Periodic Properties Flashcards
Periodic law
The chemical properties of the elements are dependent upon their atomic numbers
Representative elements
Have s or p sublevels as their outermost orbitals. Groups IA through VIIA
Nonrepresentative elements
Transition metals, have partly filled d sublevels. Lanthanide and actinide series, have partly filled f sublevels
Effective nuclear charge (Zeff)
The net positive charge from the nucleus felt by an election.
Increase left to right. Decrease down.
Atomic radius
Equal to one-half the distance between the centers of 2 atoms of that element that are just barely touching.
Decrease across.
Increases down.
Ionic radius
The radius of a cation or anion.
Cations smaller than neutral atoms. Anions larger than neutral atoms.
Ionization energy
The energy required to completely remove an electron from its gaseous state. Endothermic.
Increase across.
Decreases down.
Electron affinity
The energy change when an electron is added to a gaseous atom. The higher the Zeff = greater electron affinity.
+ = electron added; - = electron released
Electronegativity
A measure of the attraction an atom has for electrons.
Increases across.
Decreases down.
Malleability
The ability of a metal to be hammered into shapes
Ductility
The ability to be drawn into wires
Metals
Shiny solids at rt, high melting points and densities, malleable, ductile. Large atomic radius, low IE, low EN. Good conductors of heat and electricity.
Non-metals
Brittle in solid state, little or no metallic lustre. High IE, high EN. Poor conductors
Metalloids
Semimetals. Densities, boiling points, melting points fluctuate. EN and IE lies between metals and non-metals.
Alkali metals
Group IA. Metals, low densities. 1 valence e = largest atomic radii, low IE, low EN
