It's been 4 years since a lot of you guys watched this video to learn a thing or two. Meaning, you guys have since graduated and most likely moved into the cooperate world at the moment. I hope you have a blessed life with your families. We're right behind as well. And thank you khan academy for being a blessing to soo many of us. Thank you!
most professors are in actual fact hired as researchers, meaning their core function at the university is to do research, not to teach. my point is, Being good teachers is not their priority; their priority is to produce quality research papers, because universities aren't ranked according to the marks of students. They are ranked according to the most amount of quality research published.
If you have question,use their website,link is in the description,there you'll see a list of there videos, click on the one you want, if it's not already highlighted ,then scroll down to the bottom of the page,it might sometimes take a bit to show up.there they have a conversation section, where there is a whole lot of answers to questions related to that specific video. There you could also signin and ask a question for yourselves. It's great really.As far as I know khan academy don't answer questions on TH-cam's comment sections,they have integrated TH-cam to their website,I think they use it as a way of getting revenue.There is MORE info about who they are(a non profit organization) and what they offer(free education) in the description.
is it right to say VE in bonded atom?i believe since the electrons are shared, the electrons shared between one bond plus the lone pair(s) should be all considered VE? isn't better to describe it as formal charge=VE in free atom - lone pair - 1/2shared electron, it may look more complicated tho.
is there a difference tho? for memorizing purposed I think this video's explanation of it is easier. Is there any situation where this video's method would not work?
You might already know this by now because it’s been two years, but we know the hydrogen’s are attached to the oxygen because they will dissociate in water, so they must easily break off. It’s how all acids are, I believe.
U literally saved me thank-you so much😃 but in our books the formula is no.valence electron -no of unshared electrons -1/2the no of shared electrons . like if we use your formula we will get same ans in every case?
Charles Rosenthal Because compounds which exists in our nature have a formal charge of zero. Molecules with a formal charge more than zero is generally not available in nature
Why does it matter to move around the structure when the overall formal charge was already 0 because the Sulfur was +2 and the two Oxygen's were -1. 2 -1 -1 = 0. Please explain
anyone please tell me the significance of formal charge...why we calculate it?#i know how to calculate# so please don't tell me how to calculate it....just tell me why we calculate it?
Fireblaze 1998 The reason to calculate formal charge is to see which structure you would actually find in the real world. Real world structures are as close to a formal charge of zero as possible.
my techer said the formal charge is the number of valance electrons for the molecule minus the number of bonds with the molecules minus the number of unpaired electrons I have checked using this method and got same results. but might there be an exception or something?
Oxygen has 6 VE. While bond formation the Oxygen and other atom ,say Sulphur has to lend an e- to form a bond but u have drawn 7 e- in the terminal oxygen atom . How?
Naomi Castro Because compounds which exists in our nature have a formal charge of zero. Molecules with a formal charge more than zero is generally not available in nature.
Angelo Valdez the formal charge is related to the energy level of the structure. Lone pairs have higher energy level than bonded pairs so the oxygens formed a double bond. The effect of this change is minimizing the formal charge. So when drawing a structure the one with the least formal charge is probably the most accurate one because it has the least energy and is the most stable
its atomic no is 15 so arranging umm its k shell has 2 e L shell has 5 e and its outermost/valence M shell has 5 e , the group no. represents the no of valence e therefore N is in grp 5
it's atomic number is 7 and and it is in group 15 which is also known as V-A(5). And by the way you're right . Naruchi Uzumaki has explained it. But he/she is wrong about atomic number
Watch their video on formal charges and resonance Website link:- www.khanacademy.org/science/chemistry/chemical-bonds/copy-of-dot-structures/v/formal-charge?modal=1 TH-cam link:- th-cam.com/video/Kv5y3t9jsi4/w-d-xo.html The 7 electrons for oxygen or the 4 electrons for sulfur are actually not the valency electron, ever thing is explained in the videos.
The octer rule could be off, for elements in and above the third period, since sulphur is in the 3rd period,it is acceptable if it has more than 8 electrons
Why? The least electronegative atom always, or at least almost always, belongs in the center of the molecular structure. Sulfer is less electronegative than oxygen.
It's been 4 years since a lot of you guys watched this video to learn a thing or two. Meaning, you guys have since graduated and most likely moved into the cooperate world at the moment. I hope you have a blessed life with your families. We're right behind as well. And thank you khan academy for being a blessing to soo many of us. Thank you!
You taught this much better than my Chem professor and He has a PhD.....
i have to agree with you :")
most professors are in actual fact hired as researchers, meaning their core function at the university is to do research, not to teach. my point is, Being good teachers is not their priority; their priority is to produce quality research papers, because universities aren't ranked according to the marks of students. They are ranked according to the most amount of quality research published.
that explains a lot. i only go to lectures just get to my clicker points.
A PhD in chemistry, not a PhD in education. Experts don't always make good teachers.
maybe you don't pay attention in class.
whats the dot structure for a james bond?
😂😂😂
I have had 3 people try to explain to me what formal charge is and you did it in 8 mins. It isn't hard at all! Thank you!
If you have question,use their website,link is in the description,there you'll see a list of there videos, click on the one you want, if it's not already highlighted ,then scroll down to the bottom of the page,it might sometimes take a bit to show up.there they have a conversation section, where there is a whole lot of answers to questions related to that specific video.
There you could also signin and ask a question for yourselves. It's great really.As far as I know khan academy don't answer questions on TH-cam's comment sections,they have integrated TH-cam to their website,I think they use it as a way of getting revenue.There is MORE info about who they are(a non profit organization) and what they offer(free education) in the description.
is it right to say VE in bonded atom?i believe since the electrons are shared, the electrons shared between one bond plus the lone pair(s) should be all considered VE? isn't better to describe it as formal charge=VE in free atom - lone pair - 1/2shared electron, it may look more complicated tho.
is there a difference tho? for memorizing purposed I think this video's explanation of it is easier. Is there any situation where this video's method would not work?
Quick question, how do you know that the Hydrogens are attached to the oxygens rather than the sulfur?
Something to with it being an acid I think
You might already know this by now because it’s been two years, but we know the hydrogen’s are attached to the oxygen because they will dissociate in water, so they must easily break off. It’s how all acids are, I believe.
Thanks, very usefull
thank you guys so much. I couldn't understand it when my Professor lectured today.
Very nice video. I think what would make it perfect is if the sub titles did not cover some of the work. Other than that; the video was very helpful.
After watching this video. I feel that dot structure and finding charge is not that difficult
cool
life saver, thank you so much :)
U literally saved me thank-you so much😃
but in our books the formula is no.valence electron -no of unshared electrons -1/2the no of shared electrons . like if we use your formula we will get same ans in every case?
the final answer will be same as this solution. so, dont care about difference
thank you! so helpful
thumbs up if khan is ur lord and savior
u are my lord and savior
Lord and savior.........nah
only Jesus is
@@bryced2846 no
thanks so much!!!
Awesome!
So are we trying to get the formal charge of every atom to 0?
Charles Rosenthal Because compounds which exists in our nature have a formal charge of zero. Molecules with a formal charge more than zero is generally not available in nature
well put
Concise
thanks
We always did coordinate covalent bonds for sulfuric acid.
but bond pair means electron involved in making bond then have you included lone pairs electron too in the formula explain/.
thanks 😊
Haha you are Japanese. :)
Oh no ! 😂 I'm not japanese , I'm just a Naruto fan
Uhm...can I ask how to know if it is a posive or negative??
Why does it matter to move around the structure when the overall formal charge was already 0 because the Sulfur was +2 and the two Oxygen's were -1. 2 -1 -1 = 0. Please explain
anyone please tell me the significance of formal charge...why we calculate it?#i know how to calculate# so please don't tell me how to calculate it....just tell me why we calculate it?
Fireblaze 1998 The reason to calculate formal charge is to see which structure you would actually find in the real world. Real world structures are as close to a formal charge of zero as possible.
How does sulfur form 6 bonds?
+austin straub Octet rule exception
+Shawn Carlson whats the octet rule exception?
Dog that was 16 weeks ago I forgot haha
It can have a expanded octet
yeeeeeeeee
my techer said the formal charge is the number of valance electrons for the molecule minus the number of bonds with the molecules minus the number of unpaired electrons
I have checked using this method and got same results. but might there be an exception or something?
The same,its just a different way of thinking about it.
Oxygen has 6 VE. While bond formation the Oxygen and other atom ,say Sulphur has to lend an e- to form a bond but u have drawn 7 e- in the terminal oxygen atom . How?
99 duriarion
-1.-9
how does the top oxygen form a bond with S as if it has 7 electrons?
i love u
How is it that Sulfur can form 6 bonds?
nah fooooool
I may have not caught this while watching the video, but towards the end, why is he trying to get the formal charge closest to 0?
Naomi Castro Because compounds which exists in our nature have a formal charge of zero. Molecules with a formal charge more than zero is generally not available in nature.
someone pls, why need to minimize formal charge of central atom?
Angelo Valdez the formal charge is related to the energy level of the structure. Lone pairs have higher energy level than bonded pairs so the oxygens formed a double bond. The effect of this change is minimizing the formal charge. So when drawing a structure the one with the least formal charge is probably the most accurate one because it has the least energy and is the most stable
nitrogen provide one bond that two electrons are from nitrogen.
Whats a formal charge
th-cam.com/video/Kv5y3t9jsi4/w-d-xo.html
nice
9
Hello these concepts are now in class 11😅
such a simple thing dwelled on for what it seemed like hours. just get to the point
Sulur had more than 8 electrons and some were lacking. This gave me confusion because you didn't obey the octet rule
Sulfur doesn't have to obey the octet rule, it is on the 3rd row of the periodic table.
1
How is nitrogen in group 5 ?
i thought it was 15?
its atomic no is 15
so arranging umm its k shell has 2 e L shell has 5 e and its outermost/valence M shell has 5 e , the group no. represents the no of valence e therefore N is in grp 5
ohhh okay thank you
its atomic number is definitely not 15
it's atomic number is 7 and and it is in group 15 which is also known as V-A(5). And by the way you're right . Naruchi Uzumaki has explained it. But he/she is wrong about atomic number
RiSHi JagTaP Yeah yeah u're correct sry I messed up with the atomic no
N has 5 electrons, where is the last one (NH4)
+joe xtz It was NH4+. the + meaning it loses an electron. therefore it was one less.
@it 77
wait i dont get it, oxygen only has 6 valence electrons, Sulfur only has 6 valence electrons, why do you give Oxygen 7, and then sulfur 4?
Watch their video on formal charges and resonance
Website link:- www.khanacademy.org/science/chemistry/chemical-bonds/copy-of-dot-structures/v/formal-charge?modal=1
TH-cam link:- th-cam.com/video/Kv5y3t9jsi4/w-d-xo.html
The 7 electrons for oxygen or the 4 electrons for sulfur are actually not the valency electron, ever thing is explained in the videos.
slow down!!!
skrrrt
Am I the only one who thinks that the "octet" of electrons around oxygen in H2SO4 are a bit off?
@Kevin Nguyen ya i was getting really confused by it
The octer rule could be off, for elements in and above the third period, since sulphur is in the 3rd period,it is acceptable if it has more than 8 electrons
Donde esta mi hijo sal
this is wrong, the oxygens have to be more electronegative then the sulfer.
Why? The least electronegative atom always, or at least almost always, belongs in the center of the molecular structure. Sulfer is less electronegative than oxygen.
Sabhi ko english nahi aati hai sir