Draw the Lewis structure for OCl2. What is the molecular shape of this compound?
a. linear
b. trigonal planar
c. tetrahedral
d. trigonal bipyramidal
e. octahedral
f. bent
g. trigonal pyramidal
5 Answers
The Lewis structure for OCl2 is:
.. Electron geometry = Tetrahedral
Cl – O : Molecular shape = Bent
| Hybridization = sp^3
Cl Bond Angle = 109°
Keep in mind that your question asked for ‘molecular shape’ (geometry) of the molecule which is bent/angular and not the the ‘electron geometry’ of the molecule, which is tetrahedral. (To clarify things, see this forum discussion that looks at the difference between the two geometries here: http://www.chemicalforums.com/index.php?topic=4339… )
Ocl2 Lewis Structure
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Draw the Lewis structure for OCl2. What is the molecular shape of this compound?
Draw the Lewis structure for OCl2. What is the molecular shape of this compound?
a. linear
b. trigonal planar
c. tetrahedral
d. trigonal bipyramidal
e. octahedral
f. bent
g. trigonal pyramidal
The molecular structure of OCl2 is “bent”. The electron cloud geometry of the central atom (oxygen) is tetrahedral. Oxygen uses sp3 hybridization resulting in four identical hybrid orbitals directed at four corners of a tetrahedron. Two of those orbitals already have two electrons each, but the other two have only one electron each. Similar hybridization occurs in each chlorine atom, but each chlorine atom only has one hybrid orbital with only one electron in it. The incomplete orbitals on oxygen and chlorine atoms link up with the result that both chlorine atoms become attached to the same oxygen atom at two separate corners of the oxygen’s tetrahedral geometry. Linking the nucleus of the oxygen atom with each chlorine atom’s nucleus will create an angle which gives the molecule its bent shape.
Answer: f. bent
:N(-F:::)3 trigonal pyramidal around 100 deg ::Te(-Cl:::)2 bent around 109.5 deg C(-Cl:::)4 tetrahedral exactly 109.5 deg :S(=O::)2 bent around 120 deg