1. What are the period and group trends of different properties?
Periodic Trends
Essential Questions:
What are the period and group trends of different properties?
How are period and group trends in atomic radii related to electron configuration?

2. What is a periodic trend?
The predictable change the elements show when you move across a period or down a group/family

3. Atomic Radius
Is defined by how closely an atom lies to a neighboring atom
The size of the atom can vary depending on what other element its bonded to
Atomic radius decreases across a period and up a group/family

5. Atomic Radius within a Period
As you move across a period the atomic radius decreases
As you move across the period you are adding an extra proton and an extra electron. The nucleus has an increasing nuclear charge and the extra electron arranges itself into the same energy level.
As the positive charge increases in the nucleus the electrons are pulled closer to the nucleus

6. Atomic Radius within a group/family
Increases down a group/family
Increasing positive charge in the nucleus but the extra electrons are arranged into the next energy level.

7. Ionic Radius Anions: gain electrons so they become larger because
Cations: lose electrons and form positively charged ions, they always become smaller because
1) physically losing electrons
2) the increased positive charge pulls the other electrons closer to itself.
Anions: gain electrons so they become larger because
Adding an extra electron causes electrostatic repulsion to increase making them spread apart
Ionic Radius

10. Ionization Energy
Is the energy required to remove an electron from a gaseous atom
Removing electrons
1st ionization energy = 1 electron
2nd ionization energy = 2 electrons
3rd ionization energy = 3 electrons
*2nd & 3rd … ionization energies require significantly more energy

13. Electronegativity
Is the ability of an atom to attract an electron to it’s chemical bond

14. Octet Rule
Atoms in the s and p blocks want to be like the noble gases and have a full set of valence electrons
They will gain/lose or share electrons to have 8 electrons in the outer shell.
Exceptions to the octet rule are in d and f block

15. Octet Rule S block elements will give up their electrons
P block elements will take up electrons
Octet rule helps us determine the kind of bond formed.

16. Summary
Atomic Size decreases left to right on a period and up a family
Ionic size, ionization energy, and electronegativity increase left to right a period and up a family.
The octet rule states that atoms gain, lose or share electrons to acquire a full set of eight valence electrons

17. Review Questions:
How are the period and group trends in atomic radii related to electron configuration?
Atomic radii increase down a group b/c of increasing energy levels. And decrease across a period because of the stronger positive pull from the positively charged nucleus pulling the electrons closer

18. Review Questions: F, Br, F, F A tale of 2 elements:
Flourine or Bromine
Which has a larger electronegativity:
Which has a larger atomic radius:
Which has a smaller Ionic radius:
Which has a larger ionization energy:
F, Br, F, F

19. Practice Problems:
Which has the largest atomic radius: Mg, Si, S or Na? the smallest?
Na (largest)
S (smallest)

20. Practice Problems cont’d
Draw spheres to show the respective sizes of Helium, Krypton, and Radon

21. Practice Problems
Can you determine which of 2 unknown elements has the larger radius if the only known information is that the atomic number is of one of the elements is 20 greater than the other? Explain.

22. Review Questions:
Why would it be harder to remove the second electron from lithium than it is to remove a fourth electron from carbon?
Because Lithium’s second removed electron is an inner core electron, not a valence electron. Carbon’s fourth removed electron is still a valence electron