EXTRA CHEM

E=hf

L=nh/2pi

E=hc/wavelength

no two electrons can have the same set of quantum numbers

n

n-1

2n^2

-l to l

filling from lower to higher subshells

within a given subshell, oribital sare filled such that there are a max number of half filled orbitals with parallel spins

materials composed of atoms with unpaired electrons will orient their spins in alignment with a magnetic field, and the material will thus be weakly attracted to the magnetic field

materials consisting of atoms that have all paired electrons will be slightly repelled by a magnetic field

• measure of the net positive charge experienced by the outermost electrons
• (increases from left to right)

1/2 the distance between the centers of two atoms of an element that are briefly in contact with one another

decreases from left to right

distance from center of the nucleus to edge of its electron cloud

energy required to remove an electron from a gaseous species

increases from left to right and from bottom to top

energy distance by a gaseous species when it gains an electron

increases from left to right and decreases from top to bottom

inverse

longest are weakest (single)

shortest are strongest (triple)

measure of concentration of [H] or [OH[

metathesis

ClO-

ClO2-

k=Ae^(-Ea/RT)

• Ea is the activation energy
• R is the ideal gas constant

energy given off

energy absorbed

k=-slope 

linear line going down

curved line downward

the ln is a straight line where k=-slope

large curved line down

ln graph is a straight line going up where k=slope

concentration of products over the concentration over reactants

Keq or Kc

Kf/Kr

k forward / k reverse

there is a greater concentraiton of reactants; the forward reaction will proceed

reaction in equilibrium

there are more products; the reaction is reverse

only gaseous species are affected

increase in pressure causes a decrease in the moles of gas; shift away

NH3

product formed at higher temperatures

no exchange of heat, work, nor matter

can exchange energy (heat and work) but no matter

contant temperature

internal energy is zero; Q=W

no heat is exchanged between the system and its environment

dU= -W

pressure is constant

pressure is constant; nothing changes because volume is the same

no change in volume= no work 

dU=Q

describe pathway taken from one equilibrium state to another

Work and Heat (W and Q)

• 1 atm
• 273 K

• 298 K
• 1 atm
• 1 M

tempearture at which the vapor pressure is equal to the atmospheric pressur

as temp increases, so too does VP

deposition

heat under constant pressure

q=mL, 

where L is the latent heat to describe the isothermal process; Latent heat is another term for enthalpy

q=mcdT

dHrxn= Hproducts- Hreactants

enthalpy changes are additive

endothermic

dH(rxn)= H(bonds broken)-(bonds formed)

dS=Q(rev)/T

Qrev= heat gained or lost in a reversible reaction

+ dH and + dS is spontaneous at high T

- dH and - dH is nonspontanoues at all T

- dH and + dS is spontaneous at all T

- dH and - dS is spontaneous at low T

-RT lnKeq

dGrxn= dG^orxn + RTlnQ=RTln(Q/Keq)

N1/V1= n2/V2

PV=PV

V/T= V/T

P/T=P/T

[A]/P=[A]/P

1/2mv^2=3/2kbT 

kb is boltzmann constant

Urms=(3RT/M)^.5

Deviations due to pressure (as pressure increases the size of the particles is larger and they take up volume)

deviations due due to temperature (intermolecular attractions cause gas to have smaller volume)

moles of solute/ kg of solvent

Ksp=[A][B]

no solids or liquids in the equation; and there is no denominator

increasing temperature for non-gas solutes

decreases for gas solutes

higher pressures favor dissolution of gas solutes

same as Ksp but at a given time

IP < Ksp: solutes continue to dissolve

IP= Ksp: solution saturated and at equilibrium

IP > Ksp: precipitation occurs

xT=ikm

where i is the van't Hoff factor; kb is proportionality constant, and m is molality

II=iMRT

-log[H+]

-log(n*10^-m)=-log(n)-log(10^-m)=m-log(n)

p value=m-0.n

7

very low 

very basic

(steepest slope)

• -above 7
• - low
• - basic

- less than 7

aka: dismutation

specific type of redox in which an element undergoes both oxidation and reduction in producing its products

anode is site of oxidation

reduction occurs at the cathode

cathode to anode

connecting two solutions is a salt bridge

charge begins to flow

redox is spontaneous

A--> C

anode|anode solution || cathode solution | cathode

= phase boundary

= salt bridge

nonspontaneous and require input of energy

mol M= It/nF

ex: Calculating moles of Metal, It is not Fun

anode of galvanic cell is considered negative; cathode is considered positive (electrons move from negative to positive, while current is from positive to negative)

anode of an electrolytic cell is positive because it is attached to external voltage; cathode is negative

the more positive reduction potential is the one that is oxidized

Ecell= Ecathode-Eanode

dG=-nFE

used for determining cell's emf under situations taht deviate from standard

Ecell=Ecell(under standard conditions)- (RT)/(nF) lnQ