chem unit 5

  1. Front: What are the general properties of metals?
    Back: Solid at room temp, malleable, ductile, good conductors.

  2. Front: What are the general properties of nonmetals?
    Back: Mostly gases at room temp, brittle, poor conductors.

  3. Front: What are metalloids, and what is their key property?
    Back: Elements with properties of metals and nonmetals; they are semiconductors.

  4. Front: What are alkali metals, and where are they found?
    Back: Group 1 elements; silvery, soft, reactive with water, not found freely in nature.

  5. Front: What are alkaline earth metals, and how do they differ from alkali metals?
    Back: Group 2 elements; harder, denser, and less reactive than alkali metals.

  6. Front: What are halogens, and why are they so reactive?
    Back: Group 17 elements; they need 1 electron to complete their outer shell.

  7. Front: What are noble gases, and why are they unreactive?
    Back: Group 18 elements; they have full outer electron shells.

Section 5.2: Electron Configuration and the Periodic Table

  1. Front: What is the octet rule?
    Back: Atoms gain, lose, or share electrons to achieve 8 valence electrons.

  2. Front: What are the two ways elements achieve a full octet?
    Back: By gaining/losing electrons (ions) or sharing electrons (covalent bonding).

Section 5.3: Trends in Periodic Properties

  1. Front: What is effective nuclear charge (Zeff)?
    Back: The net positive charge experienced by an electron, calculated as Z−SZ - SZ−S.

  2. Front: How does atomic radius change across a period?
    Back: It decreases due to increasing Zeff, pulling electrons closer to the nucleus.

  3. Front: How does atomic radius change down a group?
    Back: It increases because electrons are added to higher energy levels.

  4. Front: What is ionization energy?
    Back: The energy required to remove an electron from an atom.

  5. Front: How does ionization energy change across a period?
    Back: It increases because Zeff strengthens the attraction to outer electrons.

  6. Front: How does ionization energy change down a group?
    Back: It decreases because outer electrons are farther from the nucleus and shielded.

  7. Front: What is electronegativity?
    Back: An atom’s ability to attract electrons in a chemical bond.

  8. Front: How does electronegativity trend on the periodic table?
    Back: It increases across a period and decreases down a group.

  9. Front: What is electron affinity?
    Back: The energy change when an atom gains an electron; often releases energy (negative).

  10. Front: How do cations and anions differ in size from their parent atoms?
    Back: Cations are smaller; anions are larger.

  11. Front: Which element has the highest electronegativity?
    Back: Fluorine, with a value of 4.0.

  12. Front: What element has the lowest electronegativity?
    Back: Francium, with a value of 0.7.