Atomic Structure Flashcards
Energy of an electron
1.6 x 10^-19 C
Atomic number (Z)
Amount of protons
On top of the element
Mass number
Protons & neutrons in the atom’s nucleus
Isotopes
Different mass numbers, bc different numbers of neutrons
Where are atomic mass and atomic number placed on an element?
Atomic mass
Atomic number
Atomic mass
in amu, of one atom, nearly equal to its mass number
Atomic weight
Weighed average of different isotopes
Lyman series
Transitions from greater than or equal to 2 down to 1
Balmer series
Transitions from greater than or equal to 3 down to 2
Paschen series
Transitions from greater than or equal to 4 down to 3
A positive E in electron emission corresponds to?
Emission
Heisenberg uncertainty principle
Impossible to simultaneously determine the momentum & position of an electron
Bohr model of electrons
Electrons are fixed in orbit
Quantum model of electron
Electrons move around localized areas of orbitals
Pauli exclusion principle
No 2 electrons in a given atom can posses the same set of 4 quantum numbers
Each has their own energy state, position, size & shape & orietation
What does a larger principal quantum number mean?
Larger energy level & radiu of electron shell
Energy difference between shells decreases when?
The shells are further from the nucleus
Parallel spins
different orbial, same ms value
Aufbau/building up principle
Electrons fill each subshell completely before filling the next one
What is the n value for those in the d block
n-1
What is the n value for those in the f block
n-2
Hund’s rule
Within a given subshell, each orbital is filled with max number of half-filled orbitals with parallel spins
Which orbitals have higher stability?
Full & half-filled orbitals , may move up in electron orbital to fill half or full
Paramagnetic
Half filled electrons shells are slightly attracted to a magnetic field
Dimagnetic
Fully filled electrons shells slightly repel magnetic field
Electrons that are usually the valence electrons?
Usually in the s & particular subshell
