Unit 1 Definitions Flashcards
(50 cards)
Electronegativity definition
Electronegativity is a measure of the attraction an atom involved in a bond has for the electrons of the bond.
Frequency definition
Frequency is the number of wavelengths that pass a fix point in one unit of time
Absorption spectrum
A spectrum consisting of dark absorption lines superimposed on a bright continuous spectrum; it shows absorption of radiation by a material over a range of wavelengths
Aufbua principal
States that orbitals are filled in order of increasing energy
Bidentate
A ligand that contains two atoms with lone pairs of electrons capable of bonding to a metal atom or ion
Complex
A complex consists of a central metal atom or ion surrounded by Ligands
Dative/coordinate bond
A covalent bonds in which one of the atoms supplies both of the electrons of the shared pair
Coordination compounds
Compounds in which a central metal atom or ion is attached to a group of surrounding molecules or ions by dative covalent bonds (also known as coordinate bonds)
Coordination number
The coordination number is the total number of dative covalent bonds to the metal atom or ion.
It is not the number of ligands attached
Dative covalent bond
In this type of covalent bonds, both the shared electrons originally came from the same atom
Degenerate
A set of atomic orbitals that are of equal energy to each other
Electromagnetic spectrum
This is the range of frequencies or wavelengths of electromagnetic radiation
Emission spectroscopy
The study of emission spectra produced by excited substances (often gaseous atoms or molecules)
Excitation energy
The minimum energy required to change a system from its ground state to a particular excited state
Ground state
This is the lowest possible electronic configuration electrons in an atom can adopt
Heisenberg’s uncertainty principle
This principle states that it is impossible to state precisely the position and the momentum of an electron at the same instant
Hexadentate
A ligand that bonds to a metal ion using electron pairs on six donor atoms
Hund’s rule
When degenerate orbitals are available, electrons fill each singly, keeping the spins parallel, before pairing starts.
Ionisation
The addition or removal of an electron to create an ion
Ionisation energy
Ionisation energy is the energy required to remove one mole of electrons from one mole of atoms in the gaseous state
Ligands
Molecules or ions that bond to the central metal atom or ion in a complex
Lone pair
A lone or non-bonding pair of electrons is a pair of outer or valence shell electrons (that have opposing spins) which are not used to form covalent bonds within the molecule
Molecular orbital
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
Monodentate
A ligand that bonds to a metal atom or ion using the electron pair of a single donor atom
