Chapter 2- Periodic Table Flashcards
Metals
Shiny, lustrous, conduct electricity well, male able and ductile.
Non metals
Dull, poor conductors or electricity, brittle.
Metalloids
Stair pattern. Obtain characteristics similar to both metals and non metals.
Effective nuclear charge Z(eff)
Net positive charge experienced by electrons in the valence shell.
Trend: increase L-R
decrease T-B
Atomic radius
Decrease L-R
Increase T-B
Ionic radius
Size of charged species.
Largest nonmetallic ionic radii, and the smallest metallic ionic radii exists at the nett aloud boundary.
Ionization energy
Amount of energy required to remove an electron from the valence shell of a gaseous species.
Increases L-R
Decreases T-B
Electron affinity
Amount of energy released when an electron is gained in the valence shell.
Increases L-R
Decreases T-B
Electronegativity
Is a measure of the attractive force of the nucleus for electrons within a bond.
Increases L-R
Decreases T-B
Alkali metals
Typically take +1 oxidation state.
Prefer to lose an electron.
Active metal.
Alkaline metals
Take on oxidation state +2.
Can lose 2 electrons.
Chalcogens
Take oxidation states -2 to +6.
Biologically important.
Halogens
Typically take on oxidation state -1.
Prefer to gain an electron.
Highest electronegativities.
Noble gases
Fully filled valence shell.
Prefer to remain no reactive.
Transition metals
Multiple oxidative states.
