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CHICHESTER QUIZ 3
chichester quiz 3, chapter 8-10 chemistry
| Question | Answer |
|---|---|
| change of state | transofrmation of a substance from 1 state to another is called this |
| What is the kinetic-molecular theory of gases? | the physical behavior of gases can b explained y assuming that they consist of particles moving rapidly at random, seperated from other particles by great distance and colliding without loss of energy |
| What are the gas laws? | boyle's law, charle's law, gay-lussac's law,combined gas law, avogadros law |
| what is boyle's law? | the volume of a fixed amount of gas at constant temperature is inversly propoortional to its pressure P1V1= P2V2 |
| What is charles law? | the volume of a fixed amount of gas at constant pressure is directly proportional to its kelvin temperatue (V1/T1)=(V2/T2) |
| What is gay-lussacs law? | the pressure of a fixed amount of gas at constant volume is directly proportional to its kelvin temperature (p1/t1)=(p2/t2) |
| what is the combined gas law? | boyles/charles/gay lussac law (p1v1/t1)=(p2v2/t2) |
| what is avogadros law? | equal volume of gases at the same temp and pressure contain the same number of moles (v1/n1)=(v2/n2) |
| what is the ideal gas law? | the four gas laws together give this, PV=nRT, which relates the edfects of temp, prrssure, volume and molar amount |
| what is partial pressure? | the amount of pressure exerted by an indiviudal gas in a mixture called the partial pressure of the gasaccording to daltons law, the total pressure exertrd by the mixture is equal to the sum of the partial pressures of the individuals gases |
| What are the major intermolecular forces? | there are 3 intermolecular forces: dipole dipole, london dispersion, and hydrogen bonding |
| what is an intermolecular force | they act to hold molecules near one another in solids and liquids |
| what is a dipole dipole force | electrical attractions that occur btwn polar molecules |
| what is a london dispersion force? | they occur between all molecules as a result of temporary molecular polarities due to unsymmetrical electron distriibution |
| what is hydrogen bonding? | the strongest of thhe three forces, and occurs between a hydrogen atom bonded to O,N or F and a near by O,N or F atom |
| What are the various kinds of solids and how do they differ? | crystalline solids, amorphous solids, molecular solids, metallic solids, ionic solids,covalent network solids |
| wha are crystalline solids? | those whose consituent particles have an ordered arrangemment |
| what are amorphous solids? | they lack internal order and do not have sharp melting points |
| what are ionic solids? | 1 of the crystalline solids- and are those like sodium chloride whose constituent particles are ions |
| what are molecular solids? | part of the crystalline solids- are those like ice, whose constituent particles are molecules held together by intermolecular forces |
| what are covalent network solid? | are those like diamond, whose atoms are linked together by covalent bonds into a ginat 3D array |
| what are metalllic solids? | such as silver or ion, also consist of large arrays of atoms, but their crystals have metallic properties such as electrical conductivity |
| what occurs during a change of state?? | at melting point, liquid becomes solidheat of fusion is amount of heat necessary to melt a given amount of a solid at its melting point |
| what is boiling point? | liquid becomes gas |
| what is heat of vaporization | amount of heat necessar to vaporize a liquid at boiling point |
| sublimation | solid straight to a gas |
| Whats the def of kinetic-molecular theory of gases? | a group of assumptions that explain the behavior of gases |
| ideal gas | a gas that obeys all the assumptions of the kinetic-molecular theory |
| pressure (p) | the force per unit area pushing against a surface |
| Gas laws | a series of laws that predict the influence of pressure, volume and temperature on any gas or mixture of gases |
| gas constant | the constant R in the ideal gas law, PV=nRT |
| Partial pressure | the contribution of a given gas in a mixture to the total pressure |
| vapor | the gas molecules in equilibrium with a liquid |
| vapor pressure | partial pressure of gas molecules in equilibrium with a liquid |
| normal bioling point | the boiling point at a pressure of exactly 1 atmosphere |
| how is the concentration of a solution expressed? | molarity, weight/weight % composition, weight/volume % composition, and ppm |
| how are dilutions carried out? | adding more solvent to an existing solution M1V1=M2V2 |
| what is an electrolyte? | substances that form ions when dissolved in water and whose water solutions therefore conduct an electric currents called these |
| how do solutions differ from pure solvents in their behaviors? | the solution has a lower vapor pressure at a given temp, a higher BP anda lower MP, |
| what is osmosis? | occurs when solutions of diff concentration are seperated by a semipermeable membrane that allows solvent molecule sto pass but blocks passage of solute ions and molecules |
| heterogenous mixture | a nonuniform mixture that has regions off different composition |
| homogenous mixture | a uniform mixture that has the same composition throughout |
| solution | a homogenous mixture that contains particles of a size of a typopical ion or small moleculee |
| colloid | a homogenous mixture that contains particles in the range2-500 nm diameter |
| solute | a substaance dissolved in a liquid |
| solvent | the liquid in which another substance is dossolved |
| solvation | the clustering of solvent molecules around a dissolved soute molecules or ion |
| hygroscopic | haviing the ability to pull water molecules from the surrounding attmosphere |
| miscible | mutually solble in all proportions |
| saturated solution | a solution that contains the max amount of disolved solute at equilibrium |
| solubility | the max anmount of a asubstance that will dissolve ina given amount of solvent at a specified temperature |
| supersaturated solution | a solution that contains more than t he maximum amount of dissolved solute;a noneqquilibirum situation |
| dilution factor | the ratio of the initial and final solution volumes (v1/v2) |
| strong electrolyte | a substance that ionizes completely when dissolved in water |
| weak electrolyte | a substance that is only partially ionized in water |
| nonelectrolyte | a substance that doesnt prodcue ions when dissolved in water |
| colligative property | a property of a solution that depennds only on the number of dissolved particles, not on their chemical identity |
| osmotic pressure | the amount of external pressure aplplied to the more concentrated solution to halt the passage of solvent molecules across a semipermeable membrane |
| osmolarity (osmol) | the sum of the molarities of all dissolved particles in a solution |
| isotonic | having the same osmolarity |
| hypotonic | having an osmolarity less than the surrounding blood plasma or cells |
| hypertonic | having an osmolarity greater than the surrounding blood plasma or cells |
| what are acids and bases? | an acid is a substance hat donates a hydrogen ion and a base accepts a hydrogen ion |
| what effect does tthe strength of acids and bases have on their on reactions? | a strong acid gives up a proton easilya weak acid gives up a proton with difficultya strong base accepts and holds a proton readilya weak base has a low affinity for a proton |
| whatt is the ion-product constant for water? | water can act as either an acid or base |
| what is the pH scale for measuring acidity | is given by uts pH below 7= acidic; 7=neutral, above 7-basic |
| how is thw acid or base concentration of a solution determined? | acid (or base) concentrations are determined in the lab by titration of a solution of unknown concentration with a base (or acid) solution of known strength |
| hydronium ion | the h3o+ ion, formed when an acid reacts with water |
| bronsted-lowry acid | a substance that can donate a hydrogen ion, H+, to another molecule or ion |
| bronsted-lowry base | a substance that can accept H+ from an acid |
| conjugate acid-base pair | two substances whose formulas differ by only a hydrogen ion, H+ |
| conjugate base | the substance formed by loss of H+ from an acid |
| conugate acid | the substance formed by addition of H+ to a base |
| amphoteric | a substance that can react either as an acid or a basr |
| strong acid | an acid that gives up H+ easily and is essentially 100% dissociated in water |
| dissociation | the splitting apart of an acid in water to give H+ and ? an anion |
| weak acid | an acid that gives up H+ with difficulty and is less than 100% dissociated in water |
| weak base | a base that has only a slight affinity for H+ |
| strong base | a base that has a high affinity for H+ and holds it tightly |
| pH | a measure of the acid strength of a solution; the negative common logarithm of hte H3O+ concentration |
| acid-base indicator | a dye that changes color depending on the pH of a solution |
| titration | a procedure for determining the total acid or base concentration of a solution |
| acid dissociation constant (Ka) | he equilibrium constant K and the water concentration together to make a new constant called this |
| ion prodcut constant for water (Kw) | the acid dissociation constant Ka and the water concentration toghether to make a new constant called this |
| normality (N) | the number of equivalents of acid or base per liter of solution |
Created by:
melissan15
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