Water (H2O)
% solution
(volume of solute/volume of solution) x 100 ***can also be mass
VSEPR Theory
Bent shape
Liquid water
Random, any shape
Deliquescent compounds
Remove enough water from moist air to become a dissolved solution
Hygroscopic hydrate
Remove water from moist air
Line on graph
Represents saturated solution
Henry's Law
S1P2=S2P1
Ice
Uniform, hexagonal shape
Water of hydration
Water in a crystal that is integral part of crystal structure
What does "•5H2O" mean when included in a chemical formula?
Compound contains 5 H2O molecules/formula unit
Hydrate
Compound itself
Electrolytes
Compound that conducts electric current when dissolved
Surfactant
Compound that prevents hydrogen bonding
Polar solvents
Dissolve ionic /polar compounds
Nonpolar solvents
Dissolve nonpolar compounds
Solvent
Dissolving medium
When a suspension of clay particles in water is filtered out, both clay and water will pass through the filter paper(T/F)
False; only for solutions
Suspension
Heterogeneous mixture in which particles settle out upon standing
Solution
Homogeneous mixture of particles in a dissolving medium
Effloresce
Hydrate that has vapor pressure greater than that of water in surrounding air (hydrate will lose water to air)
Desicant
Hygroscopic substances that remove water from air used as drying agents
Mole fraction
Mol fraction= mol of solute/mol of solution
Most important unit of concentration in chemistry
Molarity
Structure
•H2O •dihydrogen monoxide •covalent •held together by sharing e-
Properties of H2O
•high surface tension •low vapor pressure •high boiling point •solid H2O has lower density than liquid H2O
Hydrogen bonds
Attractive force between S+ H from one molecule to a S- atom of another molecule
Dilution equation
M1V1=M2V2 (can be any)
Molarity equation
M=n(solute)/v(solution)
Saturated solution
Maximum amount of solute for a given quantity of solvent at a constant temperature
Concentration [ ]
Measure of the amount of SOLUTE dissolved in a given quantity of SOLVENT
Solute
Substance being dissolved
Tyndall effect
scattering of light in all directions by colloidal particles
3 factors that influence the rate at which a solute dissolves
1. agitation 2. temperature 3. particle size
Solubility
Amount of a substance that dissolves in a given quantity of solvent at a constant temperature
What would happen if solution was filtered?
Both solute and solvent will pass through the filter paper
Insoluble
Compounds that cannot be dissolved *occus because internal bonds are so much stronger
Colloid
Heterogeneous mixture in which particles are of intermediate size between those of true solutions and suspensions
Solvation
Polar sides of water are attracted and pull apart ions from the crystal
All ionic compounds are electrolytes(T/F)
True
Finely ground particles dissolve more rapidly that larger particles because finer particles expose a greater surface area to the colliding solvent molecules(T/F)
True
Heterogeneous mixtures are not true solutions(T/F)
True
Attractions between ions in crystals of ionic compounds [(BaSO4) and (CaCO3)] are stronger than attractions between ions and water molecules(T/F)
True; because they are nearly insoluble
Miscible
Two liquids that dissolve each other
Aqueous solution
Water that contains dissolved substance
Why is ice less dense than liquid water?
When ice melts, the hexagonal framework collapses and water molecules pack closer together making it more dense
How does solubility of a gas change with an increase in temperature?
increase in temperature, decrease in solubility (inverse)
Relationship between pressure/solubility
increase pressure, increase solubility (direct)
molality
m=n(solute)/kg(SOLVENT)
Molecular polarity
•oxygen side(slightly negative) •hydrogen side(slightly positive) ***more than one H2O atom
Bond polarity
•oxygen(slightly negative) •hydrogen(slightly positive)