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1、General ChemistryName:Trends in the Periodic TableDate: Per.:1. Basic OrganizationA. A horizontal row in the Periodic Table is called a .B. A vertical column in the Periodic Table is called a or .2. OrbitalsA. Identify the orbitals being filled in the following periods (period 4 is done for you as a
2、n example):1) Period 1 .2) Period 2 .3) Period 3 .4) Period 4 4s 3d 4p.5) Period 5 .6) Period 6 (dont forget the elements 58-71) .7) Period 7 (dont forget the elements 90-103) .B. Which orbitals are being filled in groups 1, 2, and 13-18? . Which are in the transition elements? . Which are in the La
3、nthanide and Actinide series? .C. How does the position of the elements in the periodic table relate to the number of valance electrons?D. How does the position of the elements in the periodic table relate to the elements oxidation number?3. Covalent RadiusThe Graph of Covalent Radius can be used to
4、 see the periodic and group trends in covalent atomic radius. Answer the following questions from the graph. Hint: “Covalent Radius” = atomic radius and then atomic size.A. What happens to the covalent atomic radius as you go down a group? Why?B. What happens to the covalent atomic radius as you go
5、across a period? Why?4. Ionization EnergyTable K in the Reference Tables for Chemistry can be used to see the periodic and group trends in first ionization energy. You can also answer some of the following questions from the graph.A. Review what is meant by the term ionization energy.B. What is the
6、difference in magnitude between first and second ionization energy? Using your definition for ionization energy, explain this difference.C. Generally, how does the first ionization energy vary as the atomic number increases going across a period? Why?D. How does the first ionization energy vary goin
7、g down Group 1 or Group 17? Why?E. Why does the first ionization energy drop going from Group 2 to Group 13? Why?5. ElectronegativityTable K in the Reference Tables for Chemistry can be used to see the periodic and group trends in electronegativity. The same information has been graphed. Answer the
8、following questions from the graph.A. Review what is meant by the term electronegativity.B. How does electronegativity differ from ionization energy?C. Generally, how does the electronegativity vary as the atomic number increases going across a period? Why?D. How does the electronegativity vary goin
9、g down Group 1 or Group 17? Why?6. Metallic vs. Nonmetallic Nature of the ElementsUse the following information to answer the questions below Metals have a low first ionization energy and low electronegativities Nonmetals have high first ionization energies and high electronegtivities. Metals form p
10、ositively charged ions Nonmetals form negatively charged ionsA. What happens to the metallic character of an element as you go down group 1? Group 17? Why?B. What happens to the metallic character of an element as you go across a period? Why?C. Make a generalization about the reactivity of metals and nonmetals and their placement in the periodic table.7. Ionic RadiusA. How do the radii of ions of metals compare to the radii of their atoms? Why?B. How do the radii of ions of nonmetals compare to radii of their atoms? Why?0ebf9ad7525e097d52b83f01dc034a39.pdf- 2 -
