Ch 2 - The Periodic Table

• A: group 1-8 - B: transition metals, lanthanide and actinide series

• shiny (lustrous) • conduct electricity well because they have valence electrons that can move freely • malleable (ability to be hammered into shapes) and ductile (ability to be pulled or drawn into wires)

• dull • poor conductors of electricity • brittle

• characteristics of both metals and nonmetals - found at the zig zag starting under Boron, but not aluminum and oganesson

• decreased atomic radius • increased ionization energy • increased electron affinity • increased electronegativity

• increased atomic radius • decreased ionization energy • decreased electron affinity • decreased electronegativity

• the net positive charge experienced by electrons in the valence shell and forms the foundation for all periodic trends • increase from left to right with little change from top to bottom • valence electrons become increasingly separated from the nucleus as the principal energy level, n, increases from top to bottom

• size + < 0 < - increases

• amount of energy needed to remove an electron from the valence shell of a gaseous species • increases –> and bottom to top

• amount of energy released when a gaseous species gains an electron in its valence shell • increases –> and bottom to top

• measure of the attractive force of the nucleus for electrons within a bond • increases –> and bottom to top

• typically take on oxidation state of +1 • prefer to lose an electron to achieve a noble gas like configuration • most reactive to metals

• take on oxidation state of +2 - can lose 2 electrons to achieve noble gas like configuration

• group 16 • take on oxidation states of -2 to +6 (depending on whether nonmetals or metals) in order to achieve noble gas like configuration • biologically important

• typically oxidation state of -1 • prefer to gain an electron to achieve noble gas like configurations • have the highest electronegativities

• have a fully filled valence shell in their standard state and prefer not to give up o take on additional electrons • very high ionization energies • virtually non existent electronegativies and electron affinities

• unique with multiple oxidation states, which explains their ability to form colorful complexes with nonmetals in solution and their utility in certain biological systems

transition metals

• the strength with which the protons in the nucleus can pull on electrons