Answer
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The electronegativity trend is the tendency of atoms to attract shared electrons in a covalent bond. Electronegativity generally increases across a period (from left to right) and decreases down a group (from top to bottom) in the periodic table. As we move from left to right across a period, the effective nuclear charge increases, leading to a stronger attraction for electrons. On the other hand, moving down a group, the number of electron shells increases, and the distance between the nucleus and valence electrons increases, resulting in weaker electron attraction.
Hydrogen's electronegativity is relatively high compared to the alkali metals, but it is lower than that of the halogens and many other nonmetals. Hydrogen can form covalent bonds with elements on both sides of it in the periodic table, behaving like either a metal or a nonmetal, depending on the situation.
