General Chemistry Flashcards
explain the properties of liquids in terms of the intermolecular forces of attraction and the kinetic energy of the individual particles
Kinetic Molecular Model
Internal kinetic energy of matter makes its particles vibrate and wobble
The particles of matter are in constant motion
Since temperature is the measurement of the internal kinetic energy of matter, a hotter object will have faster moving particles than a older piece of the same matter
Temperature of the matter is proportional to the kinetic energy of the particles
The particles in a matter are not actually in contact with one another, even atoms in a chemical bond. The spaces between the particles allow them to vibrate and wiggle, and even slide over when deformed in the case of solids
Particles have spaces between them
Intermolecular forces of attraction/repulsion get stronger the closer the particles are
The strength of intermolecular forces of attraction is inversely proportional to the distances between particles
At any given moment, the electron of an atom may be asymmetrically distributed around the nucleus. This will create a temporary dispose in the particle
Adjacent atoms will have their electron react to the dipole
London dispersion forces
In a matter with polar molecules, the partially positive pole of a mole will be attracted to the partially negative pole of other polar molecules
Dipole-dipole forces
An especially strong type of dipole-dipole forces where molecules containing a hydrogen bonded with a highly electronegative atom creates strong dipoles
Hydrogen bond
Strongest type of intermolecular forces of attraction, A side of a polar molecule is attracted to the opposite charged ions in the mixture
Ion-dipole forces
Intermolecular forces give rise to a number of structural features and properties of liquids
Liquids
Beneath the surface of the liquid, a particle will experience attractive forces from other particles in all directions. All the pulling force equalize and result into a net force of 0
-However, particles on the surface do not have adjacent particles above them, causing unbalanced forces
Surface tension
amount of energy required to stretch or increase the surface of a liquid by a unit area
Surface tension
viscous liquids have strong intermolecular attractions with in its particles
Viscosity
spontaneous flow of a liquid into a narrow tube or porous material
Capillary action
between like molecules
Cohesion
between unlike molecules
Adhesion
partial pressure when the liquid is at equilibrium
Vapor pressure
temperature where the vapor pressure of the liquid is equal to the atmospheric pressure
Boiling point
during this transition, the temperature remains the same until the material has fully changed its phase
Molar heat of vaporization
Water molecule has a bent shape, with two partially positive hydrogen atoms and a partially negative oxygen atom. These dipoles make the overall molecule polar
Structure of water
Colorless, odorless, and tasteless liquid
Water
Solid form at 0 degree celsius and 1 atm
Water molecules can form rings or chains because of intermolecular forces
Highly ordered hree-dimensional structure of ice prevents the molecules from getting too close to one another
Low density of ice is contributed to the larger space occupied by this arrangement
Ice
distinct form in which matter can exist
Phase
transformations from one phase to another, occur when energy is added or removed from a substance
Phase change
homogeneous mixture of two or more substances
Solution
substance dissolves in a solution and is usually present in smaller amount
Solute
dissolving medium
Solute+solvent= solution
Solvent
maximum amount of solute that can dissolve in a given amount of solvent at specified temperature
Solubility
amount of solute present in a given amount of solution
Concentration
number of moles of solute per liter of solution
Molarity
number of moles of solute per kilogram of solvent
Molality
