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1st Semester Review Chemistry I Chapter 1: The Science of Chemistry Suggested Review Problems - #35, 46, 47, 52, 53, 54, 57, 73 1.1 What Chemistry is About Measurements & Units: Mass & weight; Volume; Density; Pressure Accuracy & precision Significant figures Scientific notation Dimensional analysis 1.2 Scientific Inquiry natural laws inquiry theory hypothesis experiment variable experimental variable control variables error average conclusion significant difference objective 1.2 Scientific Inquiry (cont.) repeatable procedure scientific method 1.3 Matter and Energy matter def o phases of matter energy def o Law of Conservation of Energy Chapter 2: Matter and Atoms Suggested Review Problems - #32, 39, 44, 58, 64, 66, 67, 70-73, 75 2.1 Matter and the Elements substance vs. mixture o element physical properties & physical change chemical properties & chemical change Periodic Table mole o Avogadro's number o calculations 2.2 Molecules and Compounds defs chemical formula molecular compound 2.2 Molecules and Compounds (cont.) ionic compound formula mass 2.3 Mixtures and Solutions homogeneous vs. heterogeneous solution o solute o solvent o dissolved concentration o concentrated vs. dilute o solubility o molarity o calculations percent by mass molarity mixtures of gases o molar volume o STP Chapter 5: The Structure of the Atom Suggested Review Problems - #23, 28, 32, 38 5.1 The Atom Has a Structure Historical development of atomic theory o Democritus, Dalton, Thomson, Rutherford 5.1 The Atom Has a Structure (cont.) atom interior o nucleus o electron cloud o properties of subatomic particles atomic number, atomic mass o isotope o average atomic mass ions 5.2 The Quantum Atom quantum theory o quantum state o 5 statements waves & particles o frequency o wavelength o photon o Planck's constant o relationship btwn frequency & wavelength, energy & frequency; wavelength & energy electrons as waves o allowed wavelengths orbitals energy levels o Pauli exclusion principle Periodic Table & energy levels Chapter 8: Compounds & Molecules Suggested Review Problems - #s 22, 24, 26, 27, 28, 30, 37, 38, 48, 51 8.1 Ionic Compounds Properties charges cancel Polyatomic ions Writing Formulas: total positive charge must balance total negative charge Formulas with Polyatomic ions: use parentheses NAMING: o binary ionic compounds o compounds with polyatomic ions o compounds with transition metals 8.2 Covalent Compounds Properties - molecule Small molecules Medium-sized molecules - lipid - steroid - hydrocarbon Polymers - polymer - monomer - homopolymer - copolymer 8.2 Covalent Compounds (cont.) Network covalent Formulas - empirical formula - molecular formula NAMING: o binary covalent compounds, prefixes 8.4 Formula Masses calculation of molar mass Percent Composition: formula Calculating Empirical Formulas Calculating Molecular Formulas Chapter 4: Physical and Chemical Change Suggested Review Problems - #39, 42, 45-47, 50, 56, 57, 59, 61, 70 4.1 Understanding Chemical Changes def irreversible interatomic forces vs intermolecular forces chemical bonds o covalent bond – molecule o ionic bonds enthalpy of formation reactivity 4.2 Chemical Reactions chemical reaction reactants & products balance equation coefficient endothermic vs. exothermic o activation energy 4.3 Chemical Reactions in the Lab symbols for states of matter precipitate salt precipitation reaction redox reaction acid-base reaction Chapter 13 = Acids & Bases Review Problems - #s 21, 23, 24, 27, 29, 30, 31, 32, 35, 40, 44, 52, 58, 60 13.1 The Chemical Nature of Acids & Bases - neutral - acid - base The importance of the H+ ion - Arrhenius theory - hydronium ion 13.1 The Chemical Nature of Acids & Bases (cont.) Brønsted-Lowry definition - acid - base -amphoteric Brønsted-Lowry: acid-base pairs Identifying acids/bases: acids have leading "H", strong bases have "OH" - strong - weak 13.2 The pH Scale: acids-pH<7, neutral-pH = 7, bases-pH>7 -logarithm Definition of pH Calculating pH for acids Calculating pH for bases pH indicators - indicator =