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Chemistry vocab
| Question | Answer |
|---|---|
| concentrated solution | a solution that contains a large amount of solvent. |
| colligative properties | a property that demands only upon the number of solute particles, and not upon their identity. |
| dilute solution | a solution that contains a small amount of solute. |
| Henry's Law | states that at a given temperature, the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid. |
| miscible | if two liquids dissolve in each other in all proportions. |
| immiscible | when two liquids are insoluble in one another. |
| molarity | the number of moles of a solute dissolved in one liter of a solution. |
| molality | the number of moles of a solute dissolved in 1 kilogram of solvent. |
| solubility | the amount of solute that dissolves in a given quantity of a solvent at a specified temperature and pressure to produce a saturated solution. |
| supersaturated | contains more solute than it can theoretically hold at a given temperature |
| unsaturated | a solution that contains less solute than a saturated solution at a given temperature and pressure. |
| saturated | contains the maximum amount of solute for a given quantity of solvent at a constant temperature and pressure. |
| aqueous solution | water that contains dissolved substances. |
| Brownian motion | the chaotic movement of colloidal particles. |
| colloid | a heterogeneous mixture containing particles that range in size from 1 nm to 1000 nm. |
| electrolyte | a compound that conducts an electric current when it is in an aqueous solution or in a molten state. |
| emulsion | a colloidal dispersion of a liquid in a liquid. |
| hydrate | a compound that contains water of hydration. |
| non-electrolyte | a compound that does not conduct an electric current in either an aqueous solution or the molten state. |
| solute | dissolved particles in a solution. |
| solvation | the process by which the positive and negative ions of an ionic solid become surrounded by solvent molecules. |
| solvent | the dissolving medium in a solution. |
| surfactant | any substance that interferes with the hydrogen bonding between water molecules and thereby reduces surface tension. |
| suspension | a mixture from which particles settle about standing. |
| surface tension | the inward force, or pull, that tends to minimize the surface area of liquid. |
| Tyndall effect | the scattering of visible light by colloidal particles |
| Avagadro's hypothesis | states that equal volumes of gases at the same temperature and pressure contain equal numbers of particles. |
| Avagadro's number | 6.02x10to23 |
| empirical formula | gives the lowest whole-number ratio of the atoms of the elements in a compound. |
| molecular formula | a chemical formula of a molecular compound that shows the kinds and numbers of atoms present in a molecule of a compound |
| mole | 6.02x10to23 representative particles of a substance. |
| molar mass | the mass of a mole of an element. |
| molar volume | the amount of space a mole of a substance takes up. |
| standard temperature and pressure (STP) | means a temperature of 0 degrees Celsius and a pressure of 101.3 kPA or I atmosphere (atm). |
| density units | g/ L |
| activity series | A list of elements in order of decreasing activity. |
| catalyst | A substance that increases the rate of reaction by lowering the activation-energy barrier; the catalyst is not used up in the reaction. |
| coefficients | A small whole number that appears in front of a formula in a balanced chemical equation. |
| balanced chemical equation | A chemical equation in which mass is conserved; each side of the equation has the same number of atoms of each element. |
| combination reaction | A chemical change in which two or more substances react to form a single new substance; also called a synthesis reaction. |
| combustion reaction | A chemical change in which an element or a compound reacts with oxygen, often producing energy in the form of heat and light. |
| decomposition reaction | A chemical change in which a single compound is broken down into two or more simpler products. |
| double replacement reaction | A chemical change that involves an exchange of positive ions between two compounds. |
| single replacement reaction | A chemical change in which a single compound is broken down into two or more simpler products. |
| reactant | a substance present at the start of a reaction |
| product | a substance produced in a chemical equation |
| spectator ion | An ion that is not directly involved in a chemical reaction; an ion that does not change oxidation number or composition during a reaction. |
| net ionic equation | An equation for a reaction in solution showing only those particles that are directly involved in the chemical change |
| actual yield | the amount of product that forms when a reaction is carried out in the labratory |
| theoretical yield | the amount of product that could form during a reaction calculated form a balanced chemical equation; it represents the maximum amount of product that could be formed from a given amount of reactant |
| excess reagent | a reagent present in a quantity that is more than sufficient to react with a limiting reagent is used up in a chemical reaction |
| limiting reagent | any reactant that is used up first in chemical reaction; it determines the amount of product that can be formed in the reaction |
| allotrope | two or more different molecular forms of the same element |
| atmospheric pressure | results from the collisions of atoms and molecules in air with objects |
| barometer | a tool used to measure atmospheric pressure |
| boiling point | the temperature at which the vapor pressure of the liquid is just equal to the external pressure of the liquid |
| crystal | particles are arranged in an orderly, repeating, three dimensional pattern called a crystal lattice |
| evaporation | the conversion of a liquid to a gas on the surface of a none boiling liquid |
| vaporization | the conversion of a liquid to a gas |
| kinetic energy | the energy an object has because of its motion |
| kinetic theory | all matter consists of tiny particles that are in constant motion. The particles in a gas are usually molecules or atoms. applies to the fundamental assumptions about gases |
| melting point | the temperature at which a solid changes into a liquid |
| normal boiling point | the boiling point of a liquid at a pressure of 101.3 kPa |
| phase diagram | a graph that shows the relationship among the solid, liquid, and vapor states of a substance in a sealed container |
| sublimation | the change of a substance from a solid to a vapor without passing through the liquid state |
| triple point | a point on phase diagram at which conditions of all three phases can exist in equilibrium with one another |
| unit cell | the smallest group of particles within a crystal that exhibit geometric shape of the crystal |
| vacuum | an empty space with no particles and no pressure |
| vapor pressure | a measure of the force exerted by a gas above a liquid |
| diffusion | the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout. |
| effusion | a gas escapes through a tiny hole in its container |
| partial pressure | the contribution each gas in a mixture makes to the total pressure |
| compressibility | a measure of how much the volume of matter decreases under pressure |
| Boyle's law | states that for a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure |
| Charle's law | states that the volume of a fixed mass of gas is directly proportion to its Kelvin temperature if the pressure is kept constant |
| Dalton's law of partial pressures | states that, at a constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sume of the partial pressures of the component gas |
| Gay-Lussacs law | states that the pressure of a gas is directly proportional to the Kelvin temperature if the volume remains constant |
| Graham's law of effusion | states that rate of effusion of a gas is inversely proportional to the square root of the gas's molar mass |
| endothermic process | absorbs heat from its surroundings |
| enthalpy | the heat content of a system at constant pressure |
| exothermic process | releases heat to its surrounding |
| molar heat of fusion | the heat absorbed by one mole of a solid substance as it melts to a liquid at a constant temperature |
| system | the part of the universe on which you focus your attention |
| surroundings | include everything else in the universe |
| acidic solution | one in which H+ is greater than OH- |
| alkaline solution | basic solutions |
| amphoteric | substance that can act as both an acid and a base |
| conjugate acid | the particle formed when a base gains a hydrogen ion |
| conjugate base | the particle that remains when an acid has donated a hydrogen |
| neutral solution | an aqueous solution in which H+ and OH- are equal |
| neutralization | reactions in which an acid and base react in an aqueous solution to produce a salt and water |
| ph | the negative logarithm of the hydrogen-ion concentration |
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wileyhunsaker
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