Periodic Trends (CIE IGCSE Chemistry: Co-ordinated Sciences (Double Award))

• The metallic character of the elements decreases as you move across a period on the Periodic Table, from left to right, and it increases as you move down a Group
• This trend occurs due to atoms more readily accepting electrons to fill their outer shells rather than losing them to have the previous, already full, electron shell as their outer shell
• Metals occur on the left-hand side of the Periodic Table and non-metals on the right-hand side
• Between the metals and the non-metals lie the elements which display some properties of both
• These elements are referred to as metalloids or semi-metals

Properties of metals and non-metals

Property	Metal	Non-metal
Electron arrangement	1-3 outer shell electrons (more in Periods 5+ 6)	4-7 electrons in the outer shell
Bonding	metallic	covalent
Electrical conductivity	good conductors	poor conductors
Type of oxide	basic oxide	acidic oxides
Reaction with acids	many react with acids	do not react with acids
Physical characteristics	malleable high melting and boiling point	brittle low melting and boiling point

A zig-zag line in this diagram separates the metals on the left, from the non-metals on the right

• The electronic configuration is the arrangement of electrons into shells for an atom 
  • E.g. the electronic configuration of carbon is 2,4
• There is a link between the electronic configuration of the elements and their position on the Periodic Table
• The number of notations in the electronic configuration will show the number of occupied shells of electrons the atom has, showing the period
• The last notation shows the number of outer electrons the atom has, showing the group number

Example:  Electronic configuration of chlorine:

The electronic configuration of chlorine as it should be written

 

Period: The red numbers at the bottom show the number of notations which is 3, showing that a chlorine atom has 3 shells of electrons.

Group: The final notation, which is 7 in the example, shows that a chlorine atom has 7 outer electrons and is in Group VII

The position of chlorine on the Periodic Table

 

• Elements in the same group in the Periodic Table have similar chemical properties
• When atoms collide and react, it is the outermost electrons that interact
• The similarity in their chemical properties stems from having the same number of electrons in their outer shell
• For example, both lithium and sodium are in Group 1 and can react with elements in Group 7 to form an ionic compound by reacting in a similar manner 
• As you look down a group, a full shell of electrons is added to each subsequent element
  • Lithium's electronic configuration: 2,1
  • Sodium's electronic configuration: 2,8,1
  • Potassium's electronic configuration: 2,8,8,1

Extended tier only

• Using given information about elements, we can identify trends in properties 
• An example of when this might be used is to determine the trend in reactivity of Group 1 metals 
• The table below shows the reactions of the first three elements in Group 1 with water 

Observations of lithium, sodium, and potassium with water

Element	Reaction	Observations
Li	lithium  + water   →   lithium hydroxide  +  hydrogen  2Li (s)  +  2H2O (l)   →   2LiOH (aq)  +   H2 (g)	Relatively slow reaction Fizzing Lithium moves on the surface of the water
Na	sodium + water   →   sodium hydroxide  +  hydrogen  2Na (s)  +  2H2O (l)   →   2NaOH (aq)   +   H2 (g)	More vigorous fizzing  Moves rapidly on the surface of the water Dissolves quickly
K	potassium  + water   →   potassium hydroxide  +  hydrogen  2K (s)  +  2H2O (l)   →   2KOH (aq)  +   H2 (g)	Reacts more vigorously than sodium  Burns with a lilac flame  Moves very rapidly on the surface  Dissolves very quickly

• The observations show that reactivity of the Group 1 metals increases as you go down the group
• Using this information we can predict the trend going further down Group 1 for the elements rubidium, caesium and francium
• As the reactivity of alkali metals increases down the group, rubidium, caesium and francium will react more vigorously with air and water than lithium, sodium and potassium
• Lithium will be the least reactive metal in the group at the top, and francium will be the most reactive at the bottom
• Francium is rare and radioactive so is difficult to confirm predictions

Element	Observations
Rb	Explodes with sparks
Cs	Violent explosion due to rapid production of heat and hydrogen
Fr	Too reactive to predict