Chemistry 11 Final Exam Study Guide, Study notes of Chemistry

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Unit 1: Safety in the Chemical Laboratory • ensure that you understand all the basic safety rules to follow in the chemistry laboratory • there will be a few safety questions on the final exam Unit 2: Introduction to Chemistry UNIT CONVERSIONS • you should know kilo, centi, milli and micro • use conversion factors • stop off at base unit (metre, litre, gram) • always show your work • always include the units • (unknown) = (initial) X (conversion factor) • DENSITY d = m V ACCURACY & PRECISION • significant figure = a measured or meaningful digit; includes all certain digits and one uncertain • all non-zero numbers significant • leading zeros not significant • trailing zeros significant if there is a decimal • multiplication/division - round to lowest number of s.f. • addition/subtraction - round to lowest number of decimal places • hold all numbers in your calculator and round at the end • accurate = close to correct or accepted value • precise = more significant digits Unit 3: The Physical Properties & Physical Changes of Substances DEFINITIONS qualitative, quantitative, observation, interpretation, data, experiment, hypothesis, theory, law PROPERTIES OF MATTER matter, physical property, chemical property, solid, liquid, gas, aqueous, malleability, ductility, lustre, viscosity, CLASSIFICATION OF MATTER pure substance, mixture, homogeneous, heterogeneous, solution, solute, solvent, element, atom, molecule, ion, particle, compound Chemistry 11 - Final Exam Study Guide Unit 4: Inorganic Nomenclature • metals, nonmetals, semiconductors/semi-metals/metalloids • ions, anions, cations, polyatomic ions IONIC COMPOUNDS • metal and nonmetal • criss-cross combining capacities, simplify; keep polyatomic ions together • examples: potassium oxide, calcium phosphide, tin (IV) sulphate, iron (II) phosphate • name metal and add “ide” to end of nonmetal • Roman numerals for metals with >1 possible charge • examples: CaF2, Cu2O, Ag2SO4, Pb(SO4)2 COVALENT COMPOUNDS • two nonmetals • use prefixes • examples: CO, P2O5, SiF6 • examples: phosphorus trichloride, tetrasulphide dinitride, disilicon hexaiodide PURE ELEMENTS • diatomic elements end in “gen" including halogens HYDRATES • molecules that include water molecules in their crystal structure - ex. CuSO4•5H2O • use prefix and “hydrate” to indicate number of water molecules • examples: CoCl2•4H2O, Al2O3•3H2O ACIDS • start with “H” • examples: HF, HNO3, HClO2 Unit 5: The Mole Concept • Avogadro’s Hypothesis = equal volumes of different gases, at the same temperature and pressure, contain the same number of particles • mole = the number of carbon atoms in exactly 12 g of carbon • molar mass = the mass of one mole of particles • molar mass of each element given in grams on periodic table • for molar mass of a compound, add molar masses of atoms that make up compound • molar volume = volume occupied by one mole of gas at STP = 22.7 L/mol • STP = standard temperature & pressure = 0℃ & 101.3 kPa • Avogadro’s number = 6.02 x 1023 particles per mole anion ending acid ending example “ide" hydro _____ ic HCl = hydrochloric acid “ate" ______ ic H2SO4 = sulphuric acid “ite" ______ ous HNO2 = nitrous acid THE PERIODIC TABLE • created by Dmitri Mendeleev in 1869 • organized by atomic number • metals: reflective, opaque, good conductors, ductile, malleable, solid at room T • nonmetals: gases, liquids or brittle solids at room T, poor conductors, • semiconductor: nonmetal having electrical conductivity which increases with T PERIODIC TRENDS • metallic character - increases right to left and top to bottom • atomic radius - decreases left to right; increases top to bottom • ionization energy = energy to remove an electron from outermost shell of neutral atom; increases left to right, decreases top to bottom • electronegativity = tendency of an atom to attract electrons from neighbouring atom; increases left to right, decreases top to bottom BONDING • ionic bond - electron transfer; attraction between positive and negative ions; between metal and nonmetal; very strong; high melting points • covalent bond - electrons shared equally; between nonmetals • octet rule = atoms in in groups 14-17 form covalent bonds to have 8 electrons in outer shells • double bond = sharing 4 electrons • triple bond = sharing 6 electrons • polar covalent bond = electrons shared unequally; one end slightly more negative (δ-) and one end slightly more positive (δ+) • valence electron = electrons in outer s and p orbitals • valence of an atom = number of unpaired electrons LEWIS STRUCTURES • electrons in outermost s and p orbitals shown with dots • intramolecular forces - covalent bonds between atoms in a molecule; STRONG! • intermolecular forces = van der Waals forces - hold molecules next to other molecules; WEAK! • dipole-dipole forces - due to dipole on polar molecules; ex. hydrogen bond • London forces - weakest intermolecular force; due to momentary dipoles • dipole = partial separation of charge • a molecule is polar if is partial + charge at one end and partial - charge at other end • a molecule that is not polar is nonpolar • polar molecules must be asymmetrical (uneven) • a molecule that is symmetrical is nonpolar • like dissolves like • polar/ionic solutes dissolve in polar solvents • nonpolar solutes dissolve in nonpolar solvents • VSEPR = Valence Shell Electron Pair Repulsion - predicts molecular geometry by examining bonding and non-bonding electron pairs of electrons on a molecule Unit 9: Organic Chemistry • chemistry of carbon compounds • hydrocarbon = compound containing only H and C • each carbon forms four bonds • structural isomers = compounds which have the same molecular formula but a different arrangement of atoms • saturated = contains maximum number of H-atoms • unsaturated = contain some double/triple bonds • cis-trans isomerization = arrangement around double bond • ‘cis’ isomer = 2 groups on same side of double bond • ‘trans’ isomer = 2 groups on opposed sides of double bond • resonance structure = differ in placement of double bonds • aromatic molecule = contains one or more benzene rings