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Chemistry
Chemical Bonding

How do bond energy and bond length relate?

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Wiki User
2012-12-11 13:19:03
2012-12-11 13:19:03

they dont

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bonds get bigger with the more energy

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Bond energies are the measure of strength of a chemical bond. The larger the bond energy, the stronger the bond.

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They both deal with bonding atoms. Also, the shorter the bond length, the greater the bond energy.

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i have no idea sorry maybe you should check a chemistry book

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bond energy or bond dissociation energy is relative to bond length and therefore the amount of electrons involved in the bond so figure that out and i believe you'll have your answer

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higher is the no of shared pairs of electrons higher will be the bond dissociation energy.

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A very long bond between two atoms means the two centers of attraction are far apart and the energy is lower. As short bond length means the centers of attraction are closer and the bond is thus stronger. Bond length is also related to bond order, when more electrons participate in bond formation the bond will get shorter.

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The bromine diatomic molecule has a bond energy of 190 kilojoules per mole. This translates to a bond length of 228 picometers.

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Each bond has a bonding energy which is released in a chemical reaction.

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Bond energy is a measure of the strength of a chemical bond, that is the amount of energy required to break a bond. The larger the bond energy, the stronger the bond. For covalent bonds, bond energies and bondlengths depend on many factors: electron afinities, sizes of atoms involved in the bond, differences in their electronegativity, and the overall structure of the molecule. There is a general trend in that the shorter the bondlength, the higher the bond energy and the stronger the bond.

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The distance between two bonded atoms at their minimum potential energy, that is, the average distance between two bonded atoms, is the bond length. I think that the left over valence electrons is what determines the bond length and the distance between the "howevermany" atoms are in the compound. The bond order is related to the bond length, when more electrons are in the bond formation it causes the bond to get shorter.

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Bond energy is a defined quantity, the amount of energy to convert 1 mole of compound into its constituent atoms, bond strength is not a strictly defined entity, it is sometimes used as a synonym for bond energy. Spectroscopists talk of bond strength and relate this to the resonant frequency of functional groups in say the IR/Raman spectra.Bond energy is the energy that is needed to break down one mole. Bond strength is the degree that is in a atom.

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The bond length of two atoms is the distance between the centers/ nuclei of the atoms involved in the bond. In order to break any bond, energy of a certain value has to be supplied. this means that the closer the nuclei of the bonding atoms are, a greater supply of energy is needed to separate the atoms. in other words, 'short' bond lengths require high dissociation energies to break the bond.

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the stronger the bond, the shorter the length of the bond

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The shorter the length the stronger the bond.

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at which potential energy is at a minimuim.

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Bond dissociation energy is the energy it takes to break a bond.

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Bond energy is released when the bond is broken. At that time it is called as Bond Dissociation energy.

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The bond length is similar to the Ethane (Ethz155)

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Bond Length is often measured in picometers (pm).

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Bond breaking is endothermic, which means it takes energy. An example would be breaking a window. Bond making is exothermic, which means it releases energy. An example would be burning a substance.


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