1. Trends of the periodic table

2. How are ionization energy and electron affinity related
How are ionization energy and electron affinity related? Why is this relationship important?

3. Periodic Trends
There are several important atomic characteristics that show predictable trends that you should know.
The first and most important is atomic radius.
Radius is the distance from the center of the nucleus to the “edge” of the electron cloud.

4. } Periodic Trends Radius
How do they measure it when the electron cloud has no definite edge?
Measure the Atomic Radius - this is half the distance between the two covalent radii nuclei of a diatomic molecule.
Atomic radii are usually measured in picometers (pm) or angstroms (Å). An angstrom is 1 x m. }
Radius

5. Covalent Radius
Two Br atoms bonded together are 2.86 angstroms apart. So, the radius of each atom is 1.43 Å.
2.86 Å
1.43 Å

6. Atomic Radius The trend across a horizontal period is less obvious.
What happens to atomic structure as we step from left to right?
Each step adds a proton and an electron (and 1 or 2 neutrons).
Electrons are
added to existing
Principle energy
level.

7. Atomic Radius
The effect is that the more positive nucleus has a greater pull on the electron cloud.
The nucleus is more positive and the electron cloud is more negative.
The increased
attraction pulls
the cloud in,
making atoms
smaller as we move
from left to right
across a period.

8. Effective Nuclear Charge
What keeps electrons from simply flying off into space?
Effective nuclear charge is the pull that an electron “feels” from the nucleus.
The closer an electron is to the nucleus, the more pull it feels.
As effective nuclear charge increases, the electron cloud is pulled in tighter.

9. Atomic Radius H Li Na K Rb
As we increase the atomic number (or go down a group). . .
each atom has another energy level,
so the atoms get bigger. Li Na K Rb

10. Atomic Radius Na Mg Al Si P S Cl Ar
Going from left to right across a period, the size gets smaller.
Electrons are in the same energy level.
But, there is more nuclear charge.
Outermost electrons are pulled closer. Na Mg Al Si P S Cl Ar

11. Atomic Radius Here is an animation to explain the trend.
Decreases left to right
Increases
top to
bottom

12. Shielding
As more principle energy levels are added to atoms, the inner layers of electrons shield the outer electrons from the nucleus.
The effective nuclear charge (enc) on those outer electrons is less, and so the outer electrons are less tightly held.

13. Ionization Energy This is the second important periodic trend.
If an electron is given enough energy (in the form of a photon) to overcome the effective nuclear charge holding the electron in the cloud, it can leave the atom completely.
The atom has been “ionized” or charged.
The number of protons and electrons is no longer equal.

14. Ionization Energy
The energy required to remove an electron from an atom is ionization energy. (measured in kilojoules, kJ)
The larger the atom is, the easier its electrons are to remove.
Ionization energy and atomic radius are inversely proportional.
Ionization energy is always endothermic, that is energy is added to the atom to remove the electron.

15. Ionization Energy
Decreases
top to
bottom
Increases left to right

16. Electron Affinity What does the word ‘affinity’ mean?
Electron affinity is the energy change that occurs when an atom gains an electron (also measured in kJ).
Where ionization energy is always endothermic, electron affinity is usually exothermic, but not always.

17. Electron Affinity
Electron affinity is exothermic if there is an empty or partially empty orbital for an electron to occupy.
If there are no empty spaces, a new orbital or PEL must be created, making the process endothermic.
This is true for the alkaline earth metals and the noble gases.

18. Electron Affinity
Decreases
top to
bottom
Increases left to right

19. Electronegativity
Electronegativity is a measure of an atom’s attraction for another atom’s electrons.
It is an arbitrary scale that ranges from 0 to 4.
The units of electronegativity are Paulings.
Generally, metals are electron givers and have low electronegativities.
Nonmetals are electron takers and have high electronegativities.
What do you think the noble gases electronegativity looks like?

21. Overall Reactivity
This ties all the previous trends together in one package.
However, we must treat metals and nonmetals separately.
The most reactive metals are the largest since they are the best electron givers.
The most reactive nonmetals are the smallest ones, the best electron takers.

22. Overall Reactivity

23. Ions
When an atom gains an electron, it becomes negatively charged (more electrons than protons ) and is called an anion.
In the same way that nonmetal atoms can gain electrons, metal atoms can lose electrons.
They become positively charged cations.

24. Ionic Radius Cations are always smaller than the original atom. Li Li+
The entire outer PEL is removed during ionization.
Conversely, anions are always larger than the original atom.
O O
Electrons are added to the outer Principle Energy Level.

25. Ion Group trends Each step down a group is adding an energy level
Ions therefore get bigger as you go down, because of the additional energy level.
Li1+
Na1+
K1+
Rb1+
Cs1+

26. Ion Period Trends
Across the period from left to right, the nuclear charge increases - so they get smaller.
Notice the energy level changes between anions and cations.
N3-
O2-
F1-
B3+
Li1+
Be2+
C4+