Key Concepts in Atomic Radii and Ionization Energy

This set of flashcards summarizes key vocabulary and concepts related to atomic radii and ionization energy, using information from the lecture notes.

Atomic Radius

Defined as one-half the distance between the nuclei of identical atoms that are bonded together.

Cation

A positive ion that is smaller than its atom due to the loss of one or more electrons.

Anion

A negative ion that is larger than its atom due to the addition of one or more electrons.

Ionic Radius

Refers to the size of an ion in a crystal lattice.

Ionization Energy

The energy required to remove one electron from a neutral atom of an element.

Trends Across a Period

Atomic radius tends to decrease and ionization energy tends to increase as you move from left to right.

Trends Down a Group

Atomic radius tends to increase and ionization energy tends to decrease as you move down a group.

Electron Cloud

The region surrounding the nucleus where electrons are likely to be found; its size affects atomic and ionic radii.

electronegativity

valence electrons hold atoms together in chemical compounds

The negative charge of valence electrons is concentrated closer to one atom than another

electronegativity is a measure of the ability of an atom and a chemical compound to retract electrons from another atom in the compound

Valence Electrons

Chemical compounds form because electrons are lost, gained or shared between atoms,

The electrons that interact in this manner are those in the highest energy levels,

The electro available to be lost gain or shared in the formation of chemical compounds are valence electrons

Ionic Radii

catalytic and an ionic radii decrease across a period

The electron cloud shrinks due to the increasing nuclear charge and the outer electrons in both cations and anions are in higher energy levels as one reads down a group