Review Sheet for Principles Of Chemistry I: Principles of Chemistry I | CHEM 1307, Study notes of Chemistry

Download Review Sheet for Principles Of Chemistry I: Principles of Chemistry I | CHEM 1307 and more Study notes Chemistry in PDF only on Docsity! Chem 1307 – Spring 2008 Review for Chapter 9, 11-13 Coverage Chapter 9 Sections 9.2 – 9.4, 9.6 Chapter 11 Sections 11.1 – 11.3 Chapter 12 Sections 12.1, and 12.3 Chapter 13 Sections 13.1, 13.3 except entropy, 13.4 – 13.6 Terms that you should know: Chapter 9 ionic bonding covalent bonding metallic bonding lattice energy Born – Haber cycle covalent bond bonding (shared) pair lone (unshared) pair bond order single bond double bond triple bond bond energy bond length electron “sea” model Chapter 11 valence bond (VB) theory hybridization hybrid orbital (HO) sigma (σ) bond pi (π) bond molecular orbital (MO) theory molecular orbital (MO) bonding MO antibonding MO sigma (σ) MOs pi (π) MOs MO bond order MO diagram homonuclear diatomic molecule heteronuclear diatomic molecule nonbonding MO Chapter 12 phase intermolecular forces intramolecular forces condensation/vaporization freezing/melting sublimation van der Waals radius ion-dipole forces dipole-dipole forces hydrogen bond (H-bond) polarizability dispersion (London) forces Chapter 13 solute solvent solution solubility saturated solution unsaturated solution supersaturated solution miscible heat of solution heat of salvation heat of hydration molarity molality mass percent mole fraction Henry’s Law Raoult’s Law vapor pressure lowering freezing point depression boiling point elevation molal freezing point depression constant (Kf) molal boiling point elevation constant (Kb) osmosis osmotic pressure colligative property Concepts that you should understand and skills to master: Chapter 9 Distinguish three types of bonding with respect of bonding elements, electron sharing, bond restriction, and formula; Describe essential features of ionic bonding: electron transfer to form ions, and their electrostatic attraction to form a solid via ionic lattice energy, and how lattice energy is responsible for the properties of ionic compounds; Use bond order to describe three types of covalent bonds, use bond energy to calculate standard enthalpy change (heat) of a reaction; understand the interrelationship among bond order, bond length, and bond energy; Use electron “sea” model to explain major properties of metal. Chapter 11 Understand the main idea of VB theory ⎯ orbital overlap, opposing electron spin, and hybridization Know the relationship between the electron group and hybridization of the central atom, and use molecular shape and electron group arrangement to postulate the hybrid orbitals used by central atom. Describe two modes of overlap that leads to sigma and pi bonds, and how these bonds constitute the single, double and triple bonds. Explain why π bonding restricts rotation around double bonds Distinguish the degree of delocalization of bonding orbitals between VB and MO theories Describe the types and shapes of MOs (bonding and antibonding) formed from combinations of two s and two p orbitals, and bonds in a molecule. Be able to draw MO diagram, to calculate the bond order, to determine the stability of molecular species and to explain properties of diatomic molecules, especially the magnetic property. Chapter 12 Use kinetic-molecular theory to explain the three states of matter with their difference in kinetic energy and potential energy of particles. Distinguish the intramolecular force and intermolecular forces, and their results in forming covalent solids Describe and predict the types and relative strength of intermolecular forces acting in a substance (dipole-dipole, H-bonding, dispersion), the impact of H- bonding on physical properties. Determine whether a substance can form H- bonds. Know the meanings of van der Waals radius of an atom and polarizability of a molecule and be able to rank the van der Waals radius and polarizability among atoms or molecules. Chapter 13 Describe the process of dissolving a solute in a solvent. Understand and distinguish the forces between solute and solvent particles in various solutions. Determine whether a substance is more easily soluble towards a certain solvent.