Electropositivity of elements across the periodic table normally

The electronegativity of elements across the periodic table generally follows a pattern. Electronegativity refers to the tendency of an atom to attract electrons towards itself when it is part of a chemical bond. However, in this question, we are discussing electropositivity, which is the opposite of electronegativity. Electropositivity refers to the tendency of an atom to lose electrons and form positive ions. It is essentially the measure of how easily an element gives away its valence electrons. In general, as we move across a period from left to right in the periodic table, the electropositivity of elements decreases. This means that elements on the left side of a period are more electropositive compared to those on the right side. This trend can be attributed to the increase in effective nuclear charge (the positive charge felt by the outermost electrons) as we move across the period. The stronger pull of the nucleus on the valence electrons makes it harder for the atoms to lose electrons and become positive ions. On the other hand, as we move down a group in the periodic table, the electropositivity of elements remains relatively constant or even increases. This is because the valence electrons are located in higher energy levels that are farther from the nucleus. The increased distance reduces the attractive force between the nucleus and the valence electrons, making it easier for the atoms to lose electrons and become positive ions. Therefore, based on the explanation above, the correct option is "decreases across the period."