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.
90 degrees
Bond angle can be caused by internal angle between the orbitals having bonded pair of électrons, hybridization, presence of lone pair of electrons and electronegativity of the atom. and also Bond energy
CH3 is a trigonal planar and has a hybridization of sp3
The formula looks like trans- 2-butene. The c atoms working left to right will have sp3 sp2 sp2, sp3 hybridisation. the bond angles will be tetrahedral on the sp3 centers, 120 0 on the sp2 centres which have a planar shape, with all four substituents lying in the same plane. Good picture in wikipedia. The actual bond angles will deviate slightly.
The bond angles are 120 degrees
120 degrees.
90 and 180 are the approximate bond angles.
The approximate bond angles in CHClO is 120 degrees.
sp2 with 120 degree bond angles.
180
SeF6 is a regular octahedron , all bond angles are 90 degrees
90 degrees
NOCl nitrosyl chloride has a Cl-N=O bond angle of 1130
90 i am sure
For a truly trigonal planar molecule the bond angles are 120 0 exactly.
in single bond hybridization will be sp3 and take tetrahedral shape as in CH4 in double bond hybridization will be sp2 and take planar triangle shape as in C2H4in triple bond hybridization will be sp and take linear shape as in C2H2
Bond angle can be caused by internal angle between the orbitals having bonded pair of électrons, hybridization, presence of lone pair of electrons and electronegativity of the atom. and also Bond energy