Lecture 2 Flashcards
Valence Electrons
Electrons that form bonds. Carbon has 4
VSEPR
Used to predict the shape of a molecule
Orbitals
s and p. different energy levels determine what it is
Strong Bonds
Covalent and polar covalent
Covalent Bonds
Sharing of electrons
Polar Covalent Bonds
Unequal sharing around the atom. Range .5-1.6
Electronegativity
Ability of an atom to attract electrons toward itself in a covalent bond
Weak Bonds
Ionic Bonds, Hydrogen Bonds, van der Waals interactions
van der Waals interactions
A attraction cause by a temporary change in the electrons dipole
Hydrophobic effect
Nonpolar molecules are pushed together by water. They stick together to avoid the water.
Induced dipole
The dipole changed to form a bond
Dipole moment
The distance of separation between charges
Cohesion
Water molecules sticking to each other
Heat Capacity
Specific amount of heat needed to change the temperature of a substance
Amphipathic
Molecule has a hydrophobic and hydrophilic end
Water of hydration
Water hydrates its self. Hardly ever happens. 1:555000000. Makes H3O and HO and H3O isnt stable
Micelle
Ball of hydrophilic heads on the outside and hydrophobic tails on the inside
Membrane
An enclosing or separating amphipathic layer that acts as a barrier within or around a cell
Acid
Chemical compound that, when dissolved in water, gives a solution with a hydrogen ion activity greater than in pure water; pH < 7
pH; pOH
-log[H+] = -log[H3O+]; lower the pH the more the [H+]; Concentration of H+ and OH- in a solution; -log[H+] or -log [OH-]; pH + p[OH]=14
Base
Aqueous substance that accepts protons; pH > 7
Neutral
When the concentration of hydronium ions and hydroxide ions are equivalent; pH = 7
