should be the same on both sides. Remember po that a balanced chemical equation also provides an estimate on how many reactants are needed for a reaction.
Do you think noble gases are allowed in redox reaction even though most of them doesn't have oxidation state? That maybe there will be an exemption to the rule since the elements Rn and Og have oxidation state?
Ranell: Noble gases rarely participate in redox reactions dahil stable sila with full valence shells, pero exceptions exist for heavier noble gases like radon (Rn) and oganesson (Og). Radon can form compounds like RnF₂, showing an oxidation state of +2, while Og is predicted to have oxidation states (+2 or +4) theoretically. However, dahil sobrang unstable and radioactive nila, their involvement in redox reactions is highly limited and not practical in most scenarios.
hello po noble gases are usually chill lang, like super stable sila kasi full na yung valence shells nila, kaya they don’t usually join redox reactions. Pero, wait lang, I think po may exemptions talaga. Si radon (Rn) and oganesson (Og), they can have oxidation states minsan kasi they’re heavier noble gases. Iba yung energy levels nila, so parang medyo kaya nilang mag-react in some special cases. Pero it’s super rare ha! So, in general po noble gases are like, “No thanks, I’m good,” sa redox, pero pwede silang sumama minsan kapag special occasion hahaha
The rate of redox reactions depends on factors like the nature of reactants, their concentration, temperature, surface area, use of catalysts, pressure (for gases), and pH. These affect how quickly particles collide and react.
Water can act as both an oxidizing agent (accepting electrons) and a reducing agent (donating electrons): • As an oxidizing agent: In the reaction with sodium: 2Na + 2H20 → 2NaOH + H2 Water is reduced to hydrogen gas. • As a reducing agent: In the reaction with chlorine gas: Cl + H20 - HC + HOCL Water is oxidized to hypochlorous acid
The oxidation state of chlorine in NaCl changes when it reacts with fluorine. What is the change in oxidation state of chlorine during this reaction, and what type of reaction is this?
In the reaction between sodium chloride (NaCl) and fluorine (F₂), chlorine undergoes oxidation, while fluorine undergoes reduction. The reaction is as follows: 2NaCl+F²→2NaF+Cl²
Hii! I guess it will be a matter of trial and error sa pagkuha ng oxidation state ng both elements. I also searced online and it stated that the oxidation states of elements involved in a compound that has several possible oxidation states can be determined by their electronegativity, structure, and bonding but I can't find a concrete example so yeah haha:)
In carbon dioxide (CO₂), carbon has an oxidation state of +4. How do the oxidation state rules explain why carbon has this positive value in this compound?
@@NicoleBeverlyDeza Oxygen has an oxidation state of -2. This is a general rule that applies in most compounds, including CO2. The sum of the oxidation states of all atoms in a neutral molecule is zero. CO2 is a neutral molecule, so the sum of the oxidation states of carbon and oxygen must equal zero. Let's denote the oxidation state of carbon as "x". We can set up the equation: x + 2 (-2) = 0 Solving for x: x + 2 (-2) = 0 x - 4 = 0 x = +4 It became +4 (from -4) because nailipat sya from the left side to the right of the equation and there is a rule na mapapalitan din ang sign nya if ililipat to the other side of the equation. Therefore, the oxidation state of carbon in CO2 is +4. This positive value indicates that carbon has lost electrons, which is characteristic of oxidation.
Good evening! Can you explain po how redox reactions are applied in our everyday lives? I’ve heard about their role in things like rusting and batteries, but could you provide a more detailed example?
In my own understanding, I think Yes. Because in order for the reducing agent to reduce other reactants, it MUST DONATE its electron which means it loses electron and by definition, it undergoes the oxidation reaction and oxidation in OIL rig is loss of electron
Hello! I believe po that the mnemonic is perfectly clear, and yes it is always the case talaga that the element losing electrons is the reducing agent. This is because the reducing agent is the one that donates electrons to another substance, causing it to be reduced. When the reducing agent loses electrons, nag-o oxidize siya. Therefore, the element losing electrons is called the reducing agent because it helps reduce another element by giving up its electrons.
Hello po! The ion-electron method (also known as the half-reaction method) is important in balancing redox reactions, especially complex ones, because it focuses on electron transfer. Redox reactions fundamentally involve the transfer of electrons. This method explicitly separates the overall reaction into two half-reactions: the oxidation states which loses electrons and the reduced
continuation because I accidentally touch the send button hahaha Redox reactions fundamentally involve the transfer of electrons. This method explicitly separates the overall reaction into two half-reactions: the oxidation reaction which loses electrons and the reduction reaction that gains electrons
Oxidation states help us track electron transfers in redox reactions. If oxidation state increases, na-oxidize siya (loses electrons). If it decreases naman po na-reduce siya (gains electrons). By checking these changes, you can balance the number of electrons lost and gained. This ensures the reaction is balanced both in charge and mass, making the process organized and systematic.
Hi mich, yung oxidation states kasi ay tumutulong para makita kung anong element ang oxidized (tumaas ang oxidation state) at kung alin ang reduced (bumaba ang oxidation state). Kapag alam na kasi ito , madali nang balansehin ang redox reaction gamit ang bilang ng electrons na nawala at nakuha para sure na pantay ang mga elements at charge sa mag kabilang equation.
Oxidation states tell us how many electrons an atom loses or gains in a reaction. They help us see which atoms lose electrons (oxidized) and which gain them (reduced). In a redox reaction, the number of electrons lost by one atom must equal the number of electrons gained by another. By using oxidation states, we can balance the reaction and make sure the atoms and charges are correct.
By the definition of sir miles, the 6e there accounts for the traansfer of electron REQUIRED to reduced 2 Cr atoms from +6 to +3. Firstly, we determine the number of change in oxidation number, as we can see, it decreases by 3 oxidation number. And if we look at the Cr atom at the reactant side, it has 2 atoms. So what we need to do is to multiply the 2 Cr atoms from the reactant side to the number of change in oxidation number of 3 which gives us 6.
![Intro to Chemistry & What is Chemistry? - [1-1-1]](http://i.ytimg.com/vi/pdyDmXtye2w/mqdefault.jpg)
How do oxidation and reduction help with storing and releasing energy, like in batteries and fuel cells?
Hello po! Oxidation and reduction in batteries and fuel cells involve transferring electrons, with oxidation releasing electrons and reduction accepting them. This electron movement creates an electric current, which stores or releases energy depending on the process. Oxidation and reduction help batteries and fuel cells work by moving electrons. When electrons flow, energy is either stored like nagchacharge po or released during use as electricity.
yo julz! oxidation and reduction help store and release energy in batteries and fuel cells by moving electrons. In batteries, electrons flow from one material (oxidation) to another (reduction), creating electricity to power devices. In fuel cells, fuel like hydrogen is oxidized, and oxygen is reduced, producing energy as electricity and heat. This movement of electrons is what powers many technologies we use every day.
Yes, the lecture outlines the steps for assigning oxidation states and identifying changes, I’m just wondering, what happens if we can't clearly identify the oxidation state changes in following these steps?
baks, if we cannot easily determine the oxidation state changes following these steps, it could be that the compound is complex, has mixed oxidation states, or involves a redox reaction that is not straightforward, and requires further analysis or more advanced methods to determine the oxidation states correctly.
If we can't clearly identify the oxidation state changes in a chemical reaction, we may struggle to understand the electron transfer process, which is essential for determining whether a reaction is a redox reaction, predicting reaction products, or balancing the equation correctly. It can lead to errors in analysis and calculations.
Hello sir good evening!!! My question is, In redox reactions, how do you determine the oxidation state of an element when it can have multiple possible oxidation states within a compound?
To find the oxidation states in a redox reaction, you can use either the oxidation number method (where some elements have predetermined oxidation states) or the ion-electron method (where oxidation states are determined by ion charges). Understanding both methods simplifies the process.
To determine the oxidation state of an element with multiple possible oxidation states in a compound, follow these steps:
Use known oxidation states: Start with elements that have well-known oxidation states, such as alkali metals (+1), alkaline earth metals (+2), and halogens (-1).
Sum of oxidation states: The sum of oxidation states in a neutral compound must be zero, and in a polyatomic ion, it must equal the ion's charge.
Assign based on rules: Apply general rules (e.g., oxygen is usually -2, hydrogen is +1) to find the unknown oxidation state of the element in question.
By considering these factors, you can deduce the oxidation state of the element within the compound.
Sir how did you get the 6e- in step 4 in the Ion electron method po?
What is the fundamental principle of balancing redox reactions using the ion-electron method?
Hi elleana! My answer to this po eh, the number of electrons lost during oxidation is equal to the number of electrons gained during reduction.
The ion-electron method balances redox reactions by ensuring that the number of electrons lost during oxidation equals the number of electrons gained during reduction. This principle of equal electron transfer maintains charge neutrality and ensures the conservation of mass in the overall reaction.
Sir miles defines oxidation as addition of oxygen/loss of electrons and reduction as addition of hydrogen/gain of electrons. Now my question is, why can oxidation and reduction be defined in two different ways (oxygen/hydrogen vs. electrons)?
On the ion electron method, how did you get the 6e sir?
Sir miles what is the difference between redox and oxidation in terms of electron transfer?
Can a reaction be considered redox without oxidation occurring?
The reduced element in the redox reaction examples provided by Sir Miles and those available online is typically the element or molecule containing oxygen. Do you believe that's how it always works?
That's a nice observation. If we go by definition, when we say reduction reaction, it is the adding of hydrogen and the removal of oxygen. And if an element undergoes the reduction reaction, it is the reduced element. And since reduction is the removal of oxygen, we could say that Oxygen is always the reduced element.
Hello po, the answer is yes po because from the term itself oxidation-reduction reaction (redox reaction) and if we'll go back to sir's definition of oxidation, it involves adding oxygen while the reduction, it involves removal of oxygen. Therefore, we can conclude po na oxygen will always be present in the equation.
Good Evening! How does the presence of different solvents or conditions ( for example like temperature and pressure) affect a redox reaction? Do these factors always alter the way the reaction proceeds?
(1) What is the difference between complete and incomplete combustion?
(2) Can you also provide concrete in real life examples of complete and incomplete combustion with their by-products?
Answer for Question #1)
We say can that it is complete combustion when the product in a reaction is CO2 and H20, while we can say it is incomplete combustion is when the products in a reaction consist of other element or compound (products could still react with oxygen;
where carbon or carbon monoxide are produced)
Answer for question #2)
example of complete combustion is
С3Н8+ 5O2 → 3CO2+ 4H20
example of incomplete combustion
CH4 + 02 → C + 2H20
What is the importance of redox reaction?
what's the relationship of redox reaction to chemistry?
Redox reactions are essential because they involve the transfer of electrons, which drives many natural and industrial processes, such as energy production, metabolism, corrosion, and chemical synthesis.
In chemistry, redox reactions are fundamental as they explain how substances gain or lose electrons, leading to changes in their chemical properties. This relationship helps us understand processes like combustion, electrochemistry, and the behavior of elements in the periodic table.
For a given redox reaction with unknown coefficients, what will be the step-by-step process of balancing it using the oxidation number method when the compounds are polyatomic ions
how can i identify sir if its oxidized or reduced ?
Given a complex redox reaction involving multiple elements, how would you systematically assign oxidation states to each atom and determine the electron flow?
What are the key rules for assigning oxidation states to elements in a chemical equation, and how do these rules apply to compounds such as water (H₂O) and sulfate ions (SO₄²⁻)?
The first rule states that an individual atom has an oxidation state of zero. Secondly, the total oxidation of all atoms in a neutral species is zero which is the case for the water molecule. However, for the sulfate ion, if we look at the periodic table, sulfur has numerous oxidation state so we need to solve for the sulfur's oxidation state.
What are the three most significant challenges facing the development of sustainable energy sources, and what innovative solutions are being explored to overcome them?
And my last question sir In balancing redox reactions in acidic media, why is it necessary to add H+ ions, and how do they contribute to maintaining charge neutrality?
Well in balancing redox reaction, to balance the oxygen, we need to add water molecule, the same goes to the hydrogen. In order to balance hydrogen atoms, we need to add H+ ions.
How are oxidation-reduction reactions connected to electron transfer? Can we show this with simple examples like the reaction between zinc and copper sulfate?
In a redox reaction involving transition metals, how can you determine the exact oxidation states of metals in various oxidation states, considering coordination complexes that might alter expected values?
Hello po! Transition metals can often exhibit multiple oxidation states po and the specific oxidation state in a complex depends on the ligands, their bonding to the metal, and other factors. And based on what I have searched po, the formation of a coordination complex can significantly alter the oxidation state of the central metal atom.While, Ligands are atoms, ions, or molecules that bond to the central metal atom in a coordination complex.
Sa redox reaction, what distinguishes an oxidizing agent from a reducing agent, and how do they interact?
Sa redox reaction, ang oxidizing agent ay nag-aaccept ng electrons, kaya nag-o-oxidize ang iba. Ang reducing agent naman ay nagbibigay ng electrons, kaya nag-rereduce ang iba.Oxidizing agent, "kumukuha"; reducing agent, "nagbibigay".
Hello! In a redox reaction po, the oxidizing agent is the substance that gains electrons and gets reduced. Siya yung nagpa-push sa ibang substance para mag-lose ng electrons (oxidize).
The reducing agent, on the other hand, loses electrons and gets oxidized. Siya naman yung nagpa-push sa ibang substance para mag-gain ng electrons (reduce).
So, nag-iinteract sila kasi yung reducing agent nagbibigay ng electrons, at yung oxidizing agent naman tumatanggap.
Hi sir, paano po ulit nakuha yung 6e sa may half reaction method?
Marvelous evening,sir!
How do you handle electrons as reactants or products?
Hello! In redox reactions, electrons are handled as reactants in reduction reactions, where a species gains electrons, and as products in oxidation reactions, where a species loses electrons. For example, in reduction, electrons are added to the left side of the half-reaction, such as when  gains electrons to form . In oxidation, electrons are placed on the right side, as seen when zinc metal () loses electrons to form . To ensure charge balance in the overall redox reaction, the number of electrons lost in the oxidation half-reaction must equal the number of electrons gained in the reduction half-reaction. This may require multiplying the half-reactions by appropriate factors, allowing the electrons to cancel out when the half-reactions are combined.
Why oxygen is a powerful oxidizing agent in redox reactions and how this property makes it essential for cellular energy production?
I consider oxygen to be a powerful oxidizing agent because it easily accepts electrons from other substances in redox reactions. This allows it to help other molecules lose electrons and become oxidized.
Hii! Oxygen is a powerful agent and is essential in cellular production as the final electron acceptor. Its high electronegativity and tendency to gain electrons make it effective in oxidizing other substances, and to achieve stable electron configuration, thereby facilitating the efficient production of cellular energy production or ATP.
The second rule of redox reactions, as sir. Miles mentioned, is that when determining the oxidation state of each element, we need to represent it as (x). I am just wondering, if the given compound has two elements with multiple possible oxidation states, how do you determine the oxidation state of each element?
There are two ways for you to balance oxidation redox reaction and to know the oxidation state of a compound. That is the oxidation number method and ion electron method. In oxidation redox reaction, some elements in a certain compound has already a fix oxidation states. While in ion electron method, the oxidation state of an element depends on its ion charges. It will be easier for you to identify oxidation states of an element if you know the rules of these two methods po.
As I’ve watched the video lecture in applying the rules of ion electron method in the given problem, why did the element iron was increased by 6 molecules?
Another question sir miles In redox reactions, if the standard steps for assigning oxidation states don't clearly identify the oxidation state changes, what alternative methods or considerations can be used?
In the reaction between hydrogen peroxide (H₂O₂) and potassium permanganate (KMnO₄), what happens to the oxidation states of oxygen and manganese?
how the concept of oxidation states can be applied to complex ions in redox reactions
What is the significance of noble gas compounds in the study of oxidation-reduction processes?
hello pooo
so like, noble gas compounds are important kasi they show na even super stable elements like noble gases can form bonds and undergo redox reactions. This helps scientists understand more about extreme oxidation states and bond formations, making them super useful sa advanced chemistry studies and applications.
How can I identify the neutral species?
To identify an atom if it belongs from the neutral species, you must first solve for it’s overall oxidation state. If the overall oxidation state result or answer is 0(zero) then it is a Neutral Species of atoms
A neutral species has a total charge of zero, determined by examining its formula or calculating the sum of oxidation states.
If the overall oxidation state of the compound is O then it is a nuetral species. For example, H2O.
Oxygen = -2 (oxidation state) × 1 (number of O atom in the compound)
= -2
Hydrogen = +1 (oxidation state) × 2 (number of H atom in the compound) = 2
So -2 + (+2) = 0. Therefore, H2O is a neutral species.
Are they any procedure to know and verify that the number of atoms in the reactant side and on the product side are the same ?
Are there some compounds where they are exempted in following the general rules of the oxidation state? If so, can you give some examples?
Yes po, there are compounds and elements na…, where the general rules for oxidation states have exceptions or are not strictly followed. Nangyayari siya due to unique electronic structures, bonding scenarios, or resonance effects
Ex: Peroxide
ung oxygen nya has an oxidation state of -1 instead of the usual -2
(H2O2 basically)
so in here po, each hydrogen is
+1, and each oxygen may -1
Good eve sir! In the combustion reaction po where did the 25 go po and how will you get their molecules to balance the reactant and product?
Hello po as you can see dun po sa given natin natin which is 2C8O2 - 25O2 ang naging reactants po natin which is yung nasa left side naging 16CO2 + 18H2O
yung 25 po naging constant po siya sa value ng nasa right side.
Sir miles my question is when a compound contains two elements with multiple possible oxidation states, how can we determine the oxidation state of each element in a redox reaction, following the second rule of representing each element's oxidation state as (x)?
What steps are involved in using the ion-electron method for balancing redox reactions?
How can you tell if a reaction is a redox reaction just by looking at the reactants?
You can identify a redox reaction by checking if there is a change in the oxidation states of elements in the reactants and products.
First, Assign oxidation states to each atom in the reactants. Then, Compare oxidation states before and after the reaction. If an element’s oxidation state increases, it’s oxidized (loses electrons). If an element’s oxidation state decreases, it’s reduced (gains electrons).
If both oxidation and reduction occur in the reaction, it’s a redox reaction.
How are oxidation and reduction processes related?
How does the concentration of reactants affect the rate of a redox reaction?
How do you determine the overall change in oxidation states in a redox reaction?
We can identify redox reactions using oxidation numbers, which are assigned to atoms in molecules by assuming that all bonds to the atoms are ionic. An increase in oxidation number during a reaction corresponds to oxidation, while a decreases corresponds to reduction.
Between the oxidation number method and ion-electron method, which one is more suitable for balancing complex redox reactions?
Helloo! I think po for simpler redox reactions, the oxidation number method, which focuses on assigning oxidation numbers to elements and balancing them, is mas okay na gamitin when balancing. However, for more complex example of redox reactions involving multiple electron transfers, the ion-electron method is generally preferred. This method involves breaking down the overall reaction into half-reactions, balancing each half-reaction independently, and then combining them to obtain the balanced overall equation. And it is a matter of preference na rin.
The ion-electron method is more suitable for complex redox reactions, especially in aqueous solutions, as it systematically balances electrons, atoms, and charges while accommodating acidic or basic conditions.
Goodevening Sir!
Why do elements have charges in the ion-electron method when they are not in their elemental form?
Hi! The ion-electron method focuses on understanding the transfer of electrons during chemical reactions. It uses these charges to balance the number of electrons lost and gained in redox reactions, ensuring the overall charge remains neutral.
Why is it essential to balance the electrons in oxidation and reduction half-reactions using the ion-electron method?
The number of electrons lost in the process of oxidation must equal the number gained in reduction.
If you’re solving for the oxidation state of an element, and the answer you got is not in the periodic table, is it required to follow the oxidation state of each element in the periodic table, or proceed with the answer you got?
Hello po. It is not necessarily na sundin 'yung oxidation state na nasa periodic table of elements because there will be instances talaga na 'yung oxidation state e nakadepende sa given compound
Good eve, sir!!! Can a redox reaction occur spontaneously in a completely closed system with no external energy or catalysts? If the answer is yes, kindly provide examples to deepen our understanding.
Good eve! Yes, a redox reaction can occur spontaneously in a closed system without external energy or catalysts, as long as the reaction is energetically favorable. A common example is the rusting of iron. When iron reacts with oxygen and moisture, a redox reaction happens naturally, forming iron oxide (rust). Another example is when zinc reacts with copper sulfate in a solution, causing the zinc to oxidize and copper to reduce, forming solid copper. These reactions happen because the materials involved naturally transfer electrons to reach a more stable state.
What are some real-world examples of redox reactions?
21:20 sa step two poser of assigning oxidation states for the products, if the equation was already 2x+3(-2)=0 naging 2x-6=0 then paano naging 2x=6 diretso na po ba?
iipag hihiwalay po kasi yung literal coefficient and numerical coefficient. kaya po from 2x-6=0 to 2x=6. kasi 2x is the literal coefficient so remain sa left part of equation, then yung six (numerical coefficient) ililipat mo to the right so from -6 magiging +6 na siya kasi inilipat mo. kaya po ganun :))
moreover, 2x=6 is hindi pa pwede na ma determine yung oxidation state. so idivide mo both sides by 2 para macancel yung numerical sa literal coefficient. so ang magiging sagot (yung oxidation state) is x=+3
On the ion electron method, step 3 states that if the oxidation number increases by 1, then add one e, then what if it increases by more than just 1? Are you going to still add ONE e? Or more than that?
If the oxidation number increases by more than just 1 in the ion-electron method, you will need to add the corresponding number of electrons to balance the change.
How does redox reaction can differ from other types of chemical reactions?
In the context of the ion-electron method, why is it necessary to balance the electrons for both oxidation and reduction half-reactions?
In the ion-electron method, balancing electrons for both half-reactions is necessary because the total number of electrons lost in the oxidation half-reaction must exactly equal the number of electrons gained in the reduction half-reaction . This means that the total number of electrons in the reaction stays the same ,they are not lost or gained.
How the physical state of substances like the solid, liquid, gas, and aqueous solution affects the redox reaction?
The physical state of a substance-solid, liquid, gas, or aqueous solution-significantly influences redox (reduction-oxidation) reactions by affecting the rate, mechanism, and efficiency of electron transfer. In solids, surface area and the ability to donate or accept electrons play a key role, while in liquids, the solvent’s ability to dissociate ions impacts the reaction. Gases, due to their high kinetic energy and diffusion, facilitate fast reactions, and aqueous solutions, particularly water, support ion exchange and electron transfer.
Addition to my question regarding the exemption of some compound, can you state some reasons why may exemptions?
Hello po kaya po may exepmtions to some compound because of their chemical reactions po
Sir What is the fundamental principle of balancing redox reactions using the ion-electron method?
The fundamental principle of balancing redox reactions using the ion-electron method is that the number of electrons lost during oxidation must equal the number of electrons gained during reduction.
Kindly explain the difference between the two methods.
Oxidation Number Method
This method involves tracking changes in oxidation states to balance redox equations.Ion-Electron Method (Half-Reaction Method)
This method separates the oxidation and reduction processes into two half-reactions, balances them individually, and then combines them.
What are the redox properties of lanthanides and actinides? Does their chemical properties makes them complicated in this context?
Hello po. For me, lanthanides and actinides elements po does not make the equation complicated in redox reaction kasi like any other elements, they have normal oxidation state naman if we will base it on the periodic element, unlike sa noble gases na talagang walang given oxidation state except kay Og element
Sa Lanthanides and actinides meron po silang different oxidation states, which makes their chemistry tricky. Sa Lanthanides mostly meron po silang +3 charge, but some can have +2. Actinides naman po can range from +3 to +6.Dahil po sa special electron setup and radioactivity, their reactions are harder to predict, making their redox behavior more complicated.
Can you provide po a simple, real-world example of a redox reaction that we encounter in everyday life?
What is the difference between a simple redox reaction and a reaction that involves a complex ion in terms of electron transfer and oxidation states?
In a simple redox reaction, electrons are transferred between two species, with one being oxidized (losing electrons) and the other reduced (gaining electrons). The changes in oxidation states are straightforward and typically involve individual atoms or simple ions.
How do you determine the change in oxidation states for each element in a redox reaction
To find oxidation state changes in a redox reaction, start by balancing the chemical equation. Then, assign oxidation numbers to each atom, following rules like alkali metals (+1), alkaline earth metals (+2), halogens (-1), oxygen (-2), and hydrogen (+1). Next, compare oxidation numbers before and after the reaction to identify which atoms are oxidized (increased number) and reduced (decreased number).
How do oxidation and reduction work in living things, like how cells breathe and plants make food?
In living things, oxidation and reduction are vital for processes like breathing and making food. In "cellular respiration", cells break down glucose (sugar) to get energy. During this, glucose "loses electrons" (oxidized), and oxygen "gains electrons"(reduced) to form water, releasing energy the cell uses. In "photosynthesis", plants use sunlight to convert carbon dioxide and water into glucose (food) and oxygen. Here, water "loses electrons"(oxidized) to produce oxygen, and carbon dioxide "gains electrons" (reduced) to form glucose. These processes, powered by oxidation and reduction, help cells breathe and plants create food.
Can oxidation and reduction take place alone? Why or why not?
Sir, why is it necessary to add ions when balancing this redox reaction in an acidic medium, and what role do they play in maintaining charge neutrality?
In an acidic medium, adding ions, particularly H⁺ (hydrogen ions), is essential for balancing redox reactions. These ions help maintain charge neutrality and ensure that the reaction is mass-balanced. When electrons are transferred in redox reactions, H⁺ ions are often required to balance the charge, particularly when elements are reduced (gain electrons) or oxidized (lose electrons). Additionally, in an acidic medium, H⁺ ions combine with oxygen atoms to form water (H₂O), which helps balance the number of atoms in the reaction. The inclusion of electrons ensures that the number of electrons lost in oxidation equals the number gained in reduction, further preserving charge balance. Overall, these ions are crucial for achieving both mass and charge balance in the redox equation.
Goodevening sir, sir How do you determine whether a reaction is a redox reaction?
You need to follow the step.
If changes in oxidation states and electron transfer are observed, the reaction is a redox reaction.
For exmple
Na 0 to +1 ( mean oxidizing )
Na +1 to 0 ( reduced
to check if a reaction is a redox reaction, look for electron transfer. If one substance loses electrons (oxidized) and another gains electrons (reduced), then it's a redox reaction.
Why is the transfer of electrons important in a redox reaction, and how does it connect the processes of oxidation and reduction?
Hello po. It is important po because if we go back to the definition of redox reaction, it involves transfer of electrons from a chemical substance to another. Meaning, substances cannot undergo redox reaction without transferring and accepting electrons in the process kasi we won't know which substance undergoes oxidation or reduction kung hindi natin malalaman kung ano 'yung nag bawas and nag accept ng electrons.
How do you determine the oxidation state of an atom in a complex ion, especially when the metal has multiple oxidation states?
To determine a metal's oxidation state in a complex ion we calculate the total charge contributed by the ligands. Then assign an oxidation state to the metal that when combined with the ligand charges equals the overall charge of the complex ion
How does the concept of electron transfer differ between redox reactions and other types of chemical reactions?
In redox reactions, electron transfer is the key process where one substance loses electrons (oxidation) and another gains electrons (reduction). In other types of chemical reactions, such as acid-base or precipitation reactions, no electrons are transferred; instead, other processes like proton transfer or ion exchange occur.
In redox reactions, electron transfer is the key process where one substance loses electrons (oxidation) and another gains electrons (reduction). In other types of chemical reactions, such as acid-base or precipitation reactions, no electrons are transferred; instead, other processes like proton transfer or ion exchange occur.
Another question sir, how can we see whether a given reaction will be spontaneous based on the oxidizing and reducing agents involved?
Hii Sir, is it possible for an element to undergo oxidation without forming an ion? If so, could you explain how it works?
When we say an element is in its 'elemental state,' what is its oxidation state and why?
For the step 4 in balancing Redox reaction, is it applicable to ALWAYS equate in opposite (reactant)?
YES
If in a redox reaction, the oxidation state of an element increases, what does this imply about the element's role, and how does it affect the reaction as a whole?
Hello po! When an element's oxidation state goes up in a redox reaction, it’s being oxidized-basically, it’s losing electrons. This element is the reducing agent because it gives away electrons to help another element get reduced. Redox reactions are all about this teamwork: one loses, one gains, and together they make the reaction happen.
How does the concept of electron transfer help balance a redox reaction using oxidation states?
Redox reactions involve electron transfer, where oxidation is the loss of electrons and reduction is the gain of electrons. To balance these reactions we ensure equal electron transfer between oxidizing and reducing agents, by using methods like the oxidation number or ion-electron methods.
In the oxidation method, individual elements in their elemental form have a charge of 0. Why do elements have charges in the ion-electron method?
Hello po. In the Ion-Electron Method, elements appear to have charges because we focus on oxidation states and electron transfers, not their elemental form. Sa ion electron method po kasi it tacks the electrons transferred during the reaction and assigns charges to elements or ions to reflect their new states after gaining or losing electrons.
Hydrogen peroxide is commonly used as a disinfectant in healthcare. How does it act as both an oxidizing and reducing agent?
Hi! Good eve! Hydrogen peroxide can act as both an oxidizing and reducing agent due to the presence of oxygen and because it can gain and lose electron. It can act as an oxidizing agent by gaining electrons and being reduced to water or H20 in a single process. It can operate as a reducing agent in another reaction by losing electrons and oxidizing to oxygen gas (02). Because of its dual function, hydrogen peroxide is a substance that can be used for a variety of purposes, including disinfection.
What are the most reactive elements prone to oxidation?
The most oxidation-prone elements are alkali metals (like sodium and potassium) and alkaline earth metals (like calcium and magnesium). They lose electrons easily, making them super reactive, especially with oxygen!
What about reaction with complex ions or polyatomic ions?
What is the significance of the half-reaction method in balancing redox equations?
The half-reaction method is a vital technique for balancing redox equations, as it breaks the reaction into two parts: one for oxidation and one for reduction. This approach simplifies the process by clearly separating the electron loss (oxidation) and gain (reduction), ensuring that both mass and charge are conserved. By balancing the half-reactions individually, it guarantees that the number of electrons lost during oxidation equals the number of electrons gained during reduction. Additionally, the method is adaptable to both acidic and basic solutions, making it versatile for various reactions. Overall, the half-reaction method provides a systematic and effective way to balance complex redox equations, illustrating the electron transfer process and ensuring the accuracy of the final equation.
What are the primary rules for assigning oxidation states to elements in a compound?
The primary rules for assigning oxidation states to elements in a compound ensure consistency in understanding electron transfer during chemical reactions. Elements in their pure form always have an oxidation state of 0, and monoatomic ions equal their charge. Oxygen usually has an oxidation state of -2, except in peroxides and with fluorine. Hydrogen is typically +1, except when bonded with metals in hydrides, where it is -1. The sum of oxidation states in a neutral compound is 0, and in a polyatomic ion, it equals the ion’s charge. Fluorine always has an oxidation state of -1, while other halogens typically have an oxidation state of -1, unless bonded to oxygen or fluorine, which can give them positive oxidation states. These rules help assign oxidation states systematically, enabling the understanding and balancing of redox reactions.
How would you know whether a redox reaction is taking place in an alkaline or neutral medium?
Hello! Based from what I learned from the internet, analyzing the presence of H+ or OH- ions in the balanced equation can determine the medium of the reaction.
how can you identify the substance being oxidized and the substance being reduced in a given chemical equation?
Assign an oxidation number for each element. Oxidatio numbers are a way of keeping track of how many electrons an atom has gained or lost during a reaction.
-Telan, Ma. Rielle
When an element changes during a redox reaction, how does its oxidation state change? Can we figure out if something is getting oxidized or reduced by looking at this?
We can say that an element is being oxidized if there is a loss of electron and an element is being reduced if it gains an electron. We can observe this by identifying the changes in the oxidation state between the reactant and the product
Can you briefly explain step 5 in Ion electron method? Bakit po may x6 yung Fe?
Sir, does oxidation gain electron?
Hi! No, because, oxidation is the loss of electrons and reduction is the gain of electrons.
How can you determine that the equation will use Oxidation number method in Balancing its redox reaction instead of Ion electron method and vice versa?
Use the Oxidation Number Method for simpler reactions involving changes in oxidation states. Use the Ion-Electron Method for more complex reactions, especially in acidic or basic solutions, where balancing electrons and charges is critical.
Sir pano po if hindi po balance yung chemical equation?
what is the fundamental difference between oxidation and reduction in a chemical reaction?
Why do redox reactions happen in things like rusting iron? How can we stop or slow them down?
Rusting is a redox reaction where iron reacts with oxygen and water. so to prevent rusting we must isolate iron from water and oxygen by applying protective coatings
In balancing po, why is it crucial to balance the reactant with the product?
We balance chemical reactions to adhere with the law of conservation of mass, which states that matter can not be created or destroyed in a chemical reaction.
Hello po! it's important to balance the reactants and products in order to follow po yung rules of mass and charge conservation (based on what I learned online). This means po that the number of atoms and the total charge should be the same on both sides. Remember po that a balanced chemical equation also provides an estimate on how many reactants are needed for a reaction.
Do you think noble gases are allowed in redox reaction even though most of them doesn't have oxidation state? That maybe there will be an exemption to the rule since the elements Rn and Og have oxidation state?
Ranell: Noble gases rarely participate in redox reactions dahil stable sila with full valence shells, pero exceptions exist for heavier noble gases like radon (Rn) and oganesson (Og). Radon can form compounds like RnF₂, showing an oxidation state of +2, while Og is predicted to have oxidation states (+2 or +4) theoretically. However, dahil sobrang unstable and radioactive nila, their involvement in redox reactions is highly limited and not practical in most scenarios.
hello po
noble gases are usually chill lang, like super stable sila kasi full na yung valence shells nila, kaya they don’t usually join redox reactions. Pero, wait lang, I think po may exemptions talaga. Si radon (Rn) and oganesson (Og), they can have oxidation states minsan kasi they’re heavier noble gases. Iba yung energy levels nila, so parang medyo kaya nilang mag-react in some special cases. Pero it’s super rare ha! So, in general po noble gases are like, “No thanks, I’m good,” sa redox, pero pwede silang sumama minsan kapag special occasion hahaha
What factors affect the rate of redox reactions?
The rate of redox reactions depends on factors like the nature of reactants, their concentration, temperature, surface area, use of catalysts, pressure (for gases), and pH. These affect how quickly particles collide and react.
Why is water both an oxidizing and a reducing agent in redox reactions, and what are examples of each behavior?
Water can act as both an oxidizing agent (accepting electrons) and a reducing agent (donating electrons):
• As an oxidizing agent:
In the reaction with sodium:
2Na + 2H20 → 2NaOH + H2
Water is reduced to hydrogen gas.
• As a reducing agent:
In the reaction with chlorine gas:
Cl + H20 - HC + HOCL
Water is oxidized to hypochlorous acid
How can you determine na kailangan mong ibalance yung equation?
The oxidation state of chlorine in NaCl changes when it reacts with fluorine. What is the change in oxidation state of chlorine during this reaction, and what type of reaction is this?
In the reaction between sodium chloride (NaCl) and fluorine (F₂), chlorine undergoes oxidation, while fluorine undergoes reduction. The reaction is as follows:
2NaCl+F²→2NaF+Cl²
Sir what if the elements involved in the compounds were both having a lot of oxidation state what will be the x sir?
Hii! I guess it will be a matter of trial and error sa pagkuha ng oxidation state ng both elements. I also searced online and it stated that the oxidation states of elements involved in a compound that has several possible oxidation states can be determined by their electronegativity, structure, and bonding but I can't find a concrete example so yeah haha:)
In carbon dioxide (CO₂), carbon has an oxidation state of +4. How do the oxidation state rules explain why carbon has this positive value in this compound?
@@NicoleBeverlyDeza Oxygen has an oxidation state of -2. This is a general rule that applies in most compounds, including CO2. The sum of the oxidation states of all atoms in a neutral molecule is zero. CO2 is a neutral molecule, so the sum of the oxidation states of carbon and oxygen must equal zero.
Let's denote the oxidation state of carbon as "x". We can set up the equation:
x + 2 (-2) = 0
Solving for x:
x + 2 (-2) = 0
x - 4 = 0
x = +4
It became +4 (from -4) because nailipat sya from the left side to the right of the equation and there is a rule na mapapalitan din ang sign nya if ililipat to the other side of the equation.
Therefore, the oxidation state of carbon in CO2 is +4. This positive value indicates that carbon has lost electrons, which is characteristic of oxidation.
hi sir, Miles! How do we assign oxidation states po to elements in a compound, especially in complex molecules po sir?
Good evening! Can you explain po how redox reactions are applied in our everyday lives? I’ve heard about their role in things like rusting and batteries, but could you provide a more detailed example?
Sir, the OIL RIG mnemonic, is it always the case that the element losing electrons is the reducing agent?
In my own understanding, I think Yes. Because in order for the reducing agent to reduce other reactants, it MUST DONATE its electron which means it loses electron and by definition, it undergoes the oxidation reaction and oxidation in OIL rig is loss of electron
Hello! I believe po that the mnemonic is perfectly clear, and yes it is always the case talaga that the element losing electrons is the reducing agent. This is because the reducing agent is the one that donates electrons to another substance, causing it to be reduced. When the reducing agent loses electrons, nag-o oxidize siya. Therefore, the element losing electrons is called the reducing agent because it helps reduce another element by giving up its electrons.
Hello guys! What is the importance of the ion electron method or half reaction method in balancing equations?
Hello po! The ion-electron method (also known as the half-reaction method) is important in balancing redox reactions, especially complex ones, because it focuses on electron transfer. Redox reactions fundamentally involve the transfer of electrons. This method explicitly separates the overall reaction into two half-reactions: the oxidation states which loses electrons and the reduced
continuation because I accidentally touch the send button hahaha Redox reactions fundamentally involve the transfer of electrons. This method explicitly separates the overall reaction into two half-reactions: the oxidation reaction which loses electrons and the reduction reaction that gains electrons
hi guys! can you further explain if how the concept of oxidation states helps in balancing redox reactions?
Oxidation states help us track electron transfers in redox reactions. If oxidation state increases, na-oxidize siya (loses electrons). If it decreases naman po na-reduce siya (gains electrons). By checking these changes, you can balance the number of electrons lost and gained. This ensures the reaction is balanced both in charge and mass, making the process organized and systematic.
Hi mich, yung oxidation states kasi ay tumutulong para makita kung anong element ang oxidized (tumaas ang oxidation state) at kung alin ang reduced (bumaba ang oxidation state). Kapag alam na kasi ito , madali nang balansehin ang redox reaction gamit ang bilang ng electrons na nawala at nakuha para sure na pantay ang mga elements at charge sa mag kabilang equation.
Oxidation states tell us how many electrons an atom loses or gains in a reaction. They help us see which atoms lose electrons (oxidized) and which gain them (reduced). In a redox reaction, the number of electrons lost by one atom must equal the number of electrons gained by another. By using oxidation states, we can balance the reaction and make sure the atoms and charges are correct.
In the last example (example in the Half Reaction method) a 6e suddenly appeared, what is the reason behind it?
By the definition of sir miles, the 6e there accounts for the traansfer of electron REQUIRED to reduced 2 Cr atoms from +6 to +3. Firstly, we determine the number of change in oxidation number, as we can see, it decreases by 3 oxidation number. And if we look at the Cr atom at the reactant side, it has 2 atoms. So what we need to do is to multiply the 2 Cr atoms from the reactant side to the number of change in oxidation number of 3 which gives us 6.
How can you tell if a reaction is a redox reaction by looking at the chemical equation?