| Term | Definition |
|---|---|
| chemical change | A process in which substances are rearranged into new combinations, resulting in the formation of new substances with different properties. |
| mixture | Materials that contain atoms, molecules, or formula units of two or more types, whose relative proportions can vary. |
| phase | A distinct state of matter: solid, liquid, or gas. |
| physical change | A change in matter that does not alter the chemical composition or identity of the substance. |
| precipitate | A solid substance that forms and separates from a solution during a chemical reaction. |
| Term | Definition |
|---|---|
| balanced chemical equation | A chemical equation where the number of atoms of each element is equal on both the reactant and product sides. |
| chemical change | A process in which substances are rearranged into new combinations, resulting in the formation of new substances with different properties. |
| complete ionic equation | A balanced equation that shows all ions and molecules present in solution, including spectator ions. |
| conservation of charge | The principle that the total electric charge is neither created nor destroyed in a chemical reaction; total charge is equal on both sides of the equation. |
| conservation of mass | The principle that mass is neither created nor destroyed in a chemical reaction; the total mass of reactants equals the total mass of products. |
| molecular equation | A balanced chemical equation that represents all reactants and products in their molecular form. |
| net ionic equation | A symbolic representation of a chemical reaction that shows only the ions and molecules that actually participate in the reaction, excluding spectator ions. |
| physical change | A change in matter that does not alter the chemical composition or identity of the substance. |
| Term | Definition |
|---|---|
| balanced chemical equation | A chemical equation where the number of atoms of each element is equal on both the reactant and product sides. |
| chemical reaction | A process in which substances are transformed into different substances through the breaking and forming of chemical bonds. |
| particulate model | A representation of matter showing individual atoms, molecules, or ions and their interactions to describe chemical processes at the molecular level. |
| physical process | A change in the state or properties of matter that does not alter the identity of the substances involved. |
| symbolic representation | A depiction of chemical reactions using chemical formulas, symbols, and equations to represent reactants and products. |
| Term | Definition |
|---|---|
| bond interactions | The forces between atoms or molecules, including chemical bonds and intermolecular forces, that determine the properties and behavior of substances. |
| chemical process | A transformation in which substances are converted into different substances through the breaking and forming of chemical bonds. |
| dissolution | The process by which a solute dissolves in a solvent to form a solution, involving the breaking of bonds or interactions in the solute and formation of new interactions with the solvent. |
| intermolecular interactions | Forces between molecules, such as hydrogen bonding, dipole-dipole forces, and London dispersion forces, that affect the physical and chemical properties of substances. |
| ion-dipole interactions | Attractive forces between an ion and a polar molecule, where the charged ion interacts with the partial charges on the polar molecule. |
| ionic bonds | Chemical bonds formed between positively and negatively charged ions through electrostatic attraction. |
| macroscopic characteristics | Observable properties of matter that can be seen and measured without a microscope, such as color, state, temperature, and solubility. |
| phase transition | The process by which a substance changes from one state of matter to another (solid, liquid, or gas). |
| physical process | A change in the state or properties of matter that does not alter the identity of the substances involved. |
| Term | Definition |
|---|---|
| atom conservation | The principle that atoms cannot be created, destroyed, or changed during a chemical process, so the total number and type of atoms remain constant. |
| balanced chemical equation | A chemical equation where the number of atoms of each element is equal on both the reactant and product sides. |
| coefficients | The numbers placed in front of chemical formulas in a balanced equation that indicate the relative proportions of reactants and products involved in the reaction. |
| ideal gas law | The equation PV = nRT that relates pressure, volume, number of moles, and temperature of an ideal gas. |
| molarity | A measure of solution concentration expressed as the number of moles of solute dissolved per liter of solution. |
| mole concept | A fundamental chemistry concept that relates the number of particles (atoms, molecules, or ions) to measurable quantities through Avogadro's number. |
| product | Substances formed as a result of a chemical reaction. |
| reactant | Substances that are consumed in a chemical reaction to form products. |
| stoichiometric calculations | Quantitative calculations using balanced chemical equations and mole ratios to determine amounts of reactants consumed or products formed in a chemical reaction. |
| Term | Definition |
|---|---|
| analyte | The substance in a solution whose amount or concentration is being determined during a titration. |
| endpoint | The observable event or change in property (such as color) that indicates when the equivalence point has been reached in a titration. |
| equivalence point | The point in a titration where the analyte is completely consumed by the titrant in a quantitative reaction. |
| titrant | A solution of known concentration that is added to an analyte during a titration to determine the amount of analyte present. |
| titration | An analytical procedure used to determine the amount of an analyte in solution by reacting it with a titrant of known concentration. |
| Term | Definition |
|---|---|
| acid-base reaction | A chemical reaction involving the transfer of one or more protons (H⁺ ions) between chemical species. |
| aqueous solution | A solution in which water is the solvent. |
| combustion | A type of oxidation-reduction reaction in which a species reacts with oxygen gas to produce products such as carbon dioxide and water. |
| electron transfer | The movement of one or more electrons from one chemical species to another in a redox reaction. |
| hydrocarbons | Organic compounds composed of carbon and hydrogen atoms that undergo complete combustion to produce carbon dioxide and water. |
| insoluble | Unable to dissolve in a solvent, such as water; describes compounds that form as precipitates. |
| ionic compound | Compounds formed by the electrostatic attraction between positively charged cations and negatively charged anions. |
| oxidation numbers | Numbers assigned to atoms in reactants and products to track electron transfer and identify oxidized and reduced species in a redox reaction. |
| oxidation-reduction reaction | A chemical reaction involving the transfer of one or more electrons between chemical species, indicated by changes in oxidation numbers. |
| oxidized | The process in which a species loses electrons in a redox reaction. |
| precipitation reaction | A chemical reaction in which ions in aqueous solution combine to produce an insoluble or sparingly soluble ionic compound. |
| proton transfer | The movement of a proton (H⁺) from one species to another in an acid-base reaction. |
| reduced | The process in which a species gains electrons in a redox reaction. |
| sparingly soluble | Slightly soluble in a solvent; describes ionic compounds that form precipitates when ions combine in aqueous solution. |
| Term | Definition |
|---|---|
| aqueous solution | A solution in which water is the solvent. |
| Brønsted-Lowry acid | A species that donates a proton (H⁺) in a chemical reaction. |
| Brønsted-Lowry base | A species that accepts a proton (H⁺) in a chemical reaction. |
| conjugate acid-base pair | Two species that differ by one proton, where one is the acid form and the other is the base form of the same substance. |
| ionization | The process by which an acid or base separates into ions when dissolved in water. |
| proton transfer | The movement of a proton (H⁺) from one species to another in an acid-base reaction. |
| Term | Definition |
|---|---|
| balanced redox reaction equation | A chemical equation for an oxidation-reduction reaction where the number of electrons lost equals the number of electrons gained, and all atoms and charges are balanced. |
| half-reaction | Separate equations showing either the oxidation process (loss of electrons) or the reduction process (gain of electrons) in a redox reaction. |