SeF6 is a regular octahedron , all bond angles are 90 degrees
The approximate bond angle for OCS is around 178 degrees.
The approximate bond angles in CHClO are around 109.5 degrees for the H-C-Cl bond angle, 107 degrees for the C-Cl-O bond angle, and 104.5 degrees for the H-C-O bond angle, following the expected tetrahedral geometry around carbon.
NOCl nitrosyl chloride has a Cl-N=O bond angle of 1130
For a truly trigonal planar molecule the bond angles are 120 0 exactly.
If it is non polar, the bond angles are as follows:I-P-I bond angles: 120ºBr-P-Br bond angles: 180ºI-P-Br bond angles: 90º
90 and 180 are the approximate bond angles.
The approximate bond angles in CHClO are around 109.5 degrees for the H-C-Cl bond angle, 107 degrees for the C-Cl-O bond angle, and 104.5 degrees for the H-C-O bond angle, following the expected tetrahedral geometry around carbon.
The approximate bond angle for OCS is around 178 degrees.
The approximate bond angles for BrF5 is approximately 90 degrees because there would be one lone pair of electrons left over, making the molecular shape square pyramidal... This gives an approximate bond angle of 90 degrees. AX5E, sp3d2 hybridized.
NOCl nitrosyl chloride has a Cl-N=O bond angle of 1130
For a truly trigonal planar molecule the bond angles are 120 0 exactly.
The bond angles are 120 degrees
If it is non polar, the bond angles are as follows:I-P-I bond angles: 120ºBr-P-Br bond angles: 180ºI-P-Br bond angles: 90º
In the case of ammonia (NH3), the predicted bond angle based on idealized geometry is 109.5 degrees, but the actual bond angle is around 107 degrees due to the presence of lone pairs repelling the bonded pairs. In the case of water (H2O), the predicted bond angle based on idealized geometry is 104.5 degrees, but the actual bond angle is around 104 degrees due to the presence of lone pairs repelling the bonded pairs.
Urea is sp2 hybridized, so the bond angles are ~120 degrees.
The strength of an amide bond is about 79-86 kcal/mol. It is stronger than a typical hydrogen bond but weaker than a typical covalent bond.
Selenium hexafluoride