The Periodic Table: Compounds and Molecules

These flashcards cover key terminology and concepts related to ionic bonding, lattice energies, and solubility as discussed in the chemistry lecture.

Ionic Bonding

A type of chemical bond that involves the electrostatic attraction between oppositely charged ions.

Cation

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

Anion

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

Lattice Energy

The energy change that occurs when an ionic solid is separated into its gaseous ions.

Electron Affinity

The amount of energy released when an electron is added to a neutral atom in the gas phase.

Ionization Energy

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

Isoelectronic

Ions or atoms that have the same electron configuration or the same number of electrons.

Hydration Energy

The energy released when ions are surrounded by water molecules and dissolved in solution.

Born-Haber Cycle

A thermodynamic cycle used to analyze the energy changes involved in the formation of ionic compounds.

Electrostatic Forces

The forces that hold ions together in ionic compounds, arising from their opposite charges.

Solubility

The ability of a substance to dissolve in a solvent at a particular temperature and pressure.

Lattice Energy Calculation

The Born-Haber cycle provides a method to calculate lattice energy based on various energy changes.

Hydration vs. Lattice Energy Balance

The solubility of a salt depends on the balance between lattice energy and hydration energy.

Coulomb’s Law

A law that describes the electrostatic interaction between electrically charged particles.

Magnitude of Lattice Energies

Lattice energies increase with higher ion charges and smaller ionic radii.

Complex Ionic Compounds

Ionic compounds that contain complex ions held together by covalent bonds.