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Name: ____________________________________________ Hr: ______ Date: __________ SAO: summative assessment organizer for Ch 6 & 7 Key Terms Periodic law Metals Anion Dobereiner Nonmetals Ionization energy (I.E.) Mendeleev Metalloid (semimetal) Electron affinity Groups/families Ductile Electronegativity Periods Luster Valence electrons Alkali metals Malleable Electron dot structures (aka “lewis dot Alkaline-earth metals Conductivity diagrams”) Transition metals Abbreviated electron configurations Octet rule Inner transition metals (kernel structures) Noble gas inner core Halogens S block, P block, D block, F block Inert Noble gases Ending electron configuration Ionic bond Boron group Atomic radius Ionic compound Carbon group Electron shielding (aka “shield effect”) Chemical formula Nitrogen group Ionic size Formula unit Oxygen group Cation Objectives Ch 6: The Periodic Table 6.1 Organizing the Elements 1. Explain how elements are organized in a periodic table (groups, periods, electron configuration) 2. Compare early and modern periodic tables (Dobereiner, Mendeleev, modern) 3. Locate metals, nonmetals, and metalloids on a periodic table & describe properties of each 4. Utilize the IUPAC and US system of numbering groups 5. State the periodic law 6.2 Classifying the Elements 6. Describe the information in a periodic table 7. Label groups by name, number and ending electron configuration 8. Classify elements based on electron configuration (ex: identify the element, classify as metal/nonmetal/metalloid, list general properties) 9. Distinguish representative elements, transition metals (two types!), and noble gases 10. Express electron configurations using abbreviated form (kernel method) 6.3 Periodic Trends 11. Describe trends among the elements for atomic size w/in groups and periods 12. Atomic Radius: define, label trend down a group and across a period, in which corner would largest/smallest radii be found, list the reason(s) why the trend exists 13. Explain what influences the atomic radius 14. Explain how ions form—cations and anions 15. Ionic size (NOT a “trend”): predict if ion is “bigger than atom” or “smaller than atom” based on the charge of the ion and WHY 16. Describe periodic trends for first ionization energy and electronegativity 17. Ionization Energy: define, label trend down a group and across a period, in which corner would largest/smallest I.E. be found, list the reason(s) why the trend exists (shielding effect is a huge factor!) 18. Explain why the amount of energy increases for each successive I.E. Extra Credit: Successive ionization energies (2nd ionization energy, 3rd ionization energy, etc…): after analyzing a series of successive I.E., identify the big jump in ionization energy, explain why, and predict the group the element is from 19. Electronegativty: define, label trend down a group and across a period, in which corner would largest/smallest electronegativity be found, list the reason(s) why the trend exists 20. Use figure 6.22 to add periodic trend info to your periodic table Ch 7: Ionic and Metallic Bonding 7.1 Ions 21. Determine the number of valence electrons in an atom of a representative element using group numbers, electron configuration, or orbital diagram 22. Explain how the octet rule applies to atoms of metallic and nonmetallic elements 23. Describe how cations form Name: ____________________________________________ Hr: ______ Date: __________ 24. Explain how anions form 25. Use octet rule to predict the charges of a particular ion 26. Determine likely charges for elements of a particular group based on electron configuration or orbital diagram 27. Draw lewis dot structures to represent number of valence electrons in an atom or ion 28. Use octet rule to predict how reactive or inert an element may be 7.2 Ionic Bonds and Ionic Compounds 29. Explain the electrical charge of an ionic compound 30. First learn logic of ionic bond formation, then practice “criss-cross” method 31. Predict chemical formulas for binary compounds (“binary” means made of only two elements) 32. Describe three properties of ionic compounds Label the periodic table below by group name, group number, ending electron configuration, sublevel block, expected ionic charge, anions/cations, and use arrows to label the periodic trends for atomic radius, ionization energy, and electronegativity.
