Chem Solutions Quiz

Water

Polar atom of 2H and 1 O that is symetrical and a polar atom

Structure of water

2 H and 1 O (mouse ears)

Unusual properties of water

Because of cohesion and adhesion and the unique structire of H2o it is able to both cohere and adhere

polarity

distribution of charge within a molecule

polar molecules attract

strong intermolecular force

A molecule is considered polar if it has a positive and negative end creating a dipole

cohesion

ability for molecules to stick to themselves

caused by a difference in charge

adhesion

ability for molecules to stick to or attract to other particles

hydration

water molecules interacting with and surrounding molecules while dissolving in water

solute

a substance that GETS disolved

solvent

the substance that DOES the disolving

solution

a combination of a solute and solvent

solvation

the interaction between solvent molecules and solute particles

“Like disolves like”

water is the universal solvent

polar dissolves polar

Intramolecular force

forces within the molecule

Intermolecular force

forces between molecules

Effect of IMF on Boiling and melting point

Stronger IMF—> more energy required to melt a solid or boil a loquid

Effect of IMF on viscosuty

strongest IMF’s are in the most viscous substances (tar molecules are extremely strong)

Hydrogen bonding

Hbonds are FON

the attraction between molecules and a Hydrogen atom of a different molecule

ion-Dipole force

exists between an ionic compound in water so water and ionic molecules only

London Dispersion Force (LDF)

exists between all molecules

temporary attractive force while in motion that forms temporary nonpolar dipoles

only force present when nonpolar

bigger molecule=stronger ldf

balanced LDD=nonpolar and LDF

Dipole Dipole force

2polar 2polar

polar molecules present without hbond

Rate of solvation

How fast something disolves

stirring, temperature, and particle size all effect the rate of solvation

Solubility

The amount of solute that can disolve ina given amount of solvent at a given temperature

Pressure effect on solubility

P has no effect on solids

P increases as solubility increases in gasses

Temperature effect on solubility

Solids solubility increases with temperature

gas solubility decreases while temperature increases

Saturated

solutions contain the max amount of solute at a given temp

Unsaturated

solutions contain less than the max amount of solute at a given temp

Supersaturated (and process)

contains more solute that can be disolved at a given temp

Supersaturated process)

the process of created a supersaturated solution means that the excess solute must be disolved at a high temp then allowed to cool without percipitating the solute