1. 4: Blocks of the Periodic table
h. demonstrate an understanding that electronic structure determines the chemical properties of an element
i. recall that the periodic table is divided into blocks, such as s, p and d

3. Periodic Table
The way an element reacts is particularly determined by the outermost (valence) electrons of an atom.
The Periodic table arranges the elements in order of their atomic number.
The vertical columns are called GROUPS and the horizontal rows are called PERIODS.
All elements in same group have the same number of outermost electrons.
All the elements in same period have the same number of electron shells.

4. Periodic Table and Electron Configurations
Elements in the s block have outer electrons in s subshell, Elements in the p block have outer electrons in p subshells and so on for d and f block.
Elements in same GROUP have the same outer shell electron configuration.
Elements in same PERIOD have the same number of electron shell.
s - block
p - block
d - block
f - block

5. Representative and Transition elements
6.2
In this periodic table, the colors of the boxes are used to classify representative elements and transition elements.

6. Task 1
Task 1: Answer the following questions in full sentences 1 2 3

7. Electron Configurations in Groups
6.2
The Noble Gases
The noble gases are the elements in Group 8 or 0 of the periodic table. The electron configurations for the first four noble gases in Group 8 or 0 are listed below.
Noble gases have electronic structures with full subshells. This explains why they have exceptionally high Ionisation energy.
This confirms that this electronic configuration is particularly stable one and helps to explain why Noble gases rarely react with other chemicals.

8. Electron Configurations in Groups
6.2
Electron Configurations in Groups
The Representative Elements
Elements in groups 1 to 7 are often referred to as representative elements because they display a wide range of physical and chemical properties.
The s and p sublevels of the highest occupied energy level are not completely filled.

9. Electron Configurations in Groups
6.2
Electron Configurations in Groups
In atoms of the Group 1 elements below, there is only one electron in the highest occupied energy level.
In atoms of the Group 4 elements below, there are four electrons in the highest occupied energy level.
Group 1 have electronic structures with partly filled subshells. This explains why they have low Ionisation energy.
This helps to explain why Group 1 elements are highly reactive.

10. s – block elements They have the outermost electrons in s subshell.
The s- block includes the METALS like Lithium, Sodium, Potassium, Magnesium and Calcium which are very reactive.
They have low ionization energy and have tendency to loose valence electrons to acquire a stable electronic configuration. (+ ions)

11. s – block elements
They form stable IONIC compounds with non-metals by giving away their outermost electrons.
They have lower melting point, boiling point and lower densities.
They are good conductors of electricity as they have metals in the sea of electrons – metallic bond
H and He are s- block elements but due to their non-metal like properties they are called non-metals.

12. p – block elements
The p- block elements are those in group 3,4,5,6,7and 8.
Electrons are being added to p subshell.
It contains metals, non-metals and metalloids.
Tin and lead are the p block metals. They have low metallic characteristics but they are good conductors of heat and electricity. They are relatively unreactive.

13. p – block elements Metalloids occur in a diagonal block.
They act like non-metals in most ways but they are conductors of electricity.
Silicon and Germanium are used widely for microchips.
Noble gases in group 8 are extremely unreactive.
A few compounds are made of Xenon.

14. p – block elements The non-metals form Ionic bonds with metals.
They make COVALENT BONDS with other Non-metals.
They can be solid, liquid or gas (halogens, Noble gases).
They are poor conductor of electricity.

15. d – block elements
The d- block lies between group 2 and 3 and contains elements with successive electrons being added in d orbitals.
They are called TRANSITION ELEMENTS.
They include Copper, Zinc, Iron, Silver, Gold that are much less reactive than s-block elements because inner d orbitals are being filled while outer s subshell is full.
They all conduct heat and electricity and are mostly shiny, malleable and ductile.
Mercury is an exception with low melting point and is a liquid.

16. f – block elements
In f- block elements successive electrons are filled in f subshells.
The top row is called LANTHANIDES after Lanthanum and the second row is called ACTINIDES after Actinium.
Actinides are all radioactive.

17. Homework Homework task: Due date: Criteria for Grade C:
Criteria for Grade B:
Criteria for Grade A/A*: