Formal Charge
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- Опубликовано: 8 апр 2018
- This organic chemistry video tutorial explains how to calculate the formal of an atom in a molecule using a simple formula.
Organic Chemistry - Basic Introduction: • Organic Chemistry - Ba...
Valence Bond Theory - Full 33 Minute Video:
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Formal Charge Review Notes:
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Which Bond Is More Polar?
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Condensed Structures to Skeletal Structures:
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Functional Groups Review:
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Primary, Secondary, & Tertiary Functional Groups:
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Finding Lone Pairs Using Formal Charge:
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Dipole Moment & Electronegativity:
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Predicting Bond Angles:
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Valence Bond Theory:
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This makes me so happy to see someone explain organic chemistry so fluidly! Thank you!
I like to use a mnemonic to help remember the formula:
Valence e - Lone pair e - # bonds
V-LP-B
Very little people blink
Maybe it helps some people!
ur cool
Helps sir !! :)
Professor Organic Chemistry Tutor, thank you for showing/explaining How to calculate the Formal Charge of an atom in a molecule using a simple formula in Organic Chemistry. Organic Chemistry is a unique course with many tools to learn. This is an error free video/lecture on RUclips TV with the Organic Chemistry Tutor.
Thank you mark wahlberg, this was more helpful than my 15 minutes of tutoring offered by students who are mediocre at best with chemistry at a school I pay 55k a year for. (ending my passive aggressive rant on school's tutor system now)
Have you try being better?
@@elianmndz717 Quiet scoundrel
My tutor told me to google the answers. I was a little more than upset
thank you so much im genuinely glad i found this tutorial and gave it a chance it really helped me understand
Sir, you are the best at chemistry. I tried to watch Sal Khan, the guy drives me crazy, he talks too much. Very straightforward and easy. Thank You
thanks you soo much this video helped me alot in understanding the subject
Carbocation is also what happens when I stay home and eat cake for spring break.
Quarantine
@Corbin Salvatore mhm thanks man i needed, for.. reasons
Good bless you, that is so awesome 🌼
Thanks, it helped me a lot....
Thank you! Thank you! Thank you so much!
I've said it many times, this guy is a GOAT!!!
You are a fascinating teacher
Tq sir for teaching fantastically
I am taking this class next semester and fully expect to return to this video.
OK,,,you really have nice stuff.Thanks 😊
thanks man you made this way easier to understand :)
Best explanation.. Love it
great 👏👏👏
You’re the Heisenberg of RUclips
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You’re goddam right!
Helpful vid
Many thanks
Why are their six lone pairs on the oxygen atom? Because he applied the octet rule with oxygen. It has 6 valence electrons and wants 2 more to be happy. This needs to be done before applying the formula for getting the formal charge for each atom in the molecule except hydrogen. Hydrogen does not follow the octet rule. It needs 2 electrons in its outer shell to be happy. It already has 1 valence electron in its natural state.
To be happy HAHAHAHAH, I need a passing grade in chem to be happy :(
Thank you very much dude
Thank you very much for this easy way. But please tell me the dufference between Formal charge and Oxydation number of the element. Thanks again and wish u the best.
I am very helpful from this video tq
thank you so much 👌👍
Thank you (Wed 16 Dec 2020 5:39 AM)
thank you sir...thanks so very mutch
I LOVE THIS
Thank youuuuuu
Yeah all this is okay, but what I was really looking for is the feel of formal charge ! Like I wanna understand that formula
When an atom doesn't have any valence electrons, it doesn't have a negative formal charge. The reason that the bonds equal to = -1 despite consisting of two electrons is that two atoms share the electrons and the negative charge, each getting a -1 per bond.
The reason the numbers are "-1" per electron are just because it makes it easier to count and makes sense i guess.
what if they dont give you the drawing of the structure and they just give you C02 4 example. How do you make sure the bonds are correct and therefore the dots_
Then you would need to come up with a valid structure yourself. The central atom often is first listed in many formulas.
Thanks sir ,but iam not native person but I tries to understand you .love u sir
at 2:03 why doesn't Carbon have an octet?
For instance given the structure of some alcohol, I know the oxygen has two lone pairs of electrons (because it has 6 valence electrons and only two of those electrons are being used in bonds).
Can't I use the same idea of valence electrons when looking at a molecule that has a carbon with three bonds? Can I not visualize a free non-boned valence electron? In this case wouldn't the carbon have a -1 charge?
I was wondering this as well
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Nitrogen has 5 electrons, so why ch3 has 4 out of the brackets and shouldn’t it be 3 out of the brackets?
I have my first midterm for OCHEM I tomorrow...Binge time!
You saved my life
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Question: In the first one: If one of the electrons is needed to form the covalent bond with carbon, wouldnt it be a radical?
If one of the electrons in a covalent bond with carbon is unpaired, then the molecule would be considered a radical. However, in most cases, the electrons involved in a covalent bond are paired, meaning that they are shared between the atoms in the bond. This is because the sharing of electrons allows both atoms to achieve a more stable electron configuration, usually by filling their outermost shell with electrons.
How do I know when I’m going to add the dot
how can we know which atom in a molecule to calculate the formal charge for???
Every atom has its own formal charge. Examples are randomly chosen in the video.
Which device you are using to write
Plz tell the name of it
Or name of software u r using for writing?
Sir I think it's a software for notes with a stylus on tablet or laptop.
My sir uses a similar software to teach during tuition. He used to use a macbook + pad to write and connected it to a projector but now he uses an iPad with apple pencil and connects it to a projector.
Wow🔥
How does bromine has 4 unpaired electron?
is it okay to have 0 equal?
Ok. This is fine. But how do we know if something forms a single double or triple bond? One Gen. Chem I teacher expects us to write down the Louis form, and then find formal charge, but doesn’t tell us how to find the bond information.? Maybe I’m just dumb, but I don’t get how to tell if something forms the single or double bond
Hey The Organic Chemistry Tutor!
How it can be possible that N has 4 bonds?
I was all the videos lectures and I'm really one of your students that follow your channel and lessons and sometimes I have to ask some questions!
Please and please help med because according to Lewis Structure or Lewis dots Nitrogen can have only 3 bonds and in this video I see that N has 4 4:03 bonds like Carbon! How is this?
Ok uhh
I might be wrong but I think 3 is just the typical bonding pattern and it can actually do 4 as well.... I may be wrong though
Tori L the central atom prefers to have 8 electrons. Since they’re sharing it counts as 2 electrons so usually it will either want 4 pairs or 3 pairs and 2 of its own electrons or 2 pairs and 4 of its own ect. Most want 8 but some only want 6 or some want 10 it just depends
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Shouldn't the B in the equation be divided by 2?
he is counting the number of bonds, you only divide by 2 if you count the number of bonded electrons. hope i helped
ammmmmmazingg
2:11 how come it doesn’t have any lone pairs when carbon tends to have 4 bonds and there are only 3 bonds present meaning it should then have 1 lone pair
If it had a lone pair, it would have a negative formal charge.
Excuse me but the formal charge of carbon is -1 cuz it exceeds the # of electrons then # of protons in C-R3 problem. I hope you will clear my doubts.
The formal charge of an atom in a molecule can be calculated using the formula:
Formal charge = valence electrons - non-bonded electrons - 1/2(bonded electrons)
In the case of a carbon atom in a molecule where it is attached to three identical R groups (C-R3), each R group would contribute one electron to the carbon atom in the form of a single bond. Therefore, the carbon atom would have a total of 4 valence electrons.
If we assume that each R group is a carbon atom, then each carbon atom would have 3 valence electrons, and the carbon atom in question would have a total of 10 valence electrons (4 from the central carbon atom and 3 from each of the three R groups).
If we apply the formula for formal charge to the carbon atom, we get:
Formal charge = 4 (valence electrons) - 0 (non-bonded electrons) - 1/2(6) (bonded electrons)
Formal charge = 4 - 0 - 3
Formal charge = +1
Therefore, the formal charge on the carbon atom in this molecule is +1, not -1 as you suggested. It is possible that I have misunderstood the specific problem. I hope that helps you!
@@sudaisshah9393 thanks for your wisdom
But, what is the significance of use of the formal charge on an atom?
Ok so I'm just a below avg chem student but as far as I know
It helps understand the distribution of charge in an atom
You are the Chemistry Mosiah
How come there are two versions of this formula? The other is FC = VE - [LPE - ½(BE)], and maybe I'm just stupid but, they seem to show different answers.
Edit: Nvm I figured it out. Your formula's easier.
I don't get how come It has a positive charge if It has one plus electron
@Laura Laura The plus sign on the atom doesn't indicate it has plus one electron, it shows the atom has a positive charge. That means it lost an electron and became positive. When you put a minus sign on an atom that means it has an extra electron, or it has a negative charge. So, C + (carbocation) means it's missing an electron and its a positive charge.
GOAT
How come you forget some electron on the central atom???
I'm imperfect. I make mistakes at times.
Why Carbon still has 6 non bonded electrons at 0:38? Is it suppose to be 5?
you mean the Oxygen?
@@nostro1940 My bad, it is actually Oxygen.
It's just recently that I've learned about dative bonding, so I was confused why Oxygen still has 6confusedly non-bonded electrons.
@@fromblonmenchaves6161 because of the Octet rule. It needs to be surrounded with 8 electrons. Supposedly it stole one from an hydrogen.
Just a helpful hint.....As an organic chemist......Organic molecules rarely have charges of anything other than zero, plus 1 or minus 1. This video could have been explained in a much better way. I think it could have been explained without using the formal charge equation because of how simple organic formal charges are. If you lose a bond from the typical bonding pattern, you are negative 1. If you gain a bond from your normal bonding pattern you are positive 1. As an example: Oxygen typically has 2 bonds (and 2 lone pairs). If it has 3 bonds (and 1 lone pair) it's gained a bond, meaning it's positive 1. If an oxygen has 1 bond (and 3 lone pairs) it's lost a bond, meaning it's now negative 1. Same goes for every single atom normally seen in organic chemistry. Your example of the double bonded bromine......Bromine normally has 1 bond and 3 lone pairs, so if it has 2 instead of 1, it is now positive 1. Super simple, no math. This isn't the case for general chemistry (inorganic molecules), but that's the formula is needed in those cases.....but not in orgo typically.
I disagree, I think this is a valid method of learning formal charges. In my Organic class, the formal charge equation was the method we were formally taught. It's also a simple way to double check your answer when initially learning-- especially if you occasionally forget how many bonds something is supposed to have. Use whatever works for you, but this method is efficient for first-time learners.
@@desit.302 "first time learners" of organic chemistry should already have used the formal charge equation for 2 semesters of general chemistry. They should be focusing on learning the normal patterns of organic molecules, not doing math. Math is for PChem and gen chem, not orgo. I'm not debating that people were taught to use this equation in their classes. But lots of students are taught lots of unhelpful things. I'm both a teacher and organic chemist. Sometimes we need to recognize when the old ways of teaching aren't as effective.
You just made it "click" thank you.
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That was so random
I dont understand why you have to make a formula to calculate the charge!
if a Carbon needs 4 bonds to be stable and only has 3 bonds, automatically you know it has an extra electron and therefore -1 charge.
If Br needs 1 bond to be stable but has 2 bonds, then you know it gave away one electron and therefore +1 charge.
Why the math?
While it may be true that in some cases, the charge of an ion or molecule can be determined by examining its bonding pattern, this method is not always reliable. For instance, a carbon atom that is double-bonded to another carbon and single-bonded to a hydrogen is still stable despite not having an extra electron and therefore would not have a -1 charge. Additionally, some elements can form multiple bonds, such as oxygen, which can form double or triple bonds, or nitrogen, which can form triple bonds, making it difficult to accurately determine the charge simply by counting the number of bonds.
Therefore, a formula for calculating the charge of an ion or molecule takes into account not only the number of valence electrons of all the atoms involved but also any additional electrons gained or lost during the formation of the ion or molecule. This formula provides a more consistent and reliable method of determining the charge, especially for complex molecules.
@@sudaisshah9393 hydrogen - carbon = carbon - hydrogen ?
You mean like Acetylene but double bond instead of triple bond?
I have my finals in 7 hours 🤣