THANKS! in my science book (NCERT class 10) there’s a line “Iron is not corroded even if zinc layer is broken/damaged) and this is the ONLY video in whole youtube that answered that question
One of the best explanation for a question like 'the galvanized article is protected against rusting even if the zinc coating is broken. Why and how?" thank you so much
If iron reacts with oxygen and forms iron oxide then zinc also reacts with oxygen and form zinc oxide then how does it help in preventing corrossion through sacrificial portection ,In the equation you have taken iron oxide and zinc, I think it should be zinc oxide.
This might be because.... Al displaced Fe from its compound and this displacement reaction is highly exothermic. The heat produced is sufficient to melt the metal
3:03 I’m wondering how does zinc displace iron in iron (III) oxide as iron (III) oxide is not in a solution where there are ions “floating” around. Since both zinc and iron (III) oxide are solids, how does zinc even displace/“kick out” iron?
In the sacrificial protection by zinc, both reactants are solid metals. The reaction involves solid zinc and solid iron as the cathode. The corrosion process takes place at the surface of the solid metals, and the electrons involved in the oxidation and reduction reactions are transferred directly between the solid metal surfaces. And for the reaction to take place , an electrolyte is needed (it is a solution which facilitates movement of ions), the air or moisture acts as an electrolyte and allows the reactions of solid fe and zn to take place
This video is a bit confusing but this is the video my teacher linked for the questions she added. Can someone just tell me how is galvanization done? what is galvanization?, and what is sacrificial protection?
i think galvanisation is just coating a layer of zinc to iron to prevent it from rusting. Sacrificial protection is basically using a more reactive metal and have contact with a less reactive metal so that the less reactive metal (iron in this case) won’t rust but the more reactive metal (zinc) would corrode. 👍👍
No, haven't you read the reactivity series? K Na Ca Mg Al Zn Fe Pb H Cu Hg Ag Au Zinc comes before iron in the reactivity series, thus it is more reactive than iron.
@@conceptofeverything8793 Zinc is more reactive than iron. The reasons are: • Zinc is a more electropositive element than iron. • Zinc has a bigger atomic size than that of iron and thus has more number of electrons. • The fact of having more elecetrons and a ‘d’ sub shell, gives zinc a lot of hybridisation possibilities than that of iron. Also, if we react ZnSO4 solution with Fe then no reaction will take place. But, if you react FeSO4 solution with Zn then the product will be ZnSO4 + Fe. Thus, zinc was able to displace iron from its salt solution, implying that it is more reactive than iron
@@abhi2082 Yeah but H is hydrogen. It sits where the alkali metals are on the periodic table, and all alkali metals are more reactive than iron, it seems so. Odd thing it is, to be honest. Also, on the electronegativity table, it sits higher than Ag. I mean, hydrogen can spontaneously combust, it's actually very reactive with oxygen; so not sure how they've measured the reactivity (unless it's reactivity with metals), but doesn't seem right. Unless they've measured it in the OH form, because metallic hydrogen hadn't been discovered just yet, AFAIK. I mean, besides partial evidence, I think. "In August 2018, scientists announced new observations[52] regarding the rapid transformation of fluid deuterium from an insulating to a metallic form below 2000 K. Remarkable agreement is found between the experimental data and the predictions based on Quantum Monte Carlo simulations, which is expected to be the most accurate method to date. This may help researchers better understand giant gas planets, such as Jupiter, Saturn and related exoplanets, since such planets are thought to contain a lot of liquid metallic hydrogen, which may be responsible for their observed powerful magnetic fields.[53][54] "
@@conceptofeverything8793 Bro, just because hydrogen sits near the alkali metals, doesn't mean that it is an alkali metal and has the same properties as them 💀. Also, the reactivity can't be determined by the periodic table. The reactivity can only be known by seeing the reactivity series. The reactivity series has been made by carrying out various reactions of metals and non metals with acids and bases, and displacement reactions done by scientists. The reactivity series is given below: Potassium *[MOST REACTIVE]* Sodium Lithium Barium Strontium Calcium Magnesium Aluminium Manganese Zinc Chromium Iron Cadmium Cobalt Nickel Tin Lead Hydrogen Antimony Bismuth Copper Mercury Silver Gold Platinum *[LEAST REACTIVE]* I have mentioned a shorter form of reactivity series in my first reply in this comment. You can check it out if you want And Yes, Hydrogen is more reactive than Ag (Silver). But it less reactive than Iron (Fe)
After iron get rusted, how can zinc atoms reach that area to reduce it back to iron again? is it mobile? only electrons r mobile so maybe they can go to the area where oxygen and water there and give oxygen the electrons she wants...then maybe oxygen become negatively charged and zinc on the neighborhood positively charged...and there would be electric field which make freely charged oxygen to fly to zinc ion and make the ionic bond with it.... hope my imagination is not too dump :(
@@ChemJungle if there is piece of iron rusted at some places, if i connect some zinc to it, do u think rust would be removed after some time? can zinc replace already bonded rust? or the protection is only before oxidation happen and cant be reversed? thank u.
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THANKS! in my science book (NCERT class 10) there’s a line “Iron is not corroded even if zinc layer is broken/damaged) and this is the ONLY video in whole youtube that answered that question
Same bro... Poora TH-cam chhan liya but answer nhi mila
SAME!!
Me too,got the answer from this video
I've been stuck on how zinc stops iron from rusting, and this video totally helped! Thx sooooo much!
This is a life-saver! You explain things absolutely perfectly, thank you!
You're welcome :)
One of the best explanation for a question like 'the galvanized article is protected against rusting even if the zinc coating is broken. Why and how?" thank you so much
Finally understood it. Thank you so much! lovely work!
I've finally understood it. Thanks
Thankyou thankyou very much 🙂😄
Thank you for this video i really needed this in preparation for my GSCEs
Amazingly simple, thank you.
Excellent explanation👌👌👌
Keep it up👍
Thankuuuuuuuuuuuu so much ma'am you're only who properly answer my question 😊😊😊
Very interesting video, helps me a lot in understanding how to restore my car properly
love your content
Sourav Singh Thaaaanks :)
magnificent
Nice content
It's helpful but I need more videos related to galvanizing like as addition of aluminium and nickel and how to produced of dross.
Hi Tariq - sorry this isn't on the syllabus that my students complete so there won't be a video on this :(
Thank you!
So good !
Your videos are very easy to follow :)
Glad to hear that!
Very well explained ma'am. Thank you.
Most welcome 😊
omggg i had a head ache trying to understand the topic thanks love!!!
Thank you so much😊😊
Thanks
Thanks, mam for these video 👍
“ Choose a job you love, and you will never have to work a day in your life."
thanks bruh fo real :]
h2+cl2->2hcl reprents which reaction
It has been wow
Well I used zinc spray paint and still have rust spots so how is that zinc doing the sacrificial protection?
If iron reacts with oxygen and forms iron oxide then zinc also reacts with oxygen and form zinc oxide
then how does it help in preventing corrossion through sacrificial portection ,In the equation you have taken iron oxide and zinc, I think it should be zinc oxide.
Let's say the zincoxide is formed but it's powder overtime ferroisoxide will form.
Can you tell me anti iron chemical name please?
Hi, I had a zinc based aluminum alloy (zamak 2) and treated with Fe/ Zn- Fe plating. The zamak material was fully melted. Can you explain it how ?
This might be because....
Al displaced Fe from its compound and this displacement reaction is highly exothermic. The heat produced is sufficient to melt the metal
3:03 I’m wondering how does zinc displace iron in iron (III) oxide as iron (III) oxide is not in a solution where there are ions “floating” around. Since both zinc and iron (III) oxide are solids, how does zinc even displace/“kick out” iron?
In the sacrificial protection by zinc, both reactants are solid metals. The reaction involves solid zinc and solid iron as the cathode. The corrosion process takes place at the surface of the solid metals, and the electrons involved in the oxidation and reduction reactions are transferred directly between the solid metal surfaces. And for the reaction to take place , an electrolyte is needed (it is a solution which facilitates movement of ions), the air or moisture acts as an electrolyte and allows the reactions of solid fe and zn to take place
This video is a bit confusing but this is the video my teacher linked for the questions she added.
Can someone just tell me how is galvanization done? what is galvanization?, and
what is sacrificial protection?
i think galvanisation is just coating a layer of zinc to iron to prevent it from rusting.
Sacrificial protection is basically using a more reactive metal and have contact with a less reactive metal so that the less reactive metal (iron in this case) won’t rust but the more reactive metal (zinc) would corrode. 👍👍
Can oxygen react with zinc and iron at the same time resulting in no displacement reaction ?
Shouldn’t Zinc be oxidised first?
Zinc is preferentially oxidised as it's more reactive
Maam what's your good name 😅?
But Zinc is less reactive than iron
No, haven't you read the reactivity series?
K
Na
Ca
Mg
Al
Zn
Fe
Pb
H
Cu
Hg
Ag
Au
Zinc comes before iron in the reactivity series, thus it is more reactive than iron.
@@abhi2082 H tho? Surprising. How come?
@@conceptofeverything8793 Zinc is more reactive than iron.
The reasons are:
• Zinc is a more electropositive element than iron.
• Zinc has a bigger atomic size than that of iron and thus has more number of electrons.
• The fact of having more elecetrons and a ‘d’ sub shell, gives zinc a lot of hybridisation possibilities than that of iron.
Also, if we react ZnSO4 solution with Fe then no reaction will take place. But, if you react FeSO4 solution with Zn then the product will be ZnSO4 + Fe. Thus, zinc was able to displace iron from its salt solution, implying that it is more reactive than iron
@@abhi2082
Yeah but H is hydrogen. It sits where the alkali metals are on the periodic table, and all alkali metals are more reactive than iron, it seems so.
Odd thing it is, to be honest. Also, on the electronegativity table, it sits higher than Ag.
I mean, hydrogen can spontaneously combust, it's actually very reactive with oxygen; so not sure how they've measured the reactivity (unless it's reactivity with metals), but doesn't seem right. Unless they've measured it in the OH form, because metallic hydrogen hadn't been discovered just yet, AFAIK.
I mean, besides partial evidence, I think.
"In August 2018, scientists announced new observations[52] regarding the rapid transformation of fluid deuterium from an insulating to a metallic form below 2000 K. Remarkable agreement is found between the experimental data and the predictions based on Quantum Monte Carlo simulations, which is expected to be the most accurate method to date. This may help researchers better understand giant gas planets, such as Jupiter, Saturn and related exoplanets, since such planets are thought to contain a lot of liquid metallic hydrogen, which may be responsible for their observed powerful magnetic fields.[53][54] "
@@conceptofeverything8793 Bro, just because hydrogen sits near the alkali metals, doesn't mean that it is an alkali metal and has the same properties as them 💀.
Also, the reactivity can't be determined by the periodic table.
The reactivity can only be known by seeing the reactivity series. The reactivity series has been made by carrying out various reactions of metals and non metals with acids and bases, and displacement reactions done by scientists.
The reactivity series is given below:
Potassium *[MOST REACTIVE]*
Sodium
Lithium
Barium
Strontium
Calcium
Magnesium
Aluminium
Manganese
Zinc
Chromium
Iron
Cadmium
Cobalt
Nickel
Tin
Lead
Hydrogen
Antimony
Bismuth
Copper
Mercury
Silver
Gold
Platinum *[LEAST REACTIVE]*
I have mentioned a shorter form of reactivity series in my first reply in this comment. You can check it out if you want
And Yes, Hydrogen is more reactive than Ag (Silver). But it less reactive than Iron (Fe)
After iron get rusted, how can zinc atoms reach that area to reduce it back to iron again? is it mobile?
only electrons r mobile so maybe they can go to the area where oxygen and water there and give oxygen the electrons she wants...then maybe oxygen become negatively charged and zinc on the neighborhood positively charged...and there would be electric field which make freely charged oxygen to fly to zinc ion and make the ionic bond with it....
hope my imagination is not too dump :(
The electrons being mobile is the key idea here. The electrons can move freely through the structure to form the most stable ions :)
@@ChemJungle if there is piece of iron rusted at some places, if i connect some zinc to it, do u think rust would be removed after some time? can zinc replace already bonded rust? or the protection is only before oxidation happen and cant be reversed?
thank u.
@@alaeddinredeem4570 yes it can