General Chemistry 2 Reviewer (Set 1)

• Kinetic Molecular Theory - states that the particles in a gas are constantly moving and that the particles are constantly colliding with each other
• Intermolecular Forces - are attractive forces holding the particles of substances together.
• INTRAMOLECULAR FORCES VS INTERMOLECULAR FORCES

  Intramolecular forces are the forces that hold atoms together WITHIN a molecule. Intermolecular forces are forces that exist BETWEEN molecules.
• TYPES OF INTRAMOLECULAR FORCES

  • Ionic Bond
  • Covalent Bond
  • Metallic Bond
• IONIC BOND


  This bond is formed by the complete transfer of valence

  electron(s) between atoms.
• What is Covalent Bond?

  This bond is formed between atoms that have similar

  electronegativities—the affinity or desire for electrons. They share electrons.
• Two Types of Covalent Bond

  1. Polar Covalent Bond
  2. Nonpolar Covalent Bond
• What is polar covalent bond?

  Unequal sharing of electrons.
• What is nonpolar covalent bond?

  Equal sharing
• METALLIC BOND


  This type of covalent bonding specifically occurs between atoms of metals, electron sea.
• Types of Intermolecular Forces

  • London dispersion forces (LDF)
  • Dipole-dipole interactions
  • Hydrogen Bonding
• London Dispersion Forces - result from the coulombic interactions between instantaneous dipoles.
• Dipole-dipole interactions - forces of attraction between polar molecules.
• Hydrogen Bonding - weak intermolecular forces between hydrogen and other atoms.
• Van der Waals Force - weak intermolecular forces between molecules that are not covalent bonds.
• Solution - expressed through concentration which

  may be qualitatively or quantitatively.
• Solubility - ability of a substance to dissolve a solvent to form a homogeneous solution
• Solutions - a mixture of two or more substances in which the substances are dissolved in each other.
• Solutions are composed of a solute and a solvent. The solute is the substance that is dissolved in the solvent.
• Factors Affection Solubility

  1. Nature of solute and solvent
  2. Temperature
  3. Pressure
• Colligative Properties of Solutions - The properties of a solution that depend on the number of particles in the solution.
• Three categories of solute properties:

  1. Colligative properties are properties that only depend on solute concentration and temperature. They are independent of the nature of the solute particles.
  2. Additive properties are the sum of the properties of constituent particles and depend on solute chemical composition. Mass is an example of an additive property.
  3. Constitutional properties depend on the molecular structure of a solute.
• Four Colligative Properties of Solution

  1. A lowering of the vapor pressure
  2. A lowering of the freezing point
  3. An elevation in the boiling point
  4. The development of an osmotic pressure
• Who introduced the concept of colligative properties?

  Friedrich Wilhelm Ostwald
• Where does the word "colligative" comes?

  Latin word colligatus (bound together)