This lesson introduces how electron configurations organize elements into broad categories and how metallic character shapes the behavior of representative elements. It also explains why some metals are protected from further reaction by passivation.
The periodic table reflects patterns in electron configurations. Representative elements are those in which the s or p orbitals are being filled. Transition elements fill d orbitals, while inner transition metals fill f orbitals.
All flashcards
How are transition elements distinguished from inner transition metals by orbital filling?
Transition elements fill d orbitals, whereas inner transition metals fill f orbitals.
What is metallic character?
The tendency of an element to lose its outer valence electrons.
What is passivation?
Formation of a relatively nonreactive surface film that reduces a material’s further reaction with its surroundings.
What is a sacrificial anode?
A more readily oxidized metal connected to a structure so it corrodes preferentially and protects that structure.
What is the inert pair effect?
The tendency of a heavier p-block element’s valence s-electron pair to remain relatively uninvolved in bonding.
Quiz questions
How does the reactivity of alkali metals generally change down group 1, and why?Answer: It increases because the outer electron becomes easier to remove.
How does reactivity change from zinc to mercury among the familiar group 12 metals?Answer: It decreases down the group.
How does a sacrificial anode protect a connected metal structure?Answer: The anode oxidizes preferentially, reducing oxidation of the structure.
What does it mean for an oxide or hydroxide to be amphoteric?Answer: It can react with both acids and bases.
What is tin pest?Answer: The low-temperature conversion of white tin into brittle gray tin.
Based on Chemistry 2e by Paul Flowers, Klaus Theopold, Richard Langley, William R. Robinson, PhD (OpenStax), licensed CC BY 4.0. Adapted into a summary, flashcards and quizzes.