Chapter 7 Quantum Mechanics P2 Flashcards
Electron Configuration
A representation of how electrons occupy orbitals in which orbitals are
represented as text and the number of electrons in each orbital is specified as a superscript
Aufbau Principle
Electrons fill the lowest energy orbitals first
Noble Gas Abbreviation
A method for abbreviating electron configurations and orbital diagrams. The
previous noble gas is given in brackets, and only electrons that are not part of the previous noble gas are
shown
Orbital Diagram
A representation of how electrons occupy orbitals in which orbitals are represented
as boxes and electrons are represented as arrows
Pauli Exclusion Principle
Each orbital can have a maximum of two electrons, with opposing spins
Hund’s Rule
When filling orbitals of equal energy, electrons fill them singly first, with parallel spins
Paramagnetic
Atoms or ions with unpaired electrons are paramagnetic, and are attracted to an external
magnetic field
Diamagnetic
Atoms with no unpaired electrons are diamagnetic, and are not attracted to an external
magnetic field
Valence Electrons and its importance
Electrons in the outermost principal shell of an atom. Valence electrons are held
more loosely, are more easily shared, and play a large role in determining the physical and chemical
properties of an element
Core Electrons
Electrons not in the outermost principal shell of an atom
Principal Quantum Number (n)
Specifies the principal shell of an orbital. Can be integer values
between 1 and 7
Angular Momentum Quantum Number (l)
Determines the shape of an orbital. Can be integer values
between 0 and n-1
Magnetic Quantum Number (ml)
Determines the orientation of an orbital. Can be integer values,
including 0, between -l and l
Spin Quantum Number (ms)
Specifies the spin of an electron. Two possible spins: up spin (+1⁄2) and
down spin (-½)
Effective Nuclear Charge (Zeff)
The net positive charge experienced by an electron in a multi-electron
atom
Shielding
Electrons in core orbitals screen valence electrons from the full effect of the nuclear charge
Atomic Size and trend
General term to describe the average bonding radius of an atom;
size increase down to the left
Ionization Energy and trend
Energy required to remove an electron from an atom or ion in the gaseous state; increase top right
First Ionization Energy
Energy required to remove an electron from a neutral atom in the gaseous
state
Second Ionization Energy
Energy required to remove a second electron from an already-ionized atom
in the gaseous state
metallic character trend
down to left
equation for speed of light
c=(wavelength)(Frequency v)
Energy of photon equations
E=hv; E=hc/(wavelength)
Energy of electron and transition
-2.18 x 10^-18 J (1/n^2)
-2.18 x 10^-18 J [(1/n^2f) - (1/n^2i)]
