Is it true that the greater difference in electronegativity in an ionic compound, the greater attraction between the elements in the compound?
Yes, it is true that the greater difference in electronegativity in an ionic compound leads to a greater attraction between the elements in the compound. Electronegativity is a measure of an atom's attraction for the shared pair of electrons in a bond.
To understand why the greater electronegativity difference results in a greater attraction, we need to break down the nature of ionic bonding. Ionic compounds are formed between a metal and a nonmetal. When these elements come together to form a compound, electrons are transferred from the metal (which has a lower electronegativity) to the nonmetal (which has a higher electronegativity).
The transfer of electrons creates positive and negative ions. The metal atom loses electrons, becoming a positively charged ion (cation), while the nonmetal atom gains those electrons, becoming a negatively charged ion (anion). These oppositely charged ions are then attracted to each other, leading to the formation of an ionic bond.
The difference in electronegativity between the metal and nonmetal atoms determines the extent of electron transfer and hence the polarity of the bond. The greater the electronegativity difference, the more polar the bond becomes. This increased polarity strengthens the attractive force between the positive and negative ions, resulting in a greater overall attraction between the elements in the compound.
In summary, a greater difference in electronegativity in an ionic compound indicates a stronger attractive force between the elements, leading to a more stable and tightly bonded structure.