Chem-is-try Review Sheet Exam IICh 5: ThermochemistryCalorimeter: Q=mC∆T C- Specific heat. (4.18J/g o C for water) Q- Heat kJ m- Mass g (Either convert to kilograms by dividing by 1000, oooooooooooor since you want kJ instead of J divide the calorimeter constant by 1000 orrrrrrrrrrrrrrrr just convert to kJ in the end cause Q needsto be in Q.)Enthalpy ∆H=kJ/mol ∆H= + endothermic (Generally) Less likely to happen naturally in nature ∆H= - exothermic (Generally) Very likely to happen naturally in nature (Up the hill, and down the hill theory)Bewareeeeee heat= kJ. When they ask you the heat of a molecule which has specific number grams, convert those grams to moles using the molecular mass. Once you have the number of moles you multiply that with enthalpy (∆H) because its kJ/mol, and you’re trying to get rid of the moles to get kJ.)Hess’s Law: ∆Hf-∆Hi basically the heat of the products – the heat of the reactants. Make sure to take in account the number of moles with the products and reactants, which can be found by MAKING A BALENCED EQATION!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!- The purpose of Hess’s law is to find the change in enthalpy, or the enthalpy of the entire reaction.- When comparing random enthalpy equations, with the overall enthalpy of the main equation, rearrange the random enthalpy equations to match that of the main equation. Sorry that’s the best I can explain that on text.Ch 6: Electron Structurehttp://www.pvpusd.k12.ca.us/penhi/starodub/notes/unit5/5_notes.pdfhttp://chemwiki.ucdavis.edu/@api/deki/files/8855/Single_electron_orbitals.jpgDe Broglie Relation and Wavelength:=h/mvƛ - Wavelength mƛ m- Mass kg v- Velocity m/s h- 6.626*10-34Js Planck ’s constantMass of an electron- 9.11*10-31kgc- 3.00*108m/s Speed of lightCh 7: Periodic PropertiesEffective Nuclear Charge:Zeff=Z-S Z=Number of protons (Atomic number) S=Non Valence electrons Slaters Rules:S=.35x+.8y+z X=number of valence electrons Y=n-1 Z=n-2 and any other shell S1 shell = .3Atomic Radius:SNOWMAN THEORYCations have a smaller radius than AnionsLargest SmallestP3+S2-Cl-K+Ca2+Sc3+Ionization Energy- Ionization energy (Ei) is the amount of energy required to remove an electron from a neutral gaseous atom or gaseous ion. - Electrons are attracted to positively charged nuclei; ergo removing an electron requires energy.- The process is endothermic, and so ionization energies have a positive value. - The first ionization energy (Ei1) is the energy associated with the removal of an electron from the neutral gaseous atom.- The reaction is represented for the generalized atom X as X→X++e−- The amount of energy required to remove an electron is related to the effective nuclear charge andthe stability of the electron configuration of the atom. It, therefore, shows periodic variation generally increasing from left to right in a period and from bottom to top of a group. - In general, metals have lower Ei1 values than nonmetals. - Exceptions to this general trend from left to right occur when a completely filled s subshell or half-filled p subshell is encountered, because these stable configurations have larger than expected Eil values.http://upload.wikimedia.org/wikipedia/commons/f/f1/Ionization_energy_periodic_table.svg- Removal of successive electrons always requires more energy (e.g., Ei3>Ei2>Ei1) since a negative electron is being removed for a successively higher positive charge. - This pattern of increasing values for successive ionization energies shows a drastic increase in magnitude when an electron is removed from a completely filled energy level or one that is identical to that of a noble gas.Ex. Examine the following set of ionization energy values for a certain element. How many valence electrons does an atom of the neutral element possess?Ionization stepIonization energy(kJ/mol)Ei1 1012Ei2 1903Ei3 2912Ei4 4956Ei5 6273Ei6 22233Ei7 25997Ch 10: Gas LawsEmpirical Gas Laws:PV=nRT P1V1/T1=P2V2/T2 u=√3 RT /M u=Speed of molecule in relation to 2 spacesM= Molecular MassDensity:n=PV/RT (Combo of mass/volume and empirical Gas Law.)Partial Pressures:- The sum of the partial pressure=total pressure of the mixture.- Use empirical gas formula to find the moles of the gas over the total number of moles, mole fraction. You multiply this by the total pressure found in the entire system using empirical gas