Chem 1211 1st Edition Lecture 5 Outline of Last Lecture I. Unit Factor MethodII. PercentagesIII. PropertiesIV. Heat UnitsV. Transfer Equation ConstantsOutline of Current Lecture I. Atomic NumbersII. IsotopesIII. Law of Definite ProportionsIV. Ions and Ionic CompoundsV. Complex IonsVI. MolesCurrent LectureI. Atomic Numbera. Atomic number: defines elementi. Is the number of protons or electrons (e- and p+)b. Atomic weighti. Protons and neutrons have about the same massii. Electrons have much smaller massII. Isotopes: have the same atomic number/electrons/protons, but differ in the number of neutronsa. Atomic mass comes from natural average of all forms of hydrogenIII. Law of Definite Proportions (Constant Composition)a. Ration of elements/atoms in a moleculeb. H2O means two hydrogen molecules for every oxygenc. H2O2 is different from water (hydrogen peroxide)IV. Ions and Ionic CompoundsThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.a. Ions: elements with more or fewer electrons than the corresponding atomb. Cations: positive (+) chargec. Anions: negative (-) charge d. Metals form cationse. Nonmetals form anionsf. IA- alkali metal (form +1 cations)g. IIA- Alkali earth metals (form +2 cations)h. VIIA- Halogens (form -1 anions)i. VIA- (form -2 anions)j. VA- (form -3 anions)k. Transition metals (B series) can form more than one cationV. Complex Ionsa. SO42-b. HSO4-c. H2SO4 (sulfuric acid)d. PO43-e. HPO42-f. H2PO4-g. H3PO4 (phospholic acid)h. CO32-i. HCO3-j. H2CO3 (carbonic acid)VI. Molesa. 6.022 x 1023 particles= 1 mole (Avogadro’s Number)b. Atomic mass of element i. E.g. 12.01 g Carbon = 1 moleii. 26.98 g aluminum = 1 mole= 6.022 x 10^23
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