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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 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 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 3: Temperature, Energy and Heat Suggested Review Problems - #37, 39, 43, 45, 48, 49, 64, 69, 70, 74, 76 3.1Temperature Brownian motion temp def temp scales Absolute zero 3.2 Heat and Thermal Energy definitions heat = thermal energy = units – joule, calorie, BTU Thermodynamics o 2nd Law o system – open or closed 1st Law thermal equilibrium specific heat – equation Heat transfer – conductor vs. insulator 3.3 Phase Changes def melting point, boiling point heat of fusion, heat of vaporization solving probs evaporation and condensation 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 Chapter 5: The Structure of the Atom Suggested Review Problems - #23, 28, 32, 38, 44, 46, 47, 52, 54, 56, 57, 59 5.1 The Atom Has a Structure Historical development of atomic theory o Democritus, Dalton, Thomson, Rutherford 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 5.3 Electron Configurations def writing electron configurations 5.4 Light and Spectroscopy spectrum spectrometer electromagnetic spectrum interactions between light and matter o emission spectrum o absorption spectrum Ch 20: Radioactivity Suggested Review Problems - #40, 45, 46, 54, 69 20.1 Nuclear Equations atomic number (Z) mass number (A) neutron number (N) chemical reactions vs. nuclear reactions 20.2 Nuclear Reactions nuclear reactions-def radioactivity-def radiation alpha decay o alpha radiation = alpha particle o parent nuclide o daughter nuclide beta decay o beta radiation = beta particle gamma decay positron emission o positron Chapter 6: Elements and the Periodic Table Suggested Review Problems - #14, 24, 25, 28, 29, 36, 38, 45, 46, 51, 52 6.1 The Periodic Table periodic properties Mendeleev atomic level periodic properties o atomic radius o electronegativity o ionization energy historical development orbitals & atomic radius 6.2 Properties of Groups of Elements alkali metals alkaline earth metals transition metals C, N & O halogens noble gases why compounds form: filled vs. partially filled energy levels 6.3 Valence valence electrons determining valence electrons main group elements Lewis dot diagram