Exam 2

force/area

pressure

at constant t and n…p and v=inversely proportional

P1V1=P2V2

boyles law

at constant p and n… v and t=proportional

V1/T1=V2/T2

Charles Law

at constant P and T…V and n=proppertional

V1/n1=V2/n2

Avogadros Law

at constant v and n…P and T=proportional

P1/T1=P2/T2

Amontons law/ gay-lussacs law

0 degrees celcius

22.4 L/mol

STP

volume/ moles (L/mol)

molar volume

PV=nRT

ideal gas law

.08206 L*atm/K*mol

R constant

Mm=mRT/PV

molar mass

D=MmP/RT

Density

sum of pressures=total pressures in gas mixture

Ptotal=p1+p2+p3+…

Daltons Law

fraction of moles of “a” in total moles of mixture

na/ntotal = Pa/ Ptotal

mole fraction (x)

[P+(n²a/v²)](v-nb)=nRT

Real Gases

average kinetic energy of particles and temp.=propartional

Kinetic-molecular theory

u

molecular speed notation

√3RT/Mm

u=

transfer of a gas thro space over time

Diffusion

transfer of a gas thro a membrane

Effusion

inversely proportional to molar mass

Rate of effusion and diffusion

Force*distance

Work

Heat exits system (-)

Exotherimic

Heat enters system (+)

Endothermic

E=1/2 mv²

Kinetic energy

E=mgh

potenial energy

sum of kinetic and potenial energy U

Internal energy

Etotal= kinetic energy + potential + internal

change in Etotal=0

Conservation of energy

1 J=1 N*m

Joule

energy needed to heat 1 gram of water by 1 degree celcius

calorie

1 cal = ? J

4.184 J

1 cal= ? kcal

.001 kcal

Change in energy total= change in enerfy system + change in energy surronding=0

Energy flow

remains constant

Isolated system internal energy

heat + work

q + w

Change in internal energy=

only depend on the initial and final conditions (not process used)

state functions

not state funtions

q and w are…

state functions

E and U are…

-P*change in V

w=

from hot to cold

Think ice cubes melt bc the heat from the water flows into the ice

Heat flows

bth objects have reached the same tempature

Thermal equilibrium

calculation of the amount of heat from temperature change

Caloimetry

4.184 J/g*C

Heat capacity of water

s * m * change in temp

s=spefici heat capacity

m=mass

q=

change in energy =change in heat

heat flow

q system + q surrondings= 0

q total=

m1C1ΔT1 = -m2C2ΔT2

thermal equilibrium equation

ΔH= H products- H reactants

Enthalpy (at given temp and pressure)

Δ H= q

Enthalpy at constant pressure

sumation (n ΔH products)- sumation (n ΔH reactants)

Δ H (direct method)

-must be in same phase

-reverse the reaction→ sign change

-mult. reaction——>ΔH mult. too

Δ H (indirect method)

=0

Δ H for pure elements in standard state

is diffracted

has constructive/ destructive interference

Light= wave bc…

Vλ

C=

3.00e8 m/s

Speed of light

m

wavelenth units

s^-1

Hz

frequency units

shorter

Increased energy, blank wavelength

The emision of radition/ light of a solid is assumed to be infinite for extremely short wavelengths if light followed wave patterns

It doesnt!

graphs curve back

Ultraviolet Catastrophe (blackbody radiation)

energy is quantized

all atoms of solids shake w/ certain v

Planck’s Quantum Theory

= nhv

Energy of vibration

6.626e-34 J*s

Planck’s constant

quantum number

n=

the ejection of electrons from the surface of the metals by radiation

photoelectric effect

Wave is both a particle and wave

E - energy of “particle” photon

V- frequency of the wave

Wave-particle duality

-R/n²

Electron’s energy

2.18e-18 J

R or rydberb constant=

• electrons have only specific energy levels

• only change levels when it has enough to fully transition

Bohr postulates

hv= R[(1/n²)-(1/n²)]

energy of a photon=

λ= h/mu

m-mass in kg

u-speed m/s

wavelike behavior of electrons

2L=nλ

standing waves

2 pi r= nλ

Circular standing wave

h/p

p-momentum of particle

λ in circular standing wave

mv

Momentum of particle p=

uncertianty= h/4pi

Heisenberg uncertainty principle

whole number integers

Shell where electron resides

Principal (n)

subshell

n-l

and all previous intergers starting form 0

Angular momentum (L)

spdfg

L letters

-L and +L

sum of values= # of orbitals

Magnetic (mₗ)

+1/2 or -1/2

each orbital can only have two e- that have opposite spin

Spin (mₛ)

each orbital can have at most two electrons having opposite spin

Pauli exclusion principle

Sphere

Shape of s orbital

dumbbell

Shape of p orbital

4 leaf clover

Shape of d orbital

2

max # of e in S

6

max # of e in p

10

max # of d

14

max # in f

most stable arrangemnt=subshell with greatest number of parallel spins

Hund’s

weakly attracted by a magnetic field (unpaired e)

Paramagnetic substance

not attracted by a magnetic field (paired e’s)

Diamagnetic substances

elements arranged by Z, their physical and chemical properties vary perodically

Periodic Law

r ⬇ with Z ⬆

Atomic radius in a period (row)

r ⬆

Atomic radius in a group (column)

-more pos. charge

-more pull on electrons

Shorter radius distance

-less pos charge

-less pull on electrons

longer radius distance

minimum energy needed to remove an electron from an atom

valance= easiest to remove

ionization energy

increases within any row

IE increases as Z

down

IE decreases as we go ——— in a column

less energy needed

X^+ + e

first ionization

X²+ + e

second ionization