Bhor

TEORÍA ATÓMICA DE BOHR

e ⋅ (Ze) ⋅ k Fe = − r2
Z ⋅ e2 ⋅ k Fe = − r2

Ec =

Z ⋅e ⋅k 2⋅r

2

n 2 ⋅ h2 r= 4 ⋅ π2 ⋅ m ⋅ Z ⋅ e2 ⋅ k

1 2 ⋅ π2 ⋅ m ⋅ Z 2 ⋅ e4 ⋅ k 2  1 Ef = ⋅ − 2 h  n2 n2 H L
1 1 2 ⋅ π 2 ⋅ m ⋅ Z 2 ⋅ e4 ⋅ k 2  1 ⋅ − = 3 h ⋅c λ  n2 n2 H  L
     



    

Z ⋅ e2 ⋅ k ET = − 2⋅r

h2 RB = 4 ⋅ π2 ⋅ m ⋅ e2 ⋅ k
r = RB ⋅ n2 ⋅ Z −1

Fc = −

m ⋅ v2 rE = m ⋅ c2
h⋅c Ef = λ h m ⋅v = λe 2 ⋅ π ⋅ r = n ⋅ λe

RH =

2 ⋅ π 2 ⋅ m ⋅ e4 ⋅ k 2 h3 ⋅ c
     

Z ⋅ e2 ⋅ k = m ⋅ v2 r

2 ⋅ π2 ⋅ m ⋅ Z 2 ⋅ e4 ⋅ k 2 ET = − n 2 ⋅ h2 E f = ∆E H,L = E H− E L

 1 1 1 = RH ⋅ Z 2 ⋅  − λ  n2 n2 H  L
2

ET = E P + EC

   1 1  − f = RH ⋅ Z ⋅ c ⋅   2 2 n nH   L    1 1 E f = RH ⋅ Z ⋅ h ⋅ c ⋅  −  n2 n2 H  L
2

EP = Fe ⋅ r

EH2 ⋅ π 2 ⋅ m ⋅ Z 2 ⋅ e4 ⋅ k 2 =− 2 nH ⋅ h2 2 ⋅ π 2 ⋅ m ⋅ Z 2 ⋅ e4 ⋅ k 2 2 nL ⋅ h 2

    

Z ⋅ e2 ⋅ k EP = − r
Fe = Fuerza eléctrica. Fc = Fuerza centrípeta. ET = Energía total. EP =Energía potencial. EC = Energía cinética. Ef = Energía del fotón. E = Energía de una partícula. EH = Energía de la órbita nH. EL = Energía de la órbita nL.

n⋅h m ⋅v ⋅r = 2⋅π

EL = −

∆EH,L =Diferencia de energía entre las órbitas nH y nL.
n = Órbita en la que se encuentra el electrón. nH = Órbita de alta energía. nL = Órbita de baja energía. e = Carga del electrón 1.6022x10-19 [C]. Z = Númeroatómico (Ze = Carga del núcleo). k = Constante de Coulomb 9x109 [N·m2·C-2]. r = Radio de la órbita en la que se encuentra el electrón. m = masa del electrón 9.1095x10-31 [kg].

v = Velocidad delelectrón en la órbita. c = Velocidad de la luz 2.9979x108 [m·s-1]. h = Constante de Planck 6.62617x10-34 [J·s]. λ = Longitud de la onda electromagnética. λe = Longitud de la onda asociada al electrón. RB =Radio de Bohr 5.29177x10-11 [m]. RH = Constante de Rydberg 1.09737x107 [m-1]. f = Frecuencia de la onda electromagnética.

AVM

TEORÍA ATÓMICA DE BOHR

Fe = −

Z ⋅e2 ⋅k r2
m ⋅v r
2...