15.1 - Water and its Properties
pole creates a sigma bond
triatomic molecule
bond angle of 105 degrees
high surface tension and low vapor pressure result from Hydrogen bonding
surface tension - inward force, or pull, that tends to minimize the surface area of a liquid
Water’s surface tension is higher than most — tends to hold drop of liquid in spherical shape
surfactant - any substance that interferes with H bonding
lowers surface tension
causes a bead of water to spread out
EX soaps and detergents
WATER IN THE SOLID STATE
ice cubes float in water bc solid water has a lower density than liquid water
the structure of ice is a regular open framework of water molecules arranged like a honeycomb — when it melts the structure collapses and the molecules are closer together
this is opposite for other liquids
most solids become denser and sink
ice is one of the only few solids that floats in its own liquid
MAX density of water - 1g/cm³ @ 4 degrees C
MIN density of water - 0.9168g/cm³ @ 0 degrees C
Ice melting at 0 degrees C is a high melting temp for a molecule with such low molar mass
The heat absorbed when 1g of water change from a solid to a liquid is 334J — same amt of energy is needed raise the temp of 1g of water from 0 degrees C to 80 degrees C
15.2 - Homogeneous Aqueous Systems
aqueous solution - water that contains dissolved substances
solute - what’s being dissolved
solvent - what’s doing the dissolving
water is a universal solvent for biological systems
homogenous
mixtures
can be separated but hard to do so
equally distributed
can’t be filtered by filter paper because the particles are so small
ionic compounds and polar covalent bonds dissolves most readily in water
non polar covalent bonds (methane, oil, grease, gas) cannot be dissolved by water but can be by alcohol, chloroform, and ether
“like dissolves like”
non polar solute and a non polar solvent
polar solute and polar solvent
solvation - process by which the positive and negative ions of an ionic solid become surrounded by solvent molecules
electrolytes - compound that conducts and electric current when it is in an aqueous solution or in molten state
EX HCl
all ionic compounds are electrolytes bc they dissociate into ions
non electrolytes
EX carbon, sugar, rubbing alcohol
strong electrolyte - solution in which a large portion of the solute exerts as ions
EX most soluble salts, inorganic acids, inorganic bases
weak electrolyte - conducts electricity poorly bc only a fraction of the solute in the solution exists as ions
EX ammonia, organic acids, organic bases
hydrate - a compound that contains water or hydration
when writing the formula — use a dot to connect the formula of the compound and the number of water molecules per formula unit
water of hydration and water of crystallization are contained in a crystal
efflorescent hydrate - if the hydrate vapor pressure is greater than the pressure of water vapor then the hydrate will lose its water of hydration
hygroscopic hydrate - low vapor pressure removes water from moist air
desicant - substance used to absorb moisture from the air to create a dry atmosphere
%water = mass of water/mass of hydrate x 100%
15.3 - heterogeneous aqueous systems
suspensions - a heterogeneous mixture from which particles settle out upon standing
EX blood, oj, milk, cream, salad dressing
colloid - a heterogenous mixture that contains particles that range in size from 1nm to 1000nm and can be any state of matter
EX smoke, paint, aerosol spray, fog/mist
solution particles < colloid particles < suspension particles
Tyndall effect - scattering of light due to colloid particles — a solution’s particles are too small to scatter light
Brownian movement - chaotic movement of colloidal particles which was first observed by Scottish botanist Robert Brown
coagulation - dumping of particles together in a colloid that fall out of a solution
emulsion - colloidal dispersion of a liquid in a liquid