What is a covalent bond?
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It's a bond where electrons are shared between elements.  As opposed to ionic bonds where the charges make the bond.
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Hydrogen bonding is found between the H+ of one H2O and the O- of the other H2O molecule. Also, within each H2O there are covalent bonds between the O and H.
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A coordination bond is a bond where one molecule gives both electrons to form a covalent bond. It differs from an ionic bond because the electrons are "shared" not given (e.g. the bond consists of a wavefunction, instead of discrete cations and anions)
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The bonding of what? The individual atoms to eachother........ The bonding of each sugar unit to the next..............
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1.  they are the outer most electrons \n2.  8 because that is a full orbital and a octet.. they want to get a noble gas notation\n3. Covalent shares electrons Ionic bonds donate electrons due to low electronegativity
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An ionic compound.\nA covalent compound.
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1)ionic and covalent depend on the situation and are considered generally equal \n2)network bonds are a type of covalent bond\n3)metallic bonds are weaker (this one's kinda fuzzy)\n4)intermolecular are the weakest
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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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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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Halogens, in their elemental state, are covalent. In their elemental state, they are not compounds, because they are not combined with other elements. But F2, Cl2, Br2, I2, and At2 are covalently bonded.
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A covalent bond\nThe other is an Ionic Bond which is when one atom gives an electron to another atom.
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sugars are covalent \n\nif you are specifically talking about table sugar, or sucrose, you can find out all about it here\nhttp://en.wikipedia.org/wiki/Sucrose
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Water is made of covalent bonds, but they are polar-covalent bonds.  This means that water will dissolve anything with ionic bonds (salts) and also polar-covalent bonds (sugars).
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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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In Carbon Carbon bonding:\n\nC-C is  sp3 hybridization, C=C is sp2 and C triple bond C is sp hybridisation. more s character is more strong covalent nature. Covalent character is increasing when moving multiple bonds in carbon. Covalent bond means sharing of pair of electrons (common pair) in bonding by both atoms(mutual) and hence both atoms come closer, that is lowering of bond length.
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ionic = ionic crystal\npolar-covalent = molecule with dipole bond\nnonpolar-covalent = molecule w/ no dipole bond
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covalent bonds are called the directional bonds.because the orbitals involved in bonding have specific direction where they bond.