Peridoic Table Flashcards
First ionisation energy
The minimum energy required to remove the most loosely bound electron from a NEUTRAL GASEOUS atom in its ground state
Decreases down a group
Increases across a period
Electron configuration
Shows the arrangement of electrons in the atom of an element
Aufbau principle
When building up the electron configuration of an atom in its ground state, the electrons occupy the lowest energy level available
Hund’s Rule of Maximum Multiplicity (bus seat rule)
When 2+ orbitals of equal energy are available, the electrons occupy them singly before filling in pairs
Pauli Exclusion Principle
No more than 2 electrons can occupy an orbital and they must have an opposite spin
An element
A substance that can’t be split into simpler substances by chemical means
Newland’s Octaves
Arrangements of electrons when the 1st and 8th elements have similar properties
Triad
A group of 3 elements of similar properties, where the Relative Atomic mass of the middle element is the average of the other two elements
Mendeleev’s Periodic Law
When elements are arranged in order of increasing Relative Atomic mass (atomic weight) the properties of the elements recur periodically
Recur periodically
Repeat at regular intervals
Atomic number of an atom
The amount of protons (H+) in the nucleus of an atom
Modern periodic table
An arrangement of atoms in order of increasing atomic number
Modern Periodic Law
When elements are arranged in order of increasing atomic number, the properties of the elements recur periodically
Mass number
The sum of protons+neutrons in the nucleus
Isotopes
Atoms of the same element with different mass numbers due to a different number of neutrons in the nucleus
Relative Atomic mass
The average of the mass numbers of all the isotopes as they occur naturally, taking their abundance’s into account and expressed on a scale where the atoms of carbon-12 has a mass of 12 units
Principle of Mass Spectrometry
Charged particles moving in a magnetic field are deflected to different extents according to their mass numbers
Electronegativity
The relative attraction an atom in a molecule has for the shared pair of electrons in a covalent bond
Atomic radius
Half the distance between the nuclei of 2 atoms of the same element that are joined by a single covalent bond