which is more stronger type of bond ionic or covalent?(different teachers have different opinion)?
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Well, it all depends on what kinds of atoms are involved.   For instance, a covalent bond between two atoms with very small radius is probably much greater than an ionic bond between two atoms with similar electronegative values.  What I mean is that comparing ionic and covalent bonds is a relative thing; there are many premises involved.
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1) covalent\n2) ionic
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I think knowledge of the terms electronegativity and bond energy address your question. \n\nElectronegativity refers to the difference by which two atoms tend to hold onto electrons. You should be able to find a periodic table that shows you the electronegative values of all the atoms. You can compute the electronegativity of a bond between two atoms by subtracting their values from each other (based on Linus Pauling's calculations). For example, Flourine (F) has an electronegativity value of 4 and Na = .9. The electronegative value of an F-Na bond is 3.1 (4 - .9). My old high school textbook (Heath) states that ionic bonds are those having an electronegative difference between 1.7 and 4; polar covalent bonds are between 0.2 and 1.7; covalent (non-polar) bonds are between 0 and 0.2. Thus an F-Na bond by this classification system is an ionic bond.\n\nBut I suppose to answer your question most directly, I would say the evidence that ionic bonds are strong concern something called bond energy. That is, the difference between how much energy is needed to make and break chemical bonds. Generally speaking, the higher the electronegative difference (which translates into more of an ionic bond--see calculation above), the more energy required to break such bonds. \n\nThe bottom line, is that I think this translates into something like the observed boiling points of various substances. Substances that have strong ionic bonds (again, determined by calculation above) I believe have a higher boiling point (because it takes more energy/heat) to break the bonds.
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False.\n\nIonic bonds form when 1 or more electrons from one atom are transferred to the electron cloud of another atom.  Leaving one with a net positive charge while the other has a net negative charge.  These two opposing charges will be attracted to each other, resulting in an ionic bond.
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yes, they always covalently bond with each other under any normal type conditions\n\neven if you were to conveniently have an oxygen cation and anion that you combined, they would lose their ionic nature and bind in a covalent fashion
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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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1. Covalent Bonds\n2. Ionic Bonds\n3. Hydrogen Bonds
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Ionic bonds are created by attraction of separated charges or differences in electronegativity.  This results in a dipole moment, which is a vector property, hence it is directional.
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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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You get the first answered.\nCovalent bonds are strong and don't disassociate into ions, as ionic bonds do. Watch.\nNaCl common salt, sodium and chlorine, put in solution.\n\nNa+  and Cl- they disassociate and you can follow the path of electricity Electron jumps from sodium to be accepted by chlorine. That is electron flow; conduction of electricity.
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Covalent bond: are those which one or more pairs of electrons are shared by two atoms.\nCovalent chemical bonds involve the sharing of a pair of valence electrons by two atoms, in contrast to the transfer of electrons in ionic bonds. These bonds lead to stable molecules if they share electrons in such a way as to create a noble gas configuration for each atom. \n\nHydrogen gas forms the simplest covalent bond in the diatomic hydrogen molecule. The halogens such as chlorine also exist as diatomic gases by forming covalent bonds. The nitrogen and oxygen which makes up the bulk of the atmosphere also exhibits covalent bonding in forming diatomic molecules. \n\n\n\nIonic Bonds\nIn chemical bonds, atoms can either transfer or share their valence electrons. In the extreme case where one or more atoms lose electrons and other atoms gain them in order to produce a noble gas electron configuration, the bond is called an ionic bond. \n\nTypical of ionic bonds are those in the alkali halides such as sodium chloride, NaCl\n\n\nThe below reference has some diagrams which are helpful as well.
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i think it is a polar covalent bond\nI used to remember why but I'm not in Chemistry anymore...\nHeres a website.. Look at Example #3\nhttp://users.rcn.com/jkimball.ma.ultranet/BiologyPages/E/Electronegativity.html#covalent_bond\nAnd another http://academic.brooklyn.cuny.edu/biology/bio4fv/page/polar_c.htm\nhope its not too late
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Ionic compound\n\n The crystal structure of NaCl, a typical ionic compoundIn 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.)\n\nIonic compounds have strong bonds between particles and thus generally have high melting and boiling points. They have good electrical conductivity when molten or in aqueous solution. While ionic inorganic compounds are solids at room temperature and will usually form crystals, organic ionic liquids are increasingly of interest.\n\nIonic compounds also dissolve in polarised liquids, of which water is an example, while they do not dissolve in organic liquids, such as Petrol. This is the opposite of covalent compounds.\n\nWhen an ionic compound is named, the cation is named first and then the anion. When an elemental anion is named, the suffix, -ide, is added to the name of the element. There are two common types of cations: Type I and Type II. Type I cations have only one charge and their name is simply listed when the compound is named. Type II cations have more than one charge and when the ionic compound is named, a Roman numeral is used to denote the charge of the cation. In addition, there are common polyatomic anions which do not have suffixes in their name such as hypochlorite (ClO–).\n\nRetrieved from "http://en.wikipedia.org/wiki/Ionic_compound"
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There are two types of chemical bond. The first type of chemical bond is the ionic bond. Substance with ionic bond only dissolve in water and not in organic solvents like the alcohol and tetrachloromethane. Examples of substance with ionic bond are sodium chloride, aluminium oxide and magnesuim oxide and so on. The second type of chemical bond is the covalent bond. Substance with covalent bonding DO NOT dissolve in water BUT only dissolves in organic solvents like alcohols. Therefore, substance with covalent bonding like the alcohol(includes ethanol and methanol), ammonia, methane and tetrachloromethane only dissolve in alcohol and not water.
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u do, ionic bonds results not from a sharing of electrons but from a transefer of one of more electrons from one atom to another
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in covalent compounds, the two ions being bonded share electrons.  these are called covanlence electrons.  in an ionic bond, they share the electrons in a different way.
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Covalent.\nMetallic bond (do research on the Band Theory)\nIonic.\nCovalent.\nCovalent.\nIonic.