The enthalpy of formation is defined as the enthalpy change when one mole of a compound is formed from its elements in their standard states.

The ideal gas law assumes that there are no intermolecular forces between gas particles, which is a key limitation of the model.

The triple point is the unique set of conditions at which all three phases (solid, liquid, gas) coexist in equilibrium.

A concentration cell has the same electrodes but different concentrations of the electrolyte.

Ideal gases are considered to have no volume and do not exhibit intermolecular forces.

The first law of thermodynamics states that energy cannot be created or destroyed, only transformed.

The phase transition from liquid to gas (vaporization) requires energy input (endothermic process).

Enthalpy is a state function, meaning its change depends only on the initial and final states, not the path taken.

Enthalpy is a state function, meaning it depends only on the current state of the system, not the path taken to reach that state.

The triple point on a phase diagram is the unique set of conditions at which all three phases (solid, liquid, gas) coexist in equilibrium.

Charles's Law explains that increasing temperature at constant pressure leads to an increase in volume of the gas.

The Kinetic Molecular Theory explains gas behavior by describing how gas particles are in constant motion and how this motion relates to temperature and pressure.

Le Chatelier's Principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change.

The azimuthal quantum number (l) determines the shape of the orbital, with values ranging from 0 to n-1.

Ionization energy generally increases across a period due to increasing nuclear charge, which holds electrons more tightly.

Pi bonds are formed by the side-to-side overlap of p orbitals.

A pi bond is formed by the lateral overlap of two p orbitals.

Hydrogen bonding is the dominant intermolecular force in water, leading to its relatively high boiling point.

Ionic bonds are the strongest type of intermolecular force due to the electrostatic attraction between charged ions.