Periodicity (OCR A Level Chemistry)

• The Periodic Table is a list of all known elements arranged in order of increasing atomic number, from 1 to 118.
• In addition to this, the elements are arranged so that atoms with the same number of shells are placed together, and atoms with similar electronic configurations in the outer shell are also placed together. This is achieved as follows:
  • The elements are arranged in rows and columns.
  • Elements with one shell are placed in the first row (i.e. H and He)
  • Elements with two shells are placed in the second row (Li to Ne) and so on.

• A row of elements thus arranged is called a period. The period number, n, is the outer energy level occupied by electrons.
• In addition, the elements are aligned vertically (in columns) with other elements in different rows, if they share a similar outer-shell electronic configuration
  • The outer electrons are known as the valence electrons.

• A column of elements thus arranged is called a group

The Periodic Table

• Since the electronic configurations of H and He are unusual, they do not fit comfortably into any group. They are thus allocated a group based on similarities in physical and chemical properties with other members of the group
• He is placed in group 0 on this basis, but hydrogen does not behave like any other element and so is placed in a group of its own
• The physical and chemical properties of elements in the periodic table show clear patterns related to the position of each element in the table
  • Elements in the same group show similar properties
  • Properties change gradually as you go across a period
• As atomic number increases, the properties of the elements show trends that repeat themselves in each period of the periodic table
  • These trends are known as periodic trends, and the study of these trends is known as periodicity

• All elements belong to one of four main blocks: the s-block, the p-block, the d-block and the f-block
  • The s-block elements are all those with only s electrons in the outer shell
  • The p-block elements are all those with at least one p-electron in the outer shell
  • The d-block elements are all those with at least one d-electron and at least one s-electron but no f or p electrons in the outer shell (up to 5d)
  • The f-block elements are all those with at least one f-electron and at least one s-electron but no d or p electrons in the outer shell

Trends across a period

• Each period starts with an electron in a new highest energy shell.
  
  • Across period 2, the 2s sub-shell fills with two electrons, followed by the 2p sub-shell with six electrons.
  • Across period 3,  the same pattern of filling is repeated for the 3s and 3p sub-shells,
• For each period, the s and p sub-shells are filled in the same way - a periodic pattern.