No, because two of the molecules have no bond angles at 120 °.
To answer this question, you must draw the Lewis structures of the compounds and determine their VSEPR shapes.
##”SeS”_3##
The Lewis structure of ##”SeS”_3## is
(from www.homeworklib.com)
This is an ##”AX”_3## molecule, and its geometry is trigonal planar.
All bond angles in a trigonal planar molecule are approximately 120 °.
##”SeS”_2##
The Lewis structure of ##”SeS”_2## is
##:stackrel(“. .”)(“S”)=stackrel(“. .”)(“Se”)=stackrel(“. .”)(“S”):##
This is an ##”AX”_2″E”## molecule.
Its electron geometry is trigonal planar.
The bond angle in an ##”AX”_2″E”## molecule is approximately 120 °.
##”PCl”_5##
The Lewis structure of ##”PCl”_5## is
This is an ##”AX”_5## molecule, and its geometry is trigonal pyramidal.
The equatorial bond angles in a trigonal bipyramidal molecule are all 120 °.
##”TeCl”_4##
The Lewis structure of ##”TeCl”_4## is
This is an ##”AX”_4″E”## molecule.
Its electron geometry is trigonal pyramidal.
The equatorial bond angle between the equatorial ##”Te-Cl”## bonds is approximately 120 °.
##”ICl”_3##
The Lewis structure of ##”ICl”_3## is
This is an ##”AX”_3″E”_2## molecule.
Its electron geometry is trigonal pyramidal, and its molecular geometry is T-shaped.
The ##”I-Cl”## bond angles in a T-shaped molecule are both approximately 90 °.
##”XeCl”_2##
The Lewis structure of ##”XeCl”_2## is
This is an ##”AX”_2″E”_3## molecule.
Its electron geometry is trigonal pyramidal, with the lone pairs in the equatorial positions.
The molecule is linear, with a ##”Cl-Xe-Cl”## bond angle of 180 °.
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