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Re: Polarity of CCl2H2. Postby Levina Lin 1L » Sat Nov 08, 2014 11:47 pm. The symmetry of a tetrahedral molecular structure does allow dipole moments to cancel each other - however, these dipole moments must all be the same. In CCl2H2, the central C atom is attached to 2 H atoms and 2 Cl atoms. Since H and Cl have different electronegativities ...
CCl2H2 (dichloroacetylene) is nonpolar because the molecule is symmetrically arranged, with the two chlorine atoms canceling out the dipole moments created by the hydrogen atoms. It's polar ...
Postby Chem_Mod » Wed Sep 14, 2011 2:39 am. Question: Given a formula like CCl2H2 and asked about polarity, how does one determine where the Cl and H atoms lie. For example, if there is one Cl on each side of the carbon, and one H on each side, the formal charges will cancel out. in the other setup, they won't. Top. Chem_Mod.
Re: CCl2H2. Postby MeeraBhagat » Mon Dec 09, 2019 4:11 pm. If a tetrahedral shape had all the same bonds in the same plane then the dipole moments could cancel. However, because it is a three dimensional shape, as Lavelle said, the only way for the dipole moments to cancel is if the central atom is bound to four atoms of the same element. Top.
Hello, Tetrahedral molecules are not always polar. For example, Methane, CH4, is non-polar. This is because the dipoles all cancel out. However, for a molecule like the one you mentioned, the equatorial and axial planes contain different atoms, so the tetrahedral shape means that not all dipoles will be canceled out, making the molecule polar.
405310750 wrote: Since the structure of this molecule is tetrahedral, it is not the same that it looks when drawn as a 2 d Lewis structure. Essentially a tetrahedral structure can be rotated in different ways that is not accurately depicted in a 2 d structure, so if the H's and Cl's were opposite each other the molecule would still be polar.
Postby GabrielGarciaDiscussion1i » Thu Nov 16, 2017 10:53 pm. On the topic of the polarity as a whole, CCl2 would be considered non-polar because the electronegativity vectors cancel out but be careful because, as seen on the midterm, there is a distinction between the overall polarity and the polarity of the individual bonds.
TEST 2 POLAR molecule Post by JustinHorriat_4f » Mon Dec 02, 2019 7:31 am Why is the molecule that shows the lewis structure of CCl2H2 a polar molecule, I thought that the Cl atoms are pulling different ways so it makes the overall molecule non polar?
So is this instance the cl bonds form dipoles, which can be visualized as vectors pointing towards the chlorine atoms. If the vectors are on the same side (like in cis-dichloroethene), they do not cancel and result in a polar molecule. If the chlorines are on opposite sides(in trans-dichloroethene) and the dipoles cancel then it is non-polar.
Re: Polar vs. Nonpolar. Postby Bilal Pandit 1J » Mon Nov 25, 2019 6:20 am. The reason that molecule is polar is that the shape is tetrahedral, which means the two Cl atoms aren't going to be opposite of each other. Since they aren't opposites of each other, they will not cancel out and as a result, the molecule will have a net dipole.