Chem+I+Final+Review

Chemistry Chapter 1 Atoms Molecules scientific method observation hypothesis experiments scientific law law of conservation of mass theory atomoic theory

Chapter 2 Scienfitic Notation Rules for Scientific Notation (bigger than 1 less than 10 etc) Sig Figs 8 rules for Zeros for Sig Figs Sig Figs in addition and subtraction Sig Figs in multiplication and division SI Units Converting Units Unit Prefixes (tera, giga, mega, kilo, deci, centi, milli, micro, nano, pico, femto Density: d=m/v Using density as a conversion factor

Chapter 3 matter atoms molecules states of matter: solid liquid gas solids: crystalline and amorphous Mixtures: pure substance vs mixture, elements and compounds Heterogeneous vs homogeneous Properties: physical vs chemical properties Changes: physical vs chemical changes separation: decanting, filtering, distillation vocab: volatile Energy: Units of energy types of energy: chemical, kinetic, potential, electrical Temperature: C and K scales, conversion C+273 = k Heat capacity: Q=MCDT, Q= heat, M = mass, C= heat capacity, DT = change in temperature

Chapter 4 atoms elements Atomic theory nuclear atom JJ thompson Plum Pudding model Rutherford's gold foil experiment Milikan Oil Drop Experiement proton nuetron electron, know mass and charges, these are called sub atomic particles Periodic Table: chemical symbol, atomic number, atomic mass Marie Curie Metals vs non metals metalloids semi conductors main group elements transition metals groups vs rows/periods alkali metals, alkaline earth metals, halogens, noble gases Ions: gaining or losing electrons, having charge ions and the periodic table +1, +2, +3, +-4. -3, -2, -1, 0 Isotopes: same # of protons different number of neutrons therefor different atomic masses Mass number is an average of differnt atomic masses in different percentages

Chapter 5 Law of constant composition chemical formulas: elements and subscripts use of parenthensis atomic elements (noble gases, metals) molecular elements: HINClBrOF Molecular vs Ionic Compounds Molecular: 2 or more non metals Ionic: metal and a non-metal, aka cation and anion, aka 2 different atoms/groups come together because of opposite charges Ionic Nomenclature: alkali and alkali earth metal names, transition metal names with roman numerals, non metal names with endings changed to -ide. Polyatomic ions Formula Creation: symbols, charges, switcheroo, reduce

Naming Molecular compounds: prefix, element, prefix, element, change ending to -ide Acid Nomencalture: Binary Acids Vs Oxyacids Binary: hydro-basename-ic acid Oxyacids depends on polyatomic ending for -ates it'spolyatomic name, change ending to ic acid for -ites it's polyatomic name, change ending to -ous acid

Chapter 6 Chemical composition grams to moles moles to grams moles to atoms (6.02e23) atomic mass molecular mass Mass percent Mass percent -> chemical formula Chemical formula -> mass percent empirical formulas

Chapter 7 evidence of a chemical reaction chemical equations balanced chemical equations (s), (aq), (l), (g) subscripts aqueous solutions solubility rules precipitation reactions total ionic equations, net ionic equations 5 reaction types: addition, decomposition, combustions, single displacement, double displacement

Chapter 8: stoich mole map mole to mole conversions molar ratios mass-mass convertions (gram -> mole -> mole -> gram) Limiting reagent, theoretical yield, percent yield enthalpy: heat released, conversion factor ie 200kj/mol, negative values represent exothermic reactions, positive values represent endothermic reactions

Chapter 9: quantum chem bohr model electromagnetic radiation schrodinger heisenberg types of light where light comes from according to bohr model energy levels associated with bohr model orbitals: s, p, d, f, know shapes electron configurations: filling an orbital energy diagram, aufbau, hund's rule, pauli exclusion Valence Electrons, group numbers --> valence electrons periodic trends: shielding atomic radius, ionization energy,

Chapter 10 Bonding models lewis dot theory lewis dot structures ionic compounds dots move frrom one element to the other resulting in positive and negative particles that attract molecular compounds: elements share electrons to satisfy the octet rule octet rule double bonds triple bonds lewis dot exceptions resonance VSEPR (valence shell electron pair repulsion thoery) aka 3d shapes of molecules linear, trigonal planar, tetrahedral, trigonal pyramidol, bent electronegativity: pull electrons from neighboring elements polor bonds: electrons not shared equally polar molecules: one side positive one side negative