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....._|
XeF4 is isostructural with ICl4. Both compounds have a square planar molecular geometry with bond angles of 90 degrees and are considered isostructural due to their similar arrangement of atoms in the molecule.
The approximate bond angles in CHClO are around 109.5 degrees for the H-C-Cl bond angle, 107 degrees for the C-Cl-O bond angle, and 104.5 degrees for the H-C-O bond angle, following the expected tetrahedral geometry around carbon.
The ion ICl4- is called tetrachloroiodate(1-) ion.
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 bond angles in HClO3 are approximately 109.5 degrees.
90, 120, 180.
XeF4 is isostructural with ICl4. Both compounds have a square planar molecular geometry with bond angles of 90 degrees and are considered isostructural due to their similar arrangement of atoms in the molecule.
The approximate bond angles in CHClO are around 109.5 degrees for the H-C-Cl bond angle, 107 degrees for the C-Cl-O bond angle, and 104.5 degrees for the H-C-O bond angle, following the expected tetrahedral geometry around carbon.
ICl4-'s electron domain geometry is octahedral.
The ion ICl4- is called tetrachloroiodate(1-) ion.
The bond angles are 120 degrees
The bond angles of CO2 are 180 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.
90 and 180 are the approximate bond angles.
The bond angles in HClO3 are approximately 109.5 degrees.
The bond angles in HNO2 are approximately 120 degrees.
The bond angles of SO2 are approximately 119 degrees.