Polyatomics- Acetate-CH3CO2- , Carbonate-CO32-, Bicarbonate-HCO3- , Chlorate-ClO3- , Pwechlorate-ClO4- , Chromate-CrO42- , Cyanide-CN- , DiChromate-Cr2O72- , Hydroxide-OH- , Nitrate-NO3- , Nitrite-NO2- ,Permangate-MnO4- , Phosphate-PO43- , Hydrogen Phosphate-HPO42- , DiHydrogen Phosphate-H2PO4- , Sulfate-SO42- , Hydrogen Sulfate/bisulfate-HSO4- , Sulfite-SO32- Endo ∆H > 0 Exo ∆H <0 Solubility Ions- Group 1A Cations + NH4+ , Nitrate(NO3-) , Perchlorate(ClO4-) , Acetate(CH3CO2-) , Chlorides bromides and iodides EXCEPT Ag Hg2+ Pb2+ , Sulfates EXCEPT Hg Pb Sr Ba, Insoluble Ions- Carbonate EXCEPT Group 1A + NH4 , Phosphate EXCEPT Group 1A + NH4 , Hydroxide(OH) EXCEPT Group 1A + NH4 + Sr + BaACIDS- Ide–Hydro___ic acid , Ate- ____ic Acid , Ite- _____ous Acid Extensive Property deals with size, mass, volume, and length.Intensive Property deals with everything else.Physcial Properties- Measured without changing the composition of a sample (mass, volume, color)Chemical Properties- the reactivity of a material (explosiveness, and flammability. Also the fact that gold does not react with water).Physical Change- Occurs without a change in composition of the substance (Frezzing is an example).Chemical Change- The substance is converted into a different kind of matter ( the rusting of iron or burning of wood).Homogeneous- Mixtures uniform throughoutHeterogeneous- Changes throughout mixtureAccuracy- Agreement of the measured value with the true accepted value.Precision- agreement among repeated measurementsDaltons Theory- 1. Matter is composed of small indivisible particles called atoms. The atom is the smallest unit of an element that has all the properties of that element. 2. An element is composed entirely of one type of atom. The chemical properties of all atoms of any element are the same. 3. A compound contains atoms of two or more different elements. The relative number of atoms of each element in particular compound is always the same. 4. Atoms do not change their identities in chemical reactions. Chemical reactions rearranged only how atoms are joined together.Electrolytes- refers to a substance that produces ions when dissolved in water (conducts electricity).Non-Electrolytes- water and compounds that dissolve in water.P1V1/T1=P2V2/T2PV=NRT----N=PV/RTR-values--.08206(L*atm/mol*K), 8.314(Kg*m2/s2*mol*K), 8.314(J/mol*K), 1.987(cal/mol*K)1atm=(760mmHg)or(760torr)or(101.325Kpa)1torr=(133.3Pa)Effusion- Tb/Ta=√(molar mass of b/molar mass of a)Dilution/Titrations- M1V1=M2V2Molarity=moles/liters Molar mass=g/mole Molar Volume(volume of a gas)= 22.4liters/1moleAvogadros #(moles to molecules)---6.02x1023Specific Heat- Q=MCs∆T(m=mass in grams, Cs=specific heat, T=(final-initial)Temp Conversions- Tf=Tc*(1.8/10)+32 Tc=(Tf-32)*(1/1.8)Organic Compounds-(CnH2n+2)Dissociation-separation of a compound in waterCombustion- creates CO2 and H20 in productsDaltons Law(partial pressure)- Pt=Pa+PbProperties- GAS-fluid with no definite shape or volume- LIQUID-fluid with fixed volume and no shape- SOLID- both fixed volume and shapeAverage Speed of a Particle- Urms=√[3RT/molar mass(kg)] ***thousand grams in a kilogramNeutralization- (acid+base→H20+salt)Quantum #s- N≠L L at its max=(N-1) ML is between(-L,L) Ms= -1/2 or 1/2Finding N for quantum #s- S(0)P(1)D(2)F(3)G(4) ***n is from orbitalsForces(strongest to weakest)- 1).H bonding(only to N,F,O), 2).Dipole-Dipole 3).London Dispersion.P.T. trends- ELECTRONEGATIVITY/ IONIZATION ENERGY(↑→), Size/Radius(↓←)Lattice Energy- Q1Q2/R ****the smaller R(distance) will have greater lattice energy∆Ho=(sum of moles of products)-(sum of moles of reactants)*****∆Go=gibbs free energy, ∆So=entropy****HOWEVER all equations are the same as ∆HoSteric # # of lone pair electrons on the central atom# of bonding groups (pair ofelectrons) on central atomElectron-pair GeometryMolecular Geometry Bond Angle 2 0 2 Linear Linear 1803 0 3 Trigonal Planar Trigonal Planar 1203 1 2 Trigonal Planar Bent Less than 1204 0 4 Tetrahedral Tetrahedral 109.54 1 3 Tetrahedral Trigonal PyramidalLess than 109.54 2 2 Tetrahedral Bent Less than 109.55 0 5 Trigonal BipyramidalTrigonal Bipyramidal90, 120 and 1805 1 4 Trigonal BipyramidalSeesaw 90, 120 and 1805 2 3 Trigonal BipyramidalT-shaped 90 and 1805 3 2 Trigonal BipyramidalLinear 1806 0 6 Octahedral Octahedral 90 and 1806 1 5 Octahedral Square Pyramidal90 and 1806 2 4 Octahedral Square Planar 90 and 180Electronegativity- inc. going up and over to the rightElectron Affinity- the amount of energy that is released when the electron attaches to the atomFormal charges* Valence e – (# individual bonds + the sum of each lone electron connected to the atom)Molecular orbital theory/steric#- model that combines the atomic orbitals that are shaped over the entire molecule not counting each individual bond/steric# is # of lone pairs+ # of bond regions to the central atom.Molecules that dissatisfy octet rule- Expanded octets- P,S,CL,As,Se,Br,Te,I,Xe Deficient octet- Groups 2A and 3A Lattice Energy- (Compound/energy)- LiF/1036, LiCl/853, LiBr/807, LiI/757, NaF/923, NaCl/786, NaBr/747, NaI/704, KF/821, KCl/715, KBr/682, KI/649, CsCl/657, MgF2/2957, MgCl2/2526,MgBr2/2440, MgI2/2327, CaCl2/2258, Na2O/2481, MgO/3791, CaO/3401.Lattice equation(energy)=kQ1Q2/d BOND ENERGY* enthalpy= sum of reactants- sum of productsHybridization- (steric#/orbital/bond angle) 2/sp/180, 3/sp2/120, 4/sp3/109, 5/sp3d, 6/sp3d2/90 and 180.Diamagnetic- no unpaired electrons Paramagnetic- has unpaired electronsBond order- ½(# of electrons in bonding orbital - # of electrons in antibonding orbitals)Bond order- if answer from equation is – or 0, it cant naturally occur. BUT if it is + then it can occur in nature(stable)Lewis structure process- (1)write the skeleton structure (2)Sum the valence electrons (3)subtract two electrons for each bond in the skeleton structure (4)count # of electrons needed to satisfy octet rule for each atom-if the # of electrons needed equals the # remaining, go to 5.-if fewer electrons remain, add 1 bond for every 2 additional electrons needed (5) place remaining electrons as lone pairs to satisfy octet rule for each atom(not H)Valence Bond Theory- Describes the bonds as being formed by partially filled valence orbitalsIsomers- different compounds with the same molecular formula but different structures (Cis- symmetrical Trans-