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