Unit 4 Flashcards
What are London Dispersion forces and what are they present in
Very weak and temporary; found in everything
What is the relationship between IMF and KE
disproportinal. High IMF is low KE
When do dipole-dipole interactions occur
Between polar and nonpolar molecules (partial negative and partial positive)
When do H bonds occur and what are they
Very strong dipole-dipole interaction that occurs due to a very polar bond. Occurs between H and N, O, or F
What are ion-dipole interactions
occur when the partial positive or negative region of a polar molecule is attracted to an ion of hte opposite sign
What is the order of IMFs from weakest to strongest
London Dispersion, dipole-dipole, H bonds, ion-ion, and ion dipole bonds
What is viscosity
Resistance to flow
What are the three things that Viscosity depends on
IMFs, size/ shape of molecules, and temperature
What are cohesive forces
IMFs between identical molecules (Ie. water to water)
What is surface tension
E required to increase surface area of a liquid
What are adhesive forces
IMFs between different molecules
Are adhesive or cohesive forces stronger
Adhesive
What is vapor pressure and its symbol
The pressure above a liquid at equilibirum in a closed system and vap sub P
What does vapor pressure depend on and what are the relationships
Disproportional to IMF strength and proportional to temperature
What is boiling point
T at which a liquid’s vapor pressure is equal to atmospheric pressure
What is the relationship between vapor pressure and boiling point
disproportional
What is enthalpy of vaporization and its symbol
Heat necessary to vaporize one mole of liquid and Vap sub delta H
What is enthalpy of fusion and its symbol
E needed to melt one mole of stuff and fus sub delta H
Enthalpy of fusion is always slighlty smaller of bigger than enthalpy of vaporization
Smaller
What is sublimation
solid to gas
What is deposition
gas to solid
What is the triple point
Point where all three phases exist
What is the critical point
Point where liquid/gas boundry no longer exists
Why is the phase diagram of water different from others and how is it different
Because water is heavier than ice is thus, it has a negative slope for the liquid/solid boundary
What is an ionic crystalline solid
forms crystal lattice only between metals and nonmetals
What is a metallic crystalline solid
“sea of electrons” between metals only
What is a molecular crystalline solid
forms only between nonmetals
What is a covalent network crystalline
atomic solids only
What is the relationship between temperature and solubility of gases
Increase in temperature causes a decrease in solubility
What are miscible liquids
liquids that are soluble in each other at all concentrations
What are immiscible liquids
Liquids that are not soluble in each other
What is the relationship between temperature and solubility of solids
Decrease in temperature causes a decrease in solubility
What is osmotic pressure and its symbol
pressure that a solution can exert and its symbol is small pi
What is equilibrium
State where the concentration of reactants and products is constant
What happens when the equilibrium constant is one
Reaction favors neither side
What happens when the equilibrium constant is greater than one
The reaction favors products
What happens when the equilibrium constant is less than one
Reaction favors reactants
What does the equilibrium constant depend on
temperature
What is the reaction quotient and its symbol
Way to determine if a system is at equilibrium or not and Q
What is the equilibrium constant and its symbols
Describes concentrations of a system at equilibrium and K sub eq K sub C or K
If Q is bigger than K what happens
There are too many reactants so system shifts right
If Q is smaller than K what happens
There are too many products so system shifts left
What is le Chatelier’s principle
if a system is perturbed at equilibrium, it returns to equilibrium by counteracting perturbation
When at equilibrium and K > 1 what is Gibb’s free energy?
Negative thus, spontaneous
When at equilibrium and K = 1 what is Gibb’s free energy?
Zero
When at equilibrium and K < 1 what is Gibb’s free energy?
Postive thus, non spontaneous
When are Kc and Kp equal
When there are an equal number of moles of gas on both sides
When gases are in standard states, what is their pressure
1 atm
What is the london dispersion trend?
Increases as electrons increase
What is the relationship between boiling point and IMF
Proportional
What is the relationship between viscosity and IMF
Proportional
What is the relationship between surface tension and IMF
proportional
What is the relationship between pressure and solubility of a gas
Proportional
