Chemistry Chapter 3.03 Quiz: Periodic Table Trends

Atomic Radii Trends

• Atomic radius increases from top to bottom within a group in the periodic table due to the addition of electron shells, resulting in larger atoms.
• Atomic radius decreases as one moves from left to right across a period due to the increased positive charge in the nucleus, which pulls the electrons closer.

First Ionization Energy Trends

• The first ionization energy decreases from top to bottom within a group, as increased distance from the nucleus and electron shielding reduce the energy required to remove an electron.

Electronegativity

• Electronegativity is defined as the measure of an atom's ability to attract electrons in a chemical bond; a key property that influences bond formation and molecular structure.

Comparison of Atomic Radii

• Sodium (Na) has a larger atomic radius than its ionized form, sodium ion (Na+), because removal of an electron reduces electron-electron repulsion, bringing remaining electrons closer to the nucleus.