Open Question
Why is the electron affinity of each group 5A element more positive than that of each corresponding group 4A element? Use the outer electron configurations for these columns to suggest a reason for this observation.
10. Periodic Properties of the Elements
Periodic Trend: Electron Affinity
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The affinity of an atom for an electron is also known as which of the following?
A
Electron affinity
B
Electronegativity
C
Atomic radius
D
Ionization energy
Verified step by step guidance1
Understand the definitions of the given terms: Electron affinity, Electronegativity, Atomic radius, and Ionization energy.
Electron affinity refers to the amount of energy released or absorbed when an atom gains an electron, indicating the atom's affinity for an electron.
Electronegativity is a measure of an atom's ability to attract and hold electrons in a chemical bond, not specifically the energy change when gaining an electron.
Atomic radius is the measure of the size of an atom, which is unrelated to the energy changes involved in gaining or losing electrons.
Ionization energy is the energy required to remove an electron from an atom, which is the opposite process of gaining an electron.
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