Key Concepts in Atomic Structure and Ionization

These flashcards encompass key terms related to atomic structure, ionization, and periodic trends.

Valence Electrons

Outermost electrons involved in bonding, displayed as dots around the element symbol in an electron dot (Lewis dot) structure.

Monatomic Ion

A single atom that loses or gains electrons; cations are formed by metals losing electrons, while anions are formed by nonmetals gaining electrons.

Octet Rule

Atoms gain or lose electrons to achieve a stable configuration of eight valence electrons, similar to noble gases.

Isoelectronic

Having the same electron configuration and the same number of electrons but being different elements or ions.

Effective Nuclear Charge (Z_eff)

The actual positive charge experienced by an electron in an atom, accounting for shielding from inner electrons.

Covalent Radius

A measure that determines atomic size, often exemplified by the distance between nuclei in a molecule, e.g., O₂.

Ionization Energy (IE)

The energy required to remove an electron from a gaseous atom in its ground state, higher values indicate difficulty in losing electrons.

Electron Affinity (EA)

The energy change that occurs when an electron is added to a gaseous atom; energy is released, making it an exothermic process.

Cation

A positively charged ion that forms when an atom loses one or more electrons.

Anion

A negatively charged ion that forms when an atom gains one or more electrons.