what is the best bonding element?
157419
Carbon can combine with most elments very easily and it makes the strongest bonds.
751019
The bond strength between calcium and oxygen in calcium oxide is greater. This is because in calcium oxide, calcium has given two electrons to oxygen. The ions would thus be Ca2+ and O2-. The K-F ionic bond is formed by the giving of only one electron to fluorine from potassium and is thus weaker.
714351
d) bond to carbon\n\nThis nonmetal has the interesting chemical property of being able to bond with itself and a wide variety of other elements, forming nearly ten million known compounds.
1090457
a the number of outer electron that will bond with other atoms to fill thei valence shells
333129
An element will become stable when it's outermost electron (valence) shell is full.  In most cases, the valence shell will contain 8 electrons when stable.  Hydrogen and helium only require 2 electrons.  \n\nIn order to achieve a full set, atoms can gain or lose electrons forming ionic compounds.  This normally happens between metals and nonmetals on the periodic table.  Alternatively, atoms can share electrons forming covalent compounds, which generally occurs between two nonmetals.
825051
Covalent bonds, as in NH4+
1008726
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.
195560
Atoms form bonds to get to a stable form. All atoms (besides noble gases) want to get a full shell of valence (outside) electrons. To get this full shell, they have to share electrons with others. This is called a covalent bond. \n\nOr, in the case of ionic bonds, a molecule that has extra electrons simply gives electrons to another molecule who wants them. These molecules become positive and negatively charged, and stick together because of magnetic attractions.
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metallic if it is bonded to another metal or ionic if it is bonded to a non-metal.
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Los Alamos national lab has a good periodic table/ elemental factoids.\n\nLanthanum is La.  It is the beginning of the "Lanthanides".
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In Ionic bond, elements looses or gains electron(s) and become ions and the electrostatic potential of these ions bind them\n\nIn covalent, the participating elements are bound by sharing electrons between them.
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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.
950410
Mainly H-bonding (intermolecular forces)
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The strength of C-O pi-bond is greater than that of C-C pi bond.(~ 364kJ/mol vs ~ 250 kJ/mol). Greater strength means greater stability. Thus the keto form is much favoured.
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See the two references below about metallic bonds.  The explanation is a little too long to type in this tiny space, but the first reference explains why gold is soft and both of them explain why it is a good conductor of electricity.\n\nTypes of bonding page 4 and Metallic bonds page 5: http://www.encyclopedia.com/doc/1E1-chem-bnd.html\n\nLast section on metallic and hydrogen bonds:  http://www.encyclopedia.com/doc/1E1-chem-bnd.html
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Well the reason it is so hard to obtain those pure elements is basically stability. Every atom ,but the Noble gases, wants an octet, 8, valence electrons. So these atoms bond with other atoms of other elements, rendering them as impure, to have that octet. \n\nI.E:They as in Zirconium and Hafium would rather be bonded together than pure. Though there are ways to pull the bonds apart.\nFor example is the separation of hydrogen and Oxygen when a current is pased through H2O, water.
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Actually its MgO. Magnesium is a bivalent metal Mg(2+) and Oxygen has a charge of O(2-) so they form a very strong 1:1 bond.