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ch-4

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Terms in this set (20)

  • How is the periodic table organized?
    By increasing atomic number, arranged in groups (columns) and periods (rows).
  • What defines a group in the periodic table?
    A vertical column of elements with similar chemical properties and the same number of valence electrons.
  • What defines a period in the periodic table?
    A horizontal row of elements where properties change progressively across the row.
  • What is the trend in reactivity for alkali metals down the group?
    Reactivity increases down the group due to easier loss of the outer electron.
  • What is the general trend in metallic character across a period?
    Metallic character decreases from left to right across a period.
  • What are the key properties of alkali metals?
    Highly reactive, soft metals with one valence electron, found in group 1.
  • What are halogens and their general properties?
    Group 17 elements, highly reactive nonmetals, typically form salts with metals.
  • What characterizes noble gases?
    Group 18 elements, inert gases with full valence shells, very low reactivity.
  • What are transition metals?
    Elements in groups 3-12, characterized by d-electrons, variable oxidation states, and often colored compounds.
  • How does atomic number relate to element properties?
    Atomic number determines the number of protons and electrons, influencing chemical behavior.
  • What is the trend in atomic radius across a period?
    Atomic radius decreases from left to right due to increasing nuclear charge pulling electrons closer.
  • What is the trend in atomic radius down a group?
    Atomic radius increases down a group because of added electron shells.
  • How does electronegativity change across a period?
    Electronegativity increases from left to right across a period.
  • How does electronegativity change down a group?
    Electronegativity decreases down a group.
  • What is metallic character?
    The tendency of an element to lose electrons and form positive ions; higher in metals.
  • Why are noble gases inert?
    They have full valence electron shells, making them stable and unreactive.
  • What is the significance of groups in predicting element behavior?
    Elements in the same group have similar valence electron configurations, leading to similar chemical properties.
  • What is the general trend in ionization energy across a period?
    Ionization energy increases from left to right due to stronger nuclear attraction.
  • What is the general trend in ionization energy down a group?
    Ionization energy decreases down a group because outer electrons are farther from the nucleus.
  • How do transition metals differ from main group elements?
    Transition metals have partially filled d orbitals, variable oxidation states, and often form colored ions.