Can anyone explain to me how he figures out the total valence electron before he starts drawing?? That seems to be the the one trick I'm not getting =/ haha
@SpoilerofGames Count the valence electrons by looking at atoms given and find what column they are listed in the periodic table. Ex: CO2. C atom in column 4 and 2 O atoms in column 6. 4+6+6 = 16.
@rose62892 It's a general rule for polyatomic ions with O atoms that I tell students. You can attempt to draw other configurations but you won't get a nice Lewis Structure.
@untouchedpoop The Lewis structure is C single bonded to three different H atoms. The C atom also has a lone pair of electrons. With four groups and one lone pair this species is tetrahedral (electronic geo) and trigonal planar (molecular geo). In that case, it's polar. In another sense, most say that ions are always polar because they would form ionic compounds.
@h6233w For the most part, yes. If you have a question on a particular molecule then I'm happy to comment on it. Really, it has to do with the electron cloud distribution as determined by electronegativity.
so that means, all we have to do is to just look at shape and identify if it's symmetrical or not. If it is, then it's nonpolar but if not it's polar. But what about the electronegativity, isn't there's such a way about subtracting each element's electronegativity and then basing it on a table and then u identify if it's polar or nonpolar. And what about lone pairs for? Isn't it if there's a lone pair, then that means it's a polar if none then it's nonpolar. I'm quite confused here. X(
@shinichikudoconanful Yes, look at the symmetry and that accounts for EN. Consider HF. It is linear but not symmetric, thus polar. In terms of EN, there is an obvious difference, thus polar. Same answer. Lone pairs are a determining factor in shape which leads to symmetry so that is also already accounted for. There are some examples of shapes with lone pairs that are np such as linear (with 5 or 6 groups) or square planar. See other videos of mine and let me know if you are still stuck.
@EnderlePhD Thanks a lot!!! I kinda get it. But may I ask you a question if Carbonate is polar or nonpolar? My chemistry teacher says it's polar and has a dipole moment. I don't quite get it. Thanks again!!! :D
@shinichikudoconanful Ions are hard to comment on polarity and carbonate is an ion. One could say that if it existed by itself it would be nonpolar but it would really exist with a cation. With a cation, the species would be ionic and thus polar. You should ask your instructor how to best proceed when confronted with a ion and asked about polarity.
@mrtictac94 We're learning it as freshmen (13-14 years old for most freshmen right now). I mean, I'm in Honors Integrated Science 1, but I'm pretty sure it's the same for everybody at our school.
I want to thank you for posting these videos and whether it be you, the teacher, that is uploading these videos I thank you. You're a great teacher and I like how you slowly explain everything instead of just telling us what is what. I've had teachers that just tell me the facts, without the how or why. So again, thank you!
@MsCrumplehorn The arrow demonstrates the difference in electronegativity. The C atom is more electropositive than the O atom. You could also draw a partial positive charge on the C atom and a partial negative charge on the O atom.
The answer to this matter is partially whether its symmetrical or not, but the electron negativity gives you the true aswer - if its polar or nonpolar. Why does he not explain electron negativity?
@dasistdas Typically, one uses bond dipoles to find the net dipole moment qualitatively though it is also found experimentally. Qualitatively, one can compare the EN difference for each bond and draw a resulting dipole. Through vector analysis, one can find the net dipole moment. In this video, you are just seeing the problem being solved but not the theory. Looking at molecular symmetry is a simple way to determine if there is a net dipole (same method actually).
To tell if its nonpolar or polar, cant you just ask yourself if its symmetrical? Why even bother with the dipoles :p It confuses me. so basically im asking are all symmetrical shapes nonpolar and all non-symmetrical polar?
@asdfghjkl019283 Yes, that's fine. Check out the video and you'll see I initially solved with the concept of symmetry. When students asked me for more detail, I explained using bond dipoles. To answer your last question: yes, it should be. If you think you find a counter-example, let me know and we can take a look at it.
@EnderlePhD this is not in the video, but why is PF5 nonpolar if it is not symmetrical? i have to choose between ClF3, PF3, PF5, SF4, and CH2F2. based on this logic, i'm confused as to why PF5 is nonpolar
@eerriikkaaaa First draw the PF5 Lewis structure (trigonal bipyramidal). See there are 2 Fs on the same axis (linear) which are symmetrical to each other (bond dipoles cancel). See 3 Fs that form a trigonal planar shape. The trigonal planar shape is symmetrical (bond dipoles cancel). In sum, all the bond dipoles cancel leaving the molecule polar. To say another way, any basic shape with no lone pairs on the center atom and identical atoms bonded to it is nonpolar.
Even if he is, he'd probably go for someone who can spell 'was' and 'thinking. Think you stumbled across 'drawing Lewis structures' when you meant to look for 'drawing with crayons.''
Even if he is, he'd probably go for someone who can spell 'was' and 'thinking. Think you stumbled across 'drawing Lewis structures' when you meant to look for 'drawing with crayons.''
Even if he is, he'd probably go for someone who can spell 'was' and 'thinking. Think you stumbled across 'drawing Lewis structures' when you meant to look for 'drawing with crayons.''
Even if he is, he'd probably go for someone who can spell 'was' and 'thinking. Think you stumbled across 'drawing Lewis structures' when you meant to look for 'drawing with crayons.''
Even if he is, he'd probably go for someone who can spell 'was' and 'thinking. Think you stumbled across 'drawing Lewis structures' when you meant to look for 'drawing with crayons.''
Even if he is, he'd probably go for someone who can spell 'was' and 'thinking. Think you stumbled across 'drawing Lewis structures' when you meant to look for 'drawing with crayons.''
Even if he is, he'd probably go for someone who can spell 'was' and 'thinking. Think you stumbled across 'drawing Lewis structures' when you meant to look for 'drawing with crayons.''
at 5:45 you drew the arrow pointing to oxygen the more electronegative atom, but the latest IUPAC convention points the arrow from negative to positive.
@y100269 Really? That's interesting because I've always seen it in texts pointing from the electropositive to the electronegative element. Can you post the website or reference material for us? Thanks!
@y100269 Thanks for the info. I'm not sure why different texts teach this differently. Take home application: follow whatever your chemistry instructor does. If I find more info I'll post here.
@y100269 I think that EnderlePhD direction of an arrow is correct, because it always goes from negative to positive el. for example:
from H to Cl or we can show why CO2 is unpolar, because eventough molecules do have polar bonds, because dipol bonds have oposite directions C=O=C, so dipol moment is zero! sry for my bad english! :)
@lowryderfly i did say negative to positive, he drew it from positive to negative which is fine, i'm just saying that the rule (IUPAC) has just recently changed.
@y100269 I think that EnderlePhD direction of an arrow is correct, because it always goes from negative to positive el. for example:
from H to Cl or we can show why CO2 is unpolar, because eventough molecules do have polar bonds, because dipol bonds have oposite directions C=O=C, so dipol moment is zero! sry for my bad english! :)
@y100269 I think that EnderlePhD direction of an arrow is correct, because it always goes from negative to positive el. for example:
from H to Cl or we can show why CO2 is unpolar, because eventough molecules do have polar bonds, because dipol bonds have oposite directions C=O=C, so dipol moment is zero! sry for my bad english! :)
Thank you, I am just starting organic-chem at my local community college. Hence, its been a while since high-school, so thank you so much for refreshing my memory as well as teaching me some new principle's.
You are greatly helping me cram for my exam tommorrow. It's like having mini-lectures but without all the bullshit stuffed into it to make it go for 1hr 20mins. Purified knowledge baby. I want to inject this shit.
VERY concise and appropriate way to explain this subject. You did not rush through the material too quickly although the ladies question on why the CO seems symmetrical I believe could best be answered by saying that one is more electronegative than the other, being in front of a class you did a great job overall.
Also, I relistened and saw that you did twice say that it's because theyre more electronegative and also that at the beginning of the question she answered her own question. Pretty strange, lol.
ok so, when drawing c-o. how can o have a triple bond? that makes no sense. it doesnt have a d orbital for bonding electrons so its max bonds it can make are two.......
This exercise is just drawing optimized Lewis structures without evaluating other chemistry aspects, which would be outside the scope of this class. However, the triple bond agrees with the MO diagram which shows a bond order of 3. Also, experimental data backs up the bond order of 3 (see "General Chemistry" Petrucci et al.).
This is a really good explanation, i just dont get this one thing in my chem class: why when you are drawing the shape do you draw some as a triangle/ slashed lines or just a normal line? so for example at 4:02?
That is to show u where the molecule is oriented in space the normal line means "the bond" is parallel to the chalkboard, in tetrahedral molecules which has bond angles of 109.5, meaning each bond is 109.5 degrees from the next bond. It is convenient to show the shape using triangle/ slashed lines or just a normal lines. The normal lines represent the bonds being parallel or laying on the chalkboard, usually it is convenient to show 2 "normal bonds". The slashed bond meaning behind the board.
its because hes trying to show the 3D orientation, the slashed lines means that functional group is behind the central atom, the shaded triangle line represents the bonded functional group that is infront and the line is just another bond to a functional group. good luck in ur chem class
Amazingly helpful. After sitting through college level Chemistry, and then getting ready to study for the final exam and realizing that I still had trouble with this, this video solved all my problems.
i dont get why do we have to have the valence electron?
Algerie123Foot 5 days ago
@Algerie123Foot The Lewis structure is necessary in order to answer the question and the valence electrons help us draw the correct Lewis structure.
EnderlePhD 2 days ago
lost
Sadie1307 2 weeks ago
@Sadie1307 lost what?
EnderlePhD 2 weeks ago
amazing!
nyacoub11 3 weeks ago
That shirt is SO last decade
nlading1 3 weeks ago
Can anyone explain to me how he figures out the total valence electron before he starts drawing?? That seems to be the the one trick I'm not getting =/ haha
SpoilerofGames 4 weeks ago
@SpoilerofGames Count the valence electrons by looking at atoms given and find what column they are listed in the periodic table. Ex: CO2. C atom in column 4 and 2 O atoms in column 6. 4+6+6 = 16.
EnderlePhD 4 weeks ago
@EnderlePhD Thanks a bunch =)
SpoilerofGames 3 weeks ago
Is there a reason H can only be bonded to the O in polyatomic ions? and is it only in polyatomic ions + only those elements?
rose62892 1 month ago
@rose62892 It's a general rule for polyatomic ions with O atoms that I tell students. You can attempt to draw other configurations but you won't get a nice Lewis Structure.
EnderlePhD 1 month ago
You showed in 10 minutes what my teacher couldnt show in 10 weeks
BuzzingFridge 1 month ago
i need help asap on CH3- for its molecular polarity and its dipole moments?
untouchedpoop 1 month ago
@untouchedpoop The Lewis structure is C single bonded to three different H atoms. The C atom also has a lone pair of electrons. With four groups and one lone pair this species is tetrahedral (electronic geo) and trigonal planar (molecular geo). In that case, it's polar. In another sense, most say that ions are always polar because they would form ionic compounds.
EnderlePhD 1 month ago
I am only giving it a thumbs up because the professor looks friendly :)
djumr 1 month ago
thanks young lady who asked for H2SO4
reminya25 2 months ago
Lovein the old school chalk board :D
Plackart 2 months ago
All symmetrical molecules are non-polar and all non-symmetrical are polar?
h6233w 2 months ago
@h6233w For the most part, yes. If you have a question on a particular molecule then I'm happy to comment on it. Really, it has to do with the electron cloud distribution as determined by electronegativity.
EnderlePhD 2 months ago
You are the BEST teacher in the world. Thank you so much!!
dhaccessories 3 months ago
you've taught me more in 10 minutes than my AP chem teacher has all year.
theamazingnessapril 3 months ago 5
@theamazingnessapril lol, I can relate to you :P
sruthiize 1 month ago
do you have your own website?
abiola100000 3 months ago
i must have missed one...lol
13illumination 3 months ago
so that means, all we have to do is to just look at shape and identify if it's symmetrical or not. If it is, then it's nonpolar but if not it's polar. But what about the electronegativity, isn't there's such a way about subtracting each element's electronegativity and then basing it on a table and then u identify if it's polar or nonpolar. And what about lone pairs for? Isn't it if there's a lone pair, then that means it's a polar if none then it's nonpolar. I'm quite confused here. X(
shinichikudoconanful 3 months ago
@shinichikudoconanful Yes, look at the symmetry and that accounts for EN. Consider HF. It is linear but not symmetric, thus polar. In terms of EN, there is an obvious difference, thus polar. Same answer. Lone pairs are a determining factor in shape which leads to symmetry so that is also already accounted for. There are some examples of shapes with lone pairs that are np such as linear (with 5 or 6 groups) or square planar. See other videos of mine and let me know if you are still stuck.
EnderlePhD 3 months ago
@EnderlePhD Thanks a lot!!! I kinda get it. But may I ask you a question if Carbonate is polar or nonpolar? My chemistry teacher says it's polar and has a dipole moment. I don't quite get it. Thanks again!!! :D
shinichikudoconanful 3 months ago
@shinichikudoconanful Ions are hard to comment on polarity and carbonate is an ion. One could say that if it existed by itself it would be nonpolar but it would really exist with a cation. With a cation, the species would be ionic and thus polar. You should ask your instructor how to best proceed when confronted with a ion and asked about polarity.
EnderlePhD 3 months ago
This guy is good
stevenxue1 3 months ago
I know no one's asking about this but I'm learning at 14 :) Here in the Philippines, we have less levels in our education system.
biancutie 3 months ago
i like this
clarifoamfish 4 months ago
I wish I had a chem professor like this guy. He actually teaches.
Nan15 4 months ago in playlist 10: Chemical Bonding I - Basic Concepts 14
What age are you being taught this in the USA? Cos I'm 16, English and really confused.
mrtictac94 5 months ago
@mrtictac94 hey! idk what age they teach it in the US, but here in singapore I'm learning it at 17.
ukaisukaok 5 months ago
@mrtictac94 We're learning it as freshmen (13-14 years old for most freshmen right now). I mean, I'm in Honors Integrated Science 1, but I'm pretty sure it's the same for everybody at our school.
TheAnonymouse123e 3 months ago
very helpful a lot more clear then my professor...thank you!
ibecoolyo24 5 months ago
Why did my chem textbook make dipole moment seem like some elaborate non-understandable concept? Thanks for clearing that up in the first minute.
TarynnH 5 months ago
@TarynnH ikr
RockerJack15 3 months ago
So a dipole and polar are the same thing
finally i get an answer on what dipole means
Kaperdabomb 5 months ago
my chemistry teacher gotta watch this.....
she need it much more than i do....
awesome...explaination
THEBLACK493 5 months ago
This is incredibly helpful. Thank you
vjacob89 6 months ago
i was the 100th person to like this video.
agentjucey 8 months ago
i did the 100 thumbs up!
agentjucey 8 months ago 3
You are a good teacher.I like all your videos,espeacially the one on alcohols,phenols and ethers.
exmortis123game 8 months ago
I want to thank you for posting these videos and whether it be you, the teacher, that is uploading these videos I thank you. You're a great teacher and I like how you slowly explain everything instead of just telling us what is what. I've had teachers that just tell me the facts, without the how or why. So again, thank you!
blueBruSea 9 months ago
@MsCrumplehorn The arrow demonstrates the difference in electronegativity. The C atom is more electropositive than the O atom. You could also draw a partial positive charge on the C atom and a partial negative charge on the O atom.
EnderlePhD 10 months ago
Can these be compared in terms of polarity, as in can one molecule be more polar than another?
jihadmeathello110 10 months ago
@jihadmeathello110 Yes, polarity is a similar term.
EnderlePhD 10 months ago
hi , can u explain me please how we do the lewis configuration of the CLO3F?
please reply me faster cause i have a test in 2 days
thank u
ps: u explain very well
musulmane191 10 months ago
thanks helped me alot!
ic3cr3amxx 10 months ago
The answer to this matter is partially whether its symmetrical or not, but the electron negativity gives you the true aswer - if its polar or nonpolar. Why does he not explain electron negativity?
dasistdas 10 months ago
@dasistdas Typically, one uses bond dipoles to find the net dipole moment qualitatively though it is also found experimentally. Qualitatively, one can compare the EN difference for each bond and draw a resulting dipole. Through vector analysis, one can find the net dipole moment. In this video, you are just seeing the problem being solved but not the theory. Looking at molecular symmetry is a simple way to determine if there is a net dipole (same method actually).
EnderlePhD 10 months ago
difinitoin of diPole moment
Mybuneri 11 months ago
enderle phd ? hmm.acaba buna ender ile phd de diyebilir miyiz? cevap verirsen cevabımı almış olurum zaten. thank you so much. that was very helpful.
savenature748 11 months ago
Cool teacher person.... i have a question..... why do u look like your off American Pie?
Bodhihardinge95 11 months ago
To tell if its nonpolar or polar, cant you just ask yourself if its symmetrical? Why even bother with the dipoles :p It confuses me. so basically im asking are all symmetrical shapes nonpolar and all non-symmetrical polar?
asdfghjkl019283 1 year ago
@asdfghjkl019283 Yes, that's fine. Check out the video and you'll see I initially solved with the concept of symmetry. When students asked me for more detail, I explained using bond dipoles. To answer your last question: yes, it should be. If you think you find a counter-example, let me know and we can take a look at it.
EnderlePhD 1 year ago
@EnderlePhD this is not in the video, but why is PF5 nonpolar if it is not symmetrical? i have to choose between ClF3, PF3, PF5, SF4, and CH2F2. based on this logic, i'm confused as to why PF5 is nonpolar
eerriikkaaaa 10 months ago
@eerriikkaaaa First draw the PF5 Lewis structure (trigonal bipyramidal). See there are 2 Fs on the same axis (linear) which are symmetrical to each other (bond dipoles cancel). See 3 Fs that form a trigonal planar shape. The trigonal planar shape is symmetrical (bond dipoles cancel). In sum, all the bond dipoles cancel leaving the molecule polar. To say another way, any basic shape with no lone pairs on the center atom and identical atoms bonded to it is nonpolar.
EnderlePhD 10 months ago
i wos waching and the only thing i wos thingking wos is he gay?
kilstas16 1 year ago
@kilstas16 If you have a helpful comment, I'm happy to answer it. Otherwise, you can keep your comments to yourself.
EnderlePhD 1 year ago 14
@kilstas16
Says more about then it does about him....
Even if he is, he'd probably go for someone who can spell 'was' and 'thinking. Think you stumbled across 'drawing Lewis structures' when you meant to look for 'drawing with crayons.''
ellymanster 1 year ago
@kilstas16
Says more about then it does about him....
Even if he is, he'd probably go for someone who can spell 'was' and 'thinking. Think you stumbled across 'drawing Lewis structures' when you meant to look for 'drawing with crayons.''
ellymanster 1 year ago
This has been flagged as spam show
@kilstas16 @kilstas16
Says more about than it does about him....
Even if he is, he'd probably go for someone who can spell 'was' and 'thinking. Think you stumbled across 'drawing Lewis structures' when you meant to look for 'drawing with crayons.''
ellymanster 1 year ago
This has been flagged as spam show
@kilstas16
Says more about than it does about him....
Even if he is, he'd probably go for someone who can spell 'was' and 'thinking. Think you stumbled across 'drawing Lewis structures' when you meant to look for 'drawing with crayons.''
ellymanster 1 year ago
This has been flagged as spam show
@kilstas16
Says more about than it does about him....
Even if he is, he'd probably go for someone who can spell 'was' and 'thinking. Think you stumbled across 'drawing Lewis structures' when you meant to look for 'drawing with crayons.''
ellymanster 1 year ago
This has been flagged as spam show
@kilstas16
Says more about than it does about him....
Even if he is, he'd probably go for someone who can spell 'was' and 'thinking. Think you stumbled across 'drawing Lewis structures' when you meant to look for 'drawing with crayons.''
ellymanster 1 year ago
This has been flagged as spam show
@kilstas16
Says more about than it does about him....
Even if he is, he'd probably go for someone who can spell 'was' and 'thinking. Think you stumbled across 'drawing Lewis structures' when you meant to look for 'drawing with crayons.''
ellymanster 1 year ago
PLEASE BE MY CHEM TEACHER
Dakashizzlenizzle 1 year ago
you are the man! thank you!
mikeygdawg 1 year ago
YOu are greattt!!
111000may 1 year ago
i really need this
brizelinit 1 year ago
it took me almost an hour to go through this section in my text book, and i still didnt get it...thanks for helping me understand it in 10 minutes!
zameer23 1 year ago
wow you are good!
bboydjoe 1 year ago
thank you. very helpful
Dharnoozle 1 year ago
at 5:45 you drew the arrow pointing to oxygen the more electronegative atom, but the latest IUPAC convention points the arrow from negative to positive.
y100269 1 year ago
@y100269 Really? That's interesting because I've always seen it in texts pointing from the electropositive to the electronegative element. Can you post the website or reference material for us? Thanks!
EnderlePhD 1 year ago
@EnderlePhD It's my textbook. Title: Discovering Chemistry I
2010 - 2011 edition, published by the University of Western Ontario (uwo)
authors: Dr. Kim Baines, Dr. Keith Griffiths, Dr. John Corrigan and Dr. Felix Lee
chapter: 2.1; page: 2-6 (the 6th page of chapter 2)
I'll send you Dr. Felix Lee's email (these names can be verified on uwo dot ca) i tried finding it online but it's too much of a hassle.
y100269 1 year ago
@y100269 Thanks for the info. I'm not sure why different texts teach this differently. Take home application: follow whatever your chemistry instructor does. If I find more info I'll post here.
EnderlePhD 1 year ago
@y100269 I think that EnderlePhD direction of an arrow is correct, because it always goes from negative to positive el. for example:
from H to Cl or we can show why CO2 is unpolar, because eventough molecules do have polar bonds, because dipol bonds have oposite directions C=O=C, so dipol moment is zero! sry for my bad english! :)
lowryderfly 1 year ago
@lowryderfly i did say negative to positive, he drew it from positive to negative which is fine, i'm just saying that the rule (IUPAC) has just recently changed.
y100269 1 year ago
This has been flagged as spam show
@y100269 I think that EnderlePhD direction of an arrow is correct, because it always goes from negative to positive el. for example:
from H to Cl or we can show why CO2 is unpolar, because eventough molecules do have polar bonds, because dipol bonds have oposite directions C=O=C, so dipol moment is zero! sry for my bad english! :)
lowryderfly 1 year ago
This has been flagged as spam show
@y100269 I think that EnderlePhD direction of an arrow is correct, because it always goes from negative to positive el. for example:
from H to Cl or we can show why CO2 is unpolar, because eventough molecules do have polar bonds, because dipol bonds have oposite directions C=O=C, so dipol moment is zero! sry for my bad english! :)
lowryderfly 1 year ago
@bomberfun1 Typo*... 3 PhD's if I remember correctly
arredeck 1 year ago
Thanks! Test tomorrow, and just trying to suck all the lagg info in.
tellNadia 1 year ago
my chem teacher has worked on Harvard and Oxford, has 13 PhD's and this guy in youtube answered all my questions lol
arredeck 1 year ago 2
@arredeck
Re: "my chem teacher has worked on Harvard and Oxford, has 13 PhD's"
Yeah and my name is Princess Yamamoto.
karlkarlkarl1234 1 year ago
super duper helpful thanks!
jeaniefarts 1 year ago
great vid mate helped me alot!
aurie308 1 year ago
Thank you, I am just starting organic-chem at my local community college. Hence, its been a while since high-school, so thank you so much for refreshing my memory as well as teaching me some new principle's.
TheNotoriousPIGPEN 1 year ago
your an amazing teacher - very patient. love this video. thanks. =)
YouDotTee 1 year ago
You are greatly helping me cram for my exam tommorrow. It's like having mini-lectures but without all the bullshit stuffed into it to make it go for 1hr 20mins. Purified knowledge baby. I want to inject this shit.
karlkarlkarl1234 1 year ago 42
VERY concise and appropriate way to explain this subject. You did not rush through the material too quickly although the ladies question on why the CO seems symmetrical I believe could best be answered by saying that one is more electronegative than the other, being in front of a class you did a great job overall.
dbm6969 1 year ago
Also, I relistened and saw that you did twice say that it's because theyre more electronegative and also that at the beginning of the question she answered her own question. Pretty strange, lol.
dbm6969 1 year ago
@dbm6969 Ha ha. Cool thanks!
EnderlePhD 1 year ago
good question at the end!
jacksonian321 1 year ago
ok so, when drawing c-o. how can o have a triple bond? that makes no sense. it doesnt have a d orbital for bonding electrons so its max bonds it can make are two.......
makesismehappy 1 year ago
This exercise is just drawing optimized Lewis structures without evaluating other chemistry aspects, which would be outside the scope of this class. However, the triple bond agrees with the MO diagram which shows a bond order of 3. Also, experimental data backs up the bond order of 3 (see "General Chemistry" Petrucci et al.).
EnderlePhD 1 year ago
Thank you so much. This was very helpful .
Little0Nutmeg 1 year ago
You are a very gifted teacher.
Annaleah15 2 years ago
Great video!
julius350z 2 years ago
This is a really good explanation, i just dont get this one thing in my chem class: why when you are drawing the shape do you draw some as a triangle/ slashed lines or just a normal line? so for example at 4:02?
themogmrsfreckles 2 years ago
That is to show u where the molecule is oriented in space the normal line means "the bond" is parallel to the chalkboard, in tetrahedral molecules which has bond angles of 109.5, meaning each bond is 109.5 degrees from the next bond. It is convenient to show the shape using triangle/ slashed lines or just a normal lines. The normal lines represent the bonds being parallel or laying on the chalkboard, usually it is convenient to show 2 "normal bonds". The slashed bond meaning behind the board.
leaf202 2 years ago
its because hes trying to show the 3D orientation, the slashed lines means that functional group is behind the central atom, the shaded triangle line represents the bonded functional group that is infront and the line is just another bond to a functional group. good luck in ur chem class
AZNKC 2 years ago
Amazingly helpful. After sitting through college level Chemistry, and then getting ready to study for the final exam and realizing that I still had trouble with this, this video solved all my problems.
montecarloguy09 2 years ago
Nice, very helpful.
tigerlilja1 2 years ago
Wow you're awesome man!
31w00d 2 years ago
this guy rocks! his students are soo lucky!
AnyCR87 2 years ago
this helped me a lot, i wanted to raise my hand when i watched it haha
Domenic182 2 years ago 20