Atomic Structure Flashcards
e/m of electron
1.758 x 10^11 C/kg
1.758 x 10^8 C/g
1 mole of electrons = ______C
96500 C = 1 Farad
Mass of electron
9.11 x 10^-31 kg
9.11 x 10^-28 g
Mass of electron in amu
0.00016 amu
1 mol of e- weight
0.00056g
Proton is how much heavier than electron
1840x heavier
e/m anodic is proprotional to
1/m
Anodic rays are kept in _________ pressure
0.01 torr
Positive rays give flash on
ZnS
e/m of anodic rays
9.54 x 10^7 C/kg
Mass of protons
1.67 x 10^-27 kg
1.67 x 10^-24 g
Angular momentum of Bohr’s atomic model
nh/2π
Rydberg’s constant
1.097 x 10^7 m-1
aº constant =
0.529 Aº
aº in terms of protons
n² / z
Ionization energy constant (and formula)
2.18 x 10^-18 J/atom
(z² e^4 m / 8∂² h² n²)
1 mol of H atom energy
1312.31 kJmol-1
Differences in energy gets ________ as the distance/shells increase
smaller
Ryderberg constant FORMULA
1/wavelength = (z² e^4 m / 8∂² h^3 C) (1/n1² - 1/n2²)
H spectrum series order
LBPBPf
H spectrum light types
L (Lyman) = UV
B (Balmer) = UV / Visible
P (Paschen) = Infrared
B (Brackt) = Infrared
Pf (Pfund) = Infrared
Which is the most energetic on the H spectrum series
Lyman
Stuff to find from Principle Quantum number (n)
n = number of standing waves
n² = number of orbitals
2n² = no of e- distributed in shell
Things to find from Azimuthal Quantum Number (l)
4l + 2 = no of columns in periodic table
n-l-1 = radial node