Answer:
∠
O
−
C
−
C
l
≅
120
∘
The central carbon is
s
p
2
−
hybridized........
Explanation:
And thus
∠
C
l
−
C
−
C
l
and
∠
O
−
C
−
C
l
≅
are
120
∘
to a first approximation.
Why this value? We look to
VSEPR theory
. There are 3 regions of electron density around the central carbon, and the most stable geometry is a trigonal plane. While there is a
carbonyl
group, i.e. a
C
=
O
bond, the
π
bond is conceived to lie above and below this trigonal plane.
The
carbonyl oxygen
is likewise conceived to be
s
p
2
-hybridized
, however, here, there are 2 lone pairs on the oxygen centre.
The approximate chlorine-carbon-chlorine bond angle in C2Cl4 is 120°.
The bond angle is defined as the angle between ant two bonds emanating from a common atom.
The compound C2Cl4 is tetrachloroethene. The carbon atoms are sp2 hybridized in this molecule.
Recall that the bond angle of an sp2 hybridized carbon atom is 120°. Therefore the chlorine-carbon-chlorine bond angle in C2Cl4 is 120°.
From the perspective of the VSEPR theory, the geometry of each carbon atom in C2Cl4 is trigonal planar which implies a bond angle of 120°.
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