Chemistry Chapter: Properties of Liquids

The kinetic molecular theory states that molecules are constantly in motion. The state of matter (solid, liquid, or gas) depends on the amount of motion these molecules exhibit.

Intermolecular forces (IMFs) are attractive forces between molecules. These forces oppose kinetic energy, keeping molecules close together.

A dipole moment (μ) measures the net polarity of a molecule. It is calculated by multiplying the magnitude of the charge (Q) at each end of the molecular dipole by the distance (r) between the charges.

Dipole-dipole interaction occurs between polar molecules, where one end of the molecule is slightly positive and the other is slightly negative. The positive end of one molecule is attracted to the negative end of another molecule.

A chemical bond is formed when electrons are shared between atoms, creating a strong attraction between the atoms. Example: Water molecule (H2O).

Intermolecular forces are weaker than chemical bonds. They are attractive forces between molecules that hold substances together in their liquid or solid state.

Hydrogen bonding occurs between molecules that have a hydrogen atom directly bonded to a highly electronegative atom, such as oxygen, nitrogen, or fluorine. It is the strongest type of intermolecular force.

London dispersion forces are weak intermolecular forces that occur between all molecules, even non-polar ones. They arise from temporary, fluctuating dipoles induced by the movement of electrons within the molecules.

A weak attraction that occurs when a polar molecule induces a temporary dipole in a nonpolar molecule by disturbing its electron arrangement.

An attraction between a charged ion (cation or anion) and a polar molecule.

An attraction between an ion and a nonpolar molecule, where the ion's charge induces a temporary dipole in the nonpolar molecule.

A liquid's resistance to flow. Stronger intermolecular forces lead to higher viscosity.

The property of a liquid's surface that allows it to resist external forces due to the cohesive nature of its molecules. It represents the energy required to increase the surface area of a liquid.

Attraction between molecules of the same substance. Important for surface tension.

Attraction between molecules of different substances. Important for wetting.

The pressure exerted by a vapor above a liquid in a closed container at equilibrium. It increases as the temperature rises.

The amount of heat required to vaporize one mole of a liquid at a given temperature.

The temperature at which the vapor pressure of a liquid equals the pressure surrounding the liquid.

The state of a substance that can act as both an acid and a base, donating or accepting protons.

The reaction of a substance with water, often breaking bonds and forming new molecules.

A chemical reaction involving the transfer of electrons between reactants, often resulting in changes in oxidation states

The ability of a substance to cause a separation of charges in another substance, resulting in a polar environment

The temperature at which water transitions from a liquid to a solid state.

The ability of a substance to resist flow. Water has a high viscosity due to strong intermolecular interactions.

Water's ability to dissolve many different substances, making it a crucial component in many natural processes.

A repeating pattern of atoms, ions, or molecules within a solid structure, like bricks in a wall.

Crystalline solids formed from ionic compounds, composed of positively and negatively charged ions.

Crystalline solids formed by atoms connected through strong covalent bonds, resulting in hard and durable materials.

Crystalline solids formed by molecules held together by weaker forces like hydrogen bonding or dipole-dipole interactions.

Crystalline solids formed by metal atoms with loosely bound electrons that can move freely, making them good conductors of heat and electricity.

The process by which an atom or ion captures a free electron to form a neutral atom.

A graphical representation of the different phases of a substance under varying pressure and temperature conditions.

The state of a substance when both its liquid and vapor phases are in equilibrium.

A highly compressed gas possessing properties of both gases and liquids.

The point on a phase diagram where all three phases of a substance coexist.

The component of a solution being dissolved.

The maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature and pressure.

A solid where the constituent particles are arranged randomly, lacking a repeating, long-range order. Although they may have small regions of orderly arrangement called crystallites.

Amorphous solids don't have a specific melting point but melt over a range of temperatures. For example, glass softens before melting.

The process of changing a solid into a liquid state. It's the opposite of freezing, where liquid becomes solid.

The process of changing a liquid into a gaseous state. It's the opposite of condensation, where gas becomes liquid.

The process of changing a liquid into a solid state. It's the opposite of melting, where solid becomes liquid.

The process of changing a gas into a liquid state. It's the opposite of vaporization, where liquid becomes gas.

The process of changing a solid directly into a gas, without going through the liquid state. It's the opposite of deposition.

The process of changing a gas directly into a solid, without going through the liquid state. It's the opposite of sublimation.