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UrbanXrisis
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what is the difference between bond polarity and molecular polarity?
UrbanXrisis said:so does HCl have a polar or nonpolar "molecular bond"? I wrote down polar but I think it has to be nonpolar acording to what you said
UrbanXrisis said:how is the molecule polar if the structure is symmetrical?
does this mean every polar bond must have be a polar molecule?
UrbanXrisis said:all I know is that symmetrical molecules are nonpolar molecules. That means linear and tetrahedral bonds are considered nonpolar molecules. However, if the EN is between .5-1.7 then it has a polar BOND. So, back to HCl
H-Cl has a linear bond, that means it is a nonpolar molecule.
However, HCl is a EN difference over .5 which means it is a polar bond.
Why is HCl a polar molecule as you said?
UrbanXrisis said:what about H2CO? it's a polar molecule and also has a polar bond right?
UrbanXrisis said:would this molecular structure be called bent or pyramidal? or is it called something else?
great job... way to help someone learn...t!m said:The structure of [tex]H_2CO[/tex] would be trigonal planar, with 120 degree bond angles.
t!m said:Ack, this sort of thing really depends on teacher. No bond is truly nonpolar except for bonds between identical atoms, i.e. C-C bonds. If you're following the rules for END, then yes, I suppose, C=N is a nonpolar bond.
t!m said:Linear bonds are not always nonpolar. I think you're overgeneralizing the concept of symmetry. HCN is actually a polar molecule. Also, both bonds are polar as well, which is actually the reason for the molecule's polarity. Try http://onsager.bd.psu/~jircitano/polar.html site.
Bond polarity refers to the unequal distribution of electrons between two atoms in a chemical bond. Molecular polarity, on the other hand, refers to the overall distribution of charge within a molecule.
Bond polarity affects the overall molecular polarity of a molecule. If a molecule has polar bonds, it will have a polar overall molecular polarity. However, a molecule can also have nonpolar bonds and still have a polar overall molecular polarity if the shape of the molecule causes an unequal distribution of charge.
The electronegativity difference between the atoms involved in the bond is the main factor that determines bond polarity. The larger the difference in electronegativity, the more polar the bond will be.
Molecular polarity is measured using a property called dipole moment. This is a vector quantity that represents the separation of positive and negative charges within a molecule. A higher dipole moment indicates a more polar molecule.
Examples of molecules with polar bonds include water (H2O), ammonia (NH3), and hydrogen fluoride (HF). Examples of molecules with nonpolar bonds include carbon dioxide (CO2), methane (CH4), and oxygen (O2).