Part B HoS The two sigma bonds form between a p orbital on S and an s orbital on
ID: 580491 • Letter: P
Question
Part B HoS The two sigma bonds form between a p orbital on S and an s orbital on H The two sigma bonds form between a hybrid sp orbital on S and an s orbital on H The two signa bonds form between a hybrid sp orbital on Sand an s orbital on H The two sigma bonds form between a hybrid sp? orbital on S and an s orbital on H O O Submit My Answers Give Up Incorrect, Try Again; 5 attempts remaining Start by drawing the Lewis structure for H2S, then determine the hybridization (or lack thereof) for each atom Each o bond is an end-to-end overlap of orbitals, and hy proper orientation. You can use the electron geometry from the Lewis structure to determine the hybridization scheme Part C ICN o one bond forms between a hybrid sp2 orbital on and apo ital on O One bond forms between a hybrid spa or ital on C and a P orbital on o one bond forms between a hybrid sp2 orbital on C and a p orbital on One bond forms between a hybrid sporttal on Cand a porbital on :one bond forms between a hybrid spor ital on Cand a pot talo N one bond form s between a hybrid s'orbaal on C and a port ital on N : one bond for ns between a hybrid aps orbital on Cand a port tal on N one bond forms between a hybrid ap tital on Cand a hybrid sp orbital on N Submit My Answers Give Ug a DOLLExplanation / Answer
Part B :
H2S
CN = 1/2 (NO of valence eleactron + number of monovalent atom around central ) = 1/2(6+2) = 4
CN = 4 ---> sp3 hybridisation (sp3 hybrid orbitals)
So answer is
Two sigma bonds formed between sp3 hybrid orbitals on S and s orbital on Hydrogen
Part C
ICN ---> linear molecule
Carbon is sp hybridised (triple bond)
So answer is the 4th option
Part A :
H2S
Both dispersion and dipole dipole forces ( Hydrgen bonding only in F , O , N)
Part B
N2O
Both dispersion and dipole dipole
Part C :
C2H5OH
All three forces
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