The methylene radical CH2 has just 6 electrons around the central carbon. The lowest energy methylene is "triplet" methylene with two unpaired electrons. Simple VSEPR cannot predict the bond angle which is measured as being 133 0. A slightly higher energy form has no unpaired electrons and the angle is measured at 102 0. This is in accord with simple VSEPR theory which would predict a decrease in bond angle from 120 0 due to repulsion of the lone pair.
In compounds the -CH2- unit in alkanes such as propane the bond angles are close to 109 0 the tetrahedral angle (sp3 hybridisation). When =CH2 terminates an alkene such as ethene (ethylene) the bond angle is close to 120 0, (sp2 hybridisation)
The bond angle for H2S is approximately 92 degrees.
The bond angle in NI3 is approximately 107 degrees.
The bond angle for AsF3 is approximately 87.5 degrees.
The bond angle for NBr3 is approximately 107 degrees.
The bond angle for IO2 is around 120 degrees.
HNC stand for "Higher National Certificate"
The bond angle for H2S is approximately 92 degrees.
CH2NH2 is trigonal pyramidal. It has a central nitrogen atom with three bonded atoms and one lone pair, resulting in a trigonal pyramidal geometry.
The bond angle in NI3 is approximately 107 degrees.
The bond angle for AsF3 is approximately 87.5 degrees.
The bond angle for NBr3 is approximately 107 degrees.
The bond angle for IO2 is around 120 degrees.
The water molecule's bond angle is about 104.45 degrees.
The bond angle for SBr2 is approximately 102 degrees.
No, the bond angle for linear structure is 180 degrees.
The bond angle of a hydrogen molecule is 180 degrees.
The answer would be bond angle, for number 19#