Oxidation/Reduction help?
S(s) + 6HNO3(aq) ---> H2SO4(aq) + 6NO2(g) + 2H2O(l) On left of arrow: S(s)=0 In HNO3: H = +1; O = -2; N = +5 On Right of Arrow: In H2SO4: H = +1; O = -2; S = +6 In NO2: O = -2; N = +4 In H2O: H = +1, O = -2 So, S is oxidized from 0 to +6 and N is reduced from +5 to +4
Oxidation and reduction in chemistry?
Since chloride is the more electronegative element, we assign its normal ionic charge of -1 each. The four chloride ions therefore have a total charge of -4. Since the net charge is -2, the Cu must have +2 to make it so.
Redox and Oxidation Help?
A. is a redox reaction,you could determine by using the lose or gain of oxygen, as you can see, FeO lose oygen and being reduced to Fe and CO gained an oxygen and being oxidized to CO2. B. isn't a redox reaction because there is no electron transfer between the molecules. C. is a redox reaction, Mg is being oxidised to Mg^2 due to the increase of oxidation number of it from 0 to 2.And you knew that if one release electron, another must receive it, therefore,the electron released is received by H3O^ ,and it is reduced to H2 . D. isnt a redox reaction because there is no electron transfer between each other,it is just a simply double displacement reaction. As we knew that equation B and D is not redox reaction,, we could ignore them at the questions below. 2) Iron is reduced..is true because it loses oxygen. Oxygen is oxidized is wrong because it is carbon atom being oxidised, not the oxygen. Hydrogen is reduced is true, because the oxidation number of Hydrogen atom is reduced from 1 to 0. 3) i)2 electrons are transferred to each iron ion is true because the oxidation number of Fe^2 decreases. from 2 to 0 ii)2 electrons are transferred from each magnesium ion is true because the oxidation number of Mg decreases from 0 to 2. Just remember the rule ,gain electron:being reduced. lose electron: being oxidised. If anything that I have said isnt clear, let me know, I will explain again.
Is this oxidation/reduction/redox?
a. magnesium is going from (0) to (+2) as a result it is oxidised because it loses electrons. reducing brokers are oxidised so a) is fake b.Si in SiCl4 is going from (+4) to (0). electrons are further to it as a result it is an oxidising agent so b) is actual. c. magnesium loses electrons as a result it is oxidised not decreased, consequently c) is fake d.SiCl4 constructive properties electrons as a result it is decreased, consequently d) is actual e.there's no replace of electrons as a result e) is fake f.N is oxidised and O is decreased as a result f) is actual
Redox Reactions - Oxidation & Reduction Help!?
No no longer all reaction are redox. reaction between metals and non-metals are in basic terms redox reaction Redox ability alleviation and oxidation, it rather is the convenience or loss of electron forming and ionic bond. Oxidation=loss of electrons alleviation= benefit of electrons e.g.a rection between a nonmetal and metallic is primary as redox reaction. Metals are oxidized Non-metasl are decreased there is exchange in oxidation state. even with the shown fact that in the process non-metals there's a covalent bonding, electrons are no longer won or lost yet incredibly is shared. it is not a redox reaction. bear in recommendations : Redox could contain metals. Metals are resposible for any redox reaction
Oxidation is a process that an electron was taken from an atom.Reduction is the process that an chemical receive an election.Thus, an oxidation taking place without reduction means that the election need to actually leave the system (your round-bottom flask) without being catched.Thus, comparing to normal chemical reactions, the electron that has been "ejected" have to possess a huge amount of energy ("speed") to escape.How do we get huge amount of energy?Well, not that huge and uncontrolable ~~A field called radiochemistry studies the chemistry of radioactive meterials.Actually, in radiochemistry reduction without oxidation is much more common than oxidation without reduction, however, here is a famous example of it, which produce highly unstable [math]BrO_4^{2-}[/math]. There is no non-radiochemistry methods to produce [math]BrO_4^{2-}[/math] ion.
The basic differences between Oxidation and Reduction are :-Oxidation is the process of loss of electrons whereas Reduction is the process of gain of electrons.Oxidation can also be gaining of oxygen atoms whereas Reduction is loss of Oxygen atoms.Oxidation can also be loss of Hydrogen atoms but Reduction is the gain of Hydrogen atoms.Oxidation State increases when Oxidation occurs while Oxidation state decreases when Reduction occurs.Oxidation increases the positive charge of a chemical species but Reduction increases the negative charge of a chemical species.Oxidation occurs in Reducing agents while Reduction occurs in Oxidising agents.
Redox reactions are the reactions which involves both reduction and complementary oxidation process. Some common examples of redox reactions are -:Rusting of Iron :4 Fe + 3 O2 ————→ 2 Fe2O3Here, the Fe loses electrons and is oxidized from 0 to +2 valency and O gains electrons and is reduced from 0 to -2 valency.Photosynthesis :6 CO2 + 6 H2O ———→ in the presence of sunlight and chlorophyll ———→ C6H12O6 + 6 O2Here, O from H2O is oxidised from -2 to 0 valency and C from CO2 is reduced from +4 to 0 valency.Electrochemical Cell :Lets say we have a Cu-Zn electrochemical cell with Cu as cathode and Zn as anode.Something like this :As we know that Zn is higher up in the reactivity series than Cu so Zn will replace Cu ions from CuSO4 solution.So, the reaction would be :Zn + CuSO4 ——→ ZnSO4 + Cui.e. Zn from anode is going in solution and Zn ions are moving to CuSO4 solution and replacing Cu and pure Cu is deposited on cathode.Here, Zn is getting oxidized from 0 to +2 valency and Cu is getting reduced from 2+ to 0 valency.Hope these examples help.
There’s no oxidation without reduction, so it depends on what you’re looking at. If rusting means the formation of iron oxide from iron, then the iron is getting oxidized, in this case by oxygen which is how the process came to be called oxidation. But at the same time, the oxygen is being reduced.
Oxidation/reduction? (Redox reactions)?
No no longer all reaction are redox. reaction between metals and non-metals are in trouble-free terms redox reaction Redox ability alleviation and oxidation, that's the ease or loss of electron forming and ionic bond. Oxidation=loss of electrons alleviation= great thing approximately electrons e.g.a rection between a nonmetal and steel is prevalent as redox reaction. Metals are oxidized Non-metasl are decreased there is replace in oxidation state. although in non-metals there's a covalent bonding, electrons are no longer gained or lost yet rather is shared. that may no longer a redox reaction. undergo in suggestions : Redox could desire to contain metals. Metals are resposible for any redox reaction