Download Electromagnetic Spectrum Wavelength Wavenumber Frequency

Electromagnetic
Spectrum
Wavelength
Wavenumber
Frequency
Velocity
Excited State
Ground State
Heinsenberg's
Uncertainty Principle
Pauli Exclusion
Principle
Degenerate
This is the range of frequencies or
wavelengths of electromagnetic
radiation
The distance between adjacent crests
or troughs of a wave.
The reciprocal of wavelength and has
the units of cm -1 (number of cycles
per cm.)
The number of wavelengths that pass a
fixed point in one second. The units are
Hertz (Hz).
Speed of light = 3.00 x 10⁸ ms-1
When an electron absorbs energy, it
goes to a higher energy level.
This is the lowest possible electronic
configuration the electrons in an atom
can adopt.
When an electron moves down to its
ground state, energy is given out.
This states that it is impossible to state
precisely the position and the
momentum of an electron at the same
instant.
This states that an orbital holds a
maximum of two electrons.
Of equal energy.
Aufbau Principle
Hund's Rule
Spectroscopic
Notation
Atomic Emission
Spectroscopy
Atomic Absorption
Spectroscopy
Complex
Ligand
Spectrochemical
Series
Dative Covalent Bond Coordination number
This states that orbitals are filled in
order of increasing energy.
When degenerate orbitals are
available, electrons fill each singly,
keeping their spins parallel before
pairing starts.
1s² 2s² 2p⁶ 3s² 3p⁶ 4s²3d¹⁰
A way of performing chemical analysis of
elements contained within a sample. The
sample is converted into a gas and then
excited using a flame/electricity. The excited
gas atoms emit light energy. The intensity of
this light can be use to determine exactly
which elements are in the sample.
A technique for determining the
concentration of a particular metal element
in a sample. The electrons are promoted to
higher energy levels by absorbing energy,
and the wavelength of the absorbed energy
can be used to determine which element is
present. The intensity of the absorbed light
can be used to determine the concentration
of the elements.
A central metal ion surrounded by
ligands.
Negative ions or uncharged molecules
with one or more lone pairs of
electrons.
When one atom provides both of the
electrons that form the bond
A list of ligands in order of the size of
the crystal field splitting caused in the
d-orbitals.
CN⁻ > NH₃ > H₂O > OH⁻ > F⁻ >Cl⁻ > Br⁻ > I⁻
This is the number of nearest
neighbours by which an atom or ion is
surrounded in a structure.
Bidentate
Coordination
compounds
Hexadentate
Molecular orbital
Monodentate
Oxidation
Oxidation number
Reduction
A ligand that contains two atoms with
lone pairs of electrons capable of
bondingto a metal ion.
Compounds in which a central metal
ion is attached to a group of
surrounding molecules or ions by
dative covalent bonds (also known as
coordinate bonds).
A ligand that bonds to a metal ion
using electron pairs on six donor
atoms.
A molecular orbital is a region in space
between the nuclei where there is a
high probability of finding electrons. It
is formed by the overlap of atomic
orbitals.
A ligand that bonds to a metal ion
using the electron pair of a single
donor atom.
This is the loss of electrons from a
substance. It can also be described as
an increase in oxidation number.
The formal charge assigned to each
atom in a compound according to
certain rules.
This is the gain of electrons by a
substance. It can also be described as a
decrease in oxidation number.