Unit 7- Electronic Structure Flashcards
waves
periodic disturbances- they repeat at regular intervals of time and distance
wavelength
distance between peaks
- units: m
frequency
of waves that pass a fixed point each sec
- s^-1 or Hz
speed of light (C)
3.00 x 10^8 m/s
* C = wavelength x frequency
nm to m conversion
1 nm = 10^-9 m
quantum
smallest unit of energy
energy equation
E = hv or E= hc / wavelength
h= 6.626 x 10^-34
c= speed of light
photoelectric effect
the process in which e- are ejected from a metal when it is exposed to light
spectrum
a graph of light intensity as a function of wavelength or frequency
continuum or continuous spectrum
- emitted by solids
- full rainbow spectrum
line spectrum
- emitted by gaseous atoms
- contains light only at specific wavelengths and not others (black with stripes)
wavelength equation
wavelength = h/p or h/mv
h = 6.626 x 10^-34
p = momentum
m = mass
v = velocity
wave function
give the amplitude of the e- wave at any point in space
wave fxn^2 = probability of finding the e- at any point in space
quantum #s
- n, l, m(sub l)
- describe the distribution of the e- in #D space
atomic orbital
a wave fxn of the e- for specific values of n, l, m (sub l)
Principle Quantum #, n
ENERGY and DISTANCE of the e- from the nucleus
principle shell (shell)
all atomic orbitals that have the same value of n
n = shell
Angular momentum quantum #, l
SHAPE of the orbital
- cannot equal or exceed the value of n
subshell
all possible orbits that have the same values of both n and l
value of l and its letter
0 = s
1 = p
2 = d
3 = f
4 = g
5 = h
m(vl)
ORIENTATION of the atomic orbital
-l to l, including 0
orbital
wave function described by all 3 quantum #s (n, l, m(vl))
e- spin quantum #, m(vs)
reps 1 of the 2 allowed spin values: +1/2 and -1/2
orbital shapes
s: circular
p: oval (2)
d: oval (4)
“degenerate”
s, p, d, and f orbitals in any principal shell have the same energies
e- shielding (screening)
result of the influence of e- on the effective nuclear charge
the effective nuclear charge (Z effect)
a weighted avg of the nuclear charge that affects an e- in the atom
Pauli Exclusion Principle
no 2 e- in the same atom can have the same set of 4 quantum #s
- each orbital hold a max of 2 e-
Aufbau principle
e- are assigned quantum #s of the LOWEST ENERGY orbital that is available
ground state
atom in its lowest energy state
e- configuration
lists occupied subshells (1s, 2p, etc) followed by a superscript giving # of e-
s=2e-
p=6e-
d=10e-
f=14e-
orbital diagrams
box for orbital with arrow indicting direct of spin
Hund’s Rule
1e- occupies each degenerate orbital with the same spin before a second e- is placed in an orbital
abbrev e- config
using noble gases to rep core e-
