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Applying Coulomb's law to HCl and LiF
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[QUOTE="needingtoknow, post: 4851253, member: 469601"] So electronegativity is the tendency of an atom to attract electrons in a bond. We know that fluorine has a greater electronegativity than lithium and therefore attracts more electrons. In HCl chlorine is more electronegative than hydrogen. For LiF the electronegativity difference is greater making it an ionic bond and HCl a polar attraction. Knowing this why are the charges (q1 and q2) for lithium and fluorine so much greater than the charges for hydrogen and chlorine (q1 and q2)? Is it because the fluorine atom takes more electrons from the lithium (due to its electronegativity) which increases the overall charge of fluorine to 1 C and the overall charge of lithium to -1 C, both of which are numbers that may be determined experimentally? Is my reasoning correct? [/QUOTE]
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Applying Coulomb's law to HCl and LiF
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