Pls explain this question
Answers
Explanation:
Electronegativity is a measure of an atom's ability to attract shared electrons to itself. On the periodic table, electronegativity generally increases as you move from left to right across a period and decreases as you move down a group.
Polarity Bond is the separation of electric charge along a bond, leading to a molecule or its chemical groups having an electric dipole or dipole moment. Electrons are not always shared equally between two bonding atoms.
so the more the electronegative the element is, the stronger the bond is between 2 elements.
Hopefully understandable ^-^.
Electronegativity is a property of an element. It is the property by which an element tends to attract a shared pair of electrons in a bond towards itself.
Highly electronegative elements tend to pull electrons more towards themselved than less electronegative elements. So, by taking the difference between the electronegativities of two elements, we can identify the type of bond.
In ionic bond, an element donates electrons and the other recieves it. So, the element that donates has low electronegativity as compared to the element that recieves. So, only elements of very low electronegativity tend to donate. e.g. Na, K, Cs, Ca etc
This means that if the electronegativity difference between two elements is large the bond is ionic. e.g. NaCl, KCl, CaF2
Similarly, consider covalent bonds. In covalent bond, there is sharing of electrons. Neither element is willing to give up their electrons completely. This means that, both elements have comparable electronegativities as both elements tend to pull the shared pair of electrons towards itself almost equally. e.g. N2, O2
Polarity simply means charge separation. Highly polar compounds have high charge separation (due to one element donating, getting +ve charge and other atom recieving electron, getting -ve charge) and are ionic. Lesser polarity implies lesser charge separation and hence more covalent bonds.
(Note that all ionic bonds are not 100% ionic and not all covalent bonds are 100%covalent)