CCL 1110 1st Edition Lecture 5Outline of Last Lecture II. Atomic Structuresa. DefinitionsIII. Atomic Massesa. Definitions IV. The Periodic Tablea. Group NamesV. Molecular and Ionic compoundsVI. Naming Ionic and Molecular CompoundsOutline of Current Lecture I. Chemical EquationsII. Steps to Writing a Balanced Chemical EquationIII. Patterns of Chemical ReactivityIV. Formula Weights and the MoleCurrent LectureI. Chemical Equationsa. Antoine Lavoisierb. Chemical equations- a symbolic representation of a balanced chemical reactioni. Reactants- on the left side of the equation, what the chemicals react withii. Products- on the right side of the equation, result of the chemical reactioniii. Coefficient- number of atoms or moleculesc. Based of the Law of Conservation of mass, the number and type of atoms is unchanged, which means that BOTH sides of the equation must be BALANCEDII. Steps to Writing a Balanced Chemical Equationa. Write the unbalanced equation with all components. This means all formulas are written out correctly and the states of matter are specified (s, l, g, aq)b. Start with the most complex chemical formulai. Balance equations that occur in only one other speciesii. Continue until all elements are atomically balanced1. Typically oxygen and hydrogen are the last ones balancediii. Convert coefficients to smallest integer ratio (no fractions)iv. Verify equal atom countsThese 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.1. Total number and type of atoms on left side = type and number of atoms on right sideIII. Patterns of Chemical Reactivitya. Combination reactions- occur when two or more substances (reactants) react to form one producti. Ex: 2Mg(s)+O2(g)->2MgO(s)b. Decomposition reactions- occur when one substance breaks down into two or more substancesi. Ex: 2H2O(g)->2H2(g)+O2c. Combustion reactions- generally rapid reactions that produce a flame and often involve hydrocarbons reacting with oxygen in the airi. Ex. C3H8(g)+5O2(g)->3CO2(g)+4H2O(g)IV. Formula Weights and the Molea. Mass % of element A=(mass of atoms of A/mass of all atoms)x100b. 1 mole = amount of substance that contains as many entities as there are atoms in one AMUi. Avogadro’s number of entities1. 6.022x10^232. Entities = atoms, ions, molecules, formula units3. Mole is NOT a mass conceptii. Molar mass = M = the mass in grams of 1 mole of substanceiii. A periodic table mass can be used as an average atomic mass or a molar massiv. ATOMIC MASS UNIT=MOLAR