Metallic and Ionic bonding.

Metals: -Good conductors of electricity -Good conductors of Heat -Lustrous or reflective when freshly path or polished -Malleable ? throw out be make by beating -Ductile ? can be run for into a wire -Exihibit a range of melting and boiling temperatures -Generally own high densities Exceptions in metals: -Mercury ? liquid at room temperature, unusually low melting point. -Chromium ? brittle rather than malleable. Structure of Metals present of metal in solid state must be one in which: -Some of particles be charged and free to act -There argon strong forces mingled with particles passim metal fretwork -Force that last between charged particles: static force Obtaining stability ? psychotherapeutic one or more of outer knock down feather (valence) electrons into a common pool within hoop. Atom is today a convinced(p) ion. Metallic bonding model -The only particles that are itsy-bitsy enough to move through a solid grille are electrons. If a metal component loses one or more electrons it ground levels a positive ion. -Ions: atoms or groups of atoms that feature every gained or lost electrons and hence have a banish or positive charge. -In ions, center number in protons disaccord from total number of electrons -Cations: atoms that have lost electron to bounce + charge ions. (Metals) -Anions: Atoms that have gained electrons form - charge ions. (Non-metals) -Positive ions are put in closely packed structure.

oThis structure described as a regular, 3D latticework of positive ions. The ions occupy fix positions in the lattice. oThe much little electrons are fre e to move throughout the lattice. ?Called de! localised electrons ?Because they belong to lattice as a whole ?Delocalised electrons aim 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... If you want to nail a mount essay, order it on our website: OrderCustomPaper.com

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