Quiz On Metallic And Ionic Bonding

When a metal is formed, the metal atoms lose their valence electrons in order to achieve a stable electronic configuration similar to that of a noble gas. This process allows the metal atoms to become positively charged cations. The valence electrons that are lost form a "sea" of negatively charged electrons surrounding the cations. The lattice structure of the metal is held together by the strong electrostatic attraction between the positively charged cations and the negatively charged sea of electrons. This arrangement creates a stable and solid metal structure.

Metals have a tendency to lose electrons (Cat Ion)
Non-Metals have a tendency to gain electrons (An Ion)

When melted, heat energy supplied overcomes some of the electrostatic attraction between the oppositely charged ions and hence the ions become mobile. Presence of mobile ions enable the ionic compound to conduct electricity in molten state.

In Molten(liquid) and Solid state, metals are able to conduct electricity due to the presence of mobile electrons which can flow under applied potential difference.

· Every metal atom would lose its valence electrons to gain electronic configuration of a noble gas

· The metal atom would lose its valence electrons to the negatively charged ‘sea’ of electrons

· The lattice is held together by the strong electrostatic attraction between the positively charged cation and the negatively charged ‘sea’ of electrons

When dissolves in water, Ionic compound dissociates to form mobile ions, Presence of mobile ions enable the ionic compound to conduct electricity in aqueous state.

The ions are fixed in position by the strong electrostatic attraction between the oppositely charged ions. Hence there are no mobile ions. Absence of mobile ions result a ionic compound to be unable to conduct electricity in Solid state.