I am an Indian. I learns chemistry for your chemistry lectures. I have learned as very well shell subshell and orbital etc but hybridization confusion. Million Thank you sir
Richard I am parent that utilizes the site to help my daughter with HS chemistry. Just wanted to thank you because your lessons have been extremely helpful, great job and thanks again!!!!
At 4:25 you have 1 electron in the 2s shell and 3 electrons in the 2p shell for the carbon atom. I looked at the electronic configuration for a carbon atom and it showed me 2 electrons in the 2s shell and 2 electrons in the 2p shell. Why is this so ?
Yes, initially there are 2 electrons in the 2s shell and 2 electrons in the 2p shell for carbon. However, when carbon forms bonds with other atoms, it will move an electron from a lower orbital to a higher orbital. What I drew was an electron from the 2s orbital being moved or promoted to the 2p orbital. Carbon is trying to get 8 outer electrons, and a good way for it to do that is to move one electron from 2s to an empty 2p orbital. When this occurs, there are now 4 unpaired electrons on carbon. Each unpaired electron can now pair up with an unpaired electron from another atom. When 4 unpaired electrons pair up with electrons from other atoms, carbon will now have 8 outer electrons. I probably should have included an explanation of electron promotion in this lecture. I hope this explanation helps. Here's a link that explains electron promotion and hybrid orbitals: chem.libretexts.org/Core/Physical_and_Theoretical_Chemistry/Chemical_Bonding/Fundamentals_of_Chemical_Bonding/Covalent_Bonding
Go to www.richardlouie.com and watch chemistry lecture #26 (shape of the s, p, d, and f orbitals) for a detailed explanation of how electrons actually move around the nuclei of atoms. The short answer is that electrons randomly move around a region of space around the nucleus. So yes, I guess they do buzz around in that middle section.
You had me through Ionic bonding, but this Covalent bonding is confusing. When you draw those Carbon hybrids, I get that you're showing what's going on with energy level 2, but what happened to 1s? How does that 1s orbital fit in with what's going on?
The 1s orbital continues to exists. The electrons in the 1s orbital are not involved in any type of interaction with other atoms, so we don't draw them. The main idea to remember is that in a covalent bond, the electrons are between the nuclei of atoms, and these electrons act as a glue that hold together the nuclei of different atoms, just like peanut butter holds two pieces of bread together.
I am an Indian. I learns chemistry for your chemistry lectures. I have learned as very well shell subshell and orbital etc but hybridization confusion. Million Thank you sir
Richard I am parent that utilizes the site to help my daughter with HS chemistry. Just wanted to thank you because your lessons have been extremely helpful, great job and thanks again!!!!
thank you Sir Richard your lectures have cleared my all doubts and also your way of teaching is increadible
I have learned so much from your videos but this hibridization doesn't seem too confusing
Thank you for your wonderful lessons. Regards from India.
At 4:25 you have 1 electron in the 2s shell and 3 electrons in the 2p shell for the carbon atom. I looked at the electronic configuration for a carbon atom and it showed me 2 electrons in the 2s shell and 2 electrons in the 2p shell. Why is this so ?
Yes, initially there are 2 electrons in the 2s shell and 2 electrons in the 2p shell for carbon. However, when carbon forms bonds with other atoms, it will move an electron from a lower orbital to a higher orbital. What I drew was an electron from the 2s orbital being moved or promoted to the 2p orbital. Carbon is trying to get 8 outer electrons, and a good way for it to do that is to move one electron from 2s to an empty 2p orbital. When this occurs, there are now 4 unpaired electrons on carbon. Each unpaired electron can now pair up with an unpaired electron from another atom. When 4 unpaired electrons pair up with electrons from other atoms, carbon will now have 8 outer electrons.
I probably should have included an explanation of electron promotion in this lecture. I hope this explanation helps. Here's a link that explains electron promotion and hybrid orbitals:
chem.libretexts.org/Core/Physical_and_Theoretical_Chemistry/Chemical_Bonding/Fundamentals_of_Chemical_Bonding/Covalent_Bonding
Thanks for your reply. I will have a look at the above link. I like the way you teach and explain things.
and what is electron movement? Does they buzz in that middle section, or they have complete two shells to move around? Thanks
Go to www.richardlouie.com and watch chemistry lecture #26 (shape of the s, p, d, and f orbitals) for a detailed explanation of how electrons actually move around the nuclei of atoms. The short answer is that electrons randomly move around a region of space around the nucleus. So yes, I guess they do buzz around in that middle section.
2:38 video time for question below
The videos about electron configuration, orbitals, and stuff in that concept are a precursor before watching this video
You had me through Ionic bonding, but this Covalent bonding is confusing. When you draw those Carbon hybrids, I get that you're showing what's going on with energy level 2, but what happened to 1s? How does that 1s orbital fit in with what's going on?
The 1s orbital continues to exists. The electrons in the 1s orbital are not involved in any type of interaction with other atoms, so we don't draw them.
The main idea to remember is that in a covalent bond, the electrons are between the nuclei of atoms, and these electrons act as a glue that hold together the nuclei of different atoms, just like peanut butter holds two pieces of bread together.