Vocabulary
When deciding whether 2 liquids will mix or not to form a solution, one is looking to find its...
Miscibility
Explain the difference between intermolecular forces and intramolecular forces.
inter = between different molecules
intra = between atoms within a single molecule
What is the general rule for solubility?
Name the 4 Colligative Properties
Vapor Pressure
Boiling Point
Freezing Point
Osmotic Pressure
What are the solute and solvent called in a colloid?
Dispersed phase and dispersing medium
This compares the moles of solute with the volume of solution (mol/L)
Molarity or Molar Concentration
What is the order of the inter & intra molecular forces in order of strongest to weakest?
Ionic
Metallic
Covalent
Hydrogen Bonds
Dipole-Dipole
London Dispersion
Why do we use Molality?
Molality is NOT affected by changes in temperature and pressure while Molarity is
Name 3 characteristics of Suspensions
Heterogeneous
Settles out over time
Particles > 1 micrometer
What is the relationship between the amount of solute, osmotic pressure, and osmosis?
The more solute in the solvent, the greater the osmotic pressure, the less osmosis occurs.
When a crystal forms differently at different temperatures forming different types of lattices it is called a
Allotrope
What is the relationships between viscosity and intermolecular forces?
Stronger IMF's, the more viscous
What is different about Gas Solutions when compared to Solid and Liquid Solutions?
Gas Solutions can only have a gas as the solute and as the solvent
The more solute in the solvent, the higher the boiling point, and the lower the freezing point.
What is the relationship between vapor pressure and the amount of solute?
When solute is added to the solvent it lowers the vapor pressure
The energy necessary to overcome the intermolecular forces between the solvent particles and solute particles
Thermal Energy
Name 3 characteristics of a liquid
higher kinetic energy than solid but not higher than a gas
fixed volume
non-fixed shape
more dense than gases because they cannot compress or expand
Describe the process of ionization.
- What kind of compounds go through this?
- What is formed?
- Is it reversible or irreversible?
When covalent compounds form ions when dissolved in solution
Forms new ions by a gain/loss of electrons
Irreversible Process
What is the Tyndall Effect?
Light passes through a solution without being seen because the particles are too small to disturb the light waves.
BUT when a beam of light goes through a colloid, the beam’s outline shows up distinctly
What is an amalgam?
Solution containing mercury
This is what breaks down the surface tension of water so it can wash away the oils
Surfactant
What causes London Dispersion forces to be seen in every molecule?
Momentarily electrons can become concentrated at one end of the molecule due to surrounding molecules' charges
Results from the random, unequal dispersion of electrons between molecules
1. Solutes cannot be filtered out of a solution
2. Solutes do not settle out of a solution.
3. Solutes are uniform (homogeneous).
4. Solutions are not chemically combined.
5. Solutions can vary in their concentrations.
Will sugar in water or salt in water lower the vapor pressure more? Explain.
Sugar is a pretty non polar molecule. While water is a polar molecule. Knowing “Like dissolves like”, the sugar will not dissolve/separate in the water but stay as one molecule. Adding only one molecule will only lower the Vapor Pressure a little.
Salt is an ionic compound making it very polar. Water is also polar. Knowing “Like dissolves like”, the salt will dissolve/separate in the water. Adding many molecules will lower the Vapor Pressure a lot.
Define a solution, suspension, and colloid and explain how they are different
A solution is a homogenous mixture formed when a solute dissolves in a solvent.
Suspension is a heterogeneous mixture that could appear as homogenous for a short time until it settles out over time.
Colloid is a heterogeneous mixture that shows the Tyndall Effect
Colloid Particles > 1 micrometer (Suspension) but < 1 nanometer (Solution)