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Unit 2 Exam Review: Physical Science

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  • Rank the following elements by increasing atomic radius: carbon, aluminum, oxygen, and potassium
    oxygen, carbon, aluminum, potassium
  • Define Ionization Energy
    the amount of energy needed to remove an electron from an atom.
  • What is the trend of Atomic Radius?
    Trend: Decreases from left to right across a period. Increases from top to bottom within a group.
  • How many valence electrons does F (fluorine) have?
    7
  • What is the trend for Ionization Energy?
    Trend: Increases as we go up a group. Increases from left to right across the periodic table.
  • What is the element with the lowest ionization energy: Au W S Fr Ne
    Fr
  • Give THREE examples of ions.
    Na+, Cl-, K+
  • Which has a larger atomic radius? Rb or Na Why?
    Rb. Increased atomic radii.
  • Which element is more electronegative: P or K? Why?
    P. Increasing electronegativity.
  • Define Isotopes.
    have the same atomic number (# of protons), but different mass numbers because different NEUTRONS.
  • Rank the following elements by increasing electronegativity: sulfur, oxygen, and aluminum.
    aluminum, sulfur, oxygen
  • What is the element with the lowest electronegativity: Pb C Sn Si
    Pb
  • Draw the valence electrons around Cl (chlorine).
    7 around Cl
  • What is the ionic charge of element X given: XCl
    X: +1
  • Define ionic bonding. Give two examples.
    Metal + Nonmetal. NaCl, MgS
  • Does K+ lose or gain an electron?
    loses an electron
  • Observe the following: Al3+ Is this a cation OR anion? How many electrons are lost OR gained?
    Cation. 3 electrons lost.
  • What is the element with the smallest atomic radius: Au W S Fr Ne
    Fr
  • Write the formula for magnesium bromide.
    MgBr2
  • Why do isotopes have a different mass?
    Isotopes have a different amount of NEUTRONS.
  • Arrange the following in order of increasing electronegativity: W, Pb, Ba, Po
    Ba, W, Pb, Po
  • Define Atomic Radius
    the distance between the nuclei of two identical atoms bonded together.
  • Define Valence Electrons.
    Valence electrons are the outer-shell electrons of an atom. Valence electrons determine the reactivity of an atom.
  • Define covalent bonding. Give three examples.
    2 nonmetals bonded together. CO2, NH3, HF
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