Types of Chemical Bonds: Covalent, ionic, metallicCoulomb’s LawForce = kQ1Q2/d^2We don’t care about the force, we care about the amount of energyElectrostatic Energy = charge A * charge B / distanceThe Book Refers to it this wayEel = 2.31*10^-19J*nm Q1 * Q2 / dProperties of Covalent CompoundsCovalent compounds are typically:Not hard, rigid or brittle (generally liquids or gasses)Have low melting pointsDo not conduct electricity in any stateStronger bonding forces holding atoms together within a moleculeWeaker intermolecular forcesCovalent Bonding and Nomenclature (2.7, 2.8, 9.3)Types of Chemical BondsIonic Bond: Chemical bond resulting from the electrostatic attraction of a cation and an anionProperties of Ionic CompoundsIonic Compounds are typicallyHardRigidBrittleHave high melting pointsDo not conduct electricity in the solid state but do conduct electricity when melted or dissolvedLattice EnergyThe energy required to separate 1 mole of an ionic solid into gaseous ionsElectrostatic Energy = (cation charge * anion charge) / (cation radius + anion radius)Covalent bond: Chemical bonds that results from a sharing of outermost electronsProperties of Covalent BondsNot Hard, Riid or brittleHave low melting pointsDo not conduct electricity in any stateStronger bonding forces holding atoms together within a moleculeWeaker intermolecular forcesComparing Ionic and Covalent BondsBoiling pointIonic: Very HighCovalent: Very LowBond strengthIonic: LowCovalent: HighMetallic Bond: Chemical bond consisting of the nuclei of metal atoms surrounded by a “sea” of shared electronsBond that exists between metallic elementsCHEM 111 1nd Edition Lecture 13 Outline of Last Lecture I. Atomic Radius TrendsII. Ionization Energya. Successive Ionization EnergiesIII. Electron Affinities Outline of Current Lecture II. Types of Chemical BondsIII. Coulomb’s LawIV. Properties of Covalent CompoundsV. Covalent Bonding and Nomenclature Current Lecture Types of Chemical Bonds: Covalent, ionic, metallic Coulomb’s Law- Force = kQ1Q2/d^2- We don’t care about the force, we care about the amount of energyo Electrostatic Energy = charge A * charge B / distanceo The Book Refers to it this way Eel = 2.31*10^-19J*nm Q1 * Q2 / d Properties of Covalent Compounds Covalent compounds are typically:Not hard, rigid or brittle (generally liquids or gasses)Have low melting pointsDo not conduct electricity in any stateStronger bonding forces holding atoms together within a moleculeWeaker intermolecular forcesThese 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.Covalent Bonding and Nomenclature (2.7, 2.8, 9.3)Types of Chemical Bonds- Ionic Bond: Chemical bond resulting from the electrostatic attraction of a cation and an aniono Properties of Ionic Compounds Ionic Compounds are typically- Hard- Rigid- Brittle- Have high melting points- Do not conduct electricity in the solid state but do conductelectricity when melted or dissolvedo Lattice Energy The energy required to separate 1 mole of an ionic solid into gaseous ions Electrostatic Energy = (cation charge * anion charge) / (cation radius + anion radius)- Covalent bond: Chemical bonds that results from a sharing of outermost electronso Properties of Covalent Bonds Not Hard, Riid or brittle Have low melting points Do not conduct electricity in any state Stronger bonding forces holding atoms together within a molecule Weaker intermolecular forces- Comparing Ionic and Covalent Bonds o Boiling point Ionic: Very High Covalent: Very Lowo Bond strength Ionic: Low Covalent: High- Metallic Bond: Chemical bond consisting of the nuclei of metal atoms surroundedby a “sea” of shared electronso Bond that exists between metallic