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
S P D F stands for
S = Sharpe
P = Principle
D = Defused
F = Fundamental
Magnetic Quantum numbers for S P D F
S = 0
P = -1 (Py), 0 (Pz), +1 (Px)
D = -2 (Dxy), -1 (Dyz), 0 (Dz²), +1 (Dxz), +2 (Dx² - y²)
F = -3, -2, -1, 0, +1, +2, +3
Paul’s exclusion law
Spin must be different (opposite spins) (OPP)
Hund’s Rule
If more orbitals are available then arrange e- on separate orbitals with same spin (Like if you have two hands open then hold some of the stuff in your other hand)
Auf Bau Law
Fill all subenergy levels with low “n+l” values (ABC of levels)
