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Chemistry Note

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Periodicity

Feature Title

In this chapter you should be able to:

  • Describe the arrangement of elements in the periodic table in order of increasing atomic number
  • Distinguish between the terms group and period
  • Deduce the relationship between the electron configuration of elements and their position in the periodic table
  • Describe and explain the periodic trends in atomic radii,ionic radii,ionization energies,electronegativity and melting points for the alkali metals (Li -> Cs) halogens (F -> I) and period 3 elements Na -> Ar)
  • Discuss the similarities in chemical nature of elements in the same group
  • Discuss the change in nature,from metallic to non-metallic, of the elements across period 3.
  • Explain the physical properties of the chlorides and oxides of the elements in the third period (Na -> Ar) in terms of their bonding and structure
  • Describe the chemical trends for the chlorides and oxides
  • Lis the characteristic properties of transition elements
  • Identify which elements are considered to be typical of the d-block elements
  • Describe the existence of variable oxidation states in d-block elements
  • Define the term 'ligand'
  • Describe how complexes of d-block elements are formed
  • Explain why some complexes of d-block elements are coloured
  • Outline the catalytic behaviour of d-block elements are coloured

 

 

 

Atomic Radius

 

 The position of the outermost electron can never be known,so atomic radius is defined as the half of the distance between nucleus of the two bonded atoms of the same element.The outermost electron is the highest in energy level,depends on no. of shell.

Down the group

-atomic radius increases
-no.of orbital increases

Across a period

-atomic radius decreases

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