Based on electronegativity values, which type of elements tends to have the greatest attraction for electrons in a bond?
(1) metals (3) nonmetals
(2) metalloids (4) noble gases

We can note from the periodic table that as you proceed towards the right across a period, electronegativity tends to increase. Therefore, since nonmetals exist on the right hand side of the periodic table, we can deduce that (3) nonmetals have the greatest attraction for electrons in a bond. It is also good to notice that as you travel down the periodic table along the groups, electronegativity decreases, but metallic characters increase. Therefore, we can say that there is a negative correlation between metallic characters and electronegativities, further supporting our answer.

Electronegativity shows the tendency of attracting electrons. The higher electronegativity is, the higher that element has a tendency to attract electrons.

Metals tend to give out electrons, not to attract electrons. Noble gases hardly ever attract or give out electrons, for they already have 8 valence electrons. Electronegativity of metalloids is about 1.6- 2.2, while that of nonmetals is about 3- 4. Nonmetals have the highest electronegativity among the four, and thus have the greatest attraction of electrons.

The correct answer is (3) nonmetals.

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