1. Unit 3 Part 3: Periodic Trends

2. Outline Development of the Periodic Table
Parts of the Modern Periodic Table
Representative elements, transition elements
Metals, nonmetals and metalloids
Classification of elements using electron configuration
Valence electrons and period
S, p, d, f blocks
Periodic Trends
Atomic radius, ionic radius
Ionization energy
Electronegativity

3. Development of the Periodic Table
Newlands
Meyer and Mendeleev
Moseley

4. Parts of the Modern Periodic Table
Representative elements: groups 1-2 and 13-18
Transition elements: groups 3-12
Elements are classified as metals, metalloids and nonmetals.

5. Parts of the Modern Periodic Table
Metals:
Shiny
Good conductors of electricity and heat
Malleable: can be shaped into many shapes
Ductile: can be drawn into wires

6. Parts of the Modern Periodic Table
Special metals:
Group 1 elements are called alkali metals. They are very reactive. Eg.
Group 2 elements are called alkaline earth metals. They are also very reactive. Eg.

7. Parts of the Modern Periodic Table
Transition metals:
Transition metals: Groups 3-12
Inner transition metals: lanthanide series and actinide series.

8. Parts of the Modern Periodic Table
Nonmetals:
Gas, solid, or liquid.
Brittle
Poor conductors of heat and electricity
Eg. Group 17: Halogens
Eg. Group 18: Noble gases

9. Parts of the Modern Periodic Table

10. Parts of the Modern Periodic Table
Metalloids:
Properties of both metals and non metals
Eg. Silicon, Si:

11. Using Electron Configuration
Electron configuration determines the chemical properties of an element.
Valence electrons are electrons in the highest principal energy level of an atom.
Atoms in the same group have similar chemical properties because they have the same number of valence electrons.
Eg. Group 1

12. Using Electron Configuration
Each of the representative groups (column in groups 1,2 and 13 to 18) has its own valence electron configuration.
Valence electrons and period:
The principal energy level of an element’s valence electrons = the period of the periodic table that the element is in. Eg.

13. Using Electron Configuration
s-block, p-block, d-block, and f-block elements
The periodic table has columns and rows of varying sizes.
This is because the table has been divided into sections, or blocks, representing the valence electrons’ sublevels. (ie. s, p, d, or f)

14. Using Electron Configuration
1. Which groups are the s-block elements? What do the valence electrons for these groups look like? Why are there only two groups in the s-block?
2. Which groups are the p-block elements? Why are there no p-block elements in period 1? Why are there six groups in the p-block?
3. What is a characteristic of the d-block? Example: Why are there ten groups in the d-block?
4. Which groups make up the f-block elements? Why are there 14 groups in the f-block?

15. Periodic Trends: Atomic Radius
Many properties change in a predictable way.
This pattern is called a trend.
An atom’s radius is defined by how close it can get to another atom.
This is because an atom has no clearly defined edge.

16. Periodic Trends: Atomic Radius
A metal atom’s radius is defined as half the distance between neighboring nuclei in a crystal structure.
A nonmetal’s atomic radius is defined as half the distance between nuclei of identical atoms that are bonded together.

17. Periodic Trends: Atomic Radius
The atomic radius decreases across a period.
This is because of an increasing positive charge in the nucleus, and also because the principal energy level within a period remains the same.
No additional electrons come between the valence electrons and the nucleus.

18. Periodic Trends: Atomic Radius
The atomic radius increases down a group.
Electrons are added to orbitals in higher principal energy levels =further from the nucleus.
The orbitals between the nucleus and the outer electrons shield the outer electrons from the nucleus.

19. Periodic Trends: Atomic Radius
P. 189 Q16-19

20. Periodic Trends: Ionic Radius
Atoms can gain or lose electrons to form a charged version of itself, which is called an ion.
When atoms lose electrons, they form _______________ ions called cations.
When atoms gaim electrons, they from _______________ ions called anions.

21. Periodic Trends: Ionic Radius
Atoms can gain or lose electrons to acquire a full set of eight valence electrons.
This is called the octet rule.
This is because the electron configuration of filled s and p orbitals of the same energy level is very stable.
Exception: period 1 elements. They are complete with only two valence electrons.

22. Periodic Trends: Ionic Radius
Positively charged ions:
Smaller than the “parent” atom.
Because:
1. The lost electron is a valence electron (in the outer shell) so the ion’s radius is smaller than before.
2. Less electrostatic repulsion because there are fewer electrons. So the remaining electrons experience a greater pull to the positively charged nucleus.

23. Periodic Trends: Ionic Radius
Negatively charged ions:
Larger than the “parent” atom.
Because:
More electrostatic repulsion because there are more electrons, which forces them to move further apart. The increased distance between the outer electrons results in a larger radius.

24. Periodic Trends: Ionic Radius

25. Periodic Trends: Ionic Radius
Across a period: Ionic radius decreases.
Down a group: Ionic radius increases (electrons are in higher principal energy levels = bigger radius)

26. Periodic Trends: Ionization Energy
Energy required to remove an electron from a gaseous atom.
First ionization energy:
Second ionization energy:
High ionization energy means _________
Low ionization energy means __________

27. Periodic Trends: Ionization Energy

28. Periodic Trends: Ionization Energy
Across a period: ionization energies usually increase.
Down a group: ionization energies usually decrease.
Jump in ionization energies after all the valence electrons are removed.

29. Periodic Trends: Electronegativity
The ability of an atom to attract electrons in a chemical bond.

30. Periodic Trends: Electronegativity
Across a period: increases
Down a group: decreases