Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
chadchem1
chem 1
| Question | Answer |
|---|---|
| Farenheit= | F= 1.8C + 32 |
| paramagnetic | has unpaired e- ; mostly odd number; Oxygen is a good example |
| ______is attracted to the magnetic field; _______ feels slight repulsion from the magnentic field | paramagnetic; diamagnetic |
| Diagmagnetic | NO unpaired e- |
| Pauli Exclusion principle | NO 2 e- have the same set of four quantum number |
| principle shell # | n |
| Azimuthal subshell | L |
| magnetic orientation in space | mL |
| spin quantum number | mS |
| L = ? | [0...n-1] |
| mL = ? | -L--> +L |
| n= ? | [ 1--> infiniti] |
| mS = ? | + 1/2, - 1/2 |
| Azimuthal subshell | for L --> s= 0 ; p= 1 ; d= 2; f= 3 |
| Max # of electrons per subshell | s=2; p= 6 ; d= 10; f= 14 |
| Ground state | original way to write out 1s^2....ect |
| Exctited state | occurs when light is absorbed by the ground state; means u put an e- in a higher level orbital b4 the previous orbital is full |
| 4p^4 5s^1 | excited state of Br b/c the 4p is not full yet... |
| ground state --> excited state | absorb light |
| exctied state --> ground state | emit light |
| Helium nucleus =?? | has no electrons, just protons and neutrons b/c we r in the nucleus |
| 0 ; -1 Beta (e) | elecrton |
| 0; +1 Beta | antiparticle electron |
| 0; 0 Gamma | gamma ray; strong light radiation |
| 4; 2 alpha | has no e-; just protons and neutrons ; i.e. He |
| unstable nuclei | radioactive; has a odd # of Z (protons) or N ( neutrons) |
| stable nuclei | N/Z~ 1 for z<20 ....kind of has to be an equal # of N and Z |
| stable nuclei | N/Z~ 1.6 for larger Z and LArgest N |
| stable nuclei | magic # of N and Z ; makes it stable like Oxygen |
| stable nuclei | 16; 8 O ====> N= 8 and Z= 8 ; so very stable b/c N/Z= 1 |
| E= mc^2 | c= speed of light= 3x10^8 |
| Alpha Decay (emission) | subtract 4 from the top and 2 from the bottom |
| Whats the result of alpha decay? | Reduce Mass |
| Z is greater than 83 for heavy elements | Anything over mass of 83= radioactive |
| Beta - Decay | add 0 to the top and add 1 to the bottom |
| All have to do with electrons | Beta Decay |
| Is something is Emitted then it is a _____ | Product |
| Beta + Decay | add 0 to the top and subtract one from the bottom |
| Electron Emission ( electron gets emitted from the parent nucleus) | Beta - Decay |
| Positron Emission ( gets rid of a positive charged e-) | Beta + Decay |
| Net result of beta- decay? | turn a neutron to a proton |
| Net result of Beta + decay & E- Capture | turn a proton to a neutron |
| E- capture | take in a negative charged e-, subtract 1 from the bottom; is on the reactants side when written |
| too many neutrons and not enough protons ...so N/Z is too high and is ABOVE belt of stability | N--> P Beta - decay used |
| too many protons and not enough neutrons ...so N/Z is too low and is below belt of stability | P-->N Beta + and e- capture used |
| Gamma Decay/ Emission | on product side; change nothing |
| Gamma Decay | Parent nucleus is the same as daughter nucleus; it goes to excited state and then to ground state; giving off light and energy |
| All nuclear reactions ( alpha, beta, gamma) loose mass but only ____ looses mass # | alpha |
| whats the most likely route of decay for an element?? | if the atomic number (Z) is higher than 83 then its alpha decay. if Z is lower than 83; then find the N/Z ratio. If ratio is higher than 1 for Z < 20 then do B- Decay. If N/Z is lower than 1 then do B+ decay OR E- capture |
| Radioactive Decay | 1st order process; N= Noe^-kt ;; 1/2 life is a constant |
| Mass defect in nuclear binding energy | nucleus weighs less than the p and n seperated |
| Highest nuclear binding energy per nucleon of any element ( more stable) | 56 Fe |
| Highest nuclear binding total ( very radioactive) | 235 U |
| The lower the nuclear binding energy per nucleon= | less stable; more radioactive |
| highest mass defect per nucleon= | highest nuclear binding energy |
| Anything close to 56 Fe will have the ______ binding energy per nucleon | highest |
| Effective nuclear charge equation ( this is the same as group #) | Zeff= Z-S |
| Na--> Na+ | one electron removed; electron cloud gets smaller |
| CL--> CL- | one elecrton added; electron cloud gets larger |
| cations are ___ than its neutral atom | smaller |
| anions are ___ than its neutral atom | larger |
| Cations are formed from | Metals |
| Anions are formed from | non metals |
| isoelectric series | all have the same number of e-; more positive = smaller radius; more negative = larger radius |
| ionization energy | energy needed to remove one e- , making it more positive |
| point of stability exceptions | 1. noble gasses 2. S subshell full (group 2) 3. p subshell e- are unpaired (group 5) 4. Zn, Cd, Hg |
| exceptions are.... | reverse the linear trend |
| Electron affinity is _____; IE is ____ | exothermic; endothermic |
| Exceptions of Electron Affinity | 1. Noble gasses 2. Group 2A 3. Group 5A |
| Exceptions of Electron Affinity | are slightly + b/c they do not want to loose an e- and require input of energy to accept an electron |
| Electron affinity | energy change associated with gaining an e- |
| Electron affinity is ___, IE is ____. Both deal with _____ | reduction; oxidation ; ionic bonding |
| Electronegativity | unequal sharing of e- = covalent bonding |
| ionic bonding | meta + non metal; make ionic compounds |
| covalent bonding | non metal + non metal |
| covalent bonding makes what 2 compounds: | (1) molecular compounds ( make molecules); (2) Network solid ( makes 3D structure like graphite, sand, diamond, and SiO2) |
| Metallic bonding | metal + metal; make metallic compounds |
| Ionic has a ____ MP and ___ BP | high MP; High BP; b/c has to break bonds and takes more energy |
| Ionic is brittle T of F? | TRUE |
| Covalent has a ___ MP and __ BP | low MP and LOw BP; DONT BREAK BONDS, except for solid network which has a higher BP/MP than molecular compouds. |
| BP/ MP of Network compounds in covalent bonding is similiar to which MP and BP ? | ionic |
| Metallic | lowest MP and BP. |
| Metallic characteristics: | Malleable(bendable) and ductile. HAS luster and shine. Electrally conductive. GOOD heat conductor |
| lewis dot structure | look at valence e- |
| formal charge | FC= normal( periodic) value of valence e - actual value of valence e |
| resonance | delocalized pie e= |
| double bond... | 1 sigma + 1 pie |
| triple bond... | 1 sigma + 2 pie |
| single bond | 1 sigma |
| Forces inbetween 2 seperate molecules | intermolecular forces (only look at molecular bonds) |
| hydrogen bonding= strongest intermolecular forces but weaker than... | covalent and ionic bonds |
| Capable of hydrogen bonding if... | has F, O, N with lone pairs |
| dipole - dipole | polar |
| ion dipole attraction | weak |
| induced dipole forces | very weak ( polar + non polar) |
| london dispersion forces | weakest of all |
| found everywhere, temporary dipole, non polar things, larger u are= more london u have | london dispersion ( van der waals) |
| highest VP/MP= | lowest BP |
| more branching= | lower BP, higher MP; crystalization faster at higher temp; lower SA, lower london dispersion forces |
| no branching, longest chain of C | largest SA & london dispersion forces, highest BP and MP |
| S--> L | fusion/ melting ENDO |
| L--> G | Vaporization/ boiling ENDO |
| S--> G | Sublimination ENDO |
| ENDOTHERMIC | require energy; H= + and S= + |
| G--> L | condensation EXO |
| L--> S | crystalization EXO |
| G-->S | Deposition EXO |
| EXOTHERMIC | release Energy; H= - and S= - |
| measures CO2 and H20; CALORIES | Calorimetry |
| Kinetic Molecular theory | KE is proportional to T. Hotter the temp= faster molecules travel; pressure is due to force of molecules colliding with walls |
| Ideal Gas Assumptions | 1. No molecular volume (good at low temp) 2. No attractive forces ( ALL COLLISIONS ARE ELASTIC) = no kinetic energy is lost (good at low T) |
| Pressure= | F/ A |
| The stronger the force= | higher the P |
| Smaller the Area= | higher the P |
| Ideal gas law= | PV= nRT |
| Boyles Law | PV= constant/ inversely proportional |
| charles law | V is directly proportional to T |
| Avagodros Law | V is directionally proportional to n |
| combined gas law | p1v1 / n1T1 = P2V2 / nT2 |
| Dalton's law of partial pressure | Ptot= Pa+ Pb+ Pc... |
| Partial pressure= | PA= XA * Ptot |
| Graham's law of Effusion: | r1/r2= sqrt m2/m1 |
| effusion | low ---> high ( escaping of gas from a hole) |
| diffusion | high--->low ( entropy inc) |
| KE= 1/2 mv^2 | same temp = same KE |
| lower molecular mass= | higher velocity ( smell first) |
| solvent | liquid |
| solute | dissolve in solvent--> can be L, S, or G |
| 1 L = 1 kg H20= | 1000 g H2O |
| Solubility Rules: | 1. All group 1 metals, NO3- ( nitrate) and NH4+ ( ammonium salt) are soluble. |
| Solubility Rules: | 2. MOst Ag+, Pb+, Hg2 ^2+( mercury 1) are insoluble, unless number 1 is with it. |
| AgNO3= soluble or insoluble | soluble b/c has NO3- in it |
| solids are more soluble at ____ Temps? | high |
| Gasses are less soluble at _____ Temps? | high |
| Gasses are more soluble at ____ Pressures? | high |
| colligative properties changes with ? | solute conc. and are independent of identity of solutes |
| More solute in conc. = ? | 1. lower F.P.D 2. Lower V.P.D 3. Higher B.P.E 4. Higher O.P |
| colligative properties | 1. F.P.D 2. V.P.D 3. B.P.E 4. O.P |
| No dissociation occurs if.... | something is soluble (i.e. glucose and methanol) |
| largest # of moles= | largest change in collagitive properties |
| highest V.P= | smallest change in collagative properties ( smallest # of moles) |
| freezing point Depression | DeltaTf= -(KfM) ; Kf= given and m = moles that dissociate |
| Normal freezing point of water | 0 degrees C |
| Vapor Pressure Depression | VPD= XA*PA --> PA= pure water |
| Boiling point Elevation | DeltaTb= Kb* m ; Kb= given and m = moles that dissociate |
| absolute B.p = Tb | original BP + Delta Tb |
| water boils at | 100 degrees C |
| osmotic pressure | pi= m r t; m= moles that dissociate |
| Kinetics | rate of rxn |
| THermodynamics | tells us everything except rate of rxn |
| in a rate expression | products= +; reactants= - |
| K is inversely (oppositely) proportional to Ea | so Ea1= bigger than Ea2 ...then K1<K2 |
| slowest step | Ea= largest= highest |
| nuclear decay | Always 1st order |
| Keq= only shows | gasses and AQ |
| Keq= Products / reactants | can also be written as Dalton's partial pressure same way just add P |
| T or F...Keq can never be - ? | true |
| K>1 | products favored |
| K<1 | reactants favored |
| K=1 | fair amount of both reactants and products |
| Q< K | proceeds to the right |
| Q> K | proceeds to the left |
| Q=K | at equilibrium |
| Reaction Quotient (Q) | Q= P/ R |
| Exothermic | - delta H---in products---release heat |
| Endothermic | + delta H---needed as reactants--heat is absorbed |
| an inert gas== | no shift Q=K |
| only thing that changes K is | TEMP...not even a catalyst |
| solubility | ionic solid seperating into seperate ions ( dissociating) |
| common ion effect | adding a common ion o the rxn wil shift the rxn to the left and decrease solubility of a rxn |
| If Qsp> Ksp | precipitate is formed |
| Arrhehius Defn of ACID/BASE | Arrhenius acids form hydrogen ions in aqueous solution; Arrhenius bases forming hydroxide ions. |
| Brownsted Lowry Defn of ACID/BASE | Acid= proton donor; Base= proton acceptor |
| Lewis Defn of ACID/BASE | Acid= e- pair acceptor; Base= e- pair donor |
| Best Lewis acid= | Boron b/c of it's empty P orbital |
Created by:
zrsoori
Popular DAT sets