7.100c | How to determine if Cl2CCBr2 has a dipole moment

"Identify the molecules with a dipole moment:
Cl2CCBr2"```
Molecule Cl₂CCBr₂ and Its Dipole Moment

**Cl₂CCBr₂**, also known as **1,1-dichloro-2,2-dibromoethane**, is a **polar molecule**. Let's analyze its structure to determine why it has a dipole moment:

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Structure of Cl₂CCBr₂:
*Geometry:* The central carbon atoms are connected in a *linear arrangement* (C-C) with two chlorine (Cl) atoms bonded to one carbon and two bromine (Br) atoms bonded to the other carbon, forming a *linear molecular geometry* with bond angles of **180°**.
*Polarity of Bonds:*
The *C-Cl* and *C-Br* bonds are *polar* because chlorine and bromine are more electronegative than carbon.
However, the polarities of the bonds in each part of the molecule (C-Cl and C-Br) do not cancel out due to the *asymmetric arrangement* of the chlorine and bromine atoms on either side of the carbon-carbon bond.

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Dipole Moment:
The molecule is *asymmetric* due to the different electronegativities of chlorine and bromine, resulting in an unequal distribution of electron density.
The dipoles from the *C-Cl* bonds and *C-Br* bonds do not cancel out, leading to a **net dipole moment**.

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Conclusion:
The molecule *Cl₂CCBr₂* has a *dipole moment* because of the *asymmetric distribution* of polar bonds and the differing electronegativities of chlorine and bromine.
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