Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
Bancroft Chem Vocab
Chem Vocab for Bancroft's final exam
| Term | Definition |
|---|---|
| Electromagnetic Radiation | Energy transmitted through space as oscillating electric and magnetic fields. |
| Photon | A packet of electromagnetic energy. |
| Photoelectric Effect | The emission of electrons from a material when light strikes it. |
| Atomic Spectrum | A characteristic set of wavelengths emitted or absorbed by an atom. |
| Bohr Model | A model in which electrons occupy specific quantized energy levels. |
| Quantum Mechanical Model | A model describing electrons as probability distributions rather than fixed paths. |
| Orbital | A region of space where an electron is most likely to be found. |
| Quantum Number | A value used to describe an electron's energy and location. |
| Pauli Exclusion | Principle No two electrons in an atom can have the same set of four quantum numbers. |
| Hund's Rule | Electrons occupy orbitals singly before pairing. |
| Aufbau Principle | Electrons fill the lowest-energy orbitals first. |
| Ionization Energy | The energy required to remove an electron from an atom. |
| Atomic Radius | Half the distance between the nuclei of two identical bonded atoms. |
| Ionic Bond | A bond formed by electron transfer between atoms. |
| Covalent Bond | A bond formed by sharing electrons. |
| Metallic Bond | A bond involving metal atoms and a sea of mobile electrons. |
| Electronegativity | An atom's ability to attract shared electrons. |
| Bond Polarity | Unequal sharing of electrons in a bond. |
| Dipole Moment | A measure of bond or molecular polarity. |
| Lewis Structure | A diagram showing valence electrons and bonding. |
| Octet Rule | Atoms tend to gain or share electrons to achieve eight valence electrons. |
| Resonance | Multiple valid Lewis structures for the same molecule. |
| VSEPR Model | A model predicting molecular shape from electron pair repulsions. |
| Tetrahedral | A molecular geometry with four electron domains and |
| Trigonal Planar | A molecular geometry with three electron domains and |
| Linear | A molecular geometry with two electron domains and |
| Pressure | Force per unit area. |
| Boyle's Law | Pressure and volume are inversely proportional at constant temperature. |
| Charles's Law | Volume and temperature are directly proportional at constant pressure. |
| Avogadro's Law | Volume and moles are directly proportional at constant temperature and pressure. |
| Ideal Gas Law PV=nRT. | |
| Dalton's Law | The total pressure of a gas mixture equals the sum of the partial pressures. |
| Partial Pressure | The pressure exerted by one gas in a mixture. |
| Kinetic Molecular Theory | A model describing gas behavior based on particle motion. |
| Effusion | The escape of gas through a tiny opening. |
| Diffusion | The mixing of gases due to random motion. |
| STP | Standard temperature and pressure: 273 K and |
| Molar Volume | 22.4 L/mol for an ideal gas at STP. |
| Intermolecular Forces | Attractive forces between molecules. |
| Dipole-Dipole Attraction | Attraction between polar molecules. |
| Hydrogen Bonding | A strong dipole interaction involving H bonded to N |
| London Dispersion Forces | Temporary attractions caused by fluctuating electron distributions. |
| Surface Tension | The resistance of a liquid surface to expansion. |
| Capillary Action | The movement of a liquid through a narrow space. |
| Viscosity | A liquid's resistance to flow. |
| Crystalline Solid | A solid with an orderly repeating structure. |
| Amorphous | Solid A solid lacking long-range order. |
| Lattice | A regular repeating arrangement of particles. |
| Molecular Solid | A solid composed of molecules held together by intermolecular forces. |
| Ionic Solid | A solid composed of ions. |
| Network Solid | A solid held together by a continuous network of covalent bonds. |
| Alloy | A mixture of metals. |
| Vaporization | The conversion of liquid to gas. |
| Condensation | The conversion of gas to liquid. |
| Equilibrium Vapor Pressure | The pressure exerted by vapor above a liquid at equilibrium. |
| Sublimation | The direct conversion of solid to gas. |
| Phase Diagram | A graph showing phases as a function of temperature and pressure. |
| Triple Point | The temperature and pressure at which all three phases coexist. |
| Critical Point | The temperature and pressure beyond which liquid and gas phases are indistinguishable. |
| Solution | A homogeneous mixture. |
| Solute | The substance being dissolved. |
| Solvent | The substance doing the dissolving. |
| Solubility | The maximum amount of solute that dissolves in a given amount of solvent. |
| Saturated Solution | A solution containing the maximum dissolved solute. |
| Unsaturated Solution | A solution capable of dissolving more solute. |
| Molarity | Moles of solute per liter of solution. |
| Mass Percent | Mass of solute divided by mass of solution times |
| Dilution | The process of reducing concentration by adding solvent. |
| Precipitation Reaction | A reaction producing an insoluble solid. |
| Net Ionic Equation | An equation showing only species involved in the reaction. |
| Arrhenius Acid | A substance that produces H+ in water. |
| Arrhenius Base | A substance that produces OH− in water. |
| Bronsted-Lowry Acid | A proton donor. |
| Bronsted-Lowry Base | A proton acceptor. |
| Conjugate Acid | A species formed when a base gains a proton. |
| Conjugate Base | A species formed when an acid loses a proton. |
| Amphoteric | A substance capable of acting as either an acid or a base. |
| Strong Acid | An acid that ionizes completely in water. |
| Weak Acid | An acid that ionizes partially in water. |
| Strong Base | A base that dissociates completely in water. |
| Weak Base | A base that dissociates partially in water. |
| Autoionization of Water | The reaction 2H2O ⇌ H3O+ + OH−. |
| Kw | The ion-product constant of water. |
| pH | A measure of hydrogen ion concentration. |
| pOH | A measure of hydroxide ion concentration. |
| Titration | A technique used to determine concentration by reaction with a standard solution. |
| Equivalence Point | The point in a titration where stoichiometric amounts have reacted. |
| Reaction Rate | The change in concentration per unit time. |
| Rate Law | An equation relating reaction rate to reactant concentrations. |
| Reaction Mechanism | A sequence of elementary reaction steps. |
| Activation Energy | The minimum energy needed for reaction. |
| Catalyst | A substance that speeds a reaction without being consumed. |
| Equilibrium | A state where forward and reverse reaction rates are equal. |
| Equilibrium Constant (K) | A ratio relating product and reactant concentrations at equilibrium. |
| Heterogeneous Equilibrium | An equilibrium involving multiple phases. |
| Le Chatelier's Principle | A system at equilibrium shifts to oppose a disturbance. |
| Solubility Product (Ksp) | The equilibrium constant for a sparingly soluble ionic compound. |
Created by:
C Dilly
Popular Chemistry sets