Lab Final Flashcards
Intermolecular Forces
the attractive forces between particles that are not bonded to each other.
Freezing point
the temperature at which a liquid becomes a solid
Boiling point
the temperature at which a liquid becomes a gas
Vapor pressure
the pressure exerted by the equilibrium concentration of a vapor in equilibrium with its liquid
Surface tension
a measure of how strongly molecules on the surface of a liquid attract to each other. The energy needed to pull liquid apart from itself to make a new surface.
Viscosity
a measure of how readily a fluid flows against itself. Thick fluids have high viscosity and move slowly.
Dipole
an uneven distribution of charge in a molecule
Dispersion forces
occur when an atom or molecule come near each other and the electron of one species are attracted to the protons of the other.
Dipole-Dipole
forces occur between species that have a permanent dipole, such as water molecules.
Hydrogen Bonding
a very strong form of dipole-dipole interaction that occurs in species that have H-F H-O or H-N bonds
Ion-Dipole forces
occur between permanent ions and dipoles, such as sodium ions and water.
Specific heat capacity
the amount of energy needed to raise 1g of water by 1 degree Celsius
Heat of vaporization
energy needed per mole of substance converted from liquid to gas at its boiling point, units J/mol or KJ/ mol.
Solution
Homogenous mixture of two or more substances or components containing a solvent and a solute.
solvent
majority component of a solution, which does the dissolving of a solute.
solute
minority component of a solution, which are dissolved by the solvent.
Aqueous solutions
water is the solvent and a solid, liquid or gas is the solute
solubility
the amount of a substance that can be dissolved in a given amount of solvent
miscible
two substances that are soluble in each other.
immiscible
two substances that are not soluble in each other.
Henry’s law
the higher the pressure in a gas, the more soluble the gas is in the solvent.
Buffers
anything that resists change. weak acid and conjugate base or weak base and conjugate acid.
Henderson-Hasselbalch equation
pH=pKa+log (10) {[base]/[acid]}
buffer capacity
the number of moles or added acid or base that the buffer can neutralize before it gets overwhelmed.
solubility product constant
Ksp, the equilibrium between a solids and its respective ions in a solution. Its value indicates the degree to which a compound dissociates in water
common ion effect
if [I-] is increased then [Pb+] must decrease for the Ksp to stay the same
formation constant
Kf, the stability of a complex ion can be judged by the magnitude of the equilibrium constant corresponding to the formation of the complex
Gibbs free energy
the available energy that can be used for any process.
enthalpy
the heat evolved in a chemical reaction at constant pressure.
calorimeter
measures temperature change in order to determine heat.
reduction
a chemical change where a reagent gains one or more electron, the charge becomes more negative as a result
oxidation
chemical change in which a reagent loses one or more electrons, the charge becomes more positive as a result.
anode
site of oxidation
cathode
the site of the reduction
oxidizing agent
a species that causes another to be oxidized
reducing agent
a species that causes another to be reduced
potential ( electromotive force)
the driving force for the reaction
salt bridge
allows the passage of ions to balance the electron flow
electrode
the conductor placed in each half cell
know the chemicals used in experiments
like iodine
spontaneous reaction
occurs without being driven by an outside source
Entropy
The number of specific ways where a system may be arranged
Solubility product
the equilibrium constant for a chemical equation
Colligative property
Properties of solutions that depend on the number of particles dissolved in solution, not on the type of particles
LeChatelier’s principle
When temperature, pressure, on concentration increase, equilibrium shifts to accommodate the temperature, pressure, or concentration.
