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in this video , we 're going to look at pairs of molecules and see if they relate to each other in any obvious way or maybe less than obvious way . so these first two right here , they actually look like a completely different molecules . so your gut impulse might be to say that these are completely different molecules... | and we can point to one of them because they really are the same compound . this is a meso compound . it has chiral centers . | why is a meso compound any different than an enantiomer ? |
in this video , we 're going to look at pairs of molecules and see if they relate to each other in any obvious way or maybe less than obvious way . so these first two right here , they actually look like a completely different molecules . so your gut impulse might be to say that these are completely different molecules... | just like the last one , it looks like it 's made up of the same things . you have these carbons , these carbons , these carbons and hydrogens up there . same thing over there . | can the atoms attached to the central carbons in example 3 and 4 not rotate freely ? |
in this video , we 're going to look at pairs of molecules and see if they relate to each other in any obvious way or maybe less than obvious way . so these first two right here , they actually look like a completely different molecules . so your gut impulse might be to say that these are completely different molecules... | i guess the best way to visualize it , imagine putting a mirror behind this molecule . if you put a mirror behind this molecule , what would its reflection look like ? so if you put a mirror behind it , in the image of the mirror , this hydrogen would now , since the mirror 's behind this whole molecule , this hydrogen... | you say the molecules are enatiomers which i see using the mirror , however if you just flip the molecule on the left out of the page and then back down , like you did in the first example with -- would n't you just end up with the same exact molecule as the one on the right ? |
in this video , we 're going to look at pairs of molecules and see if they relate to each other in any obvious way or maybe less than obvious way . so these first two right here , they actually look like a completely different molecules . so your gut impulse might be to say that these are completely different molecules... | but if you think about it , all you have to do is flip this guy over and you will get this molecule . these are the same molecules . so it is the same molecule . | but when you flip one of the molecules over , would n't you have the br now pointing at the pack of the page and the h now is in front ? |
in this video , we 're going to look at pairs of molecules and see if they relate to each other in any obvious way or maybe less than obvious way . so these first two right here , they actually look like a completely different molecules . so your gut impulse might be to say that these are completely different molecules... | they 're both c4h8o . so they have the same molecular formula . they 're made up of the same thing , so these are going to be isomers . | when we check enantiomers mirror put in front of molecular or side of molecular ? |
in this video , we 're going to look at pairs of molecules and see if they relate to each other in any obvious way or maybe less than obvious way . so these first two right here , they actually look like a completely different molecules . so your gut impulse might be to say that these are completely different molecules... | in this video , we 're going to look at pairs of molecules and see if they relate to each other in any obvious way or maybe less than obvious way . so these first two right here , they actually look like a completely different molecules . | what is the difference between stereorisomer and the same molecue ? |
in this video , we 're going to look at pairs of molecules and see if they relate to each other in any obvious way or maybe less than obvious way . so these first two right here , they actually look like a completely different molecules . so your gut impulse might be to say that these are completely different molecules... | even though we have two chiral centers , this is not a chiral molecule . it is the same thing as its mirror image . it is superimposable on its mirror image . it is superimposable on its mirror image . | how come the mirror image is not laterally inverted ? |
in this video , we 're going to look at pairs of molecules and see if they relate to each other in any obvious way or maybe less than obvious way . so these first two right here , they actually look like a completely different molecules . so your gut impulse might be to say that these are completely different molecules... | and it would n't be completely off , but we look a little bit closer , you see that this guy on the left has one , two , three , four carbons , and so does this guy on the right . it has one , two , three , four carbons . this guy on the left has two , four , six , seven , eight hydrogens . this guy on the right has tw... | are the 2 hydrogens , fluorine , and chlorine basically locked in place in these two molecules ? |
in this video , we 're going to look at pairs of molecules and see if they relate to each other in any obvious way or maybe less than obvious way . so these first two right here , they actually look like a completely different molecules . so your gut impulse might be to say that these are completely different molecules... | but they do n't look quite the same . are they mirror images ? well , no . | so that we ca n't rotate them in any way to superimpose the mirror images ? |
in this video , we 're going to look at pairs of molecules and see if they relate to each other in any obvious way or maybe less than obvious way . so these first two right here , they actually look like a completely different molecules . so your gut impulse might be to say that these are completely different molecules... | and over , here same thing . it 's a chiral carbon . and this has the same thing . | if a carbon has only three groups attached to it and they are all different , is it a chiral carbon or something else ? |
in this video , we 're going to look at pairs of molecules and see if they relate to each other in any obvious way or maybe less than obvious way . so these first two right here , they actually look like a completely different molecules . so your gut impulse might be to say that these are completely different molecules... | now , let 's see if they 're related in a more nuanced way . you could imagine putting a mirror behind . i guess the best way to visualize it , imagine putting a mirror behind this molecule . if you put a mirror behind this molecule , what would its reflection look like ? so if you put a mirror behind it , in the image... | in the case of the mirror behind the molecule , why does it not matter whether the hydrogen is on the left or on the right ? |
in this video , we 're going to look at pairs of molecules and see if they relate to each other in any obvious way or maybe less than obvious way . so these first two right here , they actually look like a completely different molecules . so your gut impulse might be to say that these are completely different molecules... | in this video , we 're going to look at pairs of molecules and see if they relate to each other in any obvious way or maybe less than obvious way . so these first two right here , they actually look like a completely different molecules . | is organic chemistry about amino acids and peptide chains ? |
in this video , we 're going to look at pairs of molecules and see if they relate to each other in any obvious way or maybe less than obvious way . so these first two right here , they actually look like a completely different molecules . so your gut impulse might be to say that these are completely different molecules... | and we can point to one of them because they really are the same compound . this is a meso compound . it has chiral centers . | is there no shortcut using cahn-ingold nomenclature to determine if a meso compound is present ? |
in this video , we 're going to look at pairs of molecules and see if they relate to each other in any obvious way or maybe less than obvious way . so these first two right here , they actually look like a completely different molecules . so your gut impulse might be to say that these are completely different molecules... | now , what is this one over here in blue ? just like the last one , it looks like it 's made up of the same things . you have these carbons , these carbons , these carbons and hydrogens up there . | i thought there was some trick , like , `` if every stereocenter switches ( goes from r to s ) '' then its meso , or like `` every except one stereocenter switches '' -- or is that just a trick to determine enantiomer vs. diastereomer ? |
in this video , we 're going to look at pairs of molecules and see if they relate to each other in any obvious way or maybe less than obvious way . so these first two right here , they actually look like a completely different molecules . so your gut impulse might be to say that these are completely different molecules... | in this video , we 're going to look at pairs of molecules and see if they relate to each other in any obvious way or maybe less than obvious way . so these first two right here , they actually look like a completely different molecules . so your gut impulse might be to say that these are completely different molecules... | or should we base the judgment that when we see different 3d molecules we assume they are not the same ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | so the oxidation state on the lithium here is a positive 1 . and the oxidation state on the hydrogen here is a negative . so just , once again , i really want to make sure we get the notation . | what is the oxidation state of hydrogen in acids ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | it has no charge . similarly , hydrogen , plus 1 oxidation state ; oxygen , negative 2 oxidation number or oxidation state -- you add those two together , you have a negative 1 total charge for the hydroxide anion , which is exactly the charge that we have right over there . | is the oxidation state for groups 15 , 16 , and 17 are not always -3 , -2 , and -1 right ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | and actually , let me just draw that , because it 's fun to think about it . so this is a situation where oxygen typically has -- 1 , 2 , 3 , 4 , 5 , 6 electrons . and when it 's water , you have 2 hydrogens like that . | and are groups 1 and 2 always +1 +2 ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | now , we could keep going . if we were to go right over here to the group 5 elements , typical oxidation state is negative 3 . and so you see a general trend here . | what is the oxidation state for group 4 elements ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | and you could say , well , if we 're forced to , we could say -- if we 're forced to think about this is an ionic bond , we 'll say it fully gains two electrons . so we 'll have an oxidation state of negative 2 . and once again , the notation , when you do the superscript notation for oxidation states and ionic charge ... | do group 6 elements always carry a -2 oxidation state ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . | i always thought hydrogen was part of the alkali metals , so why does he say it can be a halogen ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | if we move over one group to the left , group 6 -- and that 's where the famous oxygen sits -- we already said that oxidizing something is doing to something what oxygen would have done , that oxidation is taking electrons away from it . so these groups are typically oxidized . and oxygen is a very good oxidizing agent... | are n't there only 8 groups max ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | if you had to pretend this was n't a covalent bond , but an ionic bond , you 'd say , ok , then maybe this hydrogen would fully lose an electron , so it would get an oxidation state of plus 1 . it would be oxidized by the oxygen . and that the oxygen actually has fully gained one electron . | is the oxidization number of oxygen between h2o and oh- the same ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | now , let 's give an example where hydrogen plays the other role . let 's imagine hydroxide . so the hydroxide anion -- so you have a hydrogen and an oxygen . | so is a hydroxide ion ionic or covalent ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | but if we look at the alkali metals , the group 1 elements right over here , we 've already talked about the fact they 're not too electronegative . they have that one valence electron . they would n't mind giving away that electron . | can one find ions in nature ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | and then you have that other covalent bond to the other hydrogen . and now this hydrogen is now just a hydrogen proton . this one now has a negative charge . | how does oxygen just 'nab ' that electron and 'ditch ' the proton/hydrogen ion ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | so you could kind of view it kind of like an alkali metal . but in theory , it could have been put here on the periodic table as well . you could have put hydrogen here , because hydrogen , in order to complete its first shell , it just needs one electron . | why are the two slots empty in the periodic table ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . | what is a molecular compound ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | it has no charge . similarly , hydrogen , plus 1 oxidation state ; oxygen , negative 2 oxidation number or oxidation state -- you add those two together , you have a negative 1 total charge for the hydroxide anion , which is exactly the charge that we have right over there . | i 'm having a hard time understanding this ... how can an element have more than one oxidation number ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . | i always thought hydrogen was part of the alkali metals , so why does he say it can be a halogen ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | and actually , let me just draw that , because it 's fun to think about it . so this is a situation where oxygen typically has -- 1 , 2 , 3 , 4 , 5 , 6 electrons . and when it 's water , you have 2 hydrogens like that . and then you share . | in the video does n't there need to be 2 hydrogens in order for the charge in the oxygen to be 2- ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | there are other things that could happen . but this is a typical rule of thumb that they 're likely to want to gain an electron . if we move over one group to the left , group 6 -- and that 's where the famous oxygen sits -- we already said that oxidizing something is doing to something what oxygen would have done , th... | at 9.45am what is the rule of thumb ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | now , i mentioned that i put hydrogen aside . because if you really think about it , hydrogen , yes , hydrogen only has one electron . and so you could say , well , maybe it wants to give away that electron to get to zero electrons . | 5 , why does the oxygen atom decide to hog the electrons forming a bond to one hydrogen only , not both ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . | does h2o ionized to h3o+ and oh- every time ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | and so for them , that oxidation state might not even be a hypothetical charge . these are very good candidates for actually forming ionic bonds . and so it 's very typical that when these are in a molecule , when these form bonds , that these are the things that are being oxidized . | are oxidation numbers the same as ionic charges in ionic compounds/molecules ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | it has no charge . similarly , hydrogen , plus 1 oxidation state ; oxygen , negative 2 oxidation number or oxidation state -- you add those two together , you have a negative 1 total charge for the hydroxide anion , which is exactly the charge that we have right over there . | how does oxidation state effect quality of oxidation agent ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | now , we could keep going . if we were to go right over here to the group 5 elements , typical oxidation state is negative 3 . and so you see a general trend here . | what is the trend of oxidation agent down the group [ group 15 comparing sb ( v ) and bi ( v ) ] ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | and i keep saying typically , because these are not going to always be the case . there are other things that could happen . but this is a typical rule of thumb that they 're likely to want to gain an electron . | can oxidizing only happen with ionic compounds ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | and actually , let me just draw that , because it 's fun to think about it . so this is a situation where oxygen typically has -- 1 , 2 , 3 , 4 , 5 , 6 electrons . and when it 's water , you have 2 hydrogens like that . | i thought oxygen had 8 electrons not 6 ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | so these are typically reduced . they typically have an oxidation state of negative 1 . and i keep saying typically , because these are not going to always be the case . | is the oxidation state and the valency of an element the same ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | so you could kind of view it kind of like an alkali metal . but in theory , it could have been put here on the periodic table as well . you could have put hydrogen here , because hydrogen , in order to complete its first shell , it just needs one electron . | how does oxidising strength change in periodic table ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | so these are typically reduced . these are typically oxidized . now , we could keep going . | what does oxidized mean ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . | how can i name these compounds copper nitrate and iron oxide ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | it has no charge . similarly , hydrogen , plus 1 oxidation state ; oxygen , negative 2 oxidation number or oxidation state -- you add those two together , you have a negative 1 total charge for the hydroxide anion , which is exactly the charge that we have right over there . | why are oxidation numbers important ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | notice , the oxidation states of the molecules here , they add up to the whole -- or the oxidation state of each of the atoms in a molecule , they add up to the entire charge of the molecule . so if you add a positive 1 plus negative 1 , you get 0 . and that makes sense because the entire molecule lithium hydride is ne... | will sal have to write '1+ ' instead of '+1 ' if he has to follow the convention of writing oxidation numbers ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | it has no charge . similarly , hydrogen , plus 1 oxidation state ; oxygen , negative 2 oxidation number or oxidation state -- you add those two together , you have a negative 1 total charge for the hydroxide anion , which is exactly the charge that we have right over there . | is gain of oxygen also a oxidation ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | and actually , let me just draw that , because it 's fun to think about it . so this is a situation where oxygen typically has -- 1 , 2 , 3 , 4 , 5 , 6 electrons . and when it 's water , you have 2 hydrogens like that . | oxygen is given 4 of its own electrons and 2 of hydrogens , however , if oxygen is striving for 8 electrons then should n't it have 6 of its original electrons plus the 2 it stole from hydrogen ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | and actually , let me just draw that , because it 's fun to think about it . so this is a situation where oxygen typically has -- 1 , 2 , 3 , 4 , 5 , 6 electrons . and when it 's water , you have 2 hydrogens like that . | in the previous explanation oxygen is given its 6 electrons , so what happened to 2 of them when oxygen steals from hydrogen ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | and then you have that other covalent bond to the other hydrogen . and now this hydrogen is now just a hydrogen proton . this one now has a negative charge . | why is hydrogen sometimes part of the last column ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | it has no charge . similarly , hydrogen , plus 1 oxidation state ; oxygen , negative 2 oxidation number or oxidation state -- you add those two together , you have a negative 1 total charge for the hydroxide anion , which is exactly the charge that we have right over there . | how is oxidation different from reductio ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | so these are typically reduced . they typically have an oxidation state of negative 1 . and i keep saying typically , because these are not going to always be the case . | what is the oxidation state ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | so these groups are typically oxidized . and oxygen is a very good oxidizing agent . or another way of thinking about it is oxygen normally takes away electrons . | why is oxygen good at oxidizing ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | so these are typically reduced . they typically have an oxidation state of negative 1 . and i keep saying typically , because these are not going to always be the case . | what is the oxidation state ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | and so for them , that oxidation state might not even be a hypothetical charge . these are very good candidates for actually forming ionic bonds . and so it 's very typical that when these are in a molecule , when these form bonds , that these are the things that are being oxidized . | why is ionic bonds considered as the electrons being a valence shell in an octet structure ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | they give away an electron . so they get to -- a typical oxidation state for them would be positive 1 . if we go one group over right over here to the alkaline earth metals , two valence electrons , still not too electronegative . | how did the elements get these oxidation numbers ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | so these are typically reduced . they typically have an oxidation state of negative 1 . and i keep saying typically , because these are not going to always be the case . | what is oxidation state ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | and you could say , well , if we 're forced to , we could say -- if we 're forced to think about this is an ionic bond , we 'll say it fully gains two electrons . so we 'll have an oxidation state of negative 2 . and once again , the notation , when you do the superscript notation for oxidation states and ionic charge ... | 0 , what is the typical oxidation state of a halogen and why ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | or another way of thinking about it is oxygen normally takes away electrons . these like to take away electrons , typically two electrons . and so their oxidation state is typically negative 2 -- once again , just a rule of thumb -- or that their charge is reduced by two electrons . | if the atoms are trying to get eight valence electrons , why will the alkaline metals easily give away their last two valence electrons ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | it has no charge . similarly , hydrogen , plus 1 oxidation state ; oxygen , negative 2 oxidation number or oxidation state -- you add those two together , you have a negative 1 total charge for the hydroxide anion , which is exactly the charge that we have right over there . | what is difference between oxidation and reduction ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | it has no charge . similarly , hydrogen , plus 1 oxidation state ; oxygen , negative 2 oxidation number or oxidation state -- you add those two together , you have a negative 1 total charge for the hydroxide anion , which is exactly the charge that we have right over there . | what is oxidation and reduction and how do they differ ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | now , we could keep going . if we were to go right over here to the group 5 elements , typical oxidation state is negative 3 . and so you see a general trend here . | what about the group 14 elements , what are their oxidation states ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | they have that one valence electron . they would n't mind giving away that electron . and so for them , that oxidation state might not even be a hypothetical charge . | why do the aklaine metals do n't mind giving a away a electon ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | now , we could keep going . if we were to go right over here to the group 5 elements , typical oxidation state is negative 3 . and so you see a general trend here . | how can group 17 elements have +3 oxidation state ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | so these are typically reduced . they typically have an oxidation state of negative 1 . and i keep saying typically , because these are not going to always be the case . | how to tell which oxidation state is most stable for an element ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | so these are typically reduced . they typically have an oxidation state of negative 1 . and i keep saying typically , because these are not going to always be the case . | how to find oxidation state of element without using periodic table ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | it has no charge . similarly , hydrogen , plus 1 oxidation state ; oxygen , negative 2 oxidation number or oxidation state -- you add those two together , you have a negative 1 total charge for the hydroxide anion , which is exactly the charge that we have right over there . | how do i know what element is in group 1 and the oxidation number is 5 ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | and actually , let me just draw that , because it 's fun to think about it . so this is a situation where oxygen typically has -- 1 , 2 , 3 , 4 , 5 , 6 electrons . and when it 's water , you have 2 hydrogens like that . and then you share . | what exactly is the difference in hydrogens ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | now , we could keep going . if we were to go right over here to the group 5 elements , typical oxidation state is negative 3 . and so you see a general trend here . | what is the oxidizing state of group 4 elements ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | now , we could keep going . if we were to go right over here to the group 5 elements , typical oxidation state is negative 3 . and so you see a general trend here . | what about the oxidation states of the elements in the p block ( in the middle ) ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | it has no charge . similarly , hydrogen , plus 1 oxidation state ; oxygen , negative 2 oxidation number or oxidation state -- you add those two together , you have a negative 1 total charge for the hydroxide anion , which is exactly the charge that we have right over there . | 0 you showed that all elements in group 17 have an oxidation state of -1 .but uus ( 117th element ) is very radioactive and has a half life of just 80 milliseconds.then how can it take part in any chemical reactions ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | or another way of thinking about it is oxygen normally takes away electrons . these like to take away electrons , typically two electrons . and so their oxidation state is typically negative 2 -- once again , just a rule of thumb -- or that their charge is reduced by two electrons . | for example cu 2+ has a : 1s2 2s2 2p6 3s2 3p6 4s1 3d10 frome where does it loose the two electrons ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | it has no charge . similarly , hydrogen , plus 1 oxidation state ; oxygen , negative 2 oxidation number or oxidation state -- you add those two together , you have a negative 1 total charge for the hydroxide anion , which is exactly the charge that we have right over there . | how do you find the oxidation numbers for the transition metals ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | it has no charge . similarly , hydrogen , plus 1 oxidation state ; oxygen , negative 2 oxidation number or oxidation state -- you add those two together , you have a negative 1 total charge for the hydroxide anion , which is exactly the charge that we have right over there . | why does the non metallic elements of groups ( 4a,5a,6a,7a ) have more than one oxidation number ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | so if you 're forced to assign an ionic -- if you were to say , well , none of this partial business , just give it all away or take it , you would say , well , these would typically have an oxidation state of positive 2 . in a hypothetical ionic bonding situation , they would be more likely to give the two electrons b... | why did you not fill in the 8 ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | but if we look at the alkali metals , the group 1 elements right over here , we 've already talked about the fact they 're not too electronegative . they have that one valence electron . they would n't mind giving away that electron . | does oxidation states of a particular element varies from one compound to another ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | so it 's hogging the electrons . so when you look at it right over here , you would say , well , look , hydrogen , if we had to , if we were forced to -- remember , oxidation states is just an intellectual tool which we 'll find useful . if you had to pretend this was n't a covalent bond , but an ionic bond , you 'd sa... | how to find the hybridization of sulphur in na2s2o3 ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | or another way of thinking about it is oxygen normally takes away electrons . these like to take away electrons , typically two electrons . and so their oxidation state is typically negative 2 -- once again , just a rule of thumb -- or that their charge is reduced by two electrons . | if the electronegativity increases across a period , why does the number of electrons the elements tend to take away decrease ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | now , we could keep going . if we were to go right over here to the group 5 elements , typical oxidation state is negative 3 . and so you see a general trend here . | how can i determine the oxidation state of group 4a elements ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | and now this hydrogen is now just a hydrogen proton . this one now has a negative charge . so this is hydroxide . | if you have an acid with a negative reduction potential of e. -0.49 and a base with a positive reduction potential of +.40 which one is more likely to be reduced ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | if we go one group over right over here to the alkaline earth metals , two valence electrons , still not too electronegative . so they 're likely to fully give or partially give away two electrons . so if you 're forced to assign an ionic -- if you were to say , well , none of this partial business , just give it all a... | bases are lower on the reduction potential table so they should be more likely to be oxidized but in this case their number is higher so are they more likely to be reduced ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | so these groups are typically oxidized . and oxygen is a very good oxidizing agent . or another way of thinking about it is oxygen normally takes away electrons . these like to take away electrons , typically two electrons . and so their oxidation state is typically negative 2 -- once again , just a rule of thumb -- or... | if oxygen likes to take 2 electrons to fulfil its shell , why is n't all water oh ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | it has no charge . similarly , hydrogen , plus 1 oxidation state ; oxygen , negative 2 oxidation number or oxidation state -- you add those two together , you have a negative 1 total charge for the hydroxide anion , which is exactly the charge that we have right over there . | in the ionic compounds , is the oxidation number related to the ionization energy ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | they have that one valence electron . they would n't mind giving away that electron . and so for them , that oxidation state might not even be a hypothetical charge . | why would n't be a hypothetical charge ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | so these are typically reduced . they typically have an oxidation state of negative 1 . and i keep saying typically , because these are not going to always be the case . | why h can have +1 or -1 oxidation state ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | so these are typically reduced . they typically have an oxidation state of negative 1 . and i keep saying typically , because these are not going to always be the case . | is oxidation state related to the ions that atoms have on the out side shield ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | so these are typically reduced . they typically have an oxidation state of negative 1 . and i keep saying typically , because these are not going to always be the case . | what differentiates oxidation state from valency ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | they give away an electron . so they get to -- a typical oxidation state for them would be positive 1 . if we go one group over right over here to the alkaline earth metals , two valence electrons , still not too electronegative . | if an element ( such as fluorine ) was reduced , would you say `` oxidation state '' or `` reduction state '' ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | and you could say , well , if we 're forced to , we could say -- if we 're forced to think about this is an ionic bond , we 'll say it fully gains two electrons . so we 'll have an oxidation state of negative 2 . and once again , the notation , when you do the superscript notation for oxidation states and ionic charge ... | do group 6 elements always carry a -2 oxidation state ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | so these are typically reduced . they typically have an oxidation state of negative 1 . and i keep saying typically , because these are not going to always be the case . | what is the oxidation state ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | now , let 's give an example where hydrogen plays the other role . let 's imagine hydroxide . so the hydroxide anion -- so you have a hydrogen and an oxygen . | is n't hydroxide written as oh and not as ho ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | and then you share . and then you have covalent bond right over there sharing that pair , covalent bond sharing that right over there . to get to hydroxide , the oxygen essentially nabs both of these electrons to become -- so you get -- that pair , that pair . | why does hf form covalent bond even though having high electroneagtivity difference ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | they give away an electron . so they get to -- a typical oxidation state for them would be positive 1 . if we go one group over right over here to the alkaline earth metals , two valence electrons , still not too electronegative . | how would you assign oxidation numbers to the transition metals ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | they give away an electron . so they get to -- a typical oxidation state for them would be positive 1 . if we go one group over right over here to the alkaline earth metals , two valence electrons , still not too electronegative . | can someone show me how to get oxidation state from azide ion ( n3- ) ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | or another way of thinking about it is oxygen normally takes away electrons . these like to take away electrons , typically two electrons . and so their oxidation state is typically negative 2 -- once again , just a rule of thumb -- or that their charge is reduced by two electrons . | sal drew 6 electrons for the oxgen atom , but are n't there supposed to be 8 electrons around the nucleus ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | it has no charge . similarly , hydrogen , plus 1 oxidation state ; oxygen , negative 2 oxidation number or oxidation state -- you add those two together , you have a negative 1 total charge for the hydroxide anion , which is exactly the charge that we have right over there . | are oxidation states + and then the # or the other way around ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . | what is the strongest chemical ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | it has no charge . similarly , hydrogen , plus 1 oxidation state ; oxygen , negative 2 oxidation number or oxidation state -- you add those two together , you have a negative 1 total charge for the hydroxide anion , which is exactly the charge that we have right over there . | is there any difference between oxidation state and oxidation number ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | it has no charge . similarly , hydrogen , plus 1 oxidation state ; oxygen , negative 2 oxidation number or oxidation state -- you add those two together , you have a negative 1 total charge for the hydroxide anion , which is exactly the charge that we have right over there . | how to balance reduction and oxidation reaction using acidic and basic medium ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | now , we could keep going . if we were to go right over here to the group 5 elements , typical oxidation state is negative 3 . and so you see a general trend here . | how do you determine the transition elements ' charges ? |
let 's see if we can come up with some general rules of thumb or some general trends for oxidation states by looking at the periodic table . so first , let 's just focus on the alkali metals . and i 'll box them off . we 'll think about hydrogen in a second . well , i 'm going to box -- i 'm going to separate hydrogen ... | so these are typically reduced . they typically have an oxidation state of negative 1 . and i keep saying typically , because these are not going to always be the case . | can anyone tell how to find oxidation state in complexes ? |
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