Trends in Atomic Properties and Electron Affinity

These flashcards cover essential vocabulary related to atomic properties, trends in periodic table, and electron affinity.

Atomic Radius

Half the distance between the nuclei of two identical atoms in a molecule.

Covalent Radius

Half the distance between the nuclei of two atoms joined in a covalent bond.

Metallic Radius

Half the distance between the nuclei of adjacent atoms in a solid metal.

Trend in Atomic Radii: Group

Atomic radius increases from top to bottom within a group due to additional principal energy levels.

Trend in Atomic Radii: Period

Atomic radius decreases from left to right across a period due to increasing effective nuclear charge.

Effective Nuclear Charge (Zeff)

The net positive charge experienced by an electron in a multi-electron atom, accounting for shielding by inner electrons.

Ionization Energy

The energy required to remove an electron from a gaseous atom or ion.

Electron Affinity (EA)

The energy change that occurs when an electron is added to a gaseous atom, indicating the tendency of an atom to attract additional electrons.

Lanthanide Contraction

The decrease in atomic radii observed in the lanthanide series due to poor shielding of f electrons.

Trends in Ionization Energies

Ionization energy tends to increase across a period and decrease down a group.

Gross Trends in Atomic Properties

Decreasing atomic radius, increasing ionization energy, and more negative electron affinity across a period.

Metalloids

Elements that have properties intermediate between metals and nonmetals.

Acidic Oxides

Oxides that react with water to form acids.

Basic Oxides

Oxides that react with acids to form salts and water.

Amphoteric Oxides

Oxides that can act as either acids or bases.