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Metallic And Ionic Bonding. Essay

1305 words - 5 pages

Metals:-Good conductors of electricity-Good conductors of Heat-Lustrous or reflective when freshly cut or polished-Malleable ? can be shaped by beating-Ductile ? can be drawn into a wire-Exihibit a range of melting and boiling temperatures-Generally have high densitiesExceptions in metals:-Mercury ? liquid at room temperature, unusually low melting point.-Chromium ? brittle rather than malleable.Structure of MetalsModel of metal in solid state must be one in which:-Some of particles are charged and free to move-There are strong forces between particles throughout metal lattice-Force that exist between charged particles: electrostatic forceObtaining stability ?Releasing one or more of outer shell (valence) electrons into a common pool within lattice. Atom is now a positive ion.Metallic bonding model-The only particles that are small enough to move through a solid lattice are electrons. If a metal atom loses one or more electrons it forms a positive ion.-Ions: atoms or groups of atoms that have either gained or lost electrons and thus have a negative or positive charge.-In ions, total number in protons differ from total number of electrons-Cations: atoms that have lost electron to form + charge ions. (Metals)-Anions: Atoms that have gained electrons form - charge ions. (Non-metals)-Positive ions are arranged in closely packed structure.oThis structure described as a regular, 3D lattice of positive ions. The ions occupy fixed positions in the lattice.oThe much smaller electrons are free to move throughout the lattice.?Called delocalised electrons?Because they belong to lattice as a whole?Delocalised electrons come from valence (outer) shell. (fig 3.5)oElectrons that are not free to move throughout the lattice:?Localised electrons?Localised electrons in inner shell.-The ions are held in lattice by attraction to delocalised electrons. This attraction extends throughout lattice and is called metallic bonding.Metallic Bonding can be used to explain some properties of metals:-Delocalised electrons in metallic lattice are free to move.oIf source of electricity is supplied across metal, electrons are forced in one end and are able to flow out the othero? Thus metals are good conductors of electricity.-Delocalised electrons able to bump into one another and the cations able to transmit heat energy rapidly throughout the latticeo? Thus metals are good conductors of heat-Because of delocalised electrons in their latticeo? metals reflect light and are lustrous-Even when beaten into sheets or drawn into wires, delocalised electrons move so they still surround cations.oElectrostatic forces of attraction may change but still operate through latticeoLayers of atoms can move past one another without disrupting the force between positive ions and negative sea of electrons.o? Thus metals are malleable and ductile-For most metals large amounts of heat energy is required to overcome strong forces of attraction between cations and delocalised electrons in the metal...

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