Chemistry I 3 rd Quarter Exam Review Laws and Theories States of Matter Chemical and Physical Changes Elements and Mixtures Dalton – atom; Rutherford –

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Chemistry I 3 rd Quarter Exam Review Laws and Theories States of Matter Chemical and Physical Changes Elements and Mixtures Dalton – atom; Rutherford – gold foil, nucleus Counting elements in compounds Subatomic Particles and purpose Counting P, E, and N in atoms and ions Isotopes (neutrons change); Ions (electrons change)

Chemistry I 3 rd Quarter Exam Review Groups and their properties Binary compounds Naming compounds (polyatomics) Type I – metal & nonmetal, no split box Type II- metal & nonmetal, split box, use I, II, III Type III – both nonmetals, use prefixes Naming ions Formulas when given name Scientific notation

Chemistry I 3 rd Quarter Exam Review Metric Units – KHDBDCM Mass, volume units and mL = cc = cm 3 Significant Figures Rounding numbers Conversions Density (D = m/v) Molar mass Empirical formulas – change g to mol then divide by the smallest mol, then mult to get whole # Balancing Equations

Chemistry I 3 rd Quarter Exam Review Driving forces in reactions -formation of a solid -formation of a gas -formation of water Strong electrolyte – a substance that, when dissolved in water, produces a solution that conducts electric current very well.

Chemistry I 3 rd Quarter Exam Review Predicting products Nitrate groups are water soluble! Inside / outside groupings Naming reactions – synthesis, precipitation, acid- base, oxidation-reduction. When an acid and base react, water always forms from the H (acid) and OH (base).

Chemistry I 3 rd Quarter Exam Review Mol / mol equations – use coefficients Theoretical yields [actual / theoretical X 100] Wavelength the distance between two waves Ground state = lowest, possible energy state of an atom. Orbitals and principal energy level (valence)

Chemistry I 3 rd Quarter Exam Review Principal energy level = valence electrons “A” group numbers Electron configurations (s,p,d,f) Water – universal solvent due to it being a polar molecule. Making compounds – ionic = metal + nonmetal - covalent = both nonmetals

Chemistry I 3 rd Quarter Exam Review Lewis structures – especially negative ions