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1st Semester Review Chemistry I Chapter 1: The Science of Chemistry 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 – see vocab 1.3 Matter and Energy matter def o phases energy def o Law of Conservation of Energy Chapter 2: Matter and Atoms 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 3.1Temperature Brownian motion temp def temp scales Absolute zero 3.2 Heat and Thermal Energy def units – joule, calorie, BTU Thermodynamics o 2nd Law o system – open or closed st 1 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 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 oxidation vs. reduction acid-base reaction o pH scale Chapter 5: The Structure of the Atom 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 Chapter 6: Elements and the Periodic Table 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