OCl2 has a bond angle of 110. This is because the oxygen has 2 bonded pairs and 2 unbonded/lone pairs. To minimize electron repulsion they more apart as far as possible which creates a bent shaped molecule.
silicon oxychloride is the most popular name for this. This is a very obscure area of chemistry- not a lot is known about halosiloxanes. Molecular SiOCl2 probably does not exist., there are various reports of polymeric forms with four coordinate Si- so a reasonable guess would be that these contain tetrahedral sp3 silicon with a bond angle of 109.5.
Its bond angle will be somewhat more obtuse than the similarly structured water molecule, because of chlorine's large number of unbonded electron pairs. Perhaps 108 degrees or so. However, it will not exceed 109.5 because that's a tetrahedral bond angle, and sulfur's electron domain geometry is tetrahedral.
103 degrees and it is a bent angle. It is less than tetrahedral as the lone pairs repel more than bonding pairs (VSEPR theory)
The angle has 103 degrees.
134.3o. It is a bent molecule, but because of the additional electron pairs on the O atoms, the bond angle is deviated from 120o.
the shape is linear and the bond angle is 180 degree
It forms a linear bond. The bond angle is 180 degrees
120 degrees
105
Increases
Bond angle is 109.5 degrees.It is equal in every bond
NH4+ is tetrahedral, with bond angle of 109.5o
the f-p-f bond angle is 120the cl -p-cl bond angle is 180and the f - p - cl bond angle is 90
Bond Angle (:
The bond angle for H2S is 92.1­°.
The water molecule's bond angle is about 104.45 degrees.
the shape is bent and the bond angle is approximately 120
No, the bond angle for linear structure is 180 degrees.
The answer would be bond angle, for number 19#
The question is nonsense. WHICH bond angle? There are many of them in a molecule the size of estradiol.
SF3 is a radical, and the bond angle has not been determined. SF4 has a see-sawshape with a bond angle of 101.6 0 SF6 has an undistorted octahedral shape with a bond angle of 90 0.