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Which statement explains why the bonds between nonmetals tend to be covalent? The bonds are found to be nondirectional. They have large differences in electronegativity. They have small differences in electronegativity. They have ions that produce an electrostatic pull.

Amanda Johnson

in Chemistry

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1 answer

Nicholas Rivera on October 15, 2018

ANSWERThey have small differences in the electronegativityEXPLANATIONElectronegativity is the probability of an atom to attract the electrons of another atom.Generally speaking, non-metals have electronegativity in high levels. When we go from left to right across a period (row) in the periodic table, the electronegativity increases due to increased nuclear charge and decreasing atomic radius. (The electronegativity also increases when we go from top to bottom on a periodic table of the family.) From the non-metals are on the right side of the row, they would have large electronegativities.Because non-metals, generally, have higher electronegativities as compared with metals, non-metals have a close understanding of their own electrons.It also means that the difference of electronegativity between the non-metals are relatively small. Non-metals' tendencies to attract electrons are nearly the same force; a "tug of war" situation that occurs with respect to the attraction of the electrons. Thus, non-metals tend to end up sharing the electrons.In contrast, an ionic bond between a metal and a non metal has a large difference of electronegativity. This means that a non-metal, with its great tendency to attract electrons, very easily the valence electrons of a metal to form an ionic bond.

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