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pcat inorganic chem
pcat chem
| Question | Answer |
|---|---|
| Na | +1 |
| K | +1 |
| Mg | +2 |
| Ca | +2 |
| Ba | +2 |
| Fe | +2 or +3 |
| Co | +2 or +3 |
| Ni | +2 |
| Zn | +2 |
| Ag | +1 |
| Al | +3 |
| O | -2 |
| F | -1 |
| Cl | -1 |
| Br | -1 |
| I | -1 |
| OH | -1, hydroxide |
| CN | -1, cyanide |
| SO4 | -2, sulfate |
| PO4 | -3, phosphate |
| NO3 | -1, nitrate |
| CO3 | -2, carbonate |
| HCO3 | -1, bicarobate |
| O2 | -2, peroxide |
| MnO4 | -1, permanganate |
| NH4 | +1, ammonium |
| ClO4 | -1, perchlorate |
| ClO3 | -1, chlorate |
| ClO2 | -1, chlorite |
| ClO | -1, hyprochlorite |
| -ite | has one less O molecule then ate |
| Na + Cl | NaCl,sodium chloride |
| Mg + I | MgI2, magnesium iodide |
| Fe (3) + O | Fe2O3, iron (III) oxide OR ferric oxide |
| Al + N | AlN, aluminum nitride |
| NH4(+1) + SO4(-2) | (NH4)2SO4, ammonuim sulfate |
| Zn(+2) + (OH)(-1) | Zn(OH)2, zince hydroxide |
| Ag + NO3 | AgNO3, silver (I) nitrate |
| Ca(+2 + (PO4) | Ca3(PO4)2, calcium phosphate |
| K + MnO4 | KMnO4, potassium permangnate |
| NH4(+1) + CO3(-2) | (NH4)2CO3, ammonium carbonate |
| Co + ClO3 | CoClO3, cobalt (II) chlorate or cobaltous chlorate |
| s | 0 |
| p | 1 |
| d | 2 |
| f | 3 |
| what are the four quantum numbers | n,l,ml, and ms |
| n | shell of the electron (principle quantum) |
| l | subshell of the electron (azimuthal quantum)or (angular momentum quantum) |
| ml | orbital of the electron (magnetic quantum) |
| ms | electron's spin orientation (spin quantum) |
| formula for maximum number of electron in a shell | 2n^2 |
| what is the electron configuration for S (16) | (Ne) 3s^2 3p^4 |
| what is the electron configuration for Ni (28) | (Ne) 3s^2 3p^6 4s^2 3d^8 |
| electrons within the same orbital are represented as having parallel spins. This goes against what? | Pauil exclusion principle |
| No two electrons in a given atom can posess the same quantum number is stated by: | Pauil exclusion principle |
| Azimuthal quantum number is defined by | shape of the orbital, subshells (n-1) or (s,p,d,f) |
| The maximum number of electrons in energy level n is | 2n^2 |
| the maximum number of electrons that can exist within a subshell is given by | 4l + 2 |
| For any given principle quantum number, the value of the azimuthal quantum number ranges from | 0 to n-1 |
| the greatest value of this, is the greater energy of the subshell | l |
| the (greater or loser) value of l, the greater the energy level of the subshell | greater |
| the greater value of l, the greater | the energy of the subshell |
| the greater the value of l, the ---- energy of the subshell | greater |
| magnetic quantum number (ml) is defined by | orientation of the orbital in space all intergers (-l to l) including 0 |
| the possible value of ml are | all integers (-l to l) including 0 |
| spin quantum number (ms) is defined by | the direction of the spin (-1/2, +1/2) |
| how many electrons can be in the same orbital? | 2 |
| The Pauli exclusion principle states that whenever two electrons are in the same orbital.... | they must have opposite spins |
| subshells are ranked by increasing energy by finding | n+l |
| then lower the energy of the subshell, then the .... | lower the value of n+l |
| the lower the value of n+l, then the ..... | lower the energy of the subshell |
| Hund's rule states that | in subshells that contain more than one orbital, the orbital are filled so that there are a maximum number of half-filled orbitals with parallel spins |
| in Bohr's model of the hydrogen atom that energy of an electron is directly dependent on | principle quantum number |
| what describes the excitation exhibited when an electron jumps from its ground state to a higher energy state | atomic absorption spectrum |
| the Heisenberg uncertainty principle states that | it is impossible to determine the momentum and the position of an electron simultaneously |
| this says its is impossible to determine the momentum and the position of an electron simultaneously | Heisenberg uncertainty principle |
| what is planck's constant | 6.62E-32Js |
| what is the speed of light | 3E8 m/s |
| What is the final orbital of Ca | 4s^2 |
| how many electrons in Ca | 20 |
| what is the final orbial and number of electrons if an atom has 20 electron? | 4s^2 |
| if an atoms final orbital is 4s^2, how many total electrons does it have | 20 |
| an energy (x) corresponds to the energy of an electron in which principal energy level? what formula? | E= -RH and E=n^2x, solve for n RH is given |
| in going from 1s2s2p3s3p4s^1 to 1s2s2p3s3p^5 4s^2, an electron would | absorb energy |
| in going from from 1s2s2p3s3p^5 4s^2 to 1s2s2p3s3p4s^1 | emit energy |
| how do you find the amount of energy it takes to move an electron from one energy level to another | E=-RH ((1/ni)^2 - (1/nf)^2) RH= 2.18E-18 J/electron |
| how to determine the energy of a photon given the photon frequency? | E=hv, h=planck's constant 6.62 E-34 Js |
| how to determine the wavelength given a photon that carries an X amount of energy? | E=hc, E is wavelength, h=plank's constant 6.62E-34Js |
| on the periodic table electronegativity increases this direction? | up and to the right |
| on the periodic table ionization energy increases this direction | up and to the right |
| on the periodic table atomic radius increases this direction | down and to the left |
| dipole-dipole interactions and dispersion forces are known as | van der Waals forces |
| van der Waals forces are | dipole-dipole interactions and dispersion forces |
| dipole-dipole interaction are formed by | polar molecules arranging so that posistive sides of molecules get close to negative sides of other molecules |
| polar molecules arranging so that positive sides of molecules get close to negative sides of other molecules is called | dipole-dipole interaction |
| dipole-dipole interactions are negligible in this state phase | gaseous |
| this species tend to have higher boiling points then nonpolor species of the comparable molecular weight | polar |
| polar species ten to have higher boiling point then.... | nonpolar species of the same molecular weight |
| substances with hydrogen bonding tend to have higher boiling point compared with | compounds of similar molecular formual without H bonding |
| substances compound of similar molecular formula without H bonding tend to have lower boiling points then ... | compounds with hydrogen |
| the short lived formation of dipoles causes by the rapid polarization and counterpolarization of the boinding electron cloud | dispersion forces london forces |
| the kind of molecules possess greater dispersion forces | large |
| large molecules possess more of this intermolecular forces | london dispersion forces |
| how many moles in x grams of XY2 | mol= weight of sample(g)/ total molar weight (g/mol) |
| for the general reaction aA+bB= cC + dD rate= | rate=k(A)^x * (B)^y |
| the concentration of radioactive substances A at time t is found by | At= (Ao)e^-(kt) or ln(At)= ln(Ao)-k*e*t |
| how is the first order half-life of a reaction found | t(1/2)=ln(2/k)=0.693k |
| this enthalpy change indicates an endothermic reaction | negative |
| this enthalpy change indicates an exothermic reaction | positive |
| negative enthalpy change indicates an --- reaction | endothermic |
| positive enthalphy change indicates an ---- reaction | exothermic |
| if Keq is very large compared to 1 an equlilibrium mixture of reaction and product will contain | very little of the reactants compared to the product |
| if very little of the reactants compared to the product is contain in an equilibrium mixture of reactants and products, then | Keq is very large compared to 1 |
| if Keq is --- compared to 1 an equlibrium mixture of reactants and products will contain very little of the products compared to the reactants | very small |
| if Keq is very large compared to 1 an equlibrium mixture of reactants and products will contain | very little of the products compared to the reactants |
| if Keq is -- compared to 1 an equlibrium mixture of reactants and products will contain approximately equal amount of reactants and product | close to 1 |
| if Keq is close to 1 compared to 1 an equilibrium mixture of reactants and products will contain | approximately equal amount of reactants ans products |
| in an exothermic reaction adding heat will cause the reaction to | shift to the left |
| in an endothermic reaction adding heat will cause the reaction to | continue forward faster |
| an adiabatic process occurs when | no heat exchange occurs in a system |
| an isothermal process occurs when | temperature of the system remains constant |
| isobaric process occurs when | pressure of the system remains constant |
| an isolated system occurs when | it cannot exchange energy or matter with its surrounding |
| a closed system occurs when | it can exchange energy but not matter with its surrounding |
| an open system occurs when | |
| indicate what magnetic Co (27) is? | its a paramagnetic with 3 upe |
| indicate what magnetic Sr (38) is? | its a diamagnetic |
| indicate what magnetic Si (14) is | its a paramagnetic with 2 upe |
| what is the formula of the maximum number of electrons in a row or period? | its 2n^2 |
| elements in a column or group have the same what? | number of valence electrons |
| elements in the same row or period have the same what | same outermost valance electron in the same shell |
| Range the Halogens from lightest to heaviest | fluorine to chlorine to bromine to iodine |
| Range the noble gases from lightest to heaviest | helium to neon to argon to krypton to xenon to radon |
| what is the Ideal Gas Law? | PV = nRT, where n is moles, p is pressure in atm, v is the volume in L, T is the absolute temperature, R= 0.082 atm/mole K |
| parameters it is on opposite sides of the equal sign other | are directly proportional to each other |
| parameters it is on same sides of the equal sign other | are inversely proportional to each other |
| in a fixed volume container, 6x10^23 molecules of a gas exert a pressure of 12 N/m^2. if 12 x 10^23 molecules of gas were added to the container, what would the pressure become? | 36 N/m^2 |
| how to convert C to K? | by adding 273 to the C temp |
| how to convert mmHg or torr to atm | by dividing the mmHg or torr pressure by 760 |
| how many moles would occupy a volume of 500 ml at a pressure of 1520 mmHg and a temperature of 25C? | 0.041 mole |
| equal volume of different gasses, same temp and pressure | contain equal number of gas molecules |
| for the reaction given below, how many liters of ammonia form when 7.5 liters of hydrogen reacts? N^2 (g) + 3 H^2 (g)> 2 NH3 (g) | 5 L |
| a gas mixture containing H,O, and N has a total pressure of 12 atm and the O has a partial pressure of 3 atm, what is the partial pressure of the N gas? | 7 atm |
| for a gas collected wet one must subtract the vapor pressure of the water from | the total pressure to the pressure of the gas |
| to find the heat moved in a given process | q=m*c*dT, m-mass, c=specific heat, dT=change in temp |
| Given several reactions and their changes in enthalpy. calculate change in enthalpy for another reaction based on this | combine given reactions, multiply/factor to cancel needed compounds on either side after adding is complete so that the final reaction is the same as the one that must be calculated for. Add the reactions dHs to find the dH for the answer |
| change in entropy is given by | dS=Sfinal-Sintial, dS=q rev/T |
| change in Gibbs free energy is found by | dG=dH-TdS |
| if dG is negative this reaction is | spontaneous |
| if dG is positive the reaction is | non-spontaneous |
| if dG is zero the reaction is | in a state of equilibrium |
| if dH=TdS the reaction is | in a state of equilibrium |
| if dH>TdS the reaction is | not spontaneous |
| if dH<TdS the reaction is | spontaneous |
| if dG is --- the reaction is spontaneous | negative |
| if dG is --- the reaction is not spontaneous | positive |
| if dG is --- the reaction is in equilibrium | zero |
| the heat of formation of any element in its elemental stat is | 0 |
| P1V1= | P2V2 |
| V1/T1= | V2/T2 |
| n1/V1 | n2/V2 |
| PV= | nRT |
| at STP one mole of a gas would occupy a volume of | 22.4L |
| thus 1 mole at STP is = to how many litters | 22.4L |
| a 3 mole sample of methane gas would occupy what volume | 67.2L |
| what mass of O2 gas would occupy a volume of 1800 ml at STP? AW of O is 16 | 2.6 g |
| what are the first 3 postulates of the Kinetic-Molecular Model | 1.Gases consist of individual mol or atomes that are widely dispersed. 2.Gas mol travel in random, straight-line motion. 3.The average kinetic energy of the gas mol is directly proportional to the absolute temp of the gas |
| what are the next 3 postulates of the Kinetic-Molecular Model | 4.Collisions that the gas mol experience are perfectly elastic (no net loss of momentum). 5.the pressure of a gas is due to collisions between the gas mol and the walls of the gas's collisons. 6.Gas mol dont attract each other. |
| what are the last postulates of the Kinetic-Molecular Model | 7. the volume actually occupied by the gas mol is negligible relative to the total volume of the gas's container |
| gases tend to deviate from ideal behavior at | low temps and high pressure |
| means between molecules | intermolecular |
| means within molecules | intramolecular |
| is a measure of the capacity of the atoms of an element to attract bonded electrons | electronegativity or EN |
| non-metals have a greater EN then | metals |
| rank O,F,Ce in order of greatest to lest EN | F (4), O (3.5), Ce (0.7) |
| the greater the EN difference between the bonded atoms | the more polar (or more ionic) the bond |
| if EN is less then 0.5 then the boned is | non-polar covalent |
| if EN is less then 0.5 to 1.9 then the boned is | polar covalent |
| if EN is less then greater then 1.9 then the boned is | ionic bond |
| O=3.5,H=2.1,C=2.5,Ca=1.1,K=0.9,N=3,Br=2.8....which one will form the most ionic bond? | K-O |
| O=3.5,H=2.1,C=2.5,Ca=1.1,K=0.9,N=3,Br=2.8....determine if the following bonds are non-polar or polar 1.C-H, 2.N-H, 3.N-Br, 4.C-Br | 1. non-polar, 2. polar covalent, 3.non-polar, 4. non-polar |
| polar molecules | the EN on the bond is not the same, causing there to be a dipole moment. the mol is not symmetric |
| non-polar | the En on the bond is the same, the dipole moment is zero. the mol is symmetric |
| symmetric molecules are | non-polar |
| non-symmetric molecules are | polar |
| London Forces attractions | are the means by which neutral, non-polar molecules attract to each other, it is weakest intermolecular attraction |
| dipole-dipole attractions | polar molecules that attract each other strongly through partial charges of other molecules |
| hydrogen bonding | is very strong dipole-dipole attraction that involves a polar molecule containing H bonded to either F,O, or N |
| what are some common H-bonds | H2O, NH3, HF, alcohols, ammines, and carboxylic acids |
| ionic bonds are | metal/non-metal combination, and common polyatomic ions |
| what are some examples of ionic compounds | NaCl, MgO, NH4HO3, NH4Cl, |
| the attraction between the ions in an --- is the strongest possible intermolecular force | ionic compound |
| rank the intermolecuelar force from strongest to weakest | ion-ion> H-bonding > dipole-dipole > london |
| the stronger the intermolecular attraction, then the higher | the MP and the BP will be |
| the larger the molecules the stronger the attraction | non-polar |
| the smaller the molecule the stronger the attraction | polar molecules and ions |
| results when two atoms of the same element form a bond or when two atoms of different elements but with the same EN form a bond | non-polar bonds |
| the greater the EN difference between the atoms in a bond | the more the polar the bond will be |
| if the EN difference between the two atoms in a bond is | very large (greater than 1.9) the bond will be ionic |
| indicate which molecules in the following pairs would have the higher boiling point. 1. CH4 or CCl4, 2. H20 or H2S, 3. CH4 or NH3 4. C2H6 or C4H10 | 1. CCl since it is significantly heavier 2. H2O the H-bonder,3. NH3 the H-bonder, 4. C4H10 as it is heavier |
| Empirical Formula | the empirical formula gives the simplest whole number ratio of atoms present in the compound |
| molecular Formula | the molecular formula gives the actual number of atoms of each element that are present in the compound |
| the ---- may be the same or a multiple of the empirical formula | molecular formula |
| give the empirical formula for the following compound. 1. C2H6 , 2. C3H6O3, 3. C4H10, 4. Na2SO4, 5. (NH4)2O2, 6. NH4NO2, 7. K2S2O8 | 1. CH3, 2. CH2O, 3. C2H5, 4. Na2SO4, 5. NH4O, 6. NH2O, 7. KSO4 |
| calculate the formula weight for, 1. (NH4)2CO3, 2. Na2SO4 * 10 H2O | 1. 96G/Mol, 2. 322g/mol, |
| a 60 g sample of NaOH contains how many moles | 1.5 mole |
| what is the mass of 2.0 moles of Na2SO4 | 284 g |
| calculate the percent composition for each element in Na2CO3? | Na=43.4%, C=11.3%, O=45.3% |
| A compound contains 27.3% carbon and 72.7% oxygen by mass. what is the empirical formula for this compound? | CO2 |
| A compound is 80.0% carbone and 20.0% hydrogen by mass, and has a molecular weight of 30.0 g/mole. determine the molecular formula for this compound. | C2H6 |
| A sample of a compound contains 0.9 g of element A and 0.6 g of element B is 40 g/mole, then what is the empirical formula for this compound | AB |
| density = | mass/volume |
| what is the volume of a solid object that weighs 20g if the density of the solid is 4 g/cm^3 | 5 cm^3 |
| what is the mass of 20 ml of a liquid if the density of the liquid is 0.8 g/ml | 16g |
| specific gravity of X= | (density of X)/(density of water), with both densities measured at the same temp |
| at temps where water is a liquid SG is | essentially numerically equal to density |
| in some problems, where water is a liquid, SG can be taken as | equal to density |
| objects with a SG greater then one will | sink in water |
| KE= | (1/2)mv^2 = (3/2)kT |
| r1/r2= | sqrt(MM2/MM1) |
| natural processes want to decrease enthalpy and | increase entropy |
| any process that increase entropy and decrease enthalpy will be | spontaneous at any temp |
| any process that does this will be spontaneous at any temp | increase entropy decrease enthalpy |
| the higher the molecule mass, the -- the gas will diffuse | slower |
| the higher the molecule mass, the ... | slower the gas will diffuse |
| to find bond order from a MO diagram | subtract antibonding electron from bonding electrons and divid by two |
| what type of amine is found as an organic salt | Quaternary NH4 |
| what are the colligative properties | lowering vapor pressure boiling point elevation freezing point depression osmotic pressure |
| what functional group cannot be formed from carboxylic acid | ethers |
| the smaller the Ksp the lower the ... | solubility |
| the smaller the ---- the lower the solubility | Ksp |
| the --- the Ksp the lower the solubility | smaller |
| whatever is being oxidized is the | reducing agent |
| whatever is being reduced is the | oxidizing agent |
| a gain in charge is | oxidation |
| a loss in charge is | reduction |
| a gain in electron is | reduction |
| a loss in electrons is | oxidation |
| this hybridization is linear | sp |
| this hybridization is trigonal planar | sp2 |
| this hybridization is tetrahedral | sp3 |
| this hybridization is trigonal bipyrimidal | sp3d |
| this hybridization is octahedral | sp3d2 |
| the shape of sp is | linear |
| the shape of sp2 is | trigonal planar |
| the shape of sp3 is | tetrahedral |
| the shape of sp3d is | trigonal bipyrimidal |
| the shape of sp3d2 is | octahedral |
| which thermodynatic property tends to increase in a spontaneous process | entropy |
| what is the most advance theory of molecular bonding | MO theory |
| Ksp= | (A)^x*(B)^y |
| LeChatelier's principle states that | when a stress ( change in concentration, temp, volumn, or total pressure) is applied to a system, the equilibrium will shift to relieve that stress |
| which is the anode and which is the cathode, and what do the double represent in Cu/Cu2+//Ag+/Ag | Cu side is anode Ag side is cathode and the salt bridge |
| Cu/Cu2+//Ag+/Ag where does oxidation occur | at the anode on the left |
| Cu/Cu2+//Ag+/Ag where does reduction occur | at the cathode on the right |
| meta directors do this | help stabilize a positive charge on the meta position |
| what is the order of oxidation for functional groups from lowest to highest | alkyne, alkene, alkane, alcohol, ketone/aldehyde, COOH, CO2 |
| the dehydration of -COOH with an -OH yields what functional group | ester |
| what is the order of stability for a carbon free radical from lowest to highest | methyl, primary, secondary, tertiary |
| which of the following functional groups will have the greatest partical positive charge in carbon on the beta position to the function group? why? amine, aldehyde, alcohol, alkene | aldehyde O has a large EN so it has an inducive effect on adjacent carbons |
| what results in a free radical | homolytic cleavage |
| homolytic cleavage results in | a free radical |
| the solution for a salt with a cation of a strong base and an anion of a weak acid will form what type of solution | basic |
| the solution of a salt with a cation of a weak base and an anion of a strong acid will form what type of solution | acidic |
| the solution of a salt with a cation of a strong base and an anion of a | weak acid will form a basic solution |
| a solution of salt with a anion of a with a weak acid and ----- would form a basic solution | a cation of a strong base |
| as temp increase reaction increase was an idea from | Arrhennius |
| if a gas is only on the product side of the equation it means | entropy has increased |
| if a gas is only on the reactant side of the equation it means | entropy has decreased |
| a solute in a liquid will cause vapor pressure | depression |
| to find heat capacity do this | mass x specific heat |
| to find rate of effusion | rate 1= sqrt(MW2/MW1)rate 2 |
| wavelength x frequancy = | c (speed of light) |
| on the periodic table atomic radii tend to increase | down and to the left |
| to determine which solutes in water will raise the boiling temp the most | determine which solute produces the most moles when dissolved |
| given the initial concentration of a reactant in a first-order reaction, a rate constant, find the molarity after t seconds | ln(A0)/A)= kt |
| when pressure increase | equilibrium shifts in the direction to produce a smaller gas volume |
| when pressure decrease | equilibrium shifts in the direction to produce a larger gas volume |
| this can react with either an acid or a base and is formed by an amphoteric element, which is an element that can react as a metal or a nonmental | an amphoteric oxide |
| the larger the value of the equilibrium constant, KA | the stronger the acid/base |
| the smaller the value of the equilibrium constant, KA | the weaker the acid/base |
| what are the solubility rules | 1. all salts formed with alkali metal. 2. all ammonium salts (NH4+) and nitrate salts (NO3). 3. many chlorides bromides and iodides. 4.Many sulfates (SO4^-2) |
| these are the three steps to forming a polymer | initation, 1. formation of free radical progagation, 2. chain lengthening step termination. 3. when something bonds to the free radical and discontinues the chain growth |
| what kind of reaction is most likely to react with an aromatic compound | electrophile |
| what type of alcohol will most rapidly undergo a dehydration reaction? why? | tertiary it will have the most stable carbocation intermediate, tertiary |
| to find functional groups this spectroscopy is best | IR |
| To find molecular fragments this spectroscopy is best | MS |
| To find bonding structure this spectroscopy is best | NMR |
| 1 mole of electrons is symbolized as | 1 faraday |
| this is the only kine of nuclear decay that can increase atomic number | beta decay |
| when an aldehyde is oxidized it becomes | carboxylic acid |
| how is singlet/doublet/triplet ect determined | count the number of H on the desired C and any adjacent C |
| what represent the energy gained by given an electron to an element | electron affinity |
| Ag+ + I- > AgI what can be added to remove more silver from the solution | KI |
| in oxyacids, the ---, the stronger the acid | more oxygen present |
| in oxyacids, the more oxygen present the | stronger the acid |
| in polyprotic acids, the more hydrogen bonds of oxygen lost hydronium ions, the | stronger the acid |
| in polyprotic acids, ---, the stronger the acid | the more hydrogen bonds of oxygen lost hydronium ions |
| in equilibrim equations, ---- is not included because its will remain almost constant | H2O |
| H20 is not included in --- because its concentration will remain almost constant | equilibrium equations |
| H20 is not included in equilibrium equations because | its concentration will remain almost constant |
| this is the formation of a solid from a gas | deposition |
| causing a reaction to occur by increasing the temp increase the influence of this | entropy dG= dH-TdS |
| what kind of isomer will rotate plane polarized light | enantiomer |
| this has chiral carbons that cancel the rotation of light out on each other | diastereomer |
| what type of amine is most alkaline in water | tertiary |
| a Claisen rearrangement yields what type of compound | phenol derivative o-substituted phenol |
| either oxidizes to this | CO2 |
| Alpha decay does this | reduces atomic number by 2 |
| beta decay does this | increase the atomic number |
| when naming a benzene ring, constituents on adjacent carbons go in this order ( carbon 1,2,3) | otho, meta, para |
| a Claisen condensation will produce what | beta keto ester |
| this is the reaction of esters in the presence of sodium ethoxide | Claisen condensation |
| these are created by a dehydration reaction with a carboxylic acid and an alcohol | ester |
| these are created by a dehydration reaction with a carboxylic acid and an amine | amides |
| where as objects with a SG less than one | will float in water |
| homogenous | completely uniformed mixture with a variable concentration like, sugar dissolved in water |
| solute | what is being disolved |
| solvent | what is doing the dissolving |
| the solute is usually the | lesser part of the solvent |
| the solution always takes on the | physical state of the solvent |
| polar solvents like ---- tend to be good solvent for other polar substances | water or ammonia |
| non-polar solvents like--- tends to be a good solvent for non-ionic and non-polar substances | carbon tetrachloride or a hydrocarbon |
| concentration= | (quantity of solute/quantity of solvent or solution as a whole) |
| Molarity or M= | (# moles of solute/ V of solution in L) |
| M x VL=# of moles or V ml = | # of mmoles |
| how many moles of a solute are contained in 750 ml of a 4M solution? | 3 moles |
| a solution is prepared by dissolving 60g of NaOH in enough water to give a total volume of 500 ml. what is the molarity of the NaOH in this solution? | 3 M |
| present of mass/volume= | mass of solute x 100/ mass of solution |
| a solution that is 10% glucose by mass would contain what mass of glucose in 800 g of solution? | 80 g |
| what volume of a 5% glucose solution would contain 20g of glucose? | 400 ml |
| molality is | moles of solute/ mass of solvent in kg |
| a solution is prepared by dissolving 60 g of glucose (C6H12O6) in 500g of water. what is the molality of glucose for this solution? | 0.67 m |
| how many milligrams of solute are present in 250 ml of a 2% solution? | 5000 mg |
| mole fraction= | (# moles of i / total # of moles) |
| a solution is prepared by dissolving 0.5 moles of solute in 4.5 moles of solvent. calculate the mole faction for both the solute and the solvent | solute 0.1, solvent 0.9 |
| a colligative property of a solution is property whose value depends on the number of solute molecules that are present, not on | the nature of the solute molecules |
| Raoult's law | dissolving a non-volatile solute in a volatile solvent has the effect of lowering the vapor pressure of the resultant solution relative to that of the pure solvent. thus P (solution ) < P* (solvent alone) |
| P solution= | (X solvent) x P*, where X solution is the mole fraction of the solvent, P is the vapor pressure of the solution, and P* is the vapor pressure of the solvent |
| a solution is prepared by dissolving 2 moles of a non-volatile solute in 4 moles of a volatile solvent. if the vapor pressure of the pure solvent is 24 torr, what will be the vapor pressure of the solution? | 16 torr |
| boiling point elevation accures when dissolving a non-volatile solute in a volatile solvent has the effect of raising the BP of | the solution relative to that of the pure solvent |
| BP elevation = | TB= kB x m, where TB is the BP elevated, kB is the constant of the solvent , and m is the molality of the solute |
| what would be the boiling point of a 2 m aqueous solution? kB for water is 0.51C/m and the BP of pure water is 100C | 101.2 C |
| freezing point depression occurs when dissolving a solute in a solvent that the effect of lowering | the FP to the solution relative to that of the pure solvent. |
| FP (or how much FP is lowered) depression or TF= | kF x m, m is the molsality of the solute, kF is a constant of the solvent |
| what would be the freezing point of a 2 m aqueous solution kF for water is 1.9C/m and the FP of pure water is 0C | -3.8 C |
| osmosis | the flow of solvent through a semi-permeable membrane, in an effort to equalize concentration |
| dialysis | the flow of solute through such a membrane |
| the pressure that must be exerted on the surface of a solution to stop the flow of osmosis into that solution | osmotic pressure |
| the solution with the largest solute concentration that will yield the greatest colligtive effect is | the greatest colligative effect would be the lowest vapor pressure or the highest BP or the lowest FP or the largest osmotic pressure. |
| electrolytes | ionic solutes will have a greater con |
| ionic solutes will have a greater concentration than | non-ionic solutes (non-electrolytes) |
| non-electrolytes | non-ionic solutes |
| strong electrolytes will yield a higher effective concentration than | will weak electrolytes |
| 1 m NaCl (strong electrolyte) has a higher effective concentration | then 1 m NH3 (a weak electrolytes) |
| 1 m NH3 (a weak electrolytes) has a higher effective concentration than | 1 m glucose (a nonelectrolyte) |
| common strong electrolyte solution acid | HCl, HNO3, H2SO4 |
| common strong electrolyte solution base | NaOH, KOH |
| common strong electrolyte solution salt | NaCl, KNO3, K2SO4 |
| common weak electrolyte solution acid | CH3COOH, |
| common weak electrolyte solution base | NH3 |
| common non-electrolyte solution | sugars like glucose (C6H12O6) and sucrose (C12H22O11) |
| common non-electrolyte solution | alcohol like methanol (CH2OH) and ethanol (C2H5OH) |
| which of the following aqueous solutions would have the lowest FP? a)glucose b)NH3 C)NaCl d) C12H22O11 | C |
| which one of the following aqueous solution would have the greatest osmotic pressure? a) KCL B)K2SO4 C)NH3 D) C12H22O11 | B as K2SO4 yields 3 ions (2K ^+1 and SO4^2-) but only 2 ions (K^1+ and Cl^1-) |
| dilution, i x Vi= | f x Vf, where i is the initial (before dilution) conditions and f indicates the conditions following the dilution |
| what volume of 12 M HCl solution is needed to prepare 500ml of 0.6 M HCl? | 25ml |
| what volume of water must be added to 20 ml of a 4 M NaOH solution to yield a solution that is 0.4 M in NaOH? | 180 ml |
| what are the 3 steps of stoichimetic calculation | 1. obtain the moles of the specified starting species. 2. Use the ratio from the balanced equation to convert form the specified starting material to the target material. 3. convert from the calculated moles of the target material to the desired final |
| Al(OH)3 + 3 HNO3 > Al(NO3)3 + 3 H2O, what mass of HNO3 is needed to react with 2 moles of Al(OH)3? | 378 g |
| the law of combining volume is that gases measured at the same T and P the ratio from the balance equation is | valid in volume unite as well as in mole units |
| 2 C2H6 + 7 O2 > 4 CO2 + 6 H2O, what volume of ethane is needed to react with 21 L of oxygen? | 6 L |
| 2 A + 3 B > C + 4 D, how many moles of C could form when 3.5 moles of A are reacted with 4.8 moles of B | 1.6 mole |
| Al(OH)3 + 3 KOH > Al(OH)3 + 3 KNO3, what mass of aluminum hydroxide could form by the reaction of 40ml of 0.1 M Al(NO3)3 with an excess of 0.2 M KOH? | 0.31 g |
| 2 H3PO4 + 3 Ca(OH)2 > Ca3(PO4)2 + 6 H2O, what mass of calcium phosphate could form by the reaction of 50 ml of 0.2 M H3PO4 with 80ml of 0.1 M Ca3(PO4)2? | 0.83 g |
| common properties of acid | taste sour, turn litmus red, leave phenolphthalein colorless, yield pH's less then seven, |
| common properties of bases | taste bitter and have a slippery feel, turns litmus blue, turns phenolphthalein pink, yield pH's greater than seven |
| Arrhenius acid | generates hydronium ions (H3O^+1 or H^+1) or hydrogen ion when dissolved in water |
| Arrhenius base | generates hydroxide ion (OH^1-) when dissolved in water |
| Bronsted-Lowry acid is | a proton (H^+1) donor |
| Bronsted-Lowry base is | a proton (H^+1) acceptor |
| Lewis acid is | a electron pair donor |
| Lewis base is | a electron pair acceptor |
| strong acids and bases | undergoes the reaction completely, and also in water |
| weak acids and bases | undergoes the reaction partily, and incompletely in water |
| common strong acids | HCl, H2SO4, HClO4, HNO3 |
| hydrochloric acid | HCl |
| nitric acid | H2SO4 |
| sulfuric acid | HClO4, |
| perchloric acid | HNO3 |
| common weak acids | HC2H3O2 or CH3COOH, H2CO3, HF, H3PO4 |
| acetic acid | HC2H3O2 or CH3COOH |
| carbonic acid | H2CO3 |
| hydrofluoric acid | HF |
| phosphoric acid | H3PO4 |
| common strong base | the IA and IIA hydroxide salts are strong base, NaOH, KOH, Ca(OH)2, Ba(OH)2 |
| common weak bases | ammonia or NH3 |
| which of the following molecules is a base? A) NH4, B) N(CH3)3 C)H3NCH2Cl | b, not that N with only 3 bonds retains its lone pair and is, as a consequence, basic behavior |
| an anion obtained from the removal of a proton of a weak acid is | itself a weak base |
| an anion obtained from the removal of a proton of a strong acid is | not a base |
| HF a weak acid yields what | F^1- which is a weak base |
| protonating a weak base yields a | cation that is a weak acid |
| protonating a strong acid yields a | a cation that is not an acid |
| NH3 a weak base yields a | NH4^1+ which is a weak acid |
| NaOH a strong base yields a | Na^1+ which is not an acid |
| indicate whether the following salts would be acidic, basic, or neutral a)NaCl b)NH4Cl c)CH3COONa d) KF e) NaHCO3 | a) neutral, b)acidic, c)basic, d)basic, e)basic |
| conjugates molecules | are two molecules where there structures differ by a single H^1+ |
| molecules that has the extra H^+1 is called | conjugate acid |
| molecules that has the lack a H^+1 is called | conjugate base |
| to determine the acid or base potential of a conjugate we must consider | acid or base strength of its conjugate partner |
| Cl^1- (not a base) is the conjugate base of | HCl but in water, where HCl is a strong acid |
| F^1- (weak base in water) is the conjugate base of | HF, HF is a weak acid in water |
| what is the conjugate base and acid of HNO3 | base: NO3^1- acid: H2NO3^1+ |
| what is the conjugate base and acid of NH4 | base: NH2^1- acid: NH4^1+ |
| what is the conjugate base and acid of HPO4^2- | base: PO4^3- acid: H2PO4^1- |
| what is the conjugate base and acid of OH^1 | base: O^2- acid: H2O |
| for the following reaction indicate the conjugate acid/base pair, HNO2 + NH3 > NH4^1+ + NO2^1- | HNO2(acid)/ NO2^1-(base) and NH3(base)/ NH4^1+(acid) |
| pH= | -log(H^+1) |
| pOH= | -log(OH^1-) |
| calculate the pH for a 0.01 M HCl solution | 2 |
| calculate the pOH for a 0.001 M NaOH solution | 3 |
| (H^+1)= | in log(-pH) |
| (OH^1-)= | in log(pOH) |
| what is H^+1 for a solution whose pH is 11? | 10^-5 |
| what is OH^-1 for a solution whose pOH is 5? | 10^-11 |
| at room temp (H3O^1+)=(OH^1-)= | 10^-7 |
| pH + pOH= | 14 |
| (H3O^1+) + (OH^1-)= | 10^-14 |
| calculate (H^1+),(OH^1-), pH, and pOH for the solution that is initially 0.0001 M in HCl | H+=0.0001, OH=10^-10, pH=4, pOH=10 |
| for the solution that has a pOH equal to 4 calculate pH, (H^1+),(OH^1-) | H+=10^-10, OH=, pH=10 |
| a buffer is a | combination of a weak acid and weak base that resists changes in pH |
| indicate whether or not each of the following pairs would constitute a buffer. a)H3O+/H2O b)CH3COOH/CH3COO- c)HCl/NaCl d)CH3COOH/NH3 | buffers are b and d |
| nA x MA x VA= | nB x MB x VB |
| what is the nA of HCl | 1 |
| what is the nA of H2SO4 | 2 |
| what is the nA of H3PO4 | 3 |
| what is the nB of NaOH | 1 |
| what is the nB of Ca(OH)2 | 2 |
| what is the nB of NH3 | 1 |
| what volume of 0.1 M H2SO4 solution is needed to neutralize 40 ml of 0.2 M NaOH solution | 40 ml |
| if 25 ml of 0.2 M H3PO4 solution is needed to neutralize 60 ml of a Ba(OH)2 solution, then what is the molarity of the Ba(OH)2 solution? | 0.125 M |
| F is | always 1- |
| the IA element is Li,Na,K,Rb,Cs are | always +1 |
| the IIA element is Be,Mg,Ca,Sr,Ba are | always +2 |
| Al is always | +3 |
| H is +1 when bonded to a | non-metal |
| H is -1 when bonded to a | metal |
| O is usually | -2 |
| Cl,Br, and I are usually | -1 |
| what is the ON of Cr in Cr2O7^2- | 6 |
| what is the ON of C in CaC2O4 | +3 |
| what is the ON of P in PO4^3- | +5 |
| what is the ON of O in KO2 | -1/2 |
| what is the ON of N in NO2^1- | +5 |
| what is the ON of H in CaH2 | -1 |
| what is the ON of N in AlN | -3 |
| what is the ON of P in PH3 | -3 |
| what is the ON of F in F2 | 0 |
| what is the ON of I in ICl | +1 |
| combustion reaction consists of the | burning of a substance in air, rapid reaction with oxygen |
| the ideal product for the combustion of a hydrocarbon are | carbon dioxide and water |
| one calorie (cal) is defined as | the heat needed to raise the temp of one gram of the substance by one degree celsius |
| 1J = | 1kgm^2/sec^2 |
| one cal= | 4.18J |
| specific heat is defined as | the heat needed to raise the temp of one gram of substance by one degree celsius |
| SH of water liquid | 1.00 cal/g C= 4.18 J/g C |
| how to indicate no change in physical state | q= mass x SH X dT |
| how much heat is needed to raise the temp of 50 g of water from 20 C to 40 C | 1000 cal |
| what is the heat of fusion | is the amount of heat needed to convert one gram of solid to liquid at the substnce's melting point |
| heat of fusion of water | 80 cal/g= 334 J/g |
| how much heat is needed to melt 30g of ice at 0C | 2400 cal |
| if 500 cal are needed to melt 10 grams of a substance then what is the substances heat of fusion | 50 cal/g |
| the heat of vaporation is | the amount of hear needed to convert one gram of liquid to vapor at the liquid's boiling point |
| what is the heat of vaportation of water | 540 cal/g = 2260 J/g |
| how much heat is needed to vaporize 20 g of water at 100 C | 10,800 cal |
| what is the heat of vaporation if 10 g of a substance liberates 3000 cal upon condensing at the substance's boiling point? | 300 cal/g |
| what is the first law so Thermodynamics | in the physical universe, the sum total of mass and energy never changes. for non-nuclear reactions it is approximately true that mass is conserved as mass and energy is conserved as energy |
| what is the second law so Thermodynamics | a spontaneous reaction is favored by an increase in disorder. Or whenever a spontaneous |
| entropy (S) is the | energy equivalent of the extent of disorder present in a system |
| what is the third law so Thermodynamics | a pure, perfectly crystalline solid at absolute zero temp would have zero entropy (disorder) |
| no material can have a negative entropy as that would | imply greater order than perfect order |
| positive entropy is | disorder increases |
| negative entropy is | disorder decrease |
| dS= | S of product - S of reaction |
| other things being equal, entropy increase from a | solid to liquid to gas |
| predict the sign of dS for the following reaction: a) CaCO3 > CaO + CO2 b) N2 + 3 H2 > 2NH3 | a) + b)- |
| Enthalpy change is | the heat change for a reactio, if measure at constant temp and pressure |
| exothermic | a reaction that evolves heat and has a dH that is negative |
| endothermic | a reaction that evolves heat and has a dH that is positive |
| Gibb's free energy is | the total energy parameter, it take all energy interactions into account |
| dG= | dH - T*dS, (T must be in K) |
| if the total energy is liberated dG is negative and then | reaction is spontaneous |
| if the total energy is consumed dG is positive and then | the reaction is non-spontaneous |
| if dG is zero then the system has reached its energy | minimum and is said to be at equilibrium |
| a reaction has a loss in enthalpy and a gain a entropy. is the reaction spontaneous or not | spontaneous |
| a reaction evolves 250 kJ of heat but has a decrease in disorder of 800 J/K. calculate dG for this reaction at 27C. is the reaction spontaneous or not | -10 kJ |
| when dH is negative, | the reaction is exothermic and the favors spontaneous |
| when dH is positive | the reaction is endothermic and the favors non-spontaneous |
| when dS is negative | the disorder decrease and the favors non-spontaneous |
| when dS is positive | the disorder increase and the favors spontaneous |
| when dG is positive | the energy is consumed and the reaction is non-spontaneous |
| when dG is negative | the energy is produced and the reaction is spontaneous |
| when dG is zero | the energy is nil and the reaction is at equilibrium |
| the rate law | is the relationship of the rate of the reaction to the concentration of the reaction |
| x + y +z = | the overall order |
| the individual orders or the exponents of the concentrations in the rate law are | not necessarily the same as the respective balancing coefficients |
| the individual orders (the exponents) are usually either | 0,1, or 2 but may take on any value |
| the individual orders are determined by selectively varying the concentrations of the reactants | and seeing how the rate is affected |
| k in the rate order reaction dependent on temp, its not directly related to temp, but the increase in temp will cause an increase in k | a decrease in temp will cause a decrease in k, |
| the larger the value of k, then the | faster the reaction |
| for a particular reaction the hydroxide ion is reaction. doubling the concentration of the hydroxide ion, all other concentrations constant, changes the rate of reaction from 0.002 to 0.008. what is the order with respect to the hydroxide ion? | order is 2 as data yields 2^x=4 |
| 2A + B>products, tripling the concentration of A, dont change B, does not change the rate of the reaction. doubling the concentration of B, without changing the concentration of A, double the rate of the reaction. What is the rate law for this reaction? | rate = k(B) |
| for a particular reaction the rate law is found to be: rate=k(A)|(B)^2, if the molarity of A is tripled while the molarity of B is doubled, what will be the effect on the rate? | increase 12 fold |
| the collision theory | for molecules to react, they must collide |
| for collision to be effective what must happen | the molecules must collide with enough force to break the old (reactant molecule) bonds. the molecules must collide with the proper orientation to form the new (product molecule) bond q |
| an increase in temp | must inevitable lead to an increase in the rate of the reaction |
| the transition state theory | a short-lived, maximum energy state that reaction pass through before forming product |
| activation energy | the energy needed to boost the reaction molecules to the transition state |
| activation energy is always positive as it is the energy that | must be added to reach the maximum energy transition state |
| the larger the value of the activation energy, the | slower the reaction will be |
| activation energy forward = | E of the transition state - E of the reaction |
| activation energy revers = | E of the transition state - E of the product |
| Energy (G) = | E of the product - E of the reactants |
| for a particular reaction the transition state has an energy of -4kJ, the reactants an energy of -8kJ, and the products an energy of -15kJ. for this reaction calculate the activation energy in the forward and revers, and the E change for the reaction? | EA (for)=+4, EA (rev)=+11, dG=-7 |
| for the reaction at equilibrium the activation energy in the forward direction is equal to the activation energy in the reverse direction which means | that at equilibrium the rate of the forward reaction is equal to the rate of the reverse reaction |
| the mechanism for a reaction is a series of steps called pathways by which | the reactant molecules are converted into product molecules |
| the sum of the steps in a mechanism yields | the overall equation for the reaction |
| the rate determining step is the | step that more slower then the other step, it determines by itself the rate of the reaction |
| what is a catalyst | speeds up the reaction but unchanged by the reaction, works by altering the mechanism of the reaction leading to a lower energy transition state. it reduces the activation energy of the reaction |
| what is equilibrium | the rate of the forward and revers reaction are the same. |
| equilibrium expression | the appropriate ratio of product to reactions that yields equilibrium |
| the larger the equilibrium constant (K) for the reaction the more | complete the reaction will be |
| the exponents for the reactions and products in the equilibrium expression are always the same as the | respective balancing coefficient from the overall equation |
| the equilibrium expression is | always a ratio of products reactants |
| pure solids, pure liquids, and water when its acting as the solvent for a dilution solution are not | included in the equilibrium expression |
| write the equilibrium expression for each of the following reaction: a) N2 + 3H2 > 2NH3 b)2Hg + O2 > 2HgO | a) K= (NH3)^2/(N2)(H2)^3 b) K= 1/O2 |
| the reaction 2A + B> 2C, has an equilibrium constant equal to four. at equilibrium, the concentrations of both A and B are 1 M, then what is the concentration of C? | C= 2 |
| LeChatelier's Principle is | a system at equilibrium will respond in such a way as to relieve any stress applied to the system. the response will be either to speed up the forward or reverse reaction to until equilibrium is re-established |
| change in concentration, add reactant= | favor forward reaction (shift to right) |
| change in concentration, remove reactant= | favor forward reaction (shift to left) |
| change in concentration, add product= | favor reverse reaction (shift to left) |
| change in concentration, remove product= | favor forward reaction (shift to right) |
| consider any change in pressure to be due | to the appropriate change in volume |
| decrease in pressure | must arise from an increase in volume, shifting the reaction towards the side with more moles of gas |
| increase in pressure | must arise from a decrease in volume and this will cause the equilibrium to shift toward the side with fewer moles of gas |
| 2H2 + O2 > 2H2O, has a sudden decrease in pressure. what will occur? | increase in mole of O2 |
| endothermic reactions view heat as a | reactant component |
| exothermic reactions views heat as a | product component |
| increase in temp as the | addition of heat |
| a decrease in temp as the | removal of heat |
| temp change is treated as | a change in the concentration of heat |
| A + 2B > C + 3D, the above reaction is exothermic. a decrease in temp would cause | |
| the addition of a catalyst to a system at equilibrium has | no net effect on the position of equilibrium (ratio of product over reactant) |
| lowering the energy of the transition state the catalyst would increase the rate of both the forward and the reverse reaction but by the | same proportional factor |
| naturally radioactive isotopes or radioisotopes | are isotopes with unstable nucleii |
| radioisotopes usually decay by | emitting radiation |
| elements whose atomic number is greater then 82 have | no stable isotopes |
| an electron, -1, low to moderate penetrating power | beta |
| a positive electron, +1, low to moderate penetrating power | positron |
| a helium nucleus, +2, very low penetrating power | alpha |
| a proton, +1, low to moderate penetrating power | proton |
| a neutron, 0, very high penetrating power | neutron |
| a high energy light, 0, high penetrating power | gamma |
| in a fission nuclear reaction | a heavy radioisotope split into two lighter isotopes. can be cause by a neutron, evolves an enormous amount of energy an two or more neutrons as a side product |
| in a fusion nuclear reaction | two light isotopes unite to form on heavier isotope, requires a very high initation temp and evolve enormous amount of energy (more then fission) |
| positive charged radiation----- will always be attracted to negative plates | positron, alpha, proton |
| negative charged radiation----- will always be attracted to positive plates | beta |
| an ahydride is formed by the removal of | water from a molecule |
| H2SO4 > SO3 + H20, which is the anhyride? | SO3 is the acidic anhydride, since reversing the process yields anacid |
| Ca(OH)2 > CaO+ H20, which is the anhyride? | CaO is the basic anhydride, since reversing the process yields a base |
| given the anhydride for a) HClO4 b)KOH c)H2SO3 d) Ba(OH)2 | a)Cl2O7 b) K2O c) SO2 d) BaO |
| salt water equilibrium is reached when | the solution is saturated with ions from the salt |
| no salt has unlimited saturation in water nor | is any salt completely insoluble in water |
| for the salt of an analogous formula (both MX or both MX2) the smaller the value of Ksp, the | less soluble the salt will be |
| which is less soluble, PbCl2 with Ksp to 1.7 x 10^-5 or PbI2 with Ksp equal to 8.7 x 10^-9 | PbI2 (smaller Ksp) |
| for simple one to one salts ( formula of MX) we can easily calculate the solubiliy from the Ksp value, thus we have | x= solubility= sqrt(Ksp) |
| common ion effect | if an ion that is common to the salt is initially present in solution, the solubility of the salt in the solution will be alot lower than its solubility in pure water |
| in a saturated solution of the salt MX, the concentrations of both M+ and X- are found to be 1 x 10^-3 M. what is the value of Ksp for MX? | 1 x 10^-6 |
| for the salt MX2, the molar solubility in water would be given by | B |
| oxidation occurs at the | anode |
| reduction occurs at the | cathode |
| in a galvanic (voltaic cell) | a spontaneous redox reaction generates a flow of electricity |
| in an electrolytic cell, an external sources of electricity is used to cause a | non-spontaneous redox reaction to occur |
| if cell potential is positive the reaction would be | spontaneous |
| whereas if the cell potential is negative the reaction will be | non-spontaneous |
| half-cell potential can never be measured as absolute numbers, they are | assigned relative values |
| the standard hydrogen electrode | is assigned a half-cell potential of zero |
| all X2 types of molecules ----- are non-polar | H2, O2, N2, F2 |
| all AX type of moleucles --- are polar | CO, HCl, NO, HBr |
| the short lived formation of dipoles caused by the rapid polarization and counterpolarizationo of the bonding energy | dispersion force london forces |
| these kind of molecules possess greater dispersion forces | large molecules |
| larger molecules possess more of this intermolecular forces | london dispersion forces |
| how many moles in x grams of XY2 | mol= weight of sample (g)/ total molar weight (g/mol) |
| for the general reaction aA + Bb > cC + dD, waht is the rate= | rate= k(A)^x(B)^y |
| the concentration of radioactive substance A at time t is found by | At= (Ao)e^-(kt) or ln(At)= ln(Ao)e*k*t |
| how is the first order half life of a reaction found | t(1/2)= ln (2/k)= 0.693k |
| --- enthalphy change indicates an endothermic reaction | negative |
| --- enthalphy change indicates an exothermic reaction | positive |
| negative enthalpy change indicates an --- reaction | endothermic |
| AB3E2 | t- shaped, sp3d hybridized |
| AB2E3 | linear, shaped sp3d hybridized |
| AB5E | square, pyramidal sp3d2 hybridized |
| AB4E2 | square planar, sp3d2 hybridized |
| ion-dipole | attraction b/t an ion and the oppositely charged end of a permanent dipole possessed by a neutral molecule |
| dipole- dipole | positive end of a permanent dipole aligns itself with negative end of a permanent dipole on another molecule |
| hydrogen bond | special dipole dipole bond between an H and a N, O, or F. |
| dipole induced dipole | attraction between the opposite charge end of a permanent dipole and a temporary dipole of another molecule |
| induced dipole- induce dipole | attractive force b/t molecules resulting from movement mutual distortion of electron clouds (2 non-polar molecules) |
| increasing concentration of reactants (on rate) | increases rate |
| combustion reaction | burning of substances in air, products are CO2 and water |
| molarity | mol solute/ L of solution |
| molality | mol solute/ kg of solvent |
| dilution equation | M1V1= M2V2 |
| diamagnetic | all e- paired |
| paramagnetic | unpaired e- |
| atomic radius trend | increase down a group and decrease from left to right across period |
| ionization energy trend | decrease down a group and increase from left to right across a period |
| increasing temp cause rate to | increase |
| adding a catalyst cause rate to | increase |
| increasing surface area of reaction causes rate to | increase |
| change in temp on an equilibrium constant cause | the constante to change |
| a catalyst changes | mechanism of reaction, lowers activation energy, and rate of reaction |
| rate constant increase with | increase in temp and catalyst |
| Pauli exclusion | no 2 electrons can have the same of 4 quantum number |
| Hunds Rule | the most stable arrangement of electrons in sub-shells is the one with the greatest number of parallel spins |
| Afabau Principle | as protons are added to nucleus, electrons are also added to orbitals |
| electronegativity tend | decrease down a group and increase from left to right across a period |
| linear | sp hybridized |
| AB3, trigonal planar | sp2 hybridizes |
| AB4 | tetrahedral, sp3 |
| AB5 | trigonal bipyramidal, sp3d |
| AB6 | octahedral, sp3d |
| AB3E | bent, sp2 |
| AB3E | trigonal pyramidal, sp3 |
| AB2E2 | bent, sp3 |
| AB4E | see-saw, sp3d |
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