What are the relationships between the group configuration and number for the elements in the S, P, and D blocks?

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• 1. Who did the pioneer work on the Periodic Table we use today? 2. What important use did he make of his Periodic Table? 3. In what order are the elements listed in our present Periodic Table? 5. State the periodic law 6. What name is given to the elements in a vertical column of the Periodic Table? 7. What is given to the elements in a horizontal row of the Periodic Table? 8. What name is given to elements whose atoms usually differ in electron configuration the entrance of successive electrons in a d sublevel? 9. What name is given to elements whose atoms usually differ in electron configuration the entrance of successive electrons in a f sublevel? 10. What arrangement of outer-shell electrons identifies elements with generally similar properties? 11. Excluding the noble gases, state the location in the periodic table of (a) the most active metals (a) and (b) the most active nonmental. 12. Which of the noble gases have no known compounds? 13. What does the electron population of the outermost shell of the atoms of the transition elements reveal about their properties? 14. Why do elements of the lanthanide series have almost identical chemical properties? 15. What is the significance of the zigzag line running diagonally down and to the right near the right end of the periodic table? 16. What properties do metalloids show? 17. Why isn't the volume of an atom a completely definite quantity? 18. Describe two trends regarding the periodicity of atomic radii, across a period and down a group. a. b. 19. In the, reaction, A+ energy -> A+ + e-, (a) what kind of a particle is A+? 20. In Question 19, what kind of element is A generally if the quantity of energy (a) is low? (b) is high? 21. What two properties of the noble gases furnish strong evidence for the unusual stability of the outer-shell octet? a. b. 22. How does the ionization energy vary with atomic number within a group? a. b.why? 23. Explain the decrease in first Ionization energy between Groups 2 and 13. 24. Between which two other groups in Periods 2 and 3 is there another decrease in first ionization energy?________&_________ 25. Explain the sharp decrease in ionization energy between the last transition. 26. What apparently causes the observed irregularities in the general increase in ionization energy in each series? 27. Why is the ionization energy required to remove the second electron from Na atoms very much greater than that needed to remove the first electron? 28. Why is it easier to remove the first electron from Al atoms than it is to remove the first electron from Mg atoms? 29. Why is the ionization energy needed to remove the first two electrons from Mg atom relatively low? 30. What is electron affinity? 32. What type of energy change occurs for (a) and (b) in question 30? 34. Which elements have zero or negative electron affinities? 35. Why is there usually a decrease in the experimental values of the electron affinities the numbered families from the third through the sixth periods? 36. There is an increase in electron affinity between Groups III and IV. Explain why the addition of an electron to the atoms of these groups produces this result. 37. Of which group do the elements in each period have the highest electron affinities? 38. What are the present uses of the Periodic Table?

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