1. Section 4.5—Periodicity – Notable trends of the table

2. What is periodicity on the periodic table?
The predictable pattern by which properties of elements change across or down the periodic table.
There are always exceptions to these periodicity trends…each of the trends is a “general” trend as you move across a period or down a group.

3. Trend 1: Atomic Radii

4. What is atomic radius?
Half of the distance between the nuclei of two bonded atoms. H
Distance between nuclei
Atomic radius of hydrogen atom

5. Atomic Radii Trends Radius in picometers
What happens to the radius as you go down a group?
It Increases!
What happens to the radius as you across a period?
It Decreases!

6. Atomic Radii Trends Reasoning, Part 1
Why do atomic radii decrease across a period?
Moving left to right, the number of protons, neutrons and electrons all increase. e e
Move across the
periodic table e e n p n e e p p p n p p n
Radius decreases n n p n e
Lithium atom
Beryllium atom
As the # of protons and neutrons increase, the attraction between the positive nucleus and negative electron cloud increases.
This attraction “pulls” in on the electrons. Think of this as being similar to how larger planets have a greater pull on their objects! 

7. Atomic Radii Trends Reasoning, Part 2
Why do atomic radii increase down a group?
Protons, neutrons and electrons are also added as you move down a group. + e e +
Move down the
periodic table
Radius increases
Lithium atom
Sodium atom
However, the electrons are added in new energy levels.
The inner electrons “shield” the new outer electrons from the pull of the nucleus, therefore it doesn’t pull in like the last slide.

8. Trend 2: Ionization Energy

9. What is Ionization Energy?
The energy needed to remove the outermost electron.

10. Ionization Energy Trends
Ionization Energy in kJ/mole
What happens to the ionization energy as you go down the group?
It Decreases!
What happens to the ionization energy as you go across a period?
It Increases!

11. Ionization Energy Trends Reasoning, Part 1
Why does Ionization Energy increase across a period?
Moving left to right, the radius of the atom decreases as more protons pull on more electrons.
Move across the
periodic table e e e e n p n e e p
Radius decreases p p n p p n n n p n e
IE increases
Lithium atom
Beryllium atom
When an atom is smaller, the electrons are closer to the nucleus, and therefore feel the pull more strongly.
It is harder to pull electrons away from these smaller atoms.

12. Ionization Energy Trends Reasoning, Part 2
Why does ionization energy decrease down a group?
As you move down a group, the radius increases as more electrons shells are added. + e e +
Move down the
periodic table
Radius increases
IE decreases
Lithium atom
Sodium atom
As the outer electrons (those involved in bonding) are farther from the nucleus, they will feel the “pull” of the nucleus less.
It is easier to remove an electron from a larger atom.

13. Trend #3: Electron Affinity

14. What is Electron Affinity?
Energy released when an electron is added to an atom

15. Electron Affinity Trends
Electron Affinity in kJ/mol
What happens to the value of electron affinity as you go down a group?
It gets less negative therefore it get less favorable.
What happens to the value of electron affinity as you go left to right?
It gets more negative therefore it get more favorable.

16. Electron Affinity Trends Reasoning, Part 1
Why does Electron Affinity increase across a period?
Moving left to right, the radius of the atom decreases as more protons pull on more electrons.
Move across the
periodic table e e e e n p n e e p
Radius decreases p p n p p n n n p n e
EA increases
Lithium atom
Beryllium atom
When an atom is smaller, the electrons are closer to the nucleus, and therefore feel the pull more strongly.
A smaller atom can handle an extra electron more easily as it can be more “controlled” by the closer nucleus

17. Electron Affinity Trends Reasoning, Part 2
Why does electron affinity decrease down a group?
As you move down a group, the radius increases as more electrons shells are added. + e e +
Move down the
periodic table
Radius increases
EA decreases
Lithium atom
Sodium atom
As the outer electrons (those involved in bonding) are farther from the nucleus, they will feel the “pull” of the nucleus less.
The larger atom is less able to “control” a new electron added.

18. Ionic Charge & Radii

19. Review Some Definitions
Ion – atom with a charge.
Cation – positively charged ion. Results from loss of electrons.
Anion – negatively charged ion. Results from gain of electrons.

20. Ionic Radii—Cations
How does the radius of a cation compare to the parent atom?
Atoms lose electrons to create positive ions e +
Creating a cation,
losing electrons e +
Radius decreases
Lithium atom
Li+ ion
When electrons are lost, there are now more protons than electrons
Therefore, the protons have a greater “pull” on each of the electrons.

21. Ionic Radii—Anions
How does the radius of an anion compare to the parent atom?
Atoms gain electrons to create negative ions e + e
Creating an anion,
gaining electrons e e e e e +
Radius increases e e e e
Oxygen atom
O2- ion
When electrons are gained, there are now more electrons than protons
Therefore, the protons have a weaker “pull” on each of the electrons.

22. Summary Chart for Trends
Summary Chart for Trends! If you know radius – the other two are opposite!

23. Let’s Practice Example: List Li, Cs and K in order of increasing
Atomic radii
Ionization Energy
Electron Affinity
Example:
List Li, N and C in order of increasing
Atomic radii
Ionization Energy
Electron Affinity

24. Let’s Practice Example: List Li, Cs and K in order of increasing
Atomic radii
Ionization Energy
Electron Affinity
Li, K, Cs
Cs, K, Li
Example:
List Li, N and C in order of increasing
Atomic radii
Ionization Energy
Electron Affinity
N, C, Li
Li, C, N