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What molecule is a polar bond but is not a polar molecule?
CO2 , carbon dioxide (2 linear, opposite dipoles O=C=O)
How do polar bonds contribute to polarity of a molecule?
Polar bonds are created when there is an unequal sharing of electrons between atoms in a covalent bond. If a molecule contains polar bonds that are not canceled out by symmetry, the molecule itself will be polar. This is because the bond dipoles do not cancel each other out, leading to an overall dipole moment for the molecule.
Why might a molecule be no polar even if it's bonds are all polar?
A molecule can be nonpolar even if it contains polar bonds if its overall molecular geometry is symmetrical. In such cases, the dipole moments of the polar bonds can cancel each other out, resulting in no net dipole moment for the molecule. For example, carbon dioxide (CO2) has polar C=O bonds, but its linear shape means the dipoles are equal and opposite, making the molecule nonpolar.
What is true about a molecule which contains two polar bonds which have the different degrees of polarity will it always be polar or never be polar or only be polar if it is bent?
A molecule with two polar bonds of different polarities can still be polar if the individual bond dipoles do not cancel each other out. The overall polarity of the molecule depends on its geometry and symmetry. If the molecule is linear, it will not be polar regardless of the differing bond polarities. If it is bent or asymmetrical, it will be polar.
Is SCl6 non-polar?
Yes, sulfur hexachloride (SCl6) is a non-polar molecule. Although it has polar bonds between sulfur and chlorine, the symmetrical octahedral geometry of the molecule allows the dipoles to cancel each other out. As a result, there is no overall dipole moment, making SCl6 non-polar.
A molecule with polar bonds can be polar?
Yes, a molecule with polar bonds can be polar if the bond dipoles do not cancel each other out due to the molecule's overall geometry. This results in an uneven distribution of charge within the molecule, making it polar.
Will A molecule with polar covalent bonds will definitely be a polar molecule?
not necessarily. if the individual dipoles cancel off, then the molecule will be non-polar. As in CCl4, PCl5 etc
How does a molecule that has polar bonds be nonpolar?
A molecule with polar bonds can be overall non-polar if the bond dipoles cancel each other out. For example the following all have polar bonds but the bond dipoles cancel each other out (vector addition) to make the molecule non-polar. Linear - CO2 trigonal planar - BF3 tetrahedral molecules, CF4 trigonal bipyramidal PF5 octahedral SF6
Is it possible for a compound that contains polar bonds to be a non polar compound?
Yes, it is.A compound is non-polar if there is no net dipole.This can be achieved through one of the following:It has no polar bonds orThe shape of the molecule is such that the dipoles created cancel out.This means that a compound with polar bonds must have a symmetrical shape in order for it to be non-polar.Take CCl4 (carbon tetrachloride). The C-Cl bond is polar, however, the shape of the molecule is tetrahedral - it is symmetrical and so dipoles cancel out. Therefore, it is non-polar.
What will a molecule in which the polar covalent bonds do not cancel out be?
A molecule with polar covalent bonds that do not cancel out will be polar overall. This is because the bond dipoles do not cancel each other out, leading to an overall molecular dipole moment. Examples of such molecules include water (H2O) and ammonia (NH3).
What molecule is a polar bond but is not a polar molecule?
CO2 , carbon dioxide (2 linear, opposite dipoles O=C=O)
How do polar bonds contribute to polarity of a molecule?
Polar bonds are created when there is an unequal sharing of electrons between atoms in a covalent bond. If a molecule contains polar bonds that are not canceled out by symmetry, the molecule itself will be polar. This is because the bond dipoles do not cancel each other out, leading to an overall dipole moment for the molecule.
Why might a molecule be no polar even if it's bonds are all polar?
A molecule can be nonpolar even if it contains polar bonds if its overall molecular geometry is symmetrical. In such cases, the dipole moments of the polar bonds can cancel each other out, resulting in no net dipole moment for the molecule. For example, carbon dioxide (CO2) has polar C=O bonds, but its linear shape means the dipoles are equal and opposite, making the molecule nonpolar.
Does I2O have a dipole moment and are the bonds polar or non polar?
I2O does not have a dipole moment because the bond dipoles of the I-O bonds cancel each other out due to the linear molecular geometry. The bonds in I2O are nonpolar because the electronegativity difference between iodine and oxygen is small, resulting in a symmetrical distribution of electrons.
What is true about a molecule which contains two polar bonds which have the different degrees of polarity will it always be polar or never be polar or only be polar if it is bent?
A molecule with two polar bonds of different polarities can still be polar if the individual bond dipoles do not cancel each other out. The overall polarity of the molecule depends on its geometry and symmetry. If the molecule is linear, it will not be polar regardless of the differing bond polarities. If it is bent or asymmetrical, it will be polar.
Is CIF3 a polar covalent?
Yes, the Cl-F bonds are polar and the resultant bond dipoles do not cancel out because of the shape of the molecule, Bent T shape.
Is XeF4 a polar molecule?
Yes, XeF4 is a polar molecule. Although it has a symmetrical square planar shape, the individual bond dipoles created by the polar Xe-F bonds do not cancel each other out, resulting in a net dipole moment.
