(For mobile users) 00:07 Sketch of axes 02:05 Reducible representation for sigma orbitals 04:54 A1 irreducible representation 07:18 A2 irreducible representation 09:05 B1 irreducible representation 10:35 B2 irreducible representation 14:15 Effect of symmetry operations on representative orbital 15:00 A1 group orbital combination 16:10 B1 group orbital combination 17:30 Combining group orbitals with atomic orbitals on oxygen 21:55 Sketching energy level diagram for molecular orbitals
I don't have time to show in a video, but I probably can talk you through the few tricky parts. Pick a C2h molecule - trans1,2-dichloroethylene is a nice choice. Draw it. Draw a circle (an s orbital) around each H or Cl atom. Label one Cl "s1" and the other "s2". Label one H "s3" and the other "s4". Don't number or label the C (no need). Now, here's the tricky part; there is NO symmetry operation which can turn a H into a Cl, or vice versa. This means we have to treat them separately. Let me know if this makes sense; ask any questions. If you get his far, you are already half finished.
Each HF molecule can make two (2) hydrogen bonds; H is an H-donor and F is a H-acceptor. H₂O, on the other hand, can make up to four (4) hydrogen bonds; each of the two (2) H's are H-donors, and the oxygen atom is a double H-acceptor (it can accept two H-bonds, because it has two lone pairs.) Higher boiling point comes from greater strength of intermolecular forces. For HF and H₂O, the relevant intermolecular force is hydrogen bonding, and four (4) hydrogen bonds per molecule is stronger than two (2) hydrogen bonds per molecule. Does that make sense?
![[HỌC ZOOM LỚP 5 ] TỈ SỐ PHẦN TRĂM DẠNG TỔNG TỈ, HIỆU TỈ, CÔNG THỨC TÍNH -Thầy Khải- SĐT: 0943734664](http://i.ytimg.com/vi/kFJHNeDSrY8/mqdefault.jpg)
Hello, i finally understood. I have been dealing with subject for about a week. I just cannot thank you enough.
11:33 I was looking at screen with anticipation then you fix 1 to 2 and I got relaxed...
My professor wrote 2, 0, 0, 2 and it confuses me. I watched your video and it made sense!
(For mobile users)
00:07 Sketch of axes
02:05 Reducible representation for sigma orbitals
04:54 A1 irreducible representation
07:18 A2 irreducible representation
09:05 B1 irreducible representation
10:35 B2 irreducible representation
14:15 Effect of symmetry operations on representative orbital
15:00 A1 group orbital combination
16:10 B1 group orbital combination
17:30 Combining group orbitals with atomic orbitals on oxygen
21:55 Sketching energy level diagram for molecular orbitals
Thanks a lot, sir! It had been really helpful and well done. Thanks from Ecuador
Thank you very much sir understood very well as i wish
Thanku very much sir by providing this topic u have done a very precious work for me🙏🙏
Thanks sir .
good tutorial. and very successful
Thank u very much Sir!!!!!
Thank you sir
Thanks sir
Thanks sir.....
Hello would you PLEASEEE Show us also what the SALCs are for a c_2h group? Would help me a lot with my upcoming university exam!!!
I don't have time to show in a video, but I probably can talk you through the few tricky parts.
Pick a C2h molecule - trans1,2-dichloroethylene is a nice choice. Draw it.
Draw a circle (an s orbital) around each H or Cl atom. Label one Cl "s1" and the other "s2". Label one H "s3" and the other "s4". Don't number or label the C (no need).
Now, here's the tricky part; there is NO symmetry operation which can turn a H into a Cl, or vice versa. This means we have to treat them separately.
Let me know if this makes sense; ask any questions. If you get his far, you are already half finished.
Sir please make video of formaldehyde on this topic
Why the boiling point of H2O is higher than that HF?
Each HF molecule can make two (2) hydrogen bonds; H is an H-donor and F is a H-acceptor.
H₂O, on the other hand, can make up to four (4) hydrogen bonds; each of the two (2) H's are H-donors, and the oxygen atom is a double H-acceptor (it can accept two H-bonds, because it has two lone pairs.)
Higher boiling point comes from greater strength of intermolecular forces. For HF and H₂O, the relevant intermolecular force is hydrogen bonding, and four (4) hydrogen bonds per molecule is stronger than two (2) hydrogen bonds per molecule.
Does that make sense?
Thank you much 👏👏