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UB CHE 101 - Exam 2 Study Guide

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CHE 101Exam # 2 Study Guide Chapters: 10,6,7Chapter 10GasesCommon Units/Equations- Gravity = 14psi- P= force/area or P=gravity*height of liquid*density of liquid (SI unit: Pa)o Standard atmosphere = 1*105 Pao 1mmHg = 1torr & 1atm = 760mmHgLaws and Rules- Boyle’s Law: as P increases, V decreases P=1/V- Charles’s Law: as T increase, V increases V=T- Avogadro’s Law: as n increases, V increases V=n- Ideal Gas Law: describes how gases behave PV=nRT  Mm=mRTPV  d=MmPRTo Units of law are atm, L, mol, Ko Ideal gas constant: R= 0.08206 L*atm/mol*K or 8.314 J/mol*K- Combined Gas Law: used for 1 changing gas (PVnT)1=(PVnT)2- Dalton’s Law: Ptotal=ntotalRTV where ntotal=n1+n2+n3+…o Partial & Total P: mole fraction = ratio of mole of 1 gas to total molex1=n1ntotal∴ x=P1PtotalKinetic Molecular Theory- Explains what happens at molecular level- Particle is in constant random motion, volume is negligible and collisions are elastic- Boyle’s Law: V decreases, # of collisions increase so P increases- Charles’s Law: T increases, # of collisions increases, E increases so greater V- Avogadro’s Law: n increases, # of collisions increases so greater P- KE= ½ mu2 as T increases, u and KE increase but average KE is constantou=√3 RTMmo Heavy and light objects have same average KEGraham’s Law- Effusion = gas escapes through small hole in evacuated space- Diffusion = movement of gas through another- Effusion/diffusion rates are inversely proportional rate1rate2=√Mm1Mm2o Lighter gases effuse/diffuse fasterVander Waal’s Equation- Corrects for non-ideal gases (P+a n2V2)(V −nb)=nRT - a & b are constants found in Table 10.3Chapter 6 Electronic Structure of Atoms- Electrons can be excited to higher energies via electricity and then fall to lower energy (emit light)Wave Properties- Crest- highest point of wave  c=v : speed of waves- Wavelength ()- distance between 2 points (m)- Frequency (v)- # of crests that pass a point in 1sec- C= speed of light = 3*108 m/sRadiation- Electromagnetic spectrum, each color has different energy- Energy of quantum light (SI unit: J) E=hv or E=hc❑o h= Plank’s constant= 6.63*10-34 J*s- White light= all colors= all energies possible- Vaporized element makes atomic spectrum, only some colors line spectrum unique to elementBohr Model of H Atom- Atom doesn’t give off energy in stationary state, change in state means overall energy change Eoverall = Estate 1 – Estate 2- Quantum #, n : indicates energy and radius of electron orbito High n = high energy = bigger radiuso n=1 ground state, n>1 less stable- Bohr spectral lines: more E given when electron jump is larger- Rydberg Equation: calculates amount of E to move from initial to final stateE=−RH(1nf2−1nf2) RH= constant 2.18*10-18 Jo Negative E means E emitted, EF < EI- Matter waves: wave characteristic of particles ¿hmv (mv=mass*velocity)- Uncertainty Principle: impossible to simultaneously know momentum and position of particleQuantum Numbers1.Principle Quantum # (n): indicates size of orbital, shell #a. n=1,2,3,…2.Azimuthal Quantum # (l ) : shape of orbitala. l = 0,1,…,n-13. Magnetic Quantum # (ml ): orientation of orbital around nucleusa. ml = -l …0…l 4. Electron Spin Quantum # (ms): indicates electron spina. ms= ½ or – ½ b. clockwise or counterclockwise, 1st electron = ½ c. each box is an orbital, each row of boxes is a shell andeach cluster of boxes is a subshell5. Assigning n & l values: l by block and n by rowElectron Configuration- Use periodic table and read left to right assigning valuesl #0 1 2 3l letters p d fShape Sphere Dumbbell (2 lobes) Clover (4 lobes) Jack (8 lobes)Nodal planes 0 1 2 3- Condensed: start from previous noble gas and continue- Orbital diagrams have corresponding arrows and dasheso Cr, Mo, Cu, Ag & Au have d-subshell electron configuration exceptionsMagnetic?- Paramagnetic: 1 or more unpaired electron (attracted)- Diamagnetic: all electron paired (not attracted)Valence Electrons- Highest energy level (n), core electron = lower energy levels, group # = valence electron #- d & f electrons don’t contribute to VEs, max # of VEs = 8 (stable)Chapter 7Periodic Trends of the ElementsNuclear Charge- Attractive pull of protons on electron (pull and repulsion)- Coloumb’s Law: attraction increases when charge increases (Q) and attraction decreases when electron distance increases (d) Z =kQ1Q2d2- Not all electrons feel forces equally, core electrons can shield Zeff = Z-S (Z= protons, S= core electron)- Trends in Zeff for VEs on periodic table: left  right increases, top  bottom increasesAtomic Radius Size- Top  bottom increases and left  right size decreasesIonic Size- Cations always decrease  lose VE, Zeff increases so pulls electron closer to nucleus- Anions always get larger- Ions of same charge increase top to bottom- Ions with same # of electrons decrease when atomic # increasesIonization Energy- Removes one mole of electrons from one mole of gaseous atoms/ions- Needs energy to overcome electron-nucleus attraction, always positive- Remove outermost electron one at a time, larger = harder to removeo IE1: atom(g)  ion+ (g) + e-IE1>0o IE2: ion+(g)  ion2+ (g) + e-IE2>IE1- Left to right IE increases, top to bottom IE decreaseso Group 3>Group 2 & Group 6>Group 5Electron Affinity- Adding one mole of electron to one mole of gaseous atoms/ions- Affinity: measure of attraction to add electron (energy released)- EA1: atom(g) + e-  ion-(g) EA<0o EA of noble gas always positive, 8 VE- Left to right EA increases, top to bottom decreasesAlkali Metals- React violently when added to watero Going down a column = larger explosion (IE decreases)Alkaline Earth Metals- React differently with water, less reactiveo Harder, denser and higher IE than Group 1AHydrogen- High IEOxygen Group (6A)- Metallic properties increase top to bottom, form allotropes, oxidize other elementsHalogens (7A)- Diatomic, big negative EA, very reactive- At: extremely rare and radioactiveNoble Gases- Monoatomic,


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UB CHE 101 - Exam 2 Study Guide

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