1. The Periodic Table Classifying the Elements
In the periodic table:
The elements are arranged in order of increasing proton number
The vertical columns of elements with similar properties are called groups
The horizontal rows are called periods
Distinction in the table
METALS NON-METALS
Most of elements Fewer than metals
Particular type of bonding Much wider range of properties
They are divided by a line

4. DIFFERENCE BETWEN METALS AND NON-METALS

5. GROUPS AND PERIODS IN THE PERIODIC TABLE
MAIN-GROUP ELEMENTS
TRANSITION ELEMENTS
NOBLE GASES
Elements present in group I to VIII
These vertical groups have similar chemical and physical properties
Elements present between groups II and III
The first row occurs in period 4
Elements present in group VIII
The least reactive elemets
Group I : alkali metals, the most reactive metals
Group VII : halogens next to noble gases
In centre of the table there are the most unreactive elements

6. GROUP I: THE ALKALI METALS
They are soft solids with low melting point and low densities.
They are highly reactive
They have a silvery surface
The physical properties change as we go down the group
They react VIGOROUSLY with WATER to produce:
Increases as we go down the group
quickly tarnishes
Became dull
melting points become lower
density increases
HYDROGEN
ALKALINE SOLUTION

7. GROUP VII: THE HALOGENS
The most reactive non-metals
Their reactivity decreses down the group
They are all poisonous
They all form diatomic molecules
They all have a valency of 1
Their compounds with hydrogen are usually strong acids when dissolved in water
Each of them produces a series of compounds with other elements
They can react directly with metals to form salts
They all form negative ions carrying a single charge

8. GROUP VIII: THE NOBLE GASES
A whole group of elements remain to be discovered
They are present in Earth’s atmosphere
They are particulary unreactive
They were refered to as the inert gases
Their melting points and boiling points are extremely low
The electron arrangements of atoms are very stable
They are between the two most reactive groups of elements (groups I and VII)
So they don’t react readily with other atoms
The group VII elements gain or share electrons and the group I elements lose electrons to reach a noble gas electron arragement

9. What is an electron Configuration?
An electron configuration is a shorthand description of how electrons are arranged around of an atom.
They are important because they help us predict chemical behavior:
We can predict if two elements:
• will react or not
• what kind of reaction we are likely to have
• how strong the reaction will be

10. • Every element on the periodic table consists of atoms, composed of protons, neutrons and electrons (electrons exhibit a negative charge and are found around the nucleus of the atom in electron orbitals).
• The four different types of orbitals (s, p, d, f) have different shapes, and one orbital can hold a maximum of two electrons.
The p, d, f orbitals have different sublevels, thus can hold more electrons.

11. The Electron Configuration of each element is unique to its position on the periodic table. The energy level is determined by the period (from 1 to 7) and the number of electrons is given by the atomic number. Orbitals on different energy levels are similar to each other, but they occupy different areas in space.
The s-block is the region of alkali metals including helium (Groups I-II) The d-block are the transition metals The p-block are the main group elements (Groups III-VIII) The f-block are the lanthanides and actinides series.