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)