The difference in electronegativity causes polar bond between O and H
Electronegativity is the propensity of an atom in a molecule to draw the shared pair of electrons toward itself.
Electronegativity is an index of the tendency of an atom to attract electrons. It is proportional to the difference between an atom’s ionization potential and its electron affinity. Linus Pauling placed electronegativity values on a scale of slightly less than 1.0 for alkali metals to a maximum of 4.0 for fluorine (Figure 1.3). The alkali metals and alkaline earth metals tend to lose an electron to gain an inert gas configuration. Thus, groups I and II contain the least electronegative atoms. In fact they are electropositive.
On the other end of the scale, halogens, in group VII, tend to gain an electron to give an inert gas configuration. Thus, we find that electronegativity increases from left to right across the periodic table. Electronegativity values increase in period 2 in the order C < N < O < F. Electronegativity values decrease from top to bottom within a group of elements. We will often use these periodic trends to interpret the chemical and physical properties of organic compounds.
Hence The difference in electronegativity causes polar bond between O and H
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