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In a symmetrical molecule do the dipole charges cancel out and make the molecule nonpolar?
Yes, in a symmetrical molecule where the dipole moments generated by individual bonds cancel each other out due to symmetry, the overall molecule is nonpolar. This occurs when the molecule has a symmetric shape or an equal distribution of charge.
Can a molecule have bond dipole moments without having a net molecular dipole moment?
Yes, a molecule can exhibit bond dipole moments if there is a difference in electronegativity between the atoms that make up the bond. However, if these bond dipole moments are arranged symmetrically and cancel each other out, the molecule will not have a net molecular dipole moment.
If a molecule contains polar bonds the molecule may or may not be polar overall?
A molecule with polar bonds may or may not be polar overall, depending on its shape and symmetry. If the polar bonds are arranged symmetrically, their dipole moments can cancel each other out, resulting in a nonpolar molecule. Conversely, if the arrangement is asymmetrical, the dipole moments do not cancel, leading to an overall polar molecule. Thus, both the presence of polar bonds and the molecular geometry are crucial in determining the molecule's polarity.
What is the dipole moment of benzanilide?
The dipole moment of benzanilide is approximately zero because the molecule is symmetrical and the dipoles cancel each other out. Benzanilide consists of a benzene ring linked to an aniline group, resulting in opposing dipole moments that effectively cancel each other.
Is ccl2ch2 nonpolar?
Yes, CCl2CH2 (dichloroethylene) is a nonpolar molecule. This is because the dipole moments of the two C-Cl bonds on each side of the molecule cancel each other out due to symmetry, resulting in a net dipole moment of zero.
Is ccl4 polar or non polar?
CCl4 (carbon tetrachloride) is a nonpolar molecule because it has symmetrical tetrahedral geometry, leading to a cancellation of dipole moments. This means that the electronegativity difference between carbon and chlorine atoms results in no overall dipole moment, making the molecule nonpolar.
Is it possible for a molecule to have a bond moments and yet be nonpolar?
Yes, it is possible for a molecule to have bond dipoles (bond moments) that cancel each other out due to their symmetrical arrangement. This results in a nonpolar molecule, even though individual bonds may have a polarity.
In a symmetrical molecule do the dipole charges cancel out and make the molecule nonpolar?
Yes, in a symmetrical molecule where the dipole moments generated by individual bonds cancel each other out due to symmetry, the overall molecule is nonpolar. This occurs when the molecule has a symmetric shape or an equal distribution of charge.
Is carbon tetrachloride or chloroform more polar?
Chloroform is more polar than carbon tetrachloride. This is because chloroform has a dipole moment due to the electronegativity difference between carbon and chlorine atoms, while carbon tetrachloride is nonpolar as the four chlorine atoms cancel out any dipole moments.
Can a molecule have bond dipole moments without having a net molecular dipole moment?
Yes, a molecule can exhibit bond dipole moments if there is a difference in electronegativity between the atoms that make up the bond. However, if these bond dipole moments are arranged symmetrically and cancel each other out, the molecule will not have a net molecular dipole moment.
If a molecule contains polar bonds the molecule may or may not be polar overall?
A molecule with polar bonds may or may not be polar overall, depending on its shape and symmetry. If the polar bonds are arranged symmetrically, their dipole moments can cancel each other out, resulting in a nonpolar molecule. Conversely, if the arrangement is asymmetrical, the dipole moments do not cancel, leading to an overall polar molecule. Thus, both the presence of polar bonds and the molecular geometry are crucial in determining the molecule's polarity.
Does SiCl4 have dipole forces?
No, SiCl4 does not have dipole forces. This is because the molecule is symmetrical and the dipole moments of the chlorine atoms cancel each other out due to the tetrahedral geometry of the molecule.
How can a molecule be non polar when it consists of atoms that have different electronagativities?
A molecule can be nonpolar if its overall shape is symmetric and the individual bond dipoles cancel each other out. This occurs when the molecule has a symmetrical distribution of charge, despite the presence of atoms with different electronegativities. Examples include carbon tetrachloride (CCl4) and methane (CH4).
Does CF4 have a dipole moment?
CF4 does not have a dipole moment because the dipole moments of the C-F bonds cancel out due to the symmetric tetrahedral structure of the molecule. This results in a molecule that is nonpolar overall.
How does the shape of a molecule affect the polarity of a molecule?
The shape of a molecule affects polarity because of how bond dipoles between two atoms is affected by other atoms in the molecule. Bond dipoles are vector quantities (which means they have magnitude and direction), so when a molecule has two or more bond dipoles they can cancel each other out if they perfectly oppose each other. For example CO2 (O=C=O) has two dipole bonds, but since they equaly oppose each other they cancel out and the molecule is nonpolar. In bent molecules like H2O, the two hydrogens bonded to the oxygen have equal dipole moments, but they do not directly oppose each other so they do not cancel out. As a result the molecule is polar. So in summery the molecule's geometry affects the polarity of the molecule by dictating the direction of the vector quantities of the dipole bonds, which determines whether they will be able to cancel each other out (nonpolar) or allow for non zero dipole moments (polar).
How does the shape of a a molecule affect the polarity of the molecule?
The shape of a molecule affects polarity because of how bond dipoles between two atoms is affected by other atoms in the molecule. Bond dipoles are vector quantities (which means they have magnitude and direction), so when a molecule has two or more bond dipoles they can cancel each other out if they perfectly oppose each other. For example CO2 (O=C=O) has two dipole bonds, but since they equaly oppose each other they cancel out and the molecule is nonpolar. In bent molecules like H2O, the two hydrogens bonded to the oxygen have equal dipole moments, but they do not directly oppose each other so they do not cancel out. As a result the molecule is polar. So in summery the molecule's geometry affects the polarity of the molecule by dictating the direction of the vector quantities of the dipole bonds, which determines whether they will be able to cancel each other out (nonpolar) or allow for non zero dipole moments (polar).
Does KrBr4 have a net dipole movement?
KrBr4 does not have a net dipole moment because the molecule is symmetrical and the dipole moments of the individual bromine atoms cancel each other out.
