General Chemistry 2 Flashcards

Flashcards from General Chemistry 2 Lecture Notes

Kinetic Molecular Theory

Matter is made up of particles that are constantly moving. All particles have energy, but the energy varies depending on the temperature.

Temperature

A measure of the average kinetic energy of the particles in a substance.

Intermolecular Forces

Attractive forces between atoms/molecules that become stronger as the particles move closer together.

Solid Phase

Characterized by a small amount of kinetic energy, ordered structure, definite shape and volume, and incompressibility.

Liquid Phase

Possesses more kinetic energy than solids, lacks ordered arrangement, and does not have enough energy to escape attraction.

Ionic Bond

Transfer of electrons from one atom to another.

Covalent Bond

Sharing of electrons between atoms.

Nonpolar Covalent Bond

Equal sharing of electrons between atoms.

Polar Covalent Bond

Unequal sharing of electrons between atoms.

Ion-ion Interaction

Attractive force between ions with opposite charges; also referred to as ionic bonds.

Ion-Dipole Interaction

Attractive force between an ion and a neutral molecule with a dipole.

Hydrogen Bonding

Attraction between the hydrogen atom of one molecule and an electronegative atom (O, N, or F) of an adjacent molecule; the strongest intermolecular force.

Dipole-Dipole Interactions

Interaction where the positive end of one molecule is attracted to the negative end of another molecule.

Dispersion Forces

Caused by electron motion, creating momentary charge differences; the weakest intermolecular force.

Cohesion

Intermolecular attraction between like molecules (liquid molecules).

Adhesion

Attraction between unlike molecules (e.g., water and glass).

Surface Tension

Measure of the elastic force on the surface of a liquid.

Capillary Action

Tendency of a liquid to rise in narrow tubes or be drawn into small openings due to intermolecular attraction between the liquid and solid.

Meniscus

Curved surface of a liquid inside a container.

Viscosity

Measure of a fluid’s resistance to flow.

Vapor Pressure

The equilibrium vapor pressure is the maximum vapor pressure of a liquid at a given temperature and that it is constant at a constant temperature. It increases with temperature. Vapor pressure is independent of the amount of liquid as well as the surface area of the liquid in contact with the gas.

Molar Heat of Vaporization

The energy required to vaporize 1 mole of a liquid at a given temperature.

Crystal or Crystalline Solid

A solid material whose components are arranged in a highly ordered microscopic structure.

Electrostatic Bonding

The attraction between oppositely charged ions in a chemical compound.

Ionic Crystal

A solid made of positively and negatively charged ions held together by electrostatic forces.

Amorphous Solid

A solid that lacks long-range order and has a random arrangement of particles, similar to a supercooled liquid.

Crystal Lattice

The regular repeating three-dimensional structure in crystalline solids.

X-Ray Diffraction

Technique used to determine the atomic and molecular structure of a crystal.

Metallic Crystals

Made of atoms that readily lose electrons to form positive ions, with delocalized electrons moving around the crystal.

Ionic Crystals

Made of ions (cations and anions) that form strong electrostatic interactions within the crystal lattice.

Molecular Crystals

Made of atoms or molecules held together by a mix of hydrogen bonding/ dipole-dipole and dispersion forces.

Covalent Network Crystals

Made of atoms in which each atom is covalently bonded to its nearest neighbors.

Phase Change

Transformation of matter from one physical state to another, occurring with the addition or removal of energy.

Endothermic Processes

Phase changes that take place when heat is absorbed (heat gained).

Exothermic Processes

Phase changes that give off heat (heat lost).

Mixture

Made of 2 or more types of atoms that are NOT chemically combined together.

Solution

A homogeneous mixture that combines a solute and a solvent.

Solubility

Measure of how easily a solute will dissolve in a certain solvent.

Saturated Solution

A solution that contains the maximum amount of solute that can be dissolved into the solvent at a given temperature.

Supersaturated Solution

A solution that contains more solute than it can normally dissolve.

Molality (m)

The amount of a substance dissolved in a certain mass of solvent, measured in moles of solute per kilogram of solvent.

Molarity (M)

The amount of a substance in a certain volume of solution, measured in moles of solute per liter of solution.