1. Periodic Trends
Chp 6

2. Atomic Radii
Ionization Energy
Electronegativity

3. Look at the graph to answer the questions:
What happens to Atomic Radius for the elements in period 2 as Atomic Number increases?
What happens to Atomic Radius for the elements in period 3 as Atomic Number increases?
What can we conclude from the data?

4. Look at the graph to answer the questions:
What happens to Atomic Radius for the elements in period 2 as Atomic Number increases?
Atomic radius decreases (size decreases)
What happens to Atomic Radius for the elements in period 3 as Atomic Number increases?
What can we conclude from the data?
Moving across a period we see a trend of atomic size decreasing.

5. Look at the graph to answer the questions:
What happens to Atomic Radius for the elements in group 1 as Atomic Number increases?
What happens to Atomic Radius for the elements in group 7 as Atomic Number increases?
What can we conclude from the data?

6. Look at the graph to answer the questions:
What happens to Atomic Radius for the elements in group 1 as Atomic Number increases?
Atomic radius increases (size increases)
What happens to Atomic Radius for the elements in group 7 as Atomic Number increases?
What can we conclude from the data?
Moving down a column we see a trend of atomic size increasing.

7. Atomic Radii (Size) Trend Explanation
Atomic Radii decrease across a period because more protons increase the nuclear charge and electrons pulled closer to nucleus
Atomic Radii increase down a group because more Energy levels increases distance between nucleus and valence electrons

8. Look at the graph to answer the questions:
What happens to Ionization Energy for the elements in period 2 as Atomic Number increases?
What happens to Ionization Energy for the elements in period 3 as Atomic Number increases?
What can we conclude from the data?

9. Look at the graph to answer the questions:
What happens to Ionization Energy for the elements in period 2 as Atomic Number increases?
Ionization Energy Increases (more energy needed to remove electrons)
What happens to Ionization Energy for the elements in period 3 as Atomic Number increases?
Ionization Energy increases (more energy needed to remove electrons)
What can we conclude from the data?
As we move across a period, more ionization energy is needed to remove an electron from an atom.

10. Look at the graph to answer the questions:
What happens to Ionization Energy for the elements in group 1 as Atomic Number increases?
What happens to Ionization Energy for the elements in group 7 as Atomic Number increases?
What can we conclude from the data?

11. Look at the graph to answer the questions:
What happens to Ionization Energy for the elements in group 1 as Atomic Number increases?
Ionization Energy decreases (less energy needed to remove an electron)
What happens to Ionization Energy for the elements in group 7 as Atomic Number increases?
What can we conclude from the data?
As we move down a group, less energy is needed to remove an electron from an atom.

12. Ionization Energy Trend Explanation
Ionization Energy increases across a period because more protons increase the nuclear charge and more Energy is required to remove electrons
Ionization Energy decreases down a group because more Energy levels increase distance between nucleus and outer valence electrons (nucleus is shielded) so less Energy is required to remove electrons

13. Look at the graph to answer the questions:
What happens to Electronegativity for the elements in period 2 as Atomic Number increases?
What happens to Electronegativity for the elements in period 3 as Atomic Number increases?
What can we conclude from the data?

14. Look at the graph to answer the questions:
What happens to Electronegativity for the elements in period 2 as Atomic Number increases?
Electronegativity increases (more attraction for electrons)
What happens to Electronegativity for the elements in period 3 as Atomic Number increases?
What can we conclude from the data?
Moving across a row increases the attraction for electrons

15. Look at the graph to answer the questions:
What happens to Electronegativity for the elements in group 1 as Atomic Number increases?
What happens to Electronegativity for the elements in group 7 as Atomic Number increases?
What can we conclude from the data?

16. Look at the graph to answer the questions:
What happens to Electronegativity for the elements in group 1 as Atomic Number increases?
Electronegativity decreases (attraction for electrons decreases)
What happens to Electronegativity for the elements in group 7 as Atomic Number increases?
What can we conclude from the data?
Moving down a group decreases the attraction for electrons

17. Electronegativity Trend Explanation
Electronegativity increases across a period because more protons increase the nuclear charge and atom has stronger attraction for electrons
Electronegativity decreases down a group because more Energy levels cause nuclear charge to be shielded and decreases atom's ability to attract electrons

18. electronegativity