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
It depends on what x and y are.
The bond angles are 120 degrees
This seems like a misprint. IF6 will have one electron too many to attain an octahedral structure with 90 degree bond angles. SF6 is octahedral, for example, and does have 90 degree angles, as does PF6(-1). Perhaps IF6(+1) is the molecule in question, which will have the proper number of electrons.
The molecule of iodine heptafluoride has a bi-pyramidal pentagonal shape. All of the F-I-F angles between two fluorine atoms in axial and equatorial planes are equivalent to 90 degrees. Therefore there is five of them.
since it has a total of two atoms , its molecular shape is linear with bond angles of 180 degree.
the lone pair causes the molecule to become "bent" which makes the bond angles less than 109.5
When the central atom of a molecule has unshared electron, the bond angles will be less than when all the central atom's electrons are shared.
For a truly trigonal planar molecule the bond angles are 120 0 exactly.
No, both the bonds in CO2 are identical.
It depends on what x and y are.
H2 dihydrogen only contains two atoms there is NO bond angle in a diatomic molecule.
It is formaldehyde in which carbon atom is sp2 hybridized so it is a triangular molecule with bond angles of 1200 .
ionic
- Bond angles - Bond lengths - The location of hydrogen atoms - Chargaff's pairs (although he didn't recognize them at the time)
When a molecule expands within a hydrogen atom it is released by an incorrerated molecule inside a desticated part of the atom.
No, it doesn't. Dipole moment is the measure polarity of a polar covalent bond
The bond angles between two N-H bonds in ammonia are close to the bond angles characteristic of a tetrahedron, but the molecule as a whole is not a tetrahedron because one of the four bonds to a central atom found in an actual tetrahedral molecule is missing; there are only three hydrogen atoms bound to a central nitrogen atom in ammonia. In an ammonium ion, however, the tetrahedron is complete.