1. 200 300 400 500 100 200 300 400 500 100 200 300 400 500 100 200 300 400 500 100 200 300 400 500 100 Periodic Table Trends Chemical Properties The d BlockPotpourri

2. In the Periodic Table, reading left to right, top to bottom, elements are arranged in order of 1-1

3. Atomic number or number of protons in the nucleus

4. An element has 13 electrons orbiting the nucleus. In which group of the periodic table will it be found 1-2

5. Group 3

6. How many electrons will chlorine have in its valence shell? 1-3

7. 7 valence electrons

8. 1-4 Give the symbol of an element in the same period and another element in the same group as Sulfur

9. Anything in period 3 and anything in group 16

10. 1-5 Give the names of groups 1,2,7, and 8

11. Alkali metals, Alkaline earth metals, halogens, and Noble gases

12. What element has the highest electronegativity? 2-1

13. Fluorine

14. 2-2 Which of the following has the smallest radius K K + Ca Ca 2+

15. Ca 2+

16. 2-3 How does electronegativity change going down a group and why?

17. Decreases going down a group because of shielding of the nucleus by inner energy levels

18. 2-4 How does atomic radius change going across a period and why?

19. Decreases as nuclear charge increases and nucleus-electron attraction increases

20. 2-5 How does the radius of an anion compare with its parent atom and how does the radius of a cation compare with its parent ion?

21. Anion:Larger Cation:Smaller

22. 3-1 What properties of the halogens increases from F to I

23. Atomic Radius or Melting Point

24. 3-2 What sort of compounds form when oxygen reacts with elements on the left side of the Periodic Table?

25. Ionic compounds (Ionically bonded Oxides)

26. 3-3 Name the following Compound KBr

27. Potassium Bromide

28. 3-4 Name the following Compound AlI 3

29. Aluminum Iodide

30. 3-5 When dissolved in water, oxides bonded to hydrogen atoms act as bases to give alkaline solutions. Write out the Chemical equation for this reaction

31. See notes

32. 4-1 What is a ligand? Give an example

33. Species that can donate a pair of non-bonding electrons, ammonia, water, cyanide ion

34. 4-2 Why are transition metals frequently colored?

35. Because of the movement of electrons between d-orbitals

36. 4-3 One of these things is not like the other: What d-block elements are not considered to be transition metals and why?

37. Sc and Zn. Scandium has only 1 d-block electron and can’t have multiple oxidation states, Zn has a full 10 d-block electrons.

38. 4-4 Give an example of an oxide that would be a solid and an oxide that would be a gas at room temperature

39. 1.Any ionically bonded oxide 2.Any covalently bonded oxide

40. 4-5 Give two examples of catalysts, one industrial, one biological

41. See book

42. 5-1 Cmpd/cmpds

43. Compound/Compounds

44. 5-2 sol’n/sol’ns

45. Solution/Solutions

46. 5-3 MP, BP

47. Melting point, boiling point

48. 5-4 RT

49. Room Temperature

50. 5-5 PToE

51. Periodic Table of the Elements

52. Final Jeopardy Carbon is bonded to F, Cl, I, and Br. Draw the stereoisomers of the structure showing they are mirror images of each other.