Lewis Dot Structures for Polyatomic Ions - CLEAR & SIMPLE

[@michelle732mn]

Some teachers are just not meant to be teachers. You sir are meant to be an amazing teacher. Many thanks for explaining this!

[@josephdavies7905]

Thank you so much bro. My teacher was trying to get us to memorize a bunch of a different poly atomic ions today without explaining this or anything about why they have negative charge. It was doing my head in. I feel better now.

[@lulu462]

So helpful. Thank you! Second degree student here who is taking biochem and hasn't done chem in 7+ years. Great refresher!

[@beckwilde]

i like how you messed up and you started over again but you didnt edit it out LOL 6:49

[@abduljndli2026]

Rebecca Chen 😂😂

[@chickennuggets6910]

Now that its been 5 years how are u currently doing

[@beckwilde]

@@chickennuggets6910 I graduated and I’m not doing what I was learning in university. Thanks for checking on me 🙌

[@lucasnyman5424]

@@beckwilde woah this is wild

[@aznmayo]

@@lucasnyman5424 imma forget my password after 5 years lmfao

[@Mcbash6]

Thanks bro I have been trying to figure out where those electrons come from to complete the octate but you did it. Thanks I appreciate this. You live to educate others.

[@relemazamelela6866]

The best explanation ever! Super grateful

[@cowslane1]

Hey LENNY thanks for the link!

[@elizabethlear7299]

Thank you so much hopefully this lesson will come in handy on my chem test tomorrow!!

[@sciencepost]

Go Big!

[@alancai4280]

this is a really good video guide, thanks

[@brxxke6]

I know this is an old video so I don’t know if anyone will see this but I’m studying for an exam and I have a horrible teacher and this video was SO helpful in explaining what my teacher couldn’t. Thank you

[@-mayo-]

Very well done, very descriptive and illustrated. The video is greatly appreciated!

[@aymandaha6431]

Thanks so much man! You made my day.

[@isaiahm99]

Great beginner video, as well as a fantastic refresher on polyatomic lewis dot structures. One thing I did notice, however, was that the bond at 3:46 is actually a single bond not a double (I know I'd get confused if I didn't know already), but over all very well explained and thought out! Thanks for the vid

[@mji5678]

yea

[@GettyGoGaming]

Very helpful video! Definitely helped for my chem finals tomorrow

[@KannyNguyen]

thank u, man! I didn't understand the lesson until I watched your video :D

[@Maard00k]

you are fucking amazing are you a teacher holy shit.. I need more teachers like you in my school wow

[@riyakhan4731]

Superb video ! Just subscribed your channel for more videos .it was a great help . Thanks a lot

[@nikita-8136]

Ohhhhhhhhh this actually makes sense😛

[@jaweriasiddiqui2193]

I get it now finally! Thanks a ton!

[@kellbell6397]

Hope this helps for my chem test tomorrow!

[@sciencepost]

I hope you rock the test!

[@dzuke3127]

Thank you so much! This was so helpful!!!

[@p.c.kthianhlun4246]

excellent explanation...

[@lydiaaustin2204]

Phosphate has a 3- charge, meaning it would gain 3 e- right? So wouldn't the e- count would be 31?

[@suhannap5182]

Lydia Austin that's after another element gives phosphate the electrons. The Lewis structure he drew is before that happened, so that's how there's 29.

[@lucyqu2]

Thank you. This was very helpful :)

[@sciencepost]

That is awesome to hear! Keep being an amazing student!

[@mbabazi.o]

You have to face a Holy God on judgement day. He sees lust as adultery (Matthew 5:28) and hatred as murder. (1John 3:15) will you be guilty? Jesus took your punishment on the cross, and rose again, defeating death to save you from hell. Repent (Luke 13:5) and trust in Him today. May God soften you heart to receiving Jesus Christ, our Redeemer, as your personal LORD and Savior. Repent and trust in Him today.

[@btcmoon6058]

you are a god

[@katm9971]

Thanks. Very helpful video.

[@daniellesang6610]

So helpful! Thank you so much!

[@idresseaymu1008]

Great method 👍

[@sciencepost]

Thanks bro, you are very welcome.

[@sciencepost]

So glad it helped

[@StructuralIntegrity.]

great vid, helped alot!

[@itsjusawesome8538]

this helped a lot thanks

[@NeroxDread]

Bah, you don't use a line for shared electrons! That's one of my pet peeves for whatever reason (as legitimate as it is). Otherwise, great video.

[@zaminahmed297]

same

[@MetalcoreCarCovers]

in the second example, how come N has 5 electrons?

[@sagacioussolace7827]

Atomic no. Of nitrogen is 7 so it'll have 2 electrons in first shell n remaining 5 in outermost shell))

[@vidasinlibertad]

VERY USEFUL!

[@scitwi9164]

Your solution for PO4(3-) is *not correct*. Your ion has -3 overall charge, so it has 3 additional electrons you should account for. So there is 32 electrons in total to distribute over your molecule's atoms, not 29. You can say that it doesn't matter, since you add them at the end to one of these oxygens. But this is *still incorrect*, because now this oxygen would have a -1 formal charge (actually, all of the oxygens), and the phosphorus has +1 formal charge. Some teachers would say that it can be solved by moving one pair of electrons from one of these oxygens towards the phosphorus to make another bond (making a double bond in total), which would cancel the +1 formal charge on phosphorus and -1 on one of these oxygens. But this is still not quite right, because there are three possible choices for where we can put this double bond and which oxygen's formal charge will cancel with that of the phosphorus's. (It's usually called "resonance", although it has *nothing* to do with music or oscillations at all.) The correct answer is that this additional charge is evenly distributed between all these atoms, making a sort-of "smudged out bond" between all three oxygens and the phosphorus. It is usually being drawn as a dashed line going from one oxygen through the phosphorus to the other oxygen. But in reality, this is a molecular orbital surrounding the entire molecule. It's as if the electrons around the oxygens (which all have -1 formal charge) were attracted towards the phosphorus and leaning more towards it in their bonds, making them somewhat more than a single bond, but not yet a double bond (a 1.5 bond). This also makes these bonds shorter than single bonds, but not as short as double bonds.

[@vidasinlibertad]

how would the lewis dot stucture look like for CH3CH3O?

[@amprofiiable]

I understand ur concept but does Nitrogen have 5 electrons or 7? I'm confused.

[@pollak40]

A single nitrogen atom has 5 electrons in its VALENCE (outermost, where the chemistry happens) shell. Make sure to note, however, that nitrogen is a diatomic element. This means that nitrogen atoms tend to be found in a compound of some sort in nature, and a single nitrogen atom is extremely unstable and will find something to bond with due to its unstable nature.

[@markictakes6200]

Very helpful thanks

[@bettytiruneh5834]

Don’t you have to add the charge to the total number of electrons?

[@oshak96]

Thanks a ton man!

[@Vulecro529]

8:44 Look what we become : we become 1+ " exam grade" thank you come again XD

[@missweasleylovegoodgranger7019]

Wait it MAKES SENSE

[@marialazaro7445]

Great video :)

[@abhinithmathew304]

thanks 4 the video

[@mtg0131]

Thank you!

[@LJ-ky1ql]

can't it be (po4)1+?

[@entropyfan9417]

Thank you

[@mamtajamwal1040]

Thankyou!☺

[@mbabazi.o]

Whoever reading this, God knows what you are facing through, He heard your cry, He is going to deliver you. Just trust in Him.

[@kx85lover]

Thanks!

[@iandavidson5216]

Sounds like Cory from Trailer Park Boys

[@andrewpalladino1217]

this is wrong. Have to consider the formal charges....

[@hopscotchoblivion7564]

6:34 *Frustrated sigh*

[@abdulpali]

thanks!!!!!

[@sciencepost]

You are welcome!

[@smartcell4054]

2022 haw 🤠

[@Truevulture2000]

helped me so much but you smoked 420 lol

[@asurashi2413]

*ok*

[@PengchengZ]

If Phosphate has a -3 charge why would it want to gain electrons from other atoms? Electrons are negative. If anything it would want to give 3 electrons to make itself neutral.

[@julienl7241]

+PengchengZ I think phosphate having a -3 charge means it's _already_ gained the three electrons, three more than the total number of protons in the molecule.

[@Edward_cummington]

schrader