Unit 4: Solutions And Colligative Properties Flashcards
What type of change is the dissociation of NaCl to its constituent ions?
Physical Change
What are some important things to know about crystalline structures?
Repeating structure of atoms/molecules (ordered)
What are some important things to know about amorphous solids?
More random arrangement of the molecules/atoms.
What technique is used to determine the lattice structure of solids?
X-Ray Diffraction
What are solid state ionic lattices?
They are lattice structures that consist of ions; ion-ion forces are present in between the ions.
What are molecular solids?
They are solids consisted of molecules; for example, H2O has dipole dipole forces present in it.
What are covalent network solids?
Solids that are made up of a covalent network; bunch of covalent bonding going on.
What type of solid is MgCl2?
Ionic; Mg2+, 2Cl-
What type of solid is CO2?
Molecular
What type of solid is Si?
Covalent network solid
What is an example of a gas in liquid solution?
Carbonated water (CO2 in water)
What is an example of a liquid in liquid solution?
Gasoline (mixture of hydrocarbons)
What is an example of a solid in liquid solution?
Seawater (NaCl and other salts in water).
What are ion-dipole forces?
A type of attractive force that results from the electrostatic attraction between an ion and a neutral molecule that has a dipole. This force is present in between the water molecules and solvated ions.
What happens to the potential energy when the ionic lattice breaks apart?
Increases
When is DeltaH solution positive and when is it negative?
It is negative is the solvent-solute reactions are dominant.
It is POSITIVE when the solvent-solute reactions are NOT DOMINANT.
What are the soluble compounds? What are the exceptions?
Compounds containing the alkali metal ions and the ammonium ion- Nitrates (NO3-)- Bicarbonates (HCO3-), and Chlorate (ClO3-)-Halides-Sulfates NB-CSH
EXCEPTIONS are halides of Ag+, (Hg2)2+, and Pb2+
Sulfates of Ag+,Ca2+,Sr2+,Ba2+,Hg2+, and Pb2+
What are the insoluble compounds are what the exceptions?
Carbonates (CO3)2-, phosphates (PO4)3-, chromates (CrO4)2-, and Sulfides (S)2-, Hydroxides (OH-) CP-CSH
EXCEPTIONS are the compounds containing the alkali metal ions and the ammonium ion. Compounds containing the alkali metal ions and the Ba2+ ion.
What does “like-dissolves-like” mean?
Polar dissolves polar/ionic; non-polar dissolves non polar. Hydrophilic solutes dissolve in water and hydrophobic solitudes dissolve in hydrophobic solvents.
Do non-polar solvents have strong or weak IMFs?
Weak IMFs.
In reactions involving non-polar solvents dissolving non-polar solutes, how is the energy being driven?
It is driven by entropy, not the IMFs; more entropy is favorable.
What do aggregate hydrophobic regions do?
They push H2O into the solution (the higher the entropy, the more H-bond formation).
What generally happens to solubility when the temperature is increased?
When there is an increase in temperature, there is an increase in kinetic energy; the ions and particles interact more readily and we can increase the # of solute particles that reduce lattice energy.
What happens to the solubility of gases when the temperature of the solution is increased? T
There is a decrease in solubility; increase in temperature leads to an increase in kinetic energy. The expansion of gases makes it harder for IMFs to take place.
