2. FJ
Old Stuff
Electronegativity
Ionization
Miscellaneous
Atomic Radius
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3. Give two examples of elements that are halogens
400 old stuff
Give two examples of elements that are halogens
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4. asdgjks
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5. ID the element a metal, nonmetal, or metalloid
800 old stuff
ID the element a metal, nonmetal, or metalloid Ge
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6. Metalloid?
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7. What type of ion do the halogens form and why?
1200 old stuff
What type of ion do the halogens form and why?
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8. -1 anion, want to gain 1 e- to be stable
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9. What is coulombs attraction?
1600 old stuff
What is coulombs attraction?
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10. Discusses the pull between the positively charged nucleus and the negatively charged electrons
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11. Discuss the importance of Mendeleev’s periodic law
2000 Old Stuff
Discuss the importance of Mendeleev’s periodic law
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12. He arranged the elements by atomic mass and noticed repeating trends
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13. Electronegativity is defined as this.
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14. What is how likely an atom is to “steal” another’s electron/tendency to attract electrons?
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15. 800 Electronegativity
Describe the trend for Electronegativity as you go across and from top to bottom on the periodic table.
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16. What is increases across a period due to the increased number of protons and decreases down a group due to the addition of energy levels?
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17. Which atom has a larger electronegativity?
S or Al
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18. What is S?
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19. Which element is less likely to steal electrons while bonding?
1600 Electronegativity
Which element is less likely to steal electrons while bonding?
Na or Cl
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20. What is Na.
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21. 2000 Electronegativity
Rank the following set of atoms from lowest to highest electronegativity
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22. Ne/C/O
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23. Define Ionization Energy
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24. What is the energy required to remove an electron
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25. 800 Ionization
Describe the trend for Ionization as you go across and from top to bottom on the periodic table
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26. What is increases across because of the increased proton electron attraction and down decreases because of the addition of energy levels and shielding effect
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27. Which element has a larger first ionization energy?
Sodium or potassium
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28. What is sodium?
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29. Which element has a larger first ionization energy?
Magnesium or Phosphorus
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30. Phosphorus
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31. Which element Ba or Cu has a larger ionization energy?
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32. What is Cu.
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33. 400 Atomic Radius
Define atomic radius.
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34. What is size of the atom/ distance between two nuclei of the same atom?
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35. 800 Atomic Radius
Describe the trend for Atomic Radius as you go across and from top to bottom on the periodic table
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36. What is decreases across due to the increased protons and attraction with the electrons and increases as you go down because the addition of energy levels
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37. Which element has a larger atomic radius?
Sodium, lithium
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38. What is sodium?
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39. Which element has a larger atomic radius?
Strontium, magnesium
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40. What is strontium?
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41. Which element has a larger atomic radius?
Carbon or Germanium
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42. What is germanium?
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43. What are valence electrons and why are they so important?
400 Misc.
What are valence electrons and why are they so important?
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44. Electrons in the outermost shell; they are important because they are the electrons involved in BONDING
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45. 800 Misc.
Why are noble gases not considered when we talk about electronegativity?
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46. What is they already have a full outer shell of electrons
What is they already have a full outer shell of electrons! – they don’t want to bond with other atoms. All other atoms to “act” like them!
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47. What is an ion? What are the two types of ions? How are they formed?
1200 Misc.
What is an ion? What are the two types of ions? How are they formed?
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48. Ion is a charged atom. Two types: cation/anion
Ion is a charged atom. Two types: cation/anion. Cation formed by the loss of electrons from metals, Anions are formed from the gain of electrons from non-metals
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49. Which atom has a greater atomic radius, Mg or Mg 2+?
1600 Misc.
Which atom has a greater atomic radius, Mg or Mg 2+?
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50. What Mg because the cation loses electrons making the atom smaller?
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51. List the names of the following groups on the P.T.
2000 Misc.
List the names of the following groups on the P.T.
-Group #1 -Group #2
-Group #7 -Group #8 .
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52. #2 Alkaline Earth Metals,
What are:
#1 – Alkali Metals,
#2 Alkaline Earth Metals,
#7 – The Halogens,
#8 – The Noble Gases?
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53. Daily Double 1

54. Explain the differences between condensation, sublimation, melting, and freezing
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55. Condensation is gas turning to a liquid, sublimation is a solid to a gas, melting is a solid to a liquid and freezing is a liquid to a solid
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56. Daily Double 2

57. In the phase change diagram below, this is the reason there is a constant temperature between the solid and liquid phases.
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58. What is because the temperature stays constant until all the bonds of the solid are broken and the substance has changed to a liquid?
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59. Final Jeopardy Category

60. Label and explain what is happening in each step