How do I go about drawing an orbital diagram and hybridizing:CH3-CH (triple bonded to) CH-C (triple bonded to) C- CHOI'm completely lost.

D a Given that the spatial requirement of a lone pair is greater than that of a bond pair, explain why XeF2 has a linear molecular structure and not a bent one. The four lone pairs of XeF2 occupy the equatorial positions. The angles between lone pairs are 60°, so there is less lone pair/lone pair repulsion with this arrangement. O The two lone pairs of XeF2 occupy the equatorial positions. The angle between lone pairs is 180°, so there is less lone pair/lone pair repulsion with this arrangement. O The two lone pairs of XeF2 occupy the equatorial positions. The angle between lone pairs is 60°, so there is less lone pair/lone pair repulsion with this arrangement. O The three lone pairs of XeF2 occupy the equatorial positions. The angles between lone pairs are 120°, so there is less lone pair/lone pair repulsion with this arrangement. Submit

6. Use VSEPR to predict the geometry and bond angle for each bolded atom in the following structures. HNO₂ H₂C=CHCI CH3CCH

Answer all correctly completely this is complete question

Explain, why CH3Cl has higher dipole moment than CH3F?

Which one of the following covalent compound structures is characterized by the SMALLEST bond angles between pendant hydrogen atoms? H₂O dihydrogen monoxide H-O: H H₂O CH4 NH3 CH₂ carbon tetrahydride H H-C-H H NH₂ nitrogen trihydride H-N-H -I H

Draw correct line-bond structures for the following molecules

Match the indicated atom with the approximate bond angle around it. ... с C D A -CEC-CH2CH3 H N-H

1. Which of the following compounds contains the greatest number of sp2 hybridized carbon atoms? A) B) D) a OH -C=C-H

Please help me out, indicate bond angles at the highlighted positions.