Quick tips: Single-bonded oxygen = -1 Double-bonded oxygen = 0 ** P is from group 5, it is less electronegative than O. Hence, P = positive(+) formal charge. Consider this, since P is from group 5 = + 5. Therefore, the charge reduces by one for each single bond with oxygen. This means, when there are four (4) total single bonds with oxygen, P = +1. When there is a double bond + 3 single bonds (5 total bonds), P = 0 charge
Hello, sorry for the reply(crazy busy). Theoretically, the two double bonds would make sense. However, the highest orbital for nitrogen is 2p. Therefore, 2s and 2p can only account for maximum 8e- ( 2 on 2s and 6 on 2p = 8 maximum e-). N is unlike P that can access the 3d orbital. I hope this helps🙏
Thank you, Mr. Knight! I like how you leave the explanation of the stability factor for the molecule until the end of the discussion. This gives the learner the "why" to the unusual double bonded oxygen at the conclusion. Then when you add in the d orbital with its 10 e-s, this gives us the "how" the stable molecule is accomplished. Will there be resonance structures with this molecule?
Not how can phosphorus contain more than 8 but how do you decide to do the double bond. Calculating Formal charge for all possible structures takes so long
Quick tips: Single-bonded oxygen = -1 Double-bonded oxygen = 0 ** P is from group 5, it is less electronegative than O. Hence, P = positive(+) formal charge. Consider this, since P is from group 5 = + 5. Therefore, the charge reduces by one for each single bond with oxygen. This means, when there are four (4) total single bonds with oxygen, P = +1. When there is a double bond + 3 single bonds (5 total bonds), P = 0 charge
The octect rule still apply, but to make the lewis structure stable the d orbital should be considered. Remember, not all of the compounds of phosphorus will need to have 5 total bonds. It really depends on what makes the molecule more stable.
@@jockleyfedora8018If each oxygen atom has 6 valence electrons, and phosphorus has 5 valence electrons, where did the three additional valence electrons for phosphorus come from?
Quick tips: Single-bonded oxygen = -1
Double-bonded oxygen = 0
** P is from group 5, it is less electronegative than O. Hence, P = positive(+) formal charge.
Consider this, since P is from group 5 = + 5. Therefore, the charge reduces by one for each single bond with oxygen. This means, when there are four (4) total single bonds with oxygen, P = +1.
When there is a double bond + 3 single bonds (5 total bonds), P = 0 charge
the way you explain everything from the ground up and thoroughly is a godsend, thank you mr. knight. As you said, no more confusion!
You are welcome.
Sorry can you explain NO3-? I'm confused why it has only one double bond instead of 2, it would be more stable if it had 2 double bonds with oxygen
Hello, sorry for the reply(crazy busy). Theoretically, the two double bonds would make sense. However, the highest orbital for nitrogen is 2p. Therefore, 2s and 2p can only account for maximum 8e- ( 2 on 2s and 6 on 2p = 8 maximum e-). N is unlike P that can access the 3d orbital.
I hope this helps🙏
Thank you, Mr. Knight! I like how you leave the explanation of the stability factor for the molecule until the end of the discussion. This gives the learner the "why" to the unusual double bonded oxygen at the conclusion. Then when you add in the d orbital with its 10 e-s, this gives us the "how" the stable molecule is accomplished. Will there be resonance structures with this molecule?
You are welcome. There will be resonance, they can be achieved by shifting the double bond around.
@@science_exam Thank you Mr. Knight! I hope you will enjoy this day. I certainly will because I now have answers to my questions.
Beautiful explanation sir
Thank you.
sir So to make the structure stable we have to make anyone of their formal charge zero ?
The total formal charges must be equal to zero. The more zero charges are there on individual atoms, the more stable the structure.
Thank you sir , but if question ask on formal charge in an exam which answer is correct
You are welcome. It's best to do it for the most stable structure unless they give you a specific structure.
Thanks Mr Knight👏🏾👏🏾
You are most welcome.
Class is in session awesome 👌
😊 Thank you!
Perfect.its very well explained..
Thank you!
Not how can phosphorus contain more than 8 but how do you decide to do the double bond. Calculating Formal charge for all possible structures takes so long
Quick tips: Single-bonded oxygen = -1
Double-bonded oxygen = 0
** P is from group 5, it is less electronegative than O. Hence, P = positive(+) formal charge.
Consider this, since P is from group 5 = + 5. Therefore, the charge reduces by one for each single bond with oxygen. This means, when there are four (4) total single bonds with oxygen, P = +1.
When there is a double bond + 3 single bonds (5 total bonds), P = 0 charge
@@science_exam fuuuuck lemme read that again lmaoooo its gonna make sense before the test thank youuuu !
Can you show me all of the possible resonance structures?
All you need to do is to shift around the double and single bonds to different positions.
Can a co ordinate bond could be there with other three bonds
Yes, it is possible.
@science_exam thank you for the information.😊
You are awesome. Thank You
Thank you and you are most welcome.
So for all the compounds of phosphorous octect rule doesn't apply bcoz of the d orbital?
The octect rule still apply, but to make the lewis structure stable the d orbital should be considered. Remember, not all of the compounds of phosphorus will need to have 5 total bonds. It really depends on what makes the molecule more stable.
@@science_exam so can we consider p043- as an exception for octect rule
@@leotennison1818 When it comes to the Lewis structure yes. Primarily the rule is still applied.
@@science_exam thankyour sir for your response❤️
@@leotennison1818 You are welcome.
how many structures are their in chemistry like this it always takes time to understand and confuse us
Not much, just a few exceptions.
Very well explain
Thanks 😊
You are welcome.
Thank you
You are welcome.
Thank youuu
You are welcome
why the total n is 40 not 42 ?
Phosphorus has 8 valence electrons and 4 oxygen has 32 valence electrons total
Awesome explanation.
Please see @Jockley Fedora explanation.
@@jockleyfedora8018If each oxygen atom has 6 valence electrons, and phosphorus has 5 valence electrons, where did the three additional valence electrons for phosphorus come from?
Thanky you❤ sir
You are most welcome
Phosphorous can never be tetravalent ,so thumbnail picture busted!!😅😅
There you go👩🔬👨🔬
Can you translate it to Arabic
I will see what I can do.