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Chemistry terms
Chemistry terms chapters 8- 16
| Term | Definition |
|---|---|
| Precipitation | The formation of a solid in a chemical reaction |
| Strong Electrolyte | A substance that dissolves in water by dissociating completely into ions |
| Soluable Solid | A solid that readily dissolves in water |
| Insoluable Solid | A solid that dissolves to such a small degree that it is not detectable to the naked eye |
| Molecular Equation | A chemical equation showing the complete forms of all reactants and products |
| Complete Ionic Equation | A chemical equation for a reaction in solution representing all strong electrolytes as ions |
| Spectator Ion | An ion presents in solution that does not participate in a reaction |
| Net Ionic Equation | A chemical equation for a reaction in solution showing only those components that are in directly involved in the equation. Strong electrolytes are shown as ions |
| Acid | A substance that produce H+ ions when it is dissolved in water |
| Base | A substance that produces OH- ions in water |
| Strong Acid | An acid that completely dissociates to produce H+ ions in solution |
| Strong Base | A base that completely dissociates to produce OH- ions in solution |
| Oxidation- Reduction Reaction | A chemical reaction involving the transfer of electrons |
| Double- Displacement Reaction | AB+CD= AD+CB |
| Single- Replacement Reaction | A+ BC= B+AC |
| Combustion Reaction | A chemical reaction involving oxygen as one of the reactants that produces enough heat so that a flame results |
| Synthesis/ Combination Reaction | A chemical reaction where a compound is formed from simpler materials |
| Decomposition Reaction | A chemical reaction in which a compound is broken down into simpler compounds, or to the component elements |
| Stoichiometry | The process of using a balanced chemical equation to determine the relative masses of reactants and products involved in a reaction |
| Limiting Reactant | The reactant that is completely used up in a reaction |
| Theoretical Yield | The maximum amount of given product that can be formed when the limiting reactant is completely consumed |
| Percent Yield | The actual yield of a product as the percentage of the theoretical yield |
| Wavelength | The distance between two consecutive peaks or troughs in a wave |
| Frequency | The number of waves per second that pass a given point in space |
| Photon | A particle of electromagnetic radiation |
| Orbital | The 3- dimensional region in which there is a high probability of finding an electron in an atom |
| Electron Confirguration | The arrangement of electrons in an atom |
| Valence Electron | The electron in the outermost principal energy level of an atom |
| Core Electron | An inner electron, an electron not in the outermost principal energy level of an atom |
| Metalloids | A few elements that exhibit both metallic and nonmetallic behavior |
| Ionization Energy | The amount of energy required to remove an electron from a gaseous atom or ion |
| Chemical Bond | The force that holds two or more atoms together and makes them function as a unit |
| Bond Energy | The amount of energy required to break a chemical bond |
| Ionic Compound | The compound that results when a metal reacts with a nonmetal |
| Ionic Bonding | The attraction between oppositely charged ions |
| Covalent Bonding | A type of bonding in which atom share electron |
| Polar Covalent Bind | A covalent bond in which the electrons are not shared equally because one atom attracts the shared electrons more than the other atom |
| Electronegativity | The tendency of an atom in a molecule to attract shared electrons to itself |
| Dipole Moment | A property of a molecule in which the charge distribution can be represented by a center of positive charge and a center of negative charge |
| Lewis Structure | A representation of a molecule or polyatomic ion showing how valence electrons are arranged among the atoms in the molecule or ion |
| Bonding Pair | A pair of electrons that are shared between two atoms forming a covalent or polar- covalent bond |
| Lone Pair | Electron pairs in a Lewis structure that are not involved in bonding |
| Single Bond | A covalent or polar covalent bond in which one pair of electrons is shared by two atoms. |
| Double Bond | A covalent or polar covalent bond in which two pairs of electrons are shared by two atoms. |
| Triple Bond | A covalent or polar covalent bond in which three pairs of electrons are shared by two atoms. |
| Resonance | A condition occurring when more than one valid Lewis structure can be written for a particular molecule |
| Molecular Structure | The 3- dimensional arrangement of atoms in a molecule |
| Solution | A homogeneous mixture |
| Solvent | The dissolving medium in a solution |
| Solute | The substance dissolved in the solvent to make a solution |
| Aqueous solution | A solution with water as a solvent |
| Saturated | Describes a solution that contains as much solute as will dissolve at that temperature |
| Unsaturated | Describes a solution in which more solute can dissolve than is dissolved already at that temperature |
| Supersaturated | Describes a solution that contains more solute that a saturated solution will hold at that temperature |
| Concentrated | Describes a solution in which a relatively large amount of solute is dissolved in a solution |
| Dilute | Decribes a solution in which a relatively small amount of solute is dissolved in a solution |
| Molarity | The amount of solute in moles and the volume of the solution in liters |
| Standard Solution | A solution in which the concentration is accurately known |
| Dilution | The process of adding solvent to a solution to lower the concentration of solute |
| Equivalent of an Acid | The amount of acid that can furnish one mole of hydrogen ions (H+) |
| Equivalent of a Base | The amount of base that can furnish one mole of hydroxide ions (OH-) |
| Equivalent Weight | The mass (in grams) of one equivalent of an acid or a base |
| Colligative Property | A property that is dependent only on the number of solute particles present in solution |
| Normality | The equivalents of solute in liters of solution |
| Arrhenius Concept of Acids and Bases | Acid produce (H+) ions in solution, Bases produce (OH-) in solution |
| Conjugate Acid | The substance formed when a proton is added to a base |
| Conjugate Base | The remaining substance when a proton is lost from an acid |
| Conjugate Acid- Base Pair | Two substances related to each other by the donating and accepting of a single proton |
| Hydronium Ion | H30+ |
| Diprotic Acid | An acid that can furnish two protons |
| Oxyacid | An acid in which the acidic proton is attached to an oxygen atom |
| Organic Acid | An acid with a carbon- atom backbone and a carboxyl group |
| Amphoteric Substance | A substance that can behave either as an acid or a base |
| Indicator (acid- base) | A chemical that changes color depending on the pH of the solution |
| Indicator Paper | A strip of paper coated with a combination of acid- base indicators |
| pH Meter | A device used to measure the pH of a solution |
| Neutralization Reaction | An acid- base reaction |
| Titration | A technique in which a solution of known concentration is used to determine the concentration of another solution |
| Standard Solution | A solution in which the concentration is accurately known |
| Buret | A device used for the accurate measurement of the delivery of a given volume of a liquid or solution |
| Equivalence Point | The point in a titration when enough titrant has been added to react exactly with the substance in solution that is being titrated |
| Titration Curve | A plot of pH of solution versus volume of titrant added to a given solution |
| Buffered Solution | A solution that resists a change in pH when either an acid or a base are added |
Created by:
MartineAntonsen
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