General Chemistry 2 PDF - Intermolecular Forces, Solutions & Properties

Okay, here is the text from the images, formatted as markdown: ## GENERAL CHEMISTRY 2 12-STEM 18 2ND SEMESTER [3RD QUARTER] - AARON MARCUS DE LEON ### TOPIC OVERVIEW **A. INTERMOLECULAR FORCES OF ATTRACTION** i. Properties of Solutions ii. The Solution Process iii. Effect of Intermolecular Forces...

Okay, here is the text from the images, formatted as markdown: ## GENERAL CHEMISTRY 2 12-STEM 18 2ND SEMESTER [3RD QUARTER] - AARON MARCUS DE LEON ### TOPIC OVERVIEW **A. INTERMOLECULAR FORCES OF ATTRACTION** i. Properties of Solutions ii. The Solution Process iii. Effect of Intermolecular Forces on Solution Formation iv. Types of Solutions and Solubility v. Factors affecting Solubility vi. Ways of Expressing Concentration vii. Concentration Units **B. DILUTION AND COLLIGATION PROPERTIES** ### PROPERTIES OF SOLUTIONS | INTRAMOLECULAR | INTERMOLECULAR | | :------------------------------------------------------------------------------ | :----------------------------------------------------------------------------------------------------------- | | Holds atoms in a molecule Stronger Covalent, ionic, and metal bonds | Holds molecule in a substance Weaker Attractive forces Ion-dipole, dipole-dipole, hydrogen bonding, london dispersion | | | Note: Opposite attracts | | *Covalent:* electrons are shared *Ionic:* electrons are transferred | | ### REVIEW **POLAR MOLECULE** * Unequalized sharing of electrons * It is due to the electronegativity * If there are lone pairs in the central atom, the molecule is considered polar. **NONPOLAR MOLECULE** * Equal sharing of electrons * Examples are methane and carbon dioxide * Observe Octet Rule * If there are no dots in the central atom, it is considered nonpolar. **ELECTRONEGATIVITY** * Partial negative = partial positive * O H B, C, N, O, F * F, O, N * Ion-dipole and dipole-dipole * Hydrogen bonding and PAGE 1 DE LEON - GENERAL CHEMISTRY 2 ## GENERAL CHEMISTRY 2 12-STEM 18 2ND SEMESTER [3RD QUARTER] - AARON MARCUS DE LEON london dispersion ### A.1 TYPES OF INTERMOLECULAR FORCES **A. Ion-Dipole** * Attraction between ion and polar molecules * The strongest one * Molecules involved in attractions * Dipole: Polar Molecules **B. Dipole-Dipole** * Attraction between polar molecules * Weaker than ion-dipole * Ion-dipole attractions are stronger because they involve the interaction of a full ionic charge with a partial charge, resulting in a greater force PAGE 2 DE LEON - GENERAL CHEMISTRY 2 **C. Hydrogen Bonding** * A special dipole-dipole interaction between hydrogen and an electronegative F, O, N atom * Magnitude of the attraction is directly proportional. * Hydrogen bonding is stronger than ordinary dipole-dipole molecule * Hydrogen bond if formed between highly electroneagtive atoms and hydrogen **D. London Dispersion** * "Weaker" * It exists in polar and nonpolar molecules because they do not necessitate dipoles * LDF are transient * Temporary attraction between nonpolar molecules * Dominant * They are the only intermolecular force present. * While other intermolecular forces are stronger, they only exist in molecules with permanent dipoles or specific hydrogen bonding capabilities. * Clue: tambay lang. Nawawala at pabalik balik paminsan-minsan. ### A.2 THE SOLUTION PROCESS **Solution** In Chemistry, the term "solution" is a homogeneous mixture * **Homogeneous:** uniform, similar * Consists of solute and solvent * Solute: smallest amount * Solvent: largest amount * Examples: salt water * Solute is $NaCl$ * Solvent: water PAGE 3 DE LEON - GENERAL CHEMISTRY 2 **QI How/Why do Solutions form?** The ability of substances to form solutions depends on two factors: * The natural tendency of substances to mix and spread into larger volumes when not restrained in some way * The types of intermolecular interactions involve in the solution process * For gases or gas solutions: