2. HistoryTrends Metals, nonmetals, metalloids Groups Periods Random 10 20 30 40 50

3. Question 1 - 10 The modern periodic table lists elements in order of increasing atomic________.

4. Answer 1 – 10 Number

5. Question 1 - 20 Describe Mendeleev’s periodic table.

6. Answer 1 – 20 He arranged elements in order of increasing atomic mass.

7. Question 1 - 30 Why is Mendeleev the “Father of the Modern Periodic Table” and not Meyer or both?

8. Answer 1 – 30 Mendeleev correctly predicted physical properties of three unknown elements.

9. Question 1 - 40 How did Moseley update the Periodic Table?

10. Answer 1 – 40 After calculating the atomic number of elements, he rearranged the PT by increasing atomic number.

11. Question 1 - 50 Assess the contributions of Mendeleev and Moseley to our modern understanding of the relationship between atomic structure and atomic behavior.

12. Answer 1 – 50 Mendeleev’s PT was able to show that groups/families of elements have similar properties depending on the size of the nucleus. (able to predict properties of atomic behavior based on guessed atomic mass) Moseley expanded upon Mendeleev’s ideas with atomic number (number of protons) defining an atom and its properties.

13. Question 2 - 10 What is the trend for metallic reactivity across a period? (for example from sodium, to magnesium, then aluminum?)

14. Answer 2 – 10 Chemical reactivity of metals generally decreases across a period.

15. Question 2 - 20 What is ionization energy?

16. Answer 2 – 20 Amount of energy needed to remove an electron to form a cation.

17. Question 2 - 30 Describe the trend across a period and down a group for electronegativity.

18. Answer 2 – 30 The trend across a period for electronegativity increases. It decreases as it goes down a group.

19. Question 2 - 40 What is the trend for atomic radius on the periodic table?

20. Answer 2 – 40 It decreases across a period and increases down a group.

21. Question 2 - 50 What is the trend for ionic radii (include both ions)?

22. Answer 2 – 50 The cation is smaller than its corresponding atom, and the anion is larger than its corresponding atom.

23. Question 3 - 10 Where are the metals located on the periodic table?

24. Answer 3 – 10 To the left and cover most of the periodic table.

25. Question 3 - 20 What type of element is Tungsten?

26. Answer 3 – 20 Transition metal

27. Question 3 - 30 Where are the nonmetals located on the periodic table?

28. Answer 3 – 30 To the right and above the staircase.

29. Question 3 - 40 Where are the metalloids located? Give me three examples.

30. Answer 3 – 40 On or below the staircase Any of these three: Boron, silicon, germanium, arsenic, antimony, tellurium, polonium

31. Question 3 - 50 What are three characteristics of a metal?

32. Answer 3 – 50 Shiny luster, malleable, high melting points, good conductors of heat and electricity, form cations

33. Question 4 - 10 What group is bromine in?

34. Answer 4 – 10 The halogens

35. Question 4 - 20 What is the name of the period that Uranium belongs to?

36. Answer 4 – 20 actinides

37. Question 4 - 30 What is the name of the most reactive metallic group?

38. Answer 4 – 30 Alkali metals

39. Question 4 - 40 What family does calcium belong to?

40. Answer 4 – 40 Alkaline earth metals

41. Question 4 - 50 Which group of elements is inert and why?

42. Answer 4 – 50 Noble gases, because they have full outermost energy levels (valence electrons)

43. Question 5 - 10 What does the A and B stand for in the group labels?

44. Answer 5 – 10 A= representative elements, B = transition elements

45. Question 5 - 20 Which element has the highest amount of electronegativity?

46. Answer 5 – 20 fluorine

47. Question 5 - 30 What is the definition for electronegativity?

48. Answer 5 – 30 An atoms ability to attract an electron (or electron pair) in a compound.

49. Question 5 - 40 What type of element is hydrogen?

50. Answer 5 – 40 Non-metal

51. Question 5 - 50 Why are the halogens the most reactive non- metals?

52. Answer 5 – 50 They only need one more electron to fill their outmost energy level.