It is kind of difficult to tell the formula without using subscripts and superscripts, so here is a Lewis Dot structure to make it easier to see. (Ignore the periods.)
|.....Cl.......| 1-
|.......|.......|
|Cl - I - Cl |
|.......|.......|
|_....Cl....._|
90 degree
120 degree
180 degree
This compound has a square planar molecular geometry with equal 90o bond angle
This compound has a square planar molecular geometry. Therefore the bond angles are equal to 90 degrees.
90, 120, 180.
90 degrees
Lol
90
If it is non polar, the bond angles are as follows:I-P-I bond angles: 120ºBr-P-Br bond angles: 180ºI-P-Br bond angles: 90º
The approximate bond angles in CHClO is 120 degrees.
First off, ICl4 doesn't really exist. It should be ICl4- as the lone electron on Iodine (the central atom) will instantly pull another electron to itself to make a lone pair. Therefore iodine has two lone pairs and four elemental bonds (one to each chlorine). Since we have six total bonds (including the lone pairs) the geometrical shape will be octahedral. However, since, the lone pairs repel each other they will go to the top and bottom of the structure, making ICl4 square planar. So no, it is not bent per se, but it does deviate from the expected shape of ICl4 (3+) (which would be trigonal bipyramidal) because of the lone pairs.
jhi
SeF6 is a regular octahedron , all bond angles are 90 degrees
90, 120, 180.
ICl4-'s electron domain geometry is octahedral.
The bond angles are 120 degrees
90 and 180 are the approximate bond angles.
If it is non polar, the bond angles are as follows:I-P-I bond angles: 120ºBr-P-Br bond angles: 180ºI-P-Br bond angles: 90º
First off, ICl4 doesn't really exist. It should be ICl4- as the lone electron on Iodine (the central atom) will instantly pull another electron to itself to make a lone pair. Therefore iodine has two lone pairs and four elemental bonds (one to each chlorine). Since we have six total bonds (including the lone pairs) the geometrical shape will be octahedral. However, since, the lone pairs repel each other they will go to the top and bottom of the structure, making ICl4 square planar. So no, it is not bent per se, but it does deviate from the expected shape of ICl4 (3+) (which would be trigonal bipyramidal) because of the lone pairs.
The approximate bond angles in CHClO is 120 degrees.
Urea is sp2 hybridized, so the bond angles are ~120 degrees.
jhi
nonpolar
SeF6 is a regular octahedron , all bond angles are 90 degrees
Monoiodine tetrachloride.