Gen. Chem. for Health Science CH-84 – Flashcards

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NO3-
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Nitrate
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NO2-
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Nitrite
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NH4+
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Ammonium
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N3-
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Azide
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SO42-
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Sulfate
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HSO4-
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Bisulfate/hydrogen sulfate
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SO32-
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Sulfite
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HSO3-
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Bisulfite/ hydrogen sulfite
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S2O32-
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Thiosulfate
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PO43-
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Phosphate
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HPO42-
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Hydrogen phosphate
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H2PO4-
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Dihydrogen phosphate
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PO33-
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Phosphite
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CO32-
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Carbonate
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HCO3-
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Bicarbonate/hydrogen carbonate
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C2O42-
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Oxalate
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C2H3O2-
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Acetate
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CN-
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Cyanide
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ClO4-
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Perchlorate
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ClO3-
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Chlorate
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ClO2-
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Chlorite
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ClO-
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Hypochlorite
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H3O+
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Hydronium
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OH-
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Hydroxide
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Kinetic Molecular Theory of Mater
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a set of five statements that are used to explain the physical behabior of the three states of matter (solid, liquid, and gas)
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Pressure
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Force/area
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Boyles Law
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Pressure is inversly related to volume

 

P1V1=P2V

P=K(1/V)

PV=K

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Charles Law
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Temperature is proportional to volume

 

V1/T1=V2/T2

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Gay-Luccac's
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Pressure with constant volume is directly proportional to temperature(kalvin).

;

P1/T1=P2/T2

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Combined Gas Law
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An expression obtained by mathematically combining Boyle's and Charles Law

 

(P1*V1)/T1=(P2*V2)/T2

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Ideal Gas Law
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PV=nRT

PV/nT=.0821 (atm*L/mol*K)

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Evaporation
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The process by which molecules escape from the liquid phase to the gas phase (kenetic energy)
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Enodthermic
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Requires the input (absorbtion) of heat
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Exothermic
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Requires heat to be given up (released)
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Vapor
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Gaseous molecules of a substance at a temperature and pressure at which we ordinarily would think of the substance as a liquid or solid
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Kenetic molecular Theory
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-Matter is ultimately composed of tiny particles that have definite and characteristic size that do not change
-the particles are in constant, random motion and therefore possess kinetic energy
-the particles interact with one antoher throught attractions and repulsions and therefore possess potential energy
-the velocity of the particles increases as the temperature is increased
-the particles in a system transfer energy to each other through elastic collisions
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Elastic collision
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bounce off each other and continue
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Inelastic collision
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masses glob together with no resulting movement
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Equilibrium state
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situation in which two opposite processes take plave at the same time
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vapor pressure
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the pressure exerted by a vapor aboe a liquid when the liquid and vapor are in equilibrium
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volatile substance
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Substance that readily evaporates at room temperature because of high vapor pressure ex) gasoline
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Intermolecular force in liquids
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is an attractive force that acts between a molecule and another molecule
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Dipole-Dipole
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intermolecular force that occures between POLAR molecules
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Hydrogen Bonds
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extra strong dipole-dipole interaction between a hydrogen atom covalently bonded to a small, very electronegative atom (F,O,or N) and have a lone pair of electrons on another small very electronegative atom
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London Forces
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are weak bonds due to temporary uneven electron distributions causing slightly negative or positive charges
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Solution
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Homogeneious combination of two or more substances in which each substance retains its ownchemical identity
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Solvent
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The component of a solution that is present in the greatest amount
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Solute
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is a solution component that is present in a smaller amount relative to that of the solvent
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Solubility
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the max amount of solute that will dissolve in a given amount of solvent
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Henery's Law
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S=k#(P)....k#--solubility=partial pressure
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Unsaturated solution
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is a solution in which less solute than the max amount possible is dissolved in the solution
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saturated solution
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contains the max amount of solute that can be dissolved under the conditions at which the solution exists
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super saturated solution
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contains more than the max amount of solute (possible in some situations)
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Diluted solution
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Contains a small amount of solute relative to the amoung that could be dissolved
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Aqueous solution
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solution where water is the solvent
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nonaqueous solution
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solution in which water is not the solvent
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Factors that affect the rate of solution
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-Subdivision: partivle size--increase surface area
-Agitation: mixing or stirring
-Temperature: high temps cause more collisions between molecules
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Concentration
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the amount of solute present in a specific amoung of solution
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% Mass
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(Mass of solute/Mass of solution)X 100
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% volume
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(Volume of solute/volume of solution) X 100
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Mass-Volume %
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(Mass of solute/ Volume of solution) X 100
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Molarity
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Moles of solute/liter of solution
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Colligative properties
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Physical properties of a solution that depend only on the number (concentration) of solute partivles (molecules or ions) in a given quantity of solvent and not on their chemical identities
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Osmosis
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the passage of a solvent from a dilute solution (or pure solvent) through a semipermeable membrane into a more concentrated solution
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Osmotic pressure
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the amoung that must be applied to prevent the net flow of solvent through a semipermeable membrane from a solution of lower solute concentration to a solution of higher solute concentration
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Osmolarity
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product of its molarity and the number of partivles produced performula unit when the solute dissocrates

Osmolarity=molarity X i---i=the number of particles
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Isotonic solution
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osmotic pressure is equal to that within the cell
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Hypotonic solution
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lower osmotic pressure than that within a cell
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Hypertonic solution
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higher osmotic pressure than that within a cell
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Dialysis
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the process whihc a semipermeable membrane permits the passage of solvent, dissolved ions, and small molecules but blocks the passage of large molecules
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Combustion Reactions
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reaction of a substance with oxygen (usually from air) that proceeds with the evolution of heat and usually with a flame
CO2+H2O are products
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oxidation
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the process whereby a reactant in a chemical reaction gains one or more oxygen atoms, loses 1+ hydrogen, or loses 1+ electon
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Reduction
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the process whereby a reactant in a chemical reactions loses one or more oxygen atoms, gains 1+ hydrogen or electon
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Chemical equilibrium
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process wherein two opposing chemical reactions occur simultaneously at the same rate
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