chem 106 quiz 2 Flashcards
types of crystalline solids
molecular, ionic, atomic, network
molecular solids examples
H2O, CO2
ionic solids example
NaCl
atomic solids examples
metals; Ar(s)
network solids examples
diamond, graphite
the melting point of ionic solids is (less than/equal to/greater than) molecular solids
greater than (b/c ionic bonds over IMFs)
example of liquid solution with liquid solvent and gas solute
CO2(g) in H2O(l)
example of liquid solution with liquid solvent and solid solute
NaCl(s) in H2O(l)
example of liquid solution with liquid solvent and liquid solute
ethanol(l) in H2O(l)
example of solid solution with solid solvent and solid solute
Iron(s) in Carbon(s) (steel)
example of solid solution with solid solvent and liquid solute
Mercury(l) in Silver(s) (amalgam)
example of solid solution with solid solvent and gas solute
H2(g) in Pd(s)
what are the catalyst metals?
Ni, Pd, Pt
solution form when
the attractive forces between solvent and solute are greater than the interactions between the solute and itself; “like dissolves like”
oil and water do not mix because
oil is nonpolar and water is polar
the ΔHsolution =
ΔHsolute + ΔHsolvent + ΔHmixture
in the equation ΔHsolution = ΔHsolute + ΔHsolvent + ΔHmixture, what are the signs on each?
-, +, +, -
Henry’s Law
Solubility,gas = k * P,gas
solubility and pressure are (directly/inversely) related
directly
Henry’s constant, k, has to do with
solubility and intermolecular forces (units will be solubility/pressure)
Henry’s constant and solubility are (directly/inversely) related
directly
polarizability
ability to form instantaneous dipoles
why is CO2 soluble in H2O since it’s nonpolar?
it has a high polarizability
polarizability increases with
size
why do scuba divers have to pace themselves upon ascending?
N2 tries to bubble out of blood - too much in system because need more at higher pressure/the lower you go
mass percent equation
mass solute / total mass
parts per million equation
mass component / mass solution x 10^6
or mg/kg
mole fraction
moles solute / total moles
molarity
moles solute / volume solution
molality
moles solute / mass solvent
for a really concentrated solution, (molarity/molality) increases faster
molality
temperature affects (molarity/molality)
molarity
adding a solute to a solvent (lowers/raises) the vapor pressure of the solvent & why
lowers; the solute is blocking the vaporization (?)
P,A = ?
(X,A)(P*,A) (mole fraction times vapor pressure of pure substance)
vapor pressure of the solution decreases with (decreasing/increasing) mole fraction
decreasing
lower vapor pressure leads to a (lower/higher) boiling point
lower
alcohol by weight
g solute/g solvent ?
