Bonding+in+metals

 **//__Table of contents__//** 1. metallic bonding 2. metallic properties 3. heat conductivity 4. electrical conductivity 5. changes in shape 6. Metals 7. works cited

The properties of solid metals can be explained by the structure of metal atoms. Metals tend to have high melting points and boiling points suggesting strong bonds between the atoms. Even metals like sodium melt at a considerably higher temperature then the element which precedes it in the periodic table. The loosely held electrons in metal atoms result in a type of bonding that is characteristics of metals when metal atoms combined chemically with atoms of other elements they lose valence electrons. The sea of electrons model of solid metals explains their ability to conduct heat and electricity. Metallic bonding explains many of the common physical properties of metals and there alloys. Metals are solids at ordinary temperature and pressure with the exception. Metals have characteristic properties such as high thermal and electrical conductivity, luster and high reflectivity, malleability and ductility. They can be beaten or shaped without fracture. Heat can easily travel through the metals. Heat causes particles of matter to move faster if particles collide with cooler particles energy that is transfered to the cooler particles.The freely moving valence electrons in a metal transfer energy to atoms and other electrons nearby. Heating systems and refrigeration both rely on this type of energy to function; they function by adding or removing thermal energy from an object or area to control its temperature. **//__Electrical Conductivity__//** Electricity can flow when charged particles are free to move. Metals conduct electricity easily because the electrons in the metal can move around freely. Electrical conductivity is the ability of a material to carry electrical current in water. In a metal conductor, electrical current is the flow of electrons and is called elctronic conductance. Conductivity is is affected by temperature because water becomes less viscous and ions can move around more easily at higher temperature. **//__Changes in Shape__//** A metals ability to conduct electricity would not be useful if the metal could not be made into thin wires that could bend. They can be streched, pushed, or compressed in to different shapes. Metals act this way because the ions in metals are not attracted to the other ions. instead they are attracted to the loose electrons all around them. As the result the ions are aloud to be pushed out of its position. **//__Metals__//** Metals conduct both electricity and thermal energy. Metals mostly have high melting points and boiling points. The atom of a metal has to few electrons in its outermost shell. A nonmetal atom is packed with electrons. Most metals bond easy with oxygen because their outer electrons are sparse and the outer electrons of oxygen, a nonmetal are abundant. Metals are shiny, dense, and easy to shape. Transition metals are grouped together in the middle of the periodic table of elements because they share proporties. There are one houndred different kinds of atoms.
 * //__Metallic bonding__//**
 * //__ Metallic properties __//**
 * //__ Heat cunductivity __//**

**//__Works cited__//** Hakim, Joy. __The story of science: newton at the center.__ New york: smithsonian Books, 2005.

David V.Frank, John G. Little, and Steve Miler. __Chemical interactions__ Pearson, upper saddle river,2009.(pg 36-39)