Studied by 1 person
Looks like no one added any tags here yet for you.
Coulombic attraction
The force of attraction between charged particles, such as electrons and the nucleus.
Zeff
Effective nuclear charge, the net positive charge experienced by an electron in an atom.
PES graph
Photoelectron spectroscopy graph, a graph that shows the energy levels and number of electrons in different sublevels of an atom.
Electron configuration
The arrangement of electrons in an atom or ion.
Isotopes
Atoms of the same element that have different numbers of neutrons.
Mass spectroscopy
A technique used to measure the atomic masses of isotopes.
Group
A vertical column on the periodic table, elements in the same group have similar chemical and physical properties.
Metals
Elements located on the left side of the periodic table, typically have metallic properties.
Nonmetals
Elements located on the right side of the periodic table, typically have nonmetallic properties.
Cations
Positively charged ions, formed by removing electrons from atoms.
Anions
Negatively charged ions, formed by adding electrons to atoms.
Covalent bonds
Bonds formed by the sharing of electrons between two nonmetals.
Ionic bonds
Bonds formed by the transfer of electrons from a metal to a nonmetal.
Electronegativity
The ability of an atom to attract electrons in a chemical bond.
Combustion reactions
Reactions that involve the burning of a substance to produce carbon dioxide and water.
Bond angles
The angles between the bonds in a molecule.
Lattice energy
The energy required to break an ionic bond in a compound.
Formal charge
A calculation used to determine the distribution of electrons in a Lewis structure.
Octet rule
The tendency of atoms to gain, lose, or share electrons to achieve a stable electron configuration with eight valence electrons.
Metallic bonds
Bonds formed between metal atoms, characterized by the delocalization of electrons.
Intermolecular forces
Forces of attraction between molecules.
London Dispersion forces
The weakest intermolecular force, caused by temporary fluctuations in electron distribution.
Dipole-dipole forces
Intermolecular forces between polar molecules, caused by the attraction between positive and negative ends of the molecules.
Hydrogen bonding
A strong type of dipole-dipole force that occurs when hydrogen is bonded to a highly electronegative atom.
Ion-dipole forces
Forces of attraction between ions and polar molecules.
Boiling point
The temperature at which a substance changes from a liquid to a gas.
Melting point
The temperature at which a substance changes from a solid to a liquid.
Molecular solids
Solids composed of individual molecules held together by intermolecular forces.
Ionic solids
Solids composed of ions held together by ionic bonds.
Covalent network solids
Solids in which the atoms are bonded together in a continuous network.
Gas mixtures
Homogeneous mixtures of gases.
Compressible
The ability of a substance to be squeezed into a smaller volume.
Gas pressure
The force exerted by gas particles on the walls of a container.
Boyle's Law
The relationship between the pressure and volume of a gas, when temperature is held constant.
Charles's Law
The relationship between the volume and temperature of a gas, when pressure is held constant.
Gay-Lussac's Law
The relationship between the pressure and temperature of a gas, when volume is held constant.
Ideal gas law
The equation that relates the pressure, volume, temperature, and number of moles of a gas.
Molar mass
The mass of one mole of a substance.
Average kinetic energy
The average energy of motion of particles in a substance.
Water displacement
A method used to collect gases by displacing water in a container.
Real gases
Gases that do not behave exactly like an ideal gas due to intermolecular forces and molecular size.
Solutions
Homogeneous mixtures of two or more substances.
Mixtures
Combinations of two or more substances that are not chemically combined.
Filtering
A method used to separate mixtures based on differences in particle size.
Distillation
A method used to separate mixtures based on differences in boiling point.
Chromatography
A method used to separate mixtures based on differences in polarity.
Density
The mass per unit volume of a substance.
% composition
The percentage of each element in a compound by mass.
M1V1 = M2V2
A formula used for dilution calculations in chemistry.
Meniscus
The curved surface of a liquid in a container, used for reading the volume of a liquid.
Sig
Significant figures, the digits in a number that carry meaningful information.
Graduated cylinder
A measuring device used to measure the volume of liquids.
Volumetric flask
A measuring device with a single line to measure a specific volume of liquid.
Empirical formula
The simplest whole number ratio of atoms in a compound.
Molecular formula
The actual number of atoms of each element in a compound.
% yield
The percentage of the theoretical yield that is actually obtained in a chemical reaction.
% error
The percentage difference between the experimental and theoretical values in a measurement or calculation.
Limiting reactant
The reactant that is completely consumed in a chemical reaction and determines the amount of product formed.
Activation energy
The minimum energy required for a chemical reaction to occur.
Rate law
An equation that relates the rate of a chemical reaction to the concentrations of reactants.
Rate constant
A proportionality constant in the rate law equation.
Catalyst
A substance that increases the rate of a chemical reaction by lowering the activation energy.
Half-life
The time it takes for the concentration of a reactant to decrease by half in a first-order reaction.
Exothermic reaction
A reaction that releases heat to the surroundings.
Endothermic reaction
A reaction that absorbs heat from the surroundings.
ΔHrxn
The change in enthalpy of a reaction.
Equilibrium constant (Keq)
The ratio of the concentrations of products to reactants at equilibrium.
Le Chatelier's Principle
When a system at equilibrium is disturbed, it will shift to counteract the disturbance.
Molar solubility
The concentration of a solute in a saturated solution at equilibrium.
pH
A measure of the acidity or alkalinity of a solution.
Hydronium ion
H3O+, the ion formed when an acid donates a proton.
Strong base
A base that completely ionizes in water.
Conjugate base
The species that remains after an acid has donated a proton.
Acid-Base reaction
A chemical reaction between an acid and a base, resulting in the formation of a salt and water.
[H+]
The concentration of hydrogen ions in a solution.
[OH-]
The concentration of hydroxide ions in a solution.
% Ionization
The percentage of a weak acid or weak base that dissociates into ions in a solution.
Conjugate Base
The ion formed when an acid loses a hydrogen ion.
Conjugate Acid
The ion formed when a base gains a hydrogen ion.
Neutral Salt
A salt that does not affect the pH of a solution.
Ka Value
The acid dissociation constant, which indicates the strength of an acid.
Kb Value
The base dissociation constant, which indicates the strength of a base.
Titrations
A technique used to determine the concentration of a substance in a solution by reacting it with a known concentration of another substance.
Buffers
Solutions that resist changes in pH when small amounts of acid or base are added.
Equivalence Point
The point in a titration where the moles of acid and base are stoichiometrically equivalent.
Thermodynamically Favorable
Reactions that occur spontaneously and have a negative change in Gibbs free energy (ΔG).
ΔH
The change in enthalpy, which represents the heat absorbed or released during a reaction.
ΔS
The change in entropy, which represents the degree of disorder in a system.
Keq
The equilibrium constant, which indicates the ratio of products to reactants at equilibrium.
Activation Energy
The energy barrier that must be overcome for a reaction to occur.
Oxidation Numbers
Numbers assigned to atoms in a compound to indicate the distribution of electrons.
Anode
The electrode where oxidation occurs in both a battery and an electrolytic cell.
Cathode
The electrode where reduction occurs in both a battery and an electrolytic cell.
Salt Bridge
A pathway for the flow of ions between the two half-cells in an electrochemical cell.
Eo Cell
The standard cell potential, which indicates the voltage of a battery or electrolytic cell.
Half-Reaction
The individual oxidation or reduction reaction that occurs in an electrochemical cell.
ΔGo
The change in Gibbs free energy at standard conditions.
Electroplating
The process of depositing a layer of metal onto a surface using an electric current.
Note 
Flashcard (80)