Which of the following statements correctly explains why electronegativity generally increases from left to right across a period of the periodic table?

A) The atomic radius increases across a period, which brings bonding electrons closer to the nucleus.

B) The shielding effect of inner-shell electrons increases significantly across a period, decreasing core repulsion.

C) The effective nuclear charge increases while the principal energy level remains the same, attracting shared electrons more strongly.

D) Additional electron shells are added across a period, allowing valence electrons to experience greater nuclear pull.

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Chemistry · The Periodic Table · Chemistry · Periodic Trends

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