Periodic Trends



Periodic Trends Worksheet

1. Using the data in the table, plot the atomic radius vs the atomic number.

2. Using the data in the table, plot the 1st ionization energy vs the atomic number.

3. Using the data in the table, plot the electronegativity vs the atomic number.

Periodic Trends

|Element |Atomic Number |Atomic Radius (nm) |1st Ionization |Electronegativity |

| | | |Energy (kJ/mol) | |

|Hydrogen |1 |0.037 |1312 |2.1 |

|Helium |2 |0.050 |2372 |- |

|Lithium |3 |0.152 |519 |1.0 |

|Beryllium |4 |0.111 |900 |1.5 |

|Boron |5 |0.088 |799 |2.0 |

|Carbon |6 |0.077 |1088 |2.5 |

|Nitrogen |7 |0.070 |1406 |3.0 |

|Oxygen |8 |0.066 |1314 |3.5 |

|Fluorine |9 |0.064 |1682 |4.0 |

|Neon |10 |0.070 |2080 |- |

|Sodium |11 |0.186 |498 |1.0 |

|Magnesium |12 |0.160 |736 |1.2 |

|Aluminum |13 |0.143 |577 |1.5 |

|Silicon |14 |0.117 |787 |1.8 |

|Phosphorus |15 |0.110 |1063 |2.1 |

|Sulfur |16 |0.104 |1000 |2.5 |

|Chlorine |17 |0.099 |1255 |3.0 |

|Argon |18 |0.094 |1519 |- |

|Potassium |19 |0.231 |418 |0.9 |

|Calcium |20 |0.197 |590 |1.0 |

Conclusion

1. Examine the graph of atomic radius vs atomic number. Can a periodic trend be observed? If so, describe the trend.

2. For a given period, which group appears to have the largest atomic radii? Which group has the smallest?

3. Examine the graph of ionization energy vs atomic number. Can a periodic trend be observed? If so, describe the trend.

4. Which group or family has the highest ionization energies? Which group has the lowest?

5. Examine the graph of electronegativity vs atomic number. Can a periodic trend be observed? If so, describe the trend.

6. For a given period, which group appears to have the highest electronegativity? Which group has the smallest?

7. For the two groups you identified in question 4, draw a connection between ionization energy and the electron configuration.

8. In the graph of ionization energy vs atomic number, why are peaks observed for the noble gases?

9. Examine the graph of ionization energy vs atomic number. Use electron configuration to explain the decreases noted between beryllium and boron, nitrogen and oxygen, magnesium, and aluminum, and phosphorus and sulfur.

10. In the space below, sketch the plot you made of first ionization energy vs atomic number. (Just the shape of the curve). Add a second line, indicating the shape you think the plot would look like for the second ionization energies of the same elements. (The second ionization energy is the amount of energy required to remove a second electron from an atom). Explain your predictions.

[pic]

11. Based on your findings in question 10, how many electrons are the following atoms likely to gain or lose to attain a stable electron configuration?

Oxygen gain or lose __________ electrons

Potassium gain or lose __________ electrons

Chlorine gain or lose __________ electrons

Lithium gain or lose __________ electrons

Neon gain or lose __________ electrons

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