WHY AM I paying my tuition for my damn garbage professor that cannot teach me a single thing but I’m learning so much more from you for free.... please replace my professor 😭
It's not like ur proffesor is bad it's like ur not studying with concentration in his class and then when u miss something u come running here on TH-cam to understand with concentration
THIS IS THE METHOD FOR CALCULATION BOND ANGLES. Doesn't work for all molecules but... Every lone you have, subtract 2.5° degree from 109.5°. Eg. H2O (H=O=H) Oxygen has two long pairs. Subtract 5° from 109.5°=104.5° (109.5° is the bond angle of tetrahedral shape molecule)
but PH3 has only 1 lone pair if i substract 2.5° from 109.5° i get 107°. but the bond angle of PH3 is supposed to be 93.6° my exams are in like 3 hours.
@@fortuneless sorry for late reply. The method I used probably only work on certain molecules or compound. It was taught in my A level (highschool) text books.
An explanation as to why the NH3 and CH3CN molecules have the bond angle they do would be far more helpful here, rather than just trying to memorize them.
it’s almost like in NH3 there are 4 areas of electron density but because there are three bonds and one lone pair it is pyramidal with a diff bond angle
for the people asking, yeah you do have to memorise them (for this level of chemistry anyway) - the 3D structure of the molecule if it has X number of bonding pair electrons and Y number of lone pairs around the central atom (when you draw out the Lewis structure), and what will the angles be, and what do we call that structure (trigonal pyramidal, trigonal planar etc...) Its about how much electrons repel eachother, and lone pairs will have a higher density so sorta 'squash' the bond angle more. I'm sure there is a good video about it somewhere! :)
Last semester I watched your VSEPR theory videos over and over. It took me a while to understand this. I'm studying for the 2nd semester of O chem, and I got to this video without any issues, and THROUGH this video understanding and predicting correctly! You are an incredible teacher.
You can calculate it. Every lone you have, subtract 2.5° degree from 109.5°. Eg. H2O (H=O=H) Oxygen has two long pairs. Subtract 5° from 109.5°=104.5° (109.5° is the bond angle of tetrahedral shape molecule)
You can calculate it. Every lone you have, subtract 2.5° degree from 109.5°. Eg. H2O (H=O=H) Oxygen has two long pairs. Subtract 5° from 109.5°=104.5° (109.5° is the bond angle of tetrahedral shape molecule)
Hybridization of of Water Molecule is Sp3 and u know the concept of VSEPR Theory , Lone pair- lone pair- repulsion> lone pair- bond pair repulsion > bond pair- bond pair repulsion. So , oxygen having two lone pair in water molecule that's why bond angle of H2O is 104°
But how do we know they are those angles? Like, is this just a theory? Did someone measure the angle? What experiment proves these angles? How do we verify said angles? I'm not in college or know much about chemistry but I question how any of this is known when we can't when see these things.
This is a theory, meaning it's the closest thing to truth the universe has. We actually can see atoms using special microscopes. For measuring charges and shit I recommend looking it up online, there are tons of experiments that go into things like this
I know the lone pair electrons are involved in determining the shape but how do you know... how the lone pairs will react with the other atoms that are bonded to predict its shape?
The lone pairs will repel the electrons in the bonds with the other atoms. Thus, have smaller angles than a molecule with the same number of bonded pair...if you get what I mean. Hope it helps.
I don't think there is a specific method to find bond angles, it all depends upon hybridisation and no. of lone pairs and bond pairs !!! U can predict some but mostly memorization!!
Nope the second one has 2 bonding pairs and no lone pairs. Remember those 3 bonds N made with C we count that as 1 in bond angles! But there is no lone pair as carbon is making 4 bonds. So the central carbon makes 1 with the other carbon and makes the rest with nitrogen. It is like this C-C---N ( 3 lines are the 3 bonds). This is linear. Bent has a 120 degree angle if there are 2 bonding pairs and 1 lone pair or of there are 2 bonding pairs and 2 lone pairs!
Organic Chemistry - Video Lessons: www.video-tutor.net/organic-chemistry.html
WHY AM I paying my tuition for my damn garbage professor that cannot teach me a single thing but I’m learning so much more from you for free.... please replace my professor 😭
im with u
It's not like ur proffesor is bad it's like ur not studying with concentration in his class and then when u miss something u come running here on TH-cam to understand with concentration
@@prateeksharma2331 I mean.... I doubt you know his professer, he might as well be a bad teacher
@@prateeksharma2331 hi prof
@@prateeksharma2331 you really think bad professors don’t exist? go lick some boots lol
this is really saving me the night before my final lmao
same
how did it go lol?
My teacher is garbage
@@xuanviet807 hey! i failed!
@@elliekopanezos2550 calm down my man, next time you'll get better marks
THIS IS THE METHOD FOR CALCULATION BOND ANGLES.
Doesn't work for all molecules but...
Every lone you have, subtract 2.5° degree from 109.5°.
Eg. H2O (H=O=H)
Oxygen has two long pairs. Subtract 5° from 109.5°=104.5°
(109.5° is the bond angle of tetrahedral shape molecule)
but PH3 has only 1 lone pair
if i substract 2.5° from 109.5° i get 107°.
but the bond angle of PH3 is supposed to be 93.6°
my exams are in like 3 hours.
@@fortuneless Interesting - is PH3 maybe an exception but otherwise Jianghao's method works?
@@fortuneless sorry for late reply. The method I used probably only work on certain molecules or compound. It was taught in my A level (highschool) text books.
@@jianghaoyoutube5017 bruh i passed got 20 out of 30 (answered 21)
How does that work with the example at 1:30 .. the bond angle is 120°. doesn't work with trigonal planar.
An explanation as to why the NH3 and CH3CN molecules have the bond angle they do would be far more helpful here, rather than just trying to memorize them.
im not sure if this will help but it’s basically to make room for the lone pair of electrons
it’s almost like in NH3 there are 4 areas of electron density but because there are three bonds and one lone pair it is pyramidal with a diff bond angle
@@meghang9517whatever the fuck that means
Lone pairs will make the bond angle smaller. The more lone pairs, the smaller the angle.
for the people asking, yeah you do have to memorise them (for this level of chemistry anyway) - the 3D structure of the molecule if it has X number of bonding pair electrons and Y number of lone pairs around the central atom (when you draw out the Lewis structure), and what will the angles be, and what do we call that structure (trigonal pyramidal, trigonal planar etc...)
Its about how much electrons repel eachother, and lone pairs will have a higher density so sorta 'squash' the bond angle more. I'm sure there is a good video about it somewhere! :)
I'll pretend i understood that
Intelligent ARMY!! 💜
Last semester I watched your VSEPR theory videos over and over. It took me a while to understand this. I'm studying for the 2nd semester of O chem, and I got to this video without any issues, and THROUGH this video understanding and predicting correctly! You are an incredible teacher.
How is this useful... He's not telling us how to find the bond angles, he's only telling us what the bond angles are.
honestly yes. this is just memorization
I’m so confused rn
yea i was like wtf is this haha
Going to have my chem final on Monday! These videos have been helping me all semester. God bless you
Did you pass?
@@G.Osancity Yes I did! Then I went on to change my major and never took another chemistry class lol
i still dont get it ..
You can calculate it. Every lone you have, subtract 2.5° degree from 109.5°.
Eg. H2O (H=O=H)
Oxygen has two long pairs. Subtract 5° from 109.5°=104.5°
(109.5° is the bond angle of tetrahedral shape molecule)
Jianghao TH-cam wow, simply wow
@@notWaldont it doesn't really work for everthing. only tetrahedrals
@@jianghaoyoutube5017 does that only work for tetrahedral compounds?
I actually want to like that comment of yours but admitting it would feel like I'm losing :'(
I like the little tips you put in the explanation
Thank you Tutor , these videos have been helping me a lot !
I do love the 10-20 seconds of silence at the end of every video
This man is a genius.
Nah yu are just dumb
HeLLo I am just 12 years and I saw this vedio easy and extremely easy!!! Your vedios are really great. ThAnKs VeRy MuCh
It really helped me.. Thank you so much, wished I had known earlier about this page
So are you going to change the name of your channel ??
I just want to say that you are one of a kind! I don't think your human..Welcome to our human Earth Mr.Organic Tutor!
Yeah but how do u calculate the angle? Or do you just memorize it?
Memorization
You can calculate it. Every lone you have, subtract 2.5° degree from 109.5°.
Eg. H2O (H=O=H)
Oxygen has two long pairs. Subtract 5° from 109.5°=104.5°
(109.5° is the bond angle of tetrahedral shape molecule)
Jianghao TH-cam
But why 2.5 and why do you minus it?
@@rogersowden2369 idk but I was thought in school 😂
Mashuk Nabi you're fucking kidding me right? You're KIDDING ME! HAHAHAHAHAHA MY GRADES FUCKED!
trust me, You are awesome bro ......keep going on.... big fan ... please make videos on physical chemistry ..... 😎😎😎
I don’t even take chem but i like watching your videos for fun lmao
Lmao noice
Love you bro😭😭😭😭
You should do a video on symmetry operations/point group
everything was good till 3:30... i was like damn where did it go from 0 to 100 i just wanna pass fck straight A's
I have inorganic chemistry ....nice video.😊😊😊
good for you :)
- here's a medal
"medal"
In H2O eg why u took 2H downward and why not in a straight line which makes an angle 180??
Because The lone pairs push the hydrogen down ward
@@Hanna-gr5mv Do the lone pair electrons in Oxygen's valence shell repulse the bond pair electrons that are covalently bonded with Hydrogen?
Abrar Mahadik yes
Skull_ Brawl Stars electron repulsion pushes bonded pairs away from the lone pairs
Hybridization of of Water Molecule is Sp3 and u know the concept of VSEPR Theory ,
Lone pair- lone pair- repulsion> lone pair- bond pair repulsion > bond pair- bond pair repulsion.
So , oxygen having two lone pair in water molecule that's why bond angle of H2O is 104°
I want you to go into Mathematical Methods please 🙏.....I really struggle finding videos on TH-cam associated with it
Thank you (Wed 16 Dec 2020, 5:53 AM)
Does NH3 and PH3 and AsH3 bond angles the same
I’m literally walking to my AP Chem Exam rn, I’m 2 mins away
rip
Thanks you very much 💟
You are the best
Learn me a lot
Guys, we have to memorise these bond angles.
Is Mark Wahlberg doing the voice over?
what grade do you learn this?
11 i think
Nice❤ keep it up
But how do we know they are those angles? Like, is this just a theory? Did someone measure the angle? What experiment proves these angles? How do we verify said angles? I'm not in college or know much about chemistry but I question how any of this is known when we can't when see these things.
This is a theory, meaning it's the closest thing to truth the universe has. We actually can see atoms using special microscopes. For measuring charges and shit I recommend looking it up online, there are tons of experiments that go into things like this
wouldnt the much larger O push the H's around further on the plane? ie: make the H's closer.
I know the lone pair electrons are involved in determining the shape but how do you know... how the lone pairs will react with the other atoms that are bonded to predict its shape?
most atoms will have 8 electrons around it (octet rule)
The lone pairs will repel the electrons in the bonds with the other atoms. Thus, have smaller angles than a molecule with the same number of bonded pair...if you get what I mean. Hope it helps.
How do you know how much bonds the atoms like to form?
How many electrons it needs to become stable
This was not helpful at ALL. You just listed the angles but didn't explain how to get them. WHYYY?
lol fr
I don't think there is a specific method to find bond angles, it all depends upon hybridisation and no. of lone pairs and bond pairs !!! U can predict some but mostly memorization!!
why isnt it 90 degress for the HcH ?
MY FKKN FINALS ARE AFRER 2 WEEKS
I AM SO FKKN CONFUSED
I DON'T KNOW WHERE TO START FROM UGHHHHH
U re the best bro
huh 109°? why not 90°? is that because the bonding is in a pyramid shape?
Because carbon assumes a Tetrahedral shape when attached to 4
@@krathish01 but it looks more like 90°
The bond angle in a tetrahedron is 109°. You get this when placing the four surrounding atoms as far apart as you can in three dimensions.
@@Maryam-go3yq .
What’s the angles for C3H803?
I am twelve years old and i solve it
OH
|
HO\/\/OH
Glycerine Glossary of C3H8o3
I am twelve years old and i solve it:
OH
|
HO\/\/OH
Love from india
QUESTION - How would I know if a molecule is bent? Thanks :)
Its mostly due to lone pair repulsion, look for lone pairs.
why is the second one linear molecular shap. Isnt the molecular shape bent and tetrahedral.
Nope the second one has 2 bonding pairs and no lone pairs. Remember those 3 bonds N made with C we count that as 1 in bond angles! But there is no lone pair as carbon is making 4 bonds. So the central carbon makes 1 with the other carbon and makes the rest with nitrogen. It is like this C-C---N ( 3 lines are the 3 bonds). This is linear. Bent has a 120 degree angle if there are 2 bonding pairs and 1 lone pair or of there are 2 bonding pairs and 2 lone pairs!
Which fucking angle is it tho?? For ammonia for example,is it the n to h or h to h.like what's 107
I am twelve year old and i solve it:
Glycerine Glossary of C3H8O3;
OH
|
HO\/\/OH
girl I was playing with dolls when I was 12
@@kyle-tg7bi 😀😀😅😄
Ch2o = 120 not true . in real , the angle is 122 cause of the double bond between C and O ( 122 , 116 , 122)
1:42
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