CHEM 111 1st Edition Lecture 4Last Lecture Review:- Molecular compounds, how to write molecular formulas, how to determine the charge and how to balance chemical formulas, how to name chemicals (chemical nomenclature) Current Lecture:- Chapter 3 – Equations, Moles, Balancing EquationsBalancing Equations: When balancing equations, fractional coefficients may be obtained.C5H10+15/2O2 -----------> 5CO2 + 5 H2OMultiply all coefficients by the denominator. (2 in this case)2C5H10+15O2 ------------> 10CO2 + 10 H2ODefinitions and Rules:Neutralization: The reaction of an acid with a base to form a salt and water.Salt: An ionic compound consisting of the cation of a base and an anion of an acid.Example of Neutralization:HCl + NaOH --------------> NaCl + HOHAcid Base Salt WaterRule: The number of hydrogen ions provided by the acid must equal the number of hydroxide ions provided by the base.These 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.Combustion Reactions: The process of burning. Any chemical reaction that includes burning is a combustion reaction. - Most of these are the combination of a substance and oxygen.- When hydrocarbon burns in oxygen, the carbon is converted to CO2 and the hydrogen forms water (H2O)(CH3)2O + O2 --------> C2H6OOxidation- The loss of electrons by a substance in a reaction.Oxidation-Reduction Reaction- A reaction in which electrons are transferred from one species to another.Oxidation Number- Can be assigned to each number depending on a set of rules… - An atom in its elemental state has oxidation number of 0.- The oxidation number of monoatomic ions is the charge of the ion.- The sum of the oxidation numbers in any species must equal the charge of the species.Reduction- The gain of electrons by a substance in a reaction.Oxidation States:Reactant --------> ProductNa=0 -------> Na+= +1 OxidationCl in Cl2 = 0 ------> Cl- = -1 ReductionMOLES- One mole is the amount of substance that contains as many entities as number of atoms in exactly 12 grams of the 12C isotope Carbon.- Avogadro’s Number is equal to 6.022 x 1023Converting Moles to EntitiesMolar Mass: The molar mass (M) of any atom, molecule, or compound is the mass ingrams for exactly one mole of substance.Converting Moles and MassHow many moles of Ethylene, C2H4 are present in 16 g of that compound?About .57 moles Molar mass of C2H4 is about 28.Mass Percentage from FormulaSubscripts in formula x atomic mass / molar mass x 100Lecture Review:Avogadro’s Number (6.022 x 1023), Mass Percentage Calculation, Converting Moles and Mass, Converting Moles and Entities, Oxidation/Reduction, Neutralization, Combustion