How do metallic bonds differ from ionic and covalent  bonds?
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Metallic bonding is the bonding within metals. It involves the delocalized sharing of free electrons between a lattice of metal atoms. Thus, metallic bonds may be compared to molten salts.\n\ne.g. Iron (Fe)... Why is it so strong? Of course, metallic bonding.\n\nMetal atoms typically contain a small amount of electrons in their valence shell compared to their period or energy level. These become delocalised and form a Sea of Electrons surrounding a giant lattice of positive ions.\n\nMetals seem to have higher boiling and melting points which might suggest stronger bonds between the atoms.\n\nMetallic 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.\n\nThe metallic bond accounts for many physical characteristics of metals, such as strength, malleability, ductility, conduction of heat and electricity, and luster. See also chemical bond.\n\nMetallic bonding is the electrostatic attraction between the metal atoms or ions and the delocalised electrons. This is why atoms or layers are allowed to slide past each other, resulting in the characteristic properties of malleability and ductility.\n\nMetallic bond are different from chemical bonds. Ionic and covalent bonds are chemical bonds.\n\nCovalent bonding is a common type of bonding, in which the electronegativity difference between the bonded atoms is small or non-existent. In the latter case, the bond is sometimes referred as purely covalent. See sigma bonds and pi bonds for current LCAO-explanation of non-polar bonds.\ne.g. CH4 (methane)\n\nIonic bonding is type of electrostatic bond between atoms which have an electronegativity difference of over 1.6 (this limit is a convention). These form in a solution between two ions after the excess of the solvent is removed.\ne.g. NaCl (common salt)\n\n<BEST ANSWER>\n============================================================\nHey, I tried to draw the structures of NaCl and methane molecules but this Yahoo! made it impossible. I hope you know the structurel.
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Strong Love!\n\nIn other words, it's a covalent bond because sharing of electrons takes place in these elements when they combine with each other.
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I think you mean the covalent chemical bonds seen in metals.\n\nThey give metals their ductile and malleable properties...that is they can be stretched into wires and pounded into shapes.\n\nSuch exampels would be gold, sodium, silver and copper.\n\nThese are much different than the ionic bonds found in salts.  Metallic bonds are very covalent, that is, they share electrons among nuclei.  This allows for nuclei to "slide" by each other...macroscopically this is the maleability and ductility.  The sharing of electrons also means electrons can flow easily, and thus metals are good conductors of electricity.\n\nIonic bonds have an electron transfer from one nuclei to another, and are much more rigid in their orientation (leading to brittle materials).
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Do you mean "transition" metals?  I guess you could call them intermediate metals, I have just never heard anyone use that term.\n\nTransition [intermediate] metals tend to develop positive charges when ionized.  Two positively charged ions will repell eachother, there is not too good of a chance they will interact, much less bond.
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Alkali metals and alkali earth metals tend to form ionic bonds.  They have a +1 or +2 charge.\n\nThe halogens normally form ionic bonds when "joined" with a IA or IIA metal.\n\nTransition metals normally are ionic.\n\nNow for the trick part:  Carbon and nitrogen generally form covalent bonds.  When joined with other elements, they can produce a neutral molecule (CO, CO2).  But they also form polyatomic ions (C03- (carbonate); NO3- (nitrate) ).  \n\nGeneral rule of thumb - IA, IIA, and VIIA atoms will make ionic bonds.  \n\nHope this helps!
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If a bond has ionic nature, the electrons have a tendency to hang out by one of the atoms in the bond more than the other... On the other hand if the bond is completely covalent in nature, the electrons are shared equally by both bonded atoms.
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A covalent bond is a bond in which the atoms making up the resulting molecule "share" the electrons in the form of covalent bonds.\nAn ionic bond is an extremely one sided "sharing" of electrons, so one sided, one atom is said to have completely stripped of an electron from another atom.\n\nWhat determines if the bond is covalent or ionic is the difference in the electronegativities of the two atoms bonding.  If the electronegativity difference is high enough, the bond is said to be ionic.  If the difference in electronagativities is significant, but not quite to the level of a full ionic bond, the bond is said to be polar (which may or may not mean that the resulting molecule is polar, this depends on several things).\n\nLooking at a chart of [Pauling] electronegativities,\nhttp://www.psigate.ac.uk/newsite/reference/plambeck/chem1/p01244a.htm\none can see that most elements are somewhere in the 1 to 2 range, with only a few elements getting much lower or higher than this value.  Unless the difference is high enough (usually a difference of about 1.5 is considered ionic), then the bond will just be polar, or less so.\n\nSo, all elements have the potential to theoretically bond ionically, but only in certain combinations with other elements.\nFor example, you will never see an ionic bond between Carbon and Hydrogen since the difference is just .4, but an ionic bond between Lithium and Fluorine is easy to make with a huge difference of 3.0.
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A metal (Greek: Metallon) is an element that readily forms positive ions (cations) and has metallic bonds. Metals are sometimes described as a lattice of positive ions surrounded by a cloud of delocalized electrons. The metals are one of the three groups of elements as distinguished by their ionisation and bonding properties, along with the metalloids and nonmetals. On the periodic table, a diagonal line drawn from boron (B) to polonium (Po) separates the metals from the nonmetals. Elements on this line are metalloids, sometimes called semi-metals; elements to the lower left are metals; elements to the upper right are nonmetals.\n\nA modern definition of metals is that they have overlapping conduction bands and valence bands in their electronic structure. This definition opens up the category for metallic polymers and other organic metals, which have been made by researchers and employed in high-tech devices. These synthetic materials often have the characteristic silvery-grey reflectiveness of elemental metals.\n\nThe traditional definition focuses on the bulk properties of metals. They tend to be lustrous, ductile, malleable, and good conductors of electricity, while nonmetals are generally brittle (for solid nonmetals), lack lustre, and are insulators.\n\nRest all are non metals.
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Metallic bond is the bonding between metals. \nPositive ions of metals are arranged in a regular, 3-D lattice and these ions occupy fixed position in the lattice. The electrons are delocalised and therefore they can move freely in the lattice. Because electrons are negatively charged. There will be attraction between the positively charged ions and negatively charged delocalised electrons and this attraction force hold them together, and this is called metallic bonding!\n* ions are atoms that lost or gain one or more electrons.Metals usually form "cations" because they always lost one or more electrins to form positively charged ions *
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Not exactly sure what you're asking here either, but perhaps a better answer is that electrons that are shared equally between two atoms in a bond are covalent, while electrons that spend more time with one atom than with the other form an ionic bond.\n\nHope that helps.
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Ionic solids are indeed formed by a gain and loss of electrons.  More specifically, they are formed by a chemical reaction between a metal atom and a nonmetal atom.  For example, sodium, a metal, has a tendency to want to lose an electron, and bromine, a nonmetal, wants to gain an electron, so the sodium gives an electron to bromin(which is now called bromide).  Now sodium has lost an electron, which is negatively charged, so it has a net charge of 1+. Bromine has gained an electron, so it has a net charge of -1.  Since they are oppositely charged, they are attracted to each other (kind of like how opposite poles of magnets are atracted to each other), they ionically bond and become an ionic solid (also known as a salt).
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melting points are mostly determined by the bonding between atoms and the polarity of the atoms in the rest of the molecule (if any).  In metals, it's all about the bonding.  All metals have metallic bonding; not all metallic bonds are created equal.
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To put it very simply,\nin a covalent bond, the atoms share electrons,\nin an ionic bond, electrons from one atoms are totally removed and added to the other atom, forming ions.\n\nBut in all bonds, there is some degree of sharing, even ionic.  Atoms of different elements "pull" on electrons with different strengths, the stronger the pull (larger electron negativity), the more time the electron will be found around that atom as opposed to the other.\n\nHydrogen gas (H2) is a good example of a covalent bond between two of the same elements, in this case, they share the electrons perfectly since they both have the same electron negativity.\n\nHF, or Hydrogen Floride is an example of a very ionic bond, with an electronegativity difference of 2.0 (4.1 - 2.1).  In this case, the electrons being shared spend almost all of thier time around the Floride ion, making that side develop a negative charge whereas the Hydrogen develops a positive charge.
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If you're referring to Lewis structures, dashes represent pairs of electrons being shared between 2 atoms and dots represent one electron (see link below).  When there is more than one line connecting atoms, that means they are sharing more than one pair of electrons.  Ionic bonds aren't usually represented this way. But to do this, each atom is surrounded by dots representing the electrons present after they are transferred to bond, surrounded by brackets individually (brackets can be left off if there are no electrons after bonding), and the charge is marked in the upper right corner.  The second link shows an example with salt (NaCl).
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Any two elements from different sides of the periodic table. More specifically, one from the metal category and one from the nonmetal category.\n\nEDIT: brwneyes, sodium chloride is one example of an ionic bond, not the only kind of ionic bond.
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They all vary, depending on the size of the atoms involved.  Covalent bonds distance is defined as 1/2 the distance between the two atoms radii.  As you can see this is difficult to determine if they are not the same atom.  Most bond lengths are estimated based on similar structures.
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In chemistry, an ionic compound is a chemical compound in which ions are held together in a lattice structure by ionic bonds. The positively charged ion is usually a metal ion and the negatively charged ion is non-metallic element or molecule.\n\nIons can be single atoms, as in common table salt sodium chloride, or more complex groups such as calcium carbonate. But to be considered ions, they must carry a positive or negative charge.\n\nThus, in an ionic bond, one 'bonder' must have a positive charge and the other a negative one. By sticking to each other, they resolve, or partially resolve, their separate charge imbalances. Positive to positive and negative to negative ionic bonds do not occur. (For a real world analogy, experiment with a pair of bar magnets.)