Non-classical states of matter: plasma, glass, liquid crystal, superfluids, ionic liquidsDefinite shape Definite volume compressibilitySolid yes yes lowLiquid no yes Some whatGas no no Highly (large gaps, empty space)Pure samples:- Element (cannot be decomposed into simpler substances)- Compound (can be broken down into elements)Mixture:- Homogenous mixture/solution (composed of two or more indistinguishable elements)- Heterogeneous mixture (can visually see components, which can be separated)Physical change: change in form, not chemical compositionChemical change: substance becomes new substance(s) with different chemical composition and properties. (Bonds broken and formed)SI Base UnitsLength meter mMass kilogram kgTime second sTemperature kelvin KAmount of substance mole molElectric current ampere ALuminous intensity candela cd*kg only SI unit that cannot be measured.International Prototype Kilogram= kg stored outside of Paris taken out every 50 years, has lost ~30nanograms (1992)Light (nm)Wavelength of red light= 700nmTK=C+273.15TC=TK-273.15TF=TC(9/5)+32TC=(TF-32)(5/9)*can never have 0K*only use Celsius in class for change in temperature1 dm3 = 1L= 1000cm3=1000mL1cm3=1mL2.25 10^8 kg1.62 10^6 Ldivide by 30!Counting sig figs-Non-zeros are always significant-0’s are sometimes significsnt- leading zeroes are not significant- in-between(captive) zeroes are always significant- trailing zeroes are sometime significant, depending on decimal point. Examples: 20.000=5, 200=1, 30.=2- exact numbers: counted objects, defined amounts(1km=1000m), formula numbers[volume of a cone=(1/3)pir2], atomsinfinite sig figs- pi=1 trillion sig figsThe final number of sig figs in the answer: - in addition possible to gain sig figs- Subtraction possible to lose sig figs- 0 degrees Celsius= 3 sig figs because =273K- Multiplication and division= least precise measurement used in calculation*do not round during intermediate stepsAccuracy: how close to a particular value is true or acceptedPrecision: how close several measurement s are to each otherScanning tunneling microscopy (STM): measure topology of a surface. Magnitude of the current is sensitive to the surface and atoms. Atomic force microscopy: even more sensitive scanning.*provide full name of first 6 periods given 2 letter acronym.*know groups 1-18metalloids: B, S, As, Te, Ge, Sb, AtProperties of metals:- 75% of all metals- Malleable: can be pounded into sheets (Au most malleable)- conducts heat and electricity- solids at room temperature (except Hg)- ductile- tend to lose electrons- shiny- colorless (except Cu and Au)Nonmetals- exist in all 3 states- poor conductors of heat and electricity- solids are brittle- gin electrons on reactions (becomes anion) closer to noble gases so valence shell- found to the right of periodic table (except H)Metalloids: shiny, brittle semiconductors, gain & lose electrons.At room temperature:Hg, Br – liquids H, noble gases, N, O, F, Cl- gasMain group elements: Groups 1,2, 13-18Transition metals: groups 3-12He, Ne actual noble, the rest of the noble gases react.Alkali metals: group 1 (+1)Alkaline earth: group 2 (+2)Group 3 (+3)Group 16(-2)Halogens: group 17 (-1)Noble gases (0)Neutrino* = mass close to nothingIsotopes have different numbers of neutrons, different masses- react the same chemically- same number of protons- >90% of isotope are radioactive, every element has at least one unstable isotope.Polonium has no stable isotopes, anything after no stable isotopes.12C= exactly 12 amu1 amu= [12C mass]/12Atomic masses on periodic table reflect whichever isotope is most abundantAmu=1/12 of a CarbonCalculate atomic mass: (mass amu)(abundance)+(mass2 amu)(abundance)+…Mass Spectrometer can find the average atomic mass: two peaks with mass and % on each.Score 20Gross 144Googol 10100Ream 5001 mol= 12 g of pure 12CNA= 6.02214*1023Mass molesElement=amuCompound=molar massChapter 3: Molecules, compounds and chemical equations (skip 3.11)Covalent bonds: sharing electrons. Atomic elements (metals, noble gases) exist as single atomsMolecular elements: the same element covalently bonded to itself. (Br2, I2, N2, Cl2, H2, O2, F2) P4,S8,Se8Molecular compounds: have greater than or equal to 2 bound nonmetals. H2OIonic compounds: composed of cations and anions. NaCl1. Binary Ionic Compounds (metal +nonmetal) forms 1 cation- Cation  anion- Cation name same as on periodic table- Anion= root+ide2. Binary Ionic Compounds (metal +nonmetal) metal forms 2 or more cations, requires roman numeral.3. Binary covalent compounds (nonmetal+nonmetal)- Prefixes to indicate each atom- No mono*table 3.2 doesn’t require roman numeralAcids ionize in water to produce H+ ions (protons)No oxygen in acid: (hydro__anion root__ic acid)If anion contains oxygen:Last three letters replace with: ite ateLast three letters replace with: -ous -ic (stronger than –ous acid)Per- added as many atoms of a particular element as possible.Mass percent: the percentage by mass of its elements.Mass%= mass of element in 1 mol compound/molar mass compound (100%)Empirical formula: lowest ratio with whole numbers and correct ratios.Molecular formula: formula with the actual number of atoms in the molecule. (MFs are integer multiples of EFs).benzene Hydrogen peroxide Sodium chlorideMF: C6H6H2O2NaClEF: CH OH NaCl*All ionic formulas are empirical formulas(EF)n=MFMF/EF=nMolar mass(MF)/molar mass(EF)StoichiometryCalculating quantitates of reactants and products in a chemical reaction.-Based on the law of conservation of matter.Theoretical yield (calculated): the maximum amount of product that can form during a reaction.Actual yield (measured): the amount of pure product collected from a reaction.Actual/theoretical * 100%Exam:-memorize element name first 6 periods-show work-report units and correct sig figs-BRING: casio 260, pen, and student ID-short answer*PRACTICE EXAMMolarity (M)= moles of solute/liters of solventDilution: common to make dilute solutions from more diluted ones (stock solutions).Dilutions, more solvent is added but the amount of solute remains constant.MV=M2V2Precipitation reaction: homogenous + homogenousheterogeneous Acid-base reactionsOxidation-reduction reactionsComplete ionic equations: all strong electrolytes are written.No precipitate=no reactionAcid produces H+ in waterBase produces –OH in waterTitration: analysis of the amount of a substance by reaction with a solution of knownconcentrations uses molesDiprotic acid (H2SO4)- need twice