Periodic Table test objectives

							Chemistry
Name: ______________________________________________                   Date: __________
                            Test Objectives for Periodic Table


   Use a periodic table to determine the correct number of protons and electrons in a
    particular atom.
   Describe the basic features of the Bohr model of the atom.
   Define valence level.
   Distinguish between valence electrons and kernel electrons.
   Distinguish between ground state and excited state configurations of an atom.
   Explain the cause of spectral lines in terms of electrons and energy levels.
   Recognize the ground state configuration of an element.
   Draw Lewis Dot Structures for atoms.
   Describe the orbital model of the atom.
   Define the term principal energy level.
   Know the maximum # of electrons (2n2) in a given principal energy level.
   Know the # of sublevels for a given principal energy level.
   Define orbital.
   Know how many electrons fill an orbital and how many orbitals in a given sublevel.
   Using the periodic table, determine the correct number of valence electrons for
    “representative elements.”


   Distinguish between a period and a group on the periodic table.
   Identify an element given its period and group.
   Recognize that the elements are arranged in order of atomic number, and the
    atomic number identifies the element.
   Identify the common groups on the periodic table: alkali metals, alkaline earth
    metals, transition metals, halogens, and noble gases.
   Recognize that for groups 1, 2, and 13-18 (the A-group elements), elements in the
    same group have the same number of valence electrons and therefore have similar
    chemical properties.
Chemistry
Name: ______________________________________________                     Date: __________




   List the elements that are liquids and gases at STP.
   List the 7 diatomic elements.
   List the properties of metals, non-metals, and metalloids.
   Identify an element as a metal, non-metal, or metalloid based upon its properties.
   Memorize: “Metals are Losers; nonmetals are winners.” or LEO GER
   Predict the size and charge of ions relative to the parent atom.
   Define the term allotrope, and list some common examples.
    (for carbon and oxygen)
   Know how the modern periodic table was developed.
   Identify the common groups on the periodic table: alkali metals, alkaline earth
    metals, transition metals, halogens, and noble gases.
   Define the term “metallic character.”
   Identify the most active metal.
   Explain how the reactivity of non-metals is defined.
   Identify the most active non-metal.
   Define the terms electronegativity and ionization energy.
   Explain how the atomic radius, ionic radius, electronegativity, first ionization
    energy, and metallic or non-metallic properties change as you go down a group of
    the periodic table.
   Explain how the atomic radius, ionic radius, electronegativity, first ionization energy,
    and metallic or non-metallic properties change as you go across a period of the
    periodic table.
   Correlate changes in atomic radii with changes in ionization energy and changes in
    electronegativity.
   Recognize that elements in the same group have the same number of valence
    electrons and therefore similar chemical properties.
   Correlate changes in the number of valence electrons with typical bonding behavior.
   Predict the properties of the A-group elements from the positions of the elements in
    the periodic table.