Sir this video is very helpful. I was having so many doubts that how these Polyatomic ions are formed..... How they are different from compounds...... And many more. But after watching your video all my doubts are clear. Thank you so much sir for this much effort.
Crash Chemistry Academy ohhhh so just like when oxygen gains 2 electrons to form an Anion with a full octet, so does OH but with 1! Thank you so much for this video I’ve watched like 3 others that didn’t explain it well at all ;)
@Jake B it depends on the circumstances of the reaction. In particular, if the reaction takes place in air, such as the exchange of electrons between sodium and chlorine, then yes, you get a compound, in this case NaCl. The circumstances that lead to polyatomic ion formation will also lead to formation of a compound, which primarily occurred in the early stages of earth's formation, resulting in polyatomic ions in various types of rock. If the electron exchange takes place in water, then there is only a change in charge, rather than the formation of a compound, since ions are soluble in water. Hope that makes sense!
The best video I've watched so far about to issue, thank you so much sir! As I read in the comments section, you said those extra electrons are gained during reactions and from other atoms/molecules willing to give/take electrons Does that mean, the only way to make these molecules to exist is to separate them compounds? and they do not exist in the nature all alone? For instance can we say that, for a SO4 to form one possible way is to dissolve H2SO4? Also 1:59 why is the Oxygen on the left and said is with 3 pairs instead of 2 pairs and 2 single electrons?
In general ions do not exist independently, they exist bonded to some oppositely charged ion, the general term for which is salt. So you are correct in your assumption, polyatomic ions do not exist on their own unless dissolved in water. The SO4 ion is somewhat common in naturally occurring compounds (salts), but has become far more common for industrial purposes, which H2SO4 is by far the most prevalent, and yes, dissolving H2SO4, will release SO4 ions (more likely HSO4 ions). Any soluble salt containing a polyatomic ion (acids are not salts) will release its ions when dissolved in water, and we can extend that to all soluble salts whether or not a polyatomic ion is present. For your second question, the two electrons in the bond do not have to come from the two different atoms, they can both come from the same atom. These are called coordinate bonds. When atoms are bonding, the electrons will go to the most energetically favorable position, and that means valence electrons rearranging from their atomic orbital arrangement to the more favorable bonding arrangement.
That would certainly be a possibility, but with the same result, that of all atoms having an octet. As long as you keep track of the amount of electrons added so that all atoms have an octet, it does not matter which atoms get the electrons if there is more than one possibility.
I have a question. In my textbook it says that many polyatomic ions are formed by the loss of hydrogen ions from oxyacids. For example nitric acid which is HNO3, in water it dissociates into H+ and NO3- Is this case? Are there more than one process in forming polyatomic ions? And how’s this different from what you mentioned in the video?
The process in the video concerns what happens chemically in order for the ion to form, which is a reaction in which there is a substance willing to give up electrons during a reaction with atoms forming the negative polyatomic ion. The formation of the ion requires that it interacts with something that will give electrons to it. After such a reaction, the negative ion is free to bond with either positive ions, or as with oxy acids, form a bond with one or more hydrogens. In both of these cases, when the bonded substance is dissolve in water, the two ions break apart (dissociate) thus releasing the poly atomic ion. The same goes for oxy acids where, when dissolved in water, the H is released as H+, leaving the poly atomic ion on its own in the water. Hope that makes sense!
I have a question about the extra electron. If the polyatomic ion does gain an extra electron or however many, wouldn't it become negatively charged and the other element positively charged, and they attract? If so, would the element that gives the polyatomic ion its extra electrons be bound to it, and the new ionic compound formed be completely based on the element which gave the electrons to the polyatomic? For ex, a polyatomic CO3 gaining 2 electrons from Calcium, then CO3 has a 2- and Ca has a 2+, then it would be CaCO3. So that Calcium, the element which gave the electrons, dictates the outcome.
Everything you are saying is correct, except the last sentence I think could be worded better-- what dictates the outcome is the amount of charge. For example if sodium were giving electrons to create CO3 2-, then the resulting compound is Na2CO3. Or if aluminum was donating electrons, the compound would be Al2(CO3)3. It is just a matter of balancing charge.
how polyatomic ions are formed?i mean in CO3- , why we dont have CO2 (how this bounch of 3O AND 1C came together) ?also can polyatomic ions found free in nature? thx in advandace
Good question, hard to answer, other than saying that atoms seek to situate themselves in the lowest potential energy bonding situation given the environment they are in. CO2 is a very low PE bonding situation. CO3^2- likely has higher PE especially given that it usually is found in compounds that are not soluble in water, so one can assume that CO3 2- has a lower PE in a compound than solvated by water. Which brings us to your next question, ions in general do not exist free in nature except as aqueous ions, otherwise they are bound up in compounds due to the attraction of their charge.
so poly/ions "tend to react"..am i right? also how we have 3 oxygens?oxygen is a diatomic element..i mean where the other oxygen of 1 couple (from the molecule of oxygene) goes?
diatomic oxygen is not stable, it reacts with every other element except the noble gases, so oxygen reacting with carbon allows oxygen to go to a lower PE. Yes, ions, due to their charge, will bond to oppositely charged particles.
All bonds form in chemical reactions, which normally include changes in where electrons are (called "oxidation reduction"). So 'extra' electrons will be picked up during the chemical reaction that forms the polyatomic ion. Those electrons are given up by other atoms/compounds that become more stable by losing electrons.
YES! excellent question. So Chlorine can bond with one oxygen (the 1- hypochlorite ion), two oxygens (the 1- chlorite ion), three oxygens (the 1- chlorate ion) or four oxygens (the 1- perchlorate ion). The more oxygens, the more unstabe (lower bond energy) probably due to steric hindrance as the oxygens crowd around the chlorine and produce greater repulsions as they push up against each other. The hypochlorite and chlorite ions are more stable, likely hypochlorite being the most stable-- you can easily find bond energies on the internet. So chlorates and perchlorates are great oxidizers.
In the chlorite ion , the right hand side oxygen atom has 7 e - but in order to complete it's octet we add one more e- , MY DOUBT is where is that e- coming from out of nowhere in it's surrounding atom???
Electrons are exchanged during chemical reactions. A polyatomic ion forms in a chemical reaction, so it would obtain electrons from another species that gets stable by giving up electrons.
Sir I am so thankful of this video, it animated hoe polyatomic ions are covalently bonded. Moreover this video tells the way of finding valency.
THANKYOU SO MUCH! YOURE THE BOMB!
Sir this video is very helpful. I was having so many doubts that how these Polyatomic ions are formed..... How they are different from compounds...... And many more. But after watching your video all my doubts are clear.
Thank you so much sir for this much effort.
Thank you very much sir
THANK YOU!!!
you do not know how much my understanding was twisted, more than barbed wire; but this made everything crystal clear. thanks sooo much ❤❤❤❤❤❤❤
Great!!
Help full man
Great but from where that one extra electron in OH came from ?
Any extra electrons would be transfered to the OH or any polyatomic ions during a chemical reaction
Ooo thanks...
Crash Chemistry Academy ohhhh so just like when oxygen gains 2 electrons to form an Anion with a full octet, so does OH but with 1! Thank you so much for this video I’ve watched like 3 others that didn’t explain it well at all ;)
Thank you so much!!!!💝
In the examples you used, where would the last electrons come from. Would they just appear out of nowhere?
The electrons would come from other atoms/compounds that are willing to give up electrons in the course of a chemical reaction.
Crash Chemistry Academy thank you for clearing that up! Great video
@Jake B it depends on the circumstances of the reaction. In particular, if the reaction takes place in air, such as the exchange of electrons between sodium and chlorine, then yes, you get a compound, in this case NaCl. The circumstances that lead to polyatomic ion formation will also lead to formation of a compound, which primarily occurred in the early stages of earth's formation, resulting in polyatomic ions in various types of rock. If the electron exchange takes place in water, then there is only a change in charge, rather than the formation of a compound, since ions are soluble in water. Hope that makes sense!
thank you so much, i have never seen such explanation about polyatomic ions
The best video I've watched so far about to issue, thank you so much sir!
As I read in the comments section, you said those extra electrons are gained during reactions and from other atoms/molecules willing to give/take electrons
Does that mean, the only way to make these molecules to exist is to separate them compounds? and they do not exist in the nature all alone?
For instance can we say that, for a SO4 to form one possible way is to dissolve H2SO4?
Also 1:59 why is the Oxygen on the left and said is with 3 pairs instead of 2 pairs and 2 single electrons?
In general ions do not exist independently, they exist bonded to some oppositely charged ion, the general term for which is salt. So you are correct in your assumption, polyatomic ions do not exist on their own unless dissolved in water. The SO4 ion is somewhat common in naturally occurring compounds (salts), but has become far more common for industrial purposes, which H2SO4 is by far the most prevalent, and yes, dissolving H2SO4, will release SO4 ions (more likely HSO4 ions). Any soluble salt containing a polyatomic ion (acids are not salts) will release its ions when dissolved in water, and we can extend that to all soluble salts whether or not a polyatomic ion is present.
For your second question, the two electrons in the bond do not have to come from the two different atoms, they can both come from the same atom. These are called coordinate bonds. When atoms are bonding, the electrons will go to the most energetically favorable position, and that means valence electrons rearranging from their atomic orbital arrangement to the more favorable bonding arrangement.
Great explanation
Thank you very much Sir 🙏🙏
very helpful
good explanation
Thank youuuuuuuuuuuu soooooooooooooooooooooooo muchhhhhhhhhhhhhhhhh
in the clorite ion, why notboth Oxygens share tow pairs? and the one elecfron goes to Cl?
That would certainly be a possibility, but with the same result, that of all atoms having an octet. As long as you keep track of the amount of electrons added so that all atoms have an octet, it does not matter which atoms get the electrons if there is more than one possibility.
how does a negative charge come on cyanideplz expain sir
Where does the additional electron come from?
Electrons are lost/gained in chemical reactions, so the polyatomic ion would gain an electron during its formation from whatever it is reacting with.
I have a question. In my textbook it says that many polyatomic ions are formed by the loss of hydrogen ions from oxyacids. For example nitric acid which is HNO3, in water it dissociates into H+ and NO3-
Is this case? Are there more than one process in forming polyatomic ions? And how’s this different from what you mentioned in the video?
The process in the video concerns what happens chemically in order for the ion to form, which is a reaction in which there is a substance willing to give up electrons during a reaction with atoms forming the negative polyatomic ion. The formation of the ion requires that it interacts with something that will give electrons to it.
After such a reaction, the negative ion is free to bond with either positive ions, or as with oxy acids, form a bond with one or more hydrogens. In both of these cases, when the bonded substance is dissolve in water, the two ions break apart (dissociate) thus releasing the poly atomic ion. The same goes for oxy acids where, when dissolved in water, the H is released as H+, leaving the poly atomic ion on its own in the water.
Hope that makes sense!
I have a question about the extra electron. If the polyatomic ion does gain an extra electron or however many, wouldn't it become negatively charged and the other element positively charged, and they attract? If so, would the element that gives the polyatomic ion its extra electrons be bound to it, and the new ionic compound formed be completely based on the element which gave the electrons to the polyatomic? For ex, a polyatomic CO3 gaining 2 electrons from Calcium, then CO3 has a 2- and Ca has a 2+, then it would be CaCO3. So that Calcium, the element which gave the electrons, dictates the outcome.
Everything you are saying is correct, except the last sentence I think could be worded better-- what dictates the outcome is the amount of charge. For example if sodium were giving electrons to create CO3 2-, then the resulting compound is Na2CO3. Or if aluminum was donating electrons, the compound would be Al2(CO3)3. It is just a matter of balancing charge.
My teacher linked this video to watch
how polyatomic ions are formed?i mean in CO3- , why we dont have CO2 (how this bounch of 3O AND 1C came together) ?also can polyatomic ions found free in nature? thx in advandace
Good question, hard to answer, other than saying that atoms seek to situate themselves in the lowest potential energy bonding situation given the environment they are in. CO2 is a very low PE bonding situation. CO3^2- likely has higher PE especially given that it usually is found in compounds that are not soluble in water, so one can assume that CO3 2- has a lower PE in a compound than solvated by water. Which brings us to your next question, ions in general do not exist free in nature except as aqueous ions, otherwise they are bound up in compounds due to the attraction of their charge.
so poly/ions "tend to react"..am i right? also how we have 3 oxygens?oxygen is a diatomic element..i mean where the other oxygen of 1 couple (from the molecule of oxygene) goes?
diatomic oxygen is not stable, it reacts with every other element except the noble gases, so oxygen reacting with carbon allows oxygen to go to a lower PE. Yes, ions, due to their charge, will bond to oppositely charged particles.
ty
hey I'm in grade 9 and these things are hard for me to grasp but I want to be a chemistry major. Is it possible for me to be one?
But the question is where do the electrons come from? the extra ones
All bonds form in chemical reactions, which normally include changes in where electrons are (called "oxidation reduction"). So 'extra' electrons will be picked up during the chemical reaction that forms the polyatomic ion. Those electrons are given up by other atoms/compounds that become more stable by losing electrons.
I have a question, why did that chlorine atom go for two oxygen atoms and not one oxygen atom
it would've still gotten 1- charge right?
YES! excellent question. So Chlorine can bond with one oxygen (the 1- hypochlorite ion), two oxygens (the 1- chlorite ion), three oxygens (the 1- chlorate ion) or four oxygens (the 1- perchlorate ion). The more oxygens, the more unstabe (lower bond energy) probably due to steric hindrance as the oxygens crowd around the chlorine and produce greater repulsions as they push up against each other. The hypochlorite and chlorite ions are more stable, likely hypochlorite being the most stable-- you can easily find bond energies on the internet. So chlorates and perchlorates are great oxidizers.
Is peroxide a polyatomic ions
Yes-- it has two atoms, so that makes it polyatomic.
In the chlorite ion , the right hand side oxygen atom has 7 e - but in order to complete it's octet we add one more e- , MY DOUBT is where is that e- coming from out of nowhere in it's surrounding atom???
Electrons are exchanged during chemical reactions. A polyatomic ion forms in a chemical reaction, so it would obtain electrons from another species that gets stable by giving up electrons.
@@CrashChemistryAcademy okay thanks
plz explain the structure of cyanide
triple bond with an added electron to complete the octets for a 1- charge.
that intro music is creepy af
u can teach betr