Ccl4 molecular structure The C-Cl bonds in CCLO4 are polar, meaning that the electrons in the bond are not distributed evenly between the carbon and chlorine atoms. The chlorine atoms are more electronegative than the carbon atom, which means that they have a stronger pull on the electrons in the bond. This results in a partial negative charge on the chlorine atoms and a partial positive charge on the carbon atom. The polar nature of the C-Cl bonds in CCLO4 makes it a polar molecule, meaning that it has a net dipole moment. The dipole moment is a measure of the separation of charge in a molecule, and it is represented by a vector that points from the negative charge to the positive charge. The dipole moment of CCLO4 is approximately 1.56 Debye. The tetrahedral molecular structure of CCLO4 is also responsible for its physical properties. The tetrahedral shape of the molecule makes it more compact than if the chlorine atoms were arranged in a linear or planar fashion. This results in a higher boiling point and a higher density than if the molecule were less compact. In summary, CCLO4 is a tetrahedral molecule with a central carbon atom surrounded by four chlorine atoms. The C-Cl bonds in the molecule are polar, which makes the molecule polar and gives it a net dipole moment. The tetrahedral shape of the molecule is responsible for its physical properties, including its boiling point and density. CCLO4, also known as tetrachlorocarbane or carbon tetrachloride, is a chemical compound with the molecular formula CCl4. It is a colorless, volatile liquid with a mildly sweet odor, and it is highly soluble in organic solvents. In summary, CCLO4 is a tetrahedral molecule with a central carbon atom surrounded by four chlorine atoms. The C-Cl bonds in the molecule are polar, which makes the molecule polar and gives it a net dipole moment. The tetrahedral shape of the molecule is responsible for its physical properties, including its boiling point and density.