Question

ionization energy, electron affinity, and electronegativity increase as you move up and towards the right
○ true
○ false

Explanation:

Ionization energy is the energy required to remove an electron from an atom. Electron affinity is the energy change when an electron is added to an atom. Electronegativity is a measure of an atom's ability to attract electrons in a chemical bond. As we move up a group in the periodic table, the atomic radius decreases, and the effective nuclear charge increases, making it harder to remove an electron (higher ionization energy), easier to add an electron (higher electron affinity in general for non - metals), and more ability to attract electrons (higher electronegativity). As we move to the right across a period, the atomic radius decreases (due to increasing nuclear charge and same electron shell), leading to higher ionization energy, generally increasing electron affinity (for non - metals), and higher electronegativity.

Answer:

True