The approximate bond angles in CHClO is 120 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.
SeF6 is a regular octahedron , all bond angles are 90 degrees
The approximate bond angle for OCS is around 178 degrees.
The approximate bond angle for a molecule with a trigonal planar shape is 120 degrees.
In NOCl, the approximate bond angles are 107 degrees between the N-O bond and the N-Cl bond due to the lone pairs on the nitrogen causing repulsion and pushing the bonding pairs closer together, resulting in a slight compression of the angle from the ideal 120 degrees for trigonal planar geometry.
The approximate Cl-Si-Cl bond angle in SiCl2F2 is expected to be around 109.5 degrees. This is because the molecule adopts a tetrahedral geometry due to the presence of four electron pairs around the silicon atom, resulting in bond angles close to the ideal tetrahedral angle.
If you draw out the Lewis Structure you can see that CHClO has a central atom of C with a single bond to H, a single bond to Cl, and a double bond to O. Since C has 4 bonds it is happy with all of its 8 electrons and has no lone pair electrons; therefor there are only 3 forces off of C that we have to worry about. These 3 forces are going to want to push each other away as far as possible. While Cl is going to be stronger than H in pushing force the farthest possible is still going to be trigonal planar geometry, which is a flat 2D triangle, like what you would draw on paper when sketching the Lewis structure. The approximate bond angles in CHClO are therefor going to be 120o (360o/3 = 120o). However, for future reference, the approximate bond angles are only exact when all charge clouds are equivalent. For example, CHClO is trigonal planar with bond angles of approximately 120 degrees, but BCl3 is trigonal planar with bond angles of exactly 120 degrees. Molecules that contain a lone pair on the central atom show even more distortion in the bond angles.
90 and 180 are the approximate bond angles.
The approximate bond angle for OCS is around 178 degrees.
SeF6 is a regular octahedron , all bond angles are 90 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.
In NOCl, the approximate bond angles are 107 degrees between the N-O bond and the N-Cl bond due to the lone pairs on the nitrogen causing repulsion and pushing the bonding pairs closer together, resulting in a slight compression of the angle from the ideal 120 degrees for trigonal planar geometry.
The approximate bond angle for a molecule with a trigonal planar shape is 120 degrees.
PCl5 is covalent in the vapour phase with a trigonal biyramidal shape. It is ionic in the solid consisting of PCl4+ PCl6- In solution it can be covalent or ionic depending on the solvent.
The bond angles are 120 degrees
trigonal planar
The bond angle in COH2 is approximately 90 degrees. Each hydrogen atom is located at the corners of a triangle around the central oxygen atom, resulting in a bent molecular geometry.
Urea is sp2 hybridized, so the bond angles are ~120 degrees.