Chapter 3 - Electrons and the Periodic Table Flashcards
Absorbance
A measure of the capacity of a substance to absorb light of a specified wavelength.
Absorption Line
The individual colours of light in a continuous spectrum that are absorbed by the hydrogen atoms
Absorption Spectrum
The collection of absorption lines
Anion
A negatively charged ion
Atomic Absorption Spectroscopy (AAS)
An analytical technique that uses light absorption to measure the concentration of a metal in a sample.
Atomic Radius
A measure used for the size of atoms; determined by measuring half the distance between two adjacent atoms in a molecule or structure
Bohr Diagram
A simple diagram that shows the arrangement of electrons around the nucleus
Bohr Model
A theory of the atom proposed by Niels Bohr that states the electrons in an atom occupy fixed, circular orbits that correspond to specific energy levels.
Core Charge (or Effective Nuclear Charge)
The effective nuclear charge experienced by the outer-shell electrons in an atom. It indicates the attractive force felt by the valence electrons towards the nucleus
Cation
A positively charged ion
Electrical Conductivity
The degree to which a specified material or solution conducts an electric current.
Electromagnetic Radiation
A form of energy that moves through space. Visible light, radio waves and X-rays are forms of electromagnetic radiation.
Electromagnetic Spectrum
All possible frequencies of electromagnetic radiation shown in order of their wavelengths or frequencies.
Electron Configuration
In the shell model of an atom, the electronic configuration is a means of representing the number of electrons in each shell.
Electron Shell
In the shell model of an atom, an electron shell is a fixed energy level that corresponds to a circular orbit of electrons
Electronegativity
The ability of na atom to attract electrons in a covalent bond towards itself.
Emission Line
When an electron absorbs energy
it jumps to a higher energy state. Shortly afterwards the electron returns to the lower energy level, releasing a fixed amount of energy as a particular colour of light.
Emission Spectrum
A spectrum produced when an element is excited by heat or radiation. It appears as distinct lines characteristic of the
element.
Energy Level
One of the different shells of an atom in which an electron can be found.
Excited State
A term used to describe an atom
in which electrons occupy higher energy levels than the lowest possible energy levels.
Flame Test
Determination of the metallic elements present in a compound by inserting a
sample of the compound into anon-luminous Bunsen burner flame.
First Ionisation Energy
The energy required to remove one electron from an atom of an element in the gas phase.
Ground State
A term used to describe an atom in which the electrons occupy the lowest possible energy levels.
Group
A vertical column of
elements in the periodic table.
