Groups in the periodic table

• Metals

  • Good thermal/electric conductors​

  • Malleable

  • Ductile

  • Lustre

• Non-Metals​

  • Poor thermal/electric conductor​

  • Usually gain electrons

• Metaloids​

  • Both metallic and non-metallic properties​

  • Semi-conductors

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Atomic Radius 

• Bonding/covalent atomic radius: Half the distance between the nuclei of two bonding atoms of the same species in a covalent bond.

• ​​Non-Bonding atomic/van der Waal's radius: radius of two non bonding frozen argon atoms​

Ionic Radius​

• Cations are smaller than the atom itself

• Anions are bigger than the atom itself

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Note: you should be able to explain why each ion has a bigger or smaller radius than the atom.

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Ionization Energy

• Definition: minimum energy needed to remove one electron from a neutral gaseous atom in its gaseous state. 

• General reaction:​

Electron affinity

• Definition: energy required to detach one electron from singly charged negative ion in the gas phase.

• General reaction:​

Electronegativity

• Definition: The relative attraction that an atom has for the shared pair of electrons in a covalent bond

Metallic and non-metallic character​​

Metal and non-metal oxides

• Definition: minimum energy needed to remove one electron from a neutral gaseous atom in its gaseous state. 

Halogens​

• 7 valence electrons, therefore tends to gain one electron

• Are usually diatomic (     )

• More electronegative halogens react in ionic reactions.

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Alkali metals

• Have only one valence electron     ,therefore tends to lose the electron 

• The reaction is more vigorous down the group.

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