AP Chem Finals Vocabulary – Flashcards
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| Electronic Structure |
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| The arrangement of electrons of an atom or molecule |
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| Electronic Structure |
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| the arrangement of electrons of an atom or molecule |
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| Electromagnetic radiation |
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| a form of energy that has wave characteristics and that propagates through a vacuum at speed of light |
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| wavelength |
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| the distance betwenn identical points on successive waves. |
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| frequency |
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| the number of times per second that one complete wavelength passes a given point |
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| quantum |
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| the smallest increment of radiant energy that may be absorbed or emitted; the magnitude of radiant energy is hv |
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| photon |
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| the smallest increment of radiant energy; a photon of light with frequency v has an energy equal to hv |
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| spectrum |
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| the distribution among various wavelengths of the radiant energy emitted or absorbed by an object |
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| continous spectrum |
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| A spectrum that contains radiation distributed over all wavelengths |
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| line spectrum |
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| A spectrum that contains radiation at only certain specific wavelengths. |
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| groud state |
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| "the lowest energy, or most stable, state" |
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| excited state |
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| a higher energy state than the ground state |
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| matter waves |
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| the term used to describe the wave characteristics |
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| chemical bonds |
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| a strong attractive force that exists between two atoms |
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| ionic bond |
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| a bond between oppositely charged ions. |
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| covalent bond |
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| a bond formed between two or more atoms by a sharing of electrons |
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| lewis symbol |
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| the chemical symbol for an element with a dot for each valence electron |
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| octet rule |
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| a rule stating that bonded atoms tend to possess or share a total of eight valece shell electrons |
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| lattice energy |
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| the energy required to separate ompletely the ions in an ionic solid |
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| hess's law |
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| "The heat evolved in a given process can be expressed as the sum of the heats of several processes that, when added, yild the process of interest" |
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| isoelectronic series |
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| "a series of atoms, ions, or molecules having the same number of electrons" |
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| single bond |
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| a covalent bond involving one electron pair |
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| double bond |
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| a covalent bond involving two electron pair |
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| triple bond |
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| a covalent bond involving three electron pairs |
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| multiple bonding |
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| bonding involving two or more electron pairs |
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| nonpolar covalent |
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| a covalent bond in which the electrons are shared equally |
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| polar covalent |
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| a covalent bond in which the electrons are not shared equally |
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| electronegativity |
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| a measure of the ability of an atom that is bonded to another atom to attract electrons to itself |
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| polar molecule |
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| a molecule that possesses a nonzero dipole moment |
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| dipole |
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| a molecule with one end having a slight begative harge and the other end having a slight positive charege; a polar molecule |
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| resonance structures |
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| "two lewis structures are equally good descriptions of a single molecule, they are averaged to give correct description of the real moleule" |
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| bond enthalpy |
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| the enthalpy charge required to break a particular bond when the substance is in the gas phase |
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| conjugate base |
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| a substance formed by the loss of a proton from a bronsted lowry acid |
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| conjugate acid |
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| a substance formed by the addition of a proton from a bronsted lowry acid |
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| conjugate acid base pair |
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| an acid and a base that difer only in the presence or absence of a proton |
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| amines |
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| "a compound that has the general formula R3N, where r may be h or a hydrocarbon group" |
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| polyprotic acids |
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| a substance capable of ionizing more than one proton in water. |
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| base dissociation constant |
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| "an equilibrium constant that expresses the extent to which a base reacts with solvent water, accepting a proton and forming OH-" |
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| hydronium ion |
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| the predominant form of the proton in aqueous solution |
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| amphoteric substance |
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| capable of behaving as either an acid or a base |
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| vapors |
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| gaseous state of any substance that normally exists as a liquid or solid |
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| presure |
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| "a measure of the force exerted on a unit area. Often expressed in units of atmospheres, atm, or torr:760torr is 1 atm. Si is expressed in pascals, pa" |
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| pascal |
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| The SI unit of pressure 1 pa = n/m(squared) |
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| torr |
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| A unit of pressure 1torr=1mm Hg |
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| ideal gas |
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| "a hypothetical gas whose pressure, volume, and temperature behavior is completely described by the ideal gas equation" |
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| gas constant |
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| ® the constant of proportionality in the ideal gas equation. |
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| STP |
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| Defined as 0 celcius and 1 atm pressure; frequently used as reference conditions for a gas |
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| Partial pressures |
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| the pressure exerted by a particular gas in a mixture |
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| kinetic molecular theory |
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| "a set of assumptions about the nature of gases. These assumptions, when translated into mathmatical form, yield the ideal gas equation." |
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| solvation |
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| the clustering of solvent molecules around a solut particle |
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| hydration |
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| solvation when the solvent is water |
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| crystallization |
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| the process in which a dissolved solute comes out of solution and forms a crystalline solid |
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| saturated |
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| a solution in which undissolved solute and dissoved solute are in equilibrium |
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| solubility |
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| the amount of a substance that dissolves in a given quantity of solvent at a given temperature to form a saturated solution |
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| unsaturated |
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| solutions containing less solute than a saturated solution |
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| supersaturated |
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| solutions containg more solute than a saturated solutions |
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| miscible |
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| liquids that mix in all proportions |
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| immiscible |
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| liquids that do not mix |
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| Henry's law |
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| a law stating that the concentration of a gas in a solution is proportional to the pressure of gas over the solution |
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| mass percentage |
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| the number of grams of solute in each 100g of solution |
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| parts per million |
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| the concentration of a solution in grams of solute per million grams os solution; equals milligrams of solute per liter of solutoin for aqueous solutions |
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| parts per billion |
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| the concentration of a solution in grams of solute per billion grams os solution; equals milligrams of solute per liter of solutoin for aqueous solutions |
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| molality |
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| the concentration of a solution expressed as moles of solute per kilogram of solvent; m |
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| Raoult's law |
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| a law stating that the partial pressure of a solvent over a solution is given by the vapor pressure of the pure solvent times the mole praction of a solvent in the solution |
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| Ideal solution |
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| a solution that obeys raoults law |
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| molal boiling-point-elevation constant |
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| a constant characteristic of a particular solvent that gives the change in boiling point as a function of solution molality |
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| molal freezing-point-point-depression constant |
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| a constant characteristic of a particular solvent that gives the change in freezing point as a function of solution molality |
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| osmosis |
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| the net movement of solvent through a semipermeable membrane toward the solution with greater solute concentration |
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| osmotic pressure |
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| the pressure ethat must be applied to a solution to stop osmosis from pure solvent into the solution |
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| colloidal dispersions/colloids |
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| mixtures containing particles larger than normal solutes but small enough to remanin suspended in the dispersing medium |
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| hydrophilic |
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| water loving |
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| hydrophobic |
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| water fearing |
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| tyndall effect |
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| the scattering of a beam of visible light by the particles in a colloidal dispersion |
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| colligative properties |
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| those properties of a solvent that depend on the total conentration of solute particles present |
