Final answer:
Ionization energy is the energy needed to remove an electron from an atom, creating a cation. Electronegativity is how strongly an atom attracts electrons in a bond, influenced by the atom's ionization energy and electron affinity. As we move right across the periodic table, ionization energy tends to increase due to stronger nuclear charge.
Step-by-step explanation:
Ionization energy is defined as the amount of energy required to remove an electron from an atom in its gaseous state. This process produces a cation, which is an ion with fewer electrons than its neutral counterpart. The higher the ionization energy, the more difficult it is to remove an electron, signifying a stronger hold of the atom on its electrons. Electronegativity is a measure of how strongly an atom attracts electrons towards itself in a chemical bond. It is influenced by both the atom's ionization energy and its electron affinity, which is the energy change that occurs when an atom gains an electron. While electronegativity is not a direct measurement but a calculated value, it helps us understand the chemical behavior of atoms in molecules.
Moving across the periodic table from left to right, an atom's ionization energy generally increases due to a stronger nuclear charge, meaning a greater number of protons exerting a stronger attractive force on the electrons. Similarly, an atom with high electron affinity will release energy when it gains an electron and is more likely to form negative ions, contributing to its electronegativity.