Chemistry vocab Word Scramble
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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 |
Created by:
wileyhunsaker
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