Chapter 1 Atomic Structure Flashcards
(18 cards)
Atomic number
the number of protons
Atomic weight
the weighted average of atomic mass for all isotopes of a given atom
Isotopes
things with the same number of protons, but different number of neutrons
The principle quantum number, n, defines
what shell the electron is in (shell number), size and energy
The second quantum number, l, defines
the shape of an electrons orbital (subshell number), shape and energy
The third quantum number, m (sub) l, defines
orientation of an orbital (orbital number)
spdf:
l=0,1,2,3 for s,p,d,f respectively
s subshells
hold 1 orbital
can hold upto 2 electrons
pictured as a sphere
Subshell arranged in increasing energy
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d
for any subshell, how many electrons can be held?
4l+2 electrons
The fourth quantum number, m (sub) s
spin number, spin of electron in orbital. can either be +1/2 (spin-up) or -1/2 (spin-down)
P subshell
depicted as a dumbbell
Aufbau principle
Electrons occupy the lowest energy orbital available.
Hund’s Rule
Electrons in the same subshell occupy available orbitals singly before pairing up.
Pauli Exclusion Principle
No two electrons in the same atom can have the same set of four quantum numbers
Planck’s constant
6.6 x 10^-34
Planck’s quantum theory
electromagnetic energy is quantized (transfered from one point to another via an electromagnetic wave.)
Photoelectric effect
one to one collison of election proved that light was maded up of particles (photons)
