FINAL EXAM Flashcards
The flow of thermal energy that produces a phase change while no temperature change is observed.
Latent heat
Thermal energy that, when applied to a substance, produces a temperature change in the substance.
Sensible heat
A substance (Either an element or compound) that can occur in more than one type of crystalline form.
Polymorphous
One of two or more forms of a polymorphous element that exists in the same state.
Allotrope
The elastic “skin” that forms the surface of a liquid. It is produced by the imbalance of intermolecular forces in the surface of a liquid.
Surface tension
The curved upper surface of the column of a liquid that results from intermolecular attractions within the liquid and between the liquid and its container.
meniscus
The attractions between the particles of a liquid and the particles of other materials. (The molecules are attracted to the cup)
Adhesion
The minimum amount of kinetic energy required before colliding molecules can react
activation energy
Boiling
A physical change from liquid state to the gaseous state caused by the application of heat that occurs when the vapor pressure or a liquid equals the prevailing atmospheric pressure.
buffers
A solution that resists changes in pH when a moderate amount of either an acid or base is added.
Capillary rise
A phenomenon in which liquid spontaneously rises or falls in a narrow space such as a thin tube or in the voids of a porous material.
Catalyst
A substance that changes the reaction rate without being permanently changed in the process.
Cohesion
The reaction between the particles of a liquid.
Vapor pressure
The pressure exerted by a vapor in equilibrium with its solid or liquid state at a specified temperature.
The ability of a liquid to resist flow; the amount of internal resistance.
Viscosity
1st and 2nd Law of thermodynamics–
The first law of thermodynamics also known as the law of conservation of energy states that energy can neither be created nor destroyed, but it can be changed from one form to another.” “The second law of thermodynamics states that the entropy in an isolated system always increases.
Thermodynamics
The study of thermal energy, heat, and their useful applications.
Tyndall effect
The scattering of light by particles in a colloid.
Colloid
A mixture of small particles (between 1 and 1000 nm in size) that remain dispersed in medium. Ec: fog, foam, aerosols, and gels.
The theory that atoms and molecules must undergo forceful, properly oriented collisions before they can react.
Collision theory
Critical temperature
The highest temperature at which a gas can be liquified. Each gas has its own characteristic critical temp.
Dynamic equilibrium
A chemical equilibrium in which two or more opposing events occur at the same rate but result in no change. An example is the balancing processes of evaporation and condensation.
Enthalpy
(H) The energy content of a thermodynamic system at a constant pressure.
Entropy
The state (measure) of disorder.
A naturally occurring protein molecule that acts like a catalyst.
Enzyme
Freezing
A physical change from the liquid state to solid state.
Gibbs free energy–
(G) A substance’s ability to do work, involving both the enthalpy and entropy of a substance; also called free energy.
Kinetics
In chemistry, the study of the rates of reactions and the steps by which they occur.
Melting
A physical change from a solid state to a liquid state.
Pertaining to two liquids that are completely soluble in each other.
Miscible
Osmosis
The diffusion of pure solvent molecules, such as water, through a semipermeable membrane.
Sublimation
A physical change from a solid state directly to a gaseous state.
Unsaturated
The condition of a solution that contains less dissolved solute than it does at equilibrium.
Supersaturated
The condition of a solution that contains more dissolved solute than it does at equilibrium.
Solution
A homogeneous mixture of two or more substances that is dissolved.
Solute
The minority substance in a solution is the substance that is dissolved.
Saturated
maximum amount of solute possible at a given state of conditions.
Specific heat
The amount of thermal energy required to raise the temperature of 1 g of a substance by 1 degree C.
Solvents
The most abundant substance in a solution; the substance that does the dissolving.
Understand why like dissolves like and how that applies to polarity.
Polar solvents will dissolve polar and ionic solutes because of the attraction of the opposite charges on the solvent and solute particles. Non-polar solvents will only dissolve non-polar solutes because they cannot attract the dipoles or the ions.
Know the difference between Crystalline solid - amorphous solid
Crystalline solids have orderly shapes and form 3D patterns. They shatter into distinct shapes. Ionic, metallic, and sometimes covalent. Crystalline solids are crystals.
Amorphous solids have no distinct shape or underlying pattern. Shatter into irregular fragments. Covalent compounds are usually amorphous.
Know the steps of dissolving
Dissociation
Solvation
Diffusion
Know what usually forms when an acid and base react and neutralize.
Water and salt.
Know the difference between boiling and evaporation
Evaporation is when vaporization occurs in a non-boiling liquid while boiling is a change from liquid to gas with heat application. Evaporation only occurs in the surface of a liquid while boiling occurs throughout a liquid.
Know what the three intermolecular forces are and which is strongest
The three intermolecular forces are Dipole-Dipole, hydrogen bonds, and dispersion forces. Hydrogen bonds are the strongest.
