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.