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Topic: Metallic bond

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Double bond

Covalent bond

Bond dissociation energy

Chemical bond

Ionic bond

Coordinate covalent bond

Metal

Delocalised

Hydrogen bond

Atom

Crystal

Linus Pauling

Unit cell

Mineral

Binding energy

	Metallic bond - Wikipedia, the free encyclopedia
		Metal atoms typically contain a high number of electrons in their valence shell compared to their period or energy level.
		Metallic bonding is non-polar, in that there is no (for pure elemental metals) or very little (for alloys) electronegativity difference among the atoms participating in the bonding interaction, and the electrons involved in that interaction are delocalized across the crystalline structure of the metal.
		Metallic bonding is the electrostatic attraction between the metal atoms or ions and the delocalised electrons.
	en.wikipedia.org /wiki/Metallic_bond (255 words)

	Covalent bond - Wikipedia, the free encyclopedia
		Covalently bonded hydrogen and carbon in a molecule of methane.
		Pure covalent bonds (which are usually non-soluble, are electrically non-conductive, and tend to exist as individual molecules), and ionic bonds (which are soluble, are electrically conductive when molten or in solution, and, in general, tend to exist in a crystalline form) are on two opposite ends of the spectrum and have different properties.
		Bond order is a term that describes the number of pairs of electrons shared between atoms forming a covalent bond.
	en.wikipedia.org /wiki/Double_bond (1278 words)

	Chemical bond - Wikipedia, the free encyclopedia
		A chemical bond is the physical phenomenon of chemical species being held together by attraction of atoms to each other through sharing, as well as exchanging, of electrons or photons and is a phenomenon that is fully described by the laws of quantum mechanics.
		Coordinate covalent bonding is a special type of bonding, in which the covalent bonding electrons originate solely from one of the atoms, but are approximately equally shared by both in a molecular type bonding orbital.
		The Banana bond is a kind of bonding in which the bond bends, often due to the presence of an influencing atom in the middle of another covalent bond.
	en.wikipedia.org /wiki/Chemical_bond (2641 words)

	Covalent bond - Facts, Information, and Encyclopedia Reference article
		However, covalent bonding in metals and, particularly between metals and organic compounds is particularly important, especially in industrial catalysis and process chemistry, where many indispensible reactions depend on covalent bonding with metals.
		Pure covalent bonds (which has low melting points, are usually non-soluble, non-conductive, and tend to exist as individual molecules), and ionic bonds (which conversely have high melting points, are soluble, conductive, and generally tend to exist in a crystaline form) are on two opposite ends of the figurative spectrum, and have totally different properties.
		An example of a double bond is nitrous acid (between N and O), and an example of a triple bond is in hydrogen cyanide (between C and N).
	www.startsurfing.com /encyclopedia/c/o/v/Covalent_bond.html (1248 words)

	Bond (chemistry) - ninemsn Encarta
		When a bond is formed between atoms, energy is normally given out because the resulting compound is at a lower energy level, and therefore more stable, than the original atoms.
		Covalent bonds are formed when atoms share electrons, one from each atom in a single bond, to form electron pairs, usually making their outermost shells up to eight electrons by this means.
		Metals typically have few valency electrons, and occur in groups I, II, and III of the periodic table; reactive non-metals typically have more electrons in their outermost shells, and occur in groups IV, V, VI, and VII.
	au.encarta.msn.com /encyclopedia_761563675/Bond_(chemistry).html (1649 words)

	metallic bond - Hutchinson encyclopedia article about metallic bond (Site not responding. Last check: 2007-10-31)
		In metallic bonding, metal ions are tightly packed with their outer shell electrons overlap, so each electron becomes detached from its parent atom (delocalized).
		The metal is held together by the strong forces of attraction between the positive nuclei and the surrounding sea of delocalized electrons.
		Metals are both ductile and malleable because the bonding is not broken when metals are deformed; instead, the metal ions slide over each other to new lattice positions.
	encyclopedia.farlex.com /metallic+bond (243 words)

	metal structures
		Metals are giant structures of atoms held together by metallic bonds.
		Metals tend to have high melting and boiling points because of the strength of the metallic bond.
		The strength of the bond varies from metal to metal and depends on the number of electrons which each atom delocalises into the sea of electrons, and on the packing.
	www.chemguide.co.uk /atoms/structures/metals.html (844 words)

	Chemical Bonding Topic Overview
		For example, alkali metal and alkaline earth elements are typically metals whereas oxygen family elements and halogens are typically nonmetals.
		In such cases the bonding is called ionic bonding and the stability (lowered potential energy) is due to the mutual attraction between oppositely-charged ions in the solid crystals these compounds form.
		The metallic bond is the third and last of the generally-recognized types of chemical bonds.
	www.okstate.edu /jgelder/bondpage2.html (520 words)

	Highbeam Encyclopedia - Search Results for Metallic (Site not responding. Last check: 2007-10-31)
		metal METAL [metal] chemical element displaying certain properties by which it is normally distinguished from a nonmetal, notably its metallic luster, the capacity to lose electrons and form a positive ion, and the ability to conduct heat and electricity.
		The metallic pigment market: a renewed interest in eye-catching packaging has led to a positive year for the metallic ink market.
		Metallic pigments: with interest in and demand for the metallic look still high, metallic pigment suppliers are developing new products that can help paint formulators put a new spin on silver and other metallic finishes.
	www.encyclopedia.com /SearchResults.aspx?Q=Metallic (544 words)

	Encyclopedia :: encyclopedia : Chemical bond (Site not responding. Last check: 2007-10-31)
		A chemical bond is the phenomenon of atoms being held together in molecules or crystals.
		All chemical bonds are due to electrons interacting simultaneously with the atoms in question.
		However, more complicated compounds such as metal complexes cannot be described by valence bond theory alone, and quantum chemistry (based on quantum mechanics) has to be used.
	www.hallencyclopedia.com /Chemical_bond (482 words)

	ICSD Chem Zone: Summary of Forces & Bonds
		Ionic bonds are bonds between ions and are always formed as the result of a gain and loss of electrons.
		Metallic Bond: Atoms are held together in a solid metal or metal alloy by metallic bonds.
		However the bond between two atoms in the metal is still electrostatic, between the positive nuclei and the loosely held negative electrons.
	ithacasciencezone.com /chemzone/lessons/03bonding/bonds.htm (1334 words)

	C05-1-4-0-0-0-0:Types of chemical bonds (Site not responding. Last check: 2007-10-31)
		An ionic bond is formed by the attraction of oppositely charged atoms or groups of atoms.
		Ionic bonding is typically described to students as being the outcome of the transfer of electron(s) between two dissimilar atoms.
		A coordinate covalent bond (also called a dative bond) is formed when one atom donates both of the electrons to form a single covalent bond.
	dwb.unl.edu /Teacher/NSF/C05/C05Mats/BondTypes.html (739 words)

	Thermal barrier coating for metallic components - Patent 5236787
		Transition layers comprising a controllably positioned mixture of metallic and ceramic materials are interposed, respectively, between the bond coat and the central layer of ceramic material, and between the seal coat and the central layer of ceramic material.
		A coating for a metallic substrate, as set forth in claim 1, wherein said centric layer has a density at a position equidistant from the first and second surfaces of said layer that is less than the density of said material at said first and second surfaces.
		Both of the metallic coats, i.e, the bond coat 16 and the seal coat 18 are preferably formed by the plasma spray deposition of an oxidation resistant refractory metal powder material.
	freepatentsonline.com /5236787.html (3541 words)

	Metallic Bonding
		The nature of metals and metallic atoms is that they have loosely held electrons that can be taken away fairly easily.
		The key is in the loosely held electrons spread around and between all the metal atoms, or metal ions.
		With a little bit of thought about the position of different metals on the periodic table, how tightly they hold onto their electrons, and also the nature of metallic bonding you should be able to make some predictions about how the properties of different metals would compare to one another.
	dl.clackamas.cc.or.us /ch104-08/metallic.htm (971 words)

	Metallic bond (Site not responding. Last check: 2007-10-31)
		Metallic bonding as with covalent bonding is non-polar in that there is (for pure elemental metals) or very little alloys) electronegativity difference among the atoms participating the bonding interaction and the electrons involved that interaction are delocalized across molecular orbitals.
		is also akin to ionic bonding and distinct from covalent bonding in the interatomic forces are largely anisotropic and are extensive throughout the chemical than being confined to a discrete molecule.
		The Metallic Bond and the Structure of Metals
	www.freeglossary.com /Metallic_bond (394 words)

	Metallic bond
		The mechanism that holds a metallic bond together is the attraction between the positive kernels and the negative electron sea.
		The strength of the metallic bond is derived primarily from the charges in the system.
		The larger the magnitude of the positive charge on the metallic nuclei, the greater the strength of the metallic bond.
	www.bcpl.net /~kdrews/solids/metallics.html (575 words)

	Chapter 16 - Covalent Bonding
		An ionic bond is a chemical bond formed by the electrostatic attraction between a positive ion (cation) and a negative ion (anion).
		A bond angle is the angle between the bonds connecting atoms of a molecule.
		Since the single lone pair of electrons associated with the nitrogen atom exerts a repulsive force greater than that of the three bonding pairs of electrons in the ammonia molecule, the nitrogen-hydrogen bonds are “pushed downward” and the angle is slightly smaller than in the normal tetrahedral molecule.
	pages.prodigy.net /anderhan/Ch16Bonding.html (4773 words)

	GCSE Revision notes Ionic, Covalent, Polymer and Metallic Bonding at Doc Brown's Chemistry Clinc. btbnwpb wpbchemhelp
		The covalent bonding is caused by the mutual electrical attraction between the two positive nuclei of the two atoms of the bond, and the electrons between them.
		One single covalent bond is a sharing of 1 pair of electrons, two pairs of shared electrons between the same two atoms gives a double bond and it is possible for two atoms to share 3 pairs of electrons and give a triple bond.
		Metals are good conductors of electricity because these 'free' electrons carry the charge of an electric current when a potential difference (voltage!) is applied across a piece of metal.
	www.wpbschoolhouse.btinternet.co.uk /page04/4_72bond.htm (4294 words)

	metallic bonding
		Metals tend to have high melting points and boiling points suggesting strong bonds between the atoms.
		The metal is held together by the strong forces of attraction between the positive nuclei and the delocalised electrons.
		In a molten metal, the metallic bond is still present, although the ordered structure has been broken down.
	www.chemguide.co.uk /atoms/bonding/metallic.html (629 words)

	atomicbonds
		In a metal, the outer electrons are shared among all the atoms in the solid.
		The metallic ions are held together by virtue of their mutual attraction for the negative electron cloud.
		This is illustrated schematically in Figure 2.The metallic bond may be thought of as an extension of the covalent bond to a large number of atoms.
	info.lu.farmingdale.edu /depts/met/met205/atomicbonds.html (801 words)

	Duran: Chapter Eleven Bond Energies / Metallic & Itermolecular Bonds (Site not responding. Last check: 2007-10-31)
		In an analogous fashion, covalent bonds result in a net strong attraction between the bonding atoms.
		The bond energy is the amount of energy necessary to break one mole of covalent bonds into isolated gaseous species, it is sometimes called the bond dissociation energy or bond enthalpy.
		As the exact bond energy of a given bond varies somewhat with the species that are linked to the other side of the central atom, average bond energies are often quoted.
	chem.ufl.edu /~chm2040/Notes/Chapter_11/bond.html (175 words)

	Metallic Bonds (Site not responding. Last check: 2007-10-31)
		Extra electrons in metals are not restricted to one atom but can move throughout entire structure in what is called an electron sea.
		Metal atoms are positive charges in the electron sea.
		The metallic bond is not localized between two atoms.
	www.stedwards.edu /science/scie2320/chemistry/metallic.html (91 words)

	Metallic bond (Site not responding. Last check: 2007-10-31)
		It involves the delocalised sharing of free electrons between a lattice of metal atoms.
		Metallic bonding, as with covalent bonding is non-polar, in that there is no (for pure elemental metals) or very little (for alloys) electronegativity difference among the atoms participating in the bonding interaction, and the electrons involved in that interaction are delocalized across the crystalline structure of the metal.
		The metallic bond accounts for many physical characteristics of metals, such as malleability, ductility, conduction of heat and electricity, and luster.
	metallic-bond.ask.dyndns.dk (93 words)

	Metallic bond (Site not responding. Last check: 2007-10-31)
		It involvesthe delocalised sharing of free electrons between a lattice of metal nuclei.
		Metallic bonding, as with covalent bonding is non-polar, in that thereis no (for pure elemental metals) or very little (for alloys) electronegativity difference among the atoms participating in thebonding interaction, and the electrons involved in that interaction are delocalized across molecular orbitals.
		It is also akin to ionic bonding and distinct from covalent bonding in that the interatomic forcesare largely anisotropic and are extensive throughout the chemical, ratherthan being confined to a discrete molecule.
	www.therfcc.org /metallic-bond-83763.html (104 words)

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