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Topic: Bond energy

	Bond dissociation energy - Wikipedia, the free encyclopedia
		The bond dissociation energy is usually different from the bond energy, which is calculated from the sum of the bond dissociation energies of all bonds in a molecule.
		of bond dissociation energy, and 424.4 kJ mol
		The bond energy of the O-H bonds in water is 458.9 kJ mol
	en.wikipedia.org /wiki/Bond_dissociation_energy (305 words)

	Binding energy - Wikipedia, the free encyclopedia (Site not responding. Last check: 2007-10-26)
		At the nuclear level, the nuclear binding energy is derived from the strong nuclear force and is the energy required to disassemble a nucleus into free unbound neutrons and protons.
		At the atomic level, the binding energy of the atom is derived from electromagnetic interaction and is the energy required to disassemble an atom into free electrons and a nucleus.
		This quantity is not to be confused with the gravitational potential energy, which is the energy required to separate two bodies, such as a celestial body and a satellite, to infinite distance, keeping each intact (the latter energy is lower).
	en.wikipedia.org /wiki/Binding_energy (1409 words)

	Bond (chemistry) - MSN Encarta
		When a bond is formed between atoms, energy is normally given out because the resulting compound is at a lower energy level, and therefore more stable, than the original atoms.
		The energy required to break a bond is called its bond energy (or bond enthalpy), and is a useful quantity when the stability of compounds is being studied.
		Lattice energies, the equivalent of bond energies for covalent compounds, are of the order of 600 to 1,000 kJ/mole, for compounds containing singly charged ions, and higher if either or both of the ions has a multiple charge.
	uk.encarta.msn.com /encyclopedia_761563675/Bond_(chemistry).html (1649 words)

	Chemical Bond Data
		A chemical bond forms when it is energetically favorable, i.e., when the energy of the bonded atoms is less than the energies of the separated atoms.
		The ionization energy or ionization potential is the energy necessary to remove an electron from the neutral atom.
		The ionization energy can be thought of as a kind of counter property to electronegativity in the sense that a low ionization energy implies that an element readily gives electrons to a reaction, while a high electronegativity implies that an element strongly seeks to take electrons in a reaction.
	hyperphysics.phy-astr.gsu.edu /hbase/chemical/bondd.html (569 words)

	Strengths of Covalent Bonds (Site not responding. Last check: 2007-10-26)
		The stability of a molecule is a function of the strength of the covalent bonds holding the atoms together.
		The bond energy for a given bond is influenced by the rest of the molecule.
		However, this is a relatively small effect (suggesting that bonding electrons are localized between the bonding atoms).
	wine1.sb.fsu.edu /chm1045/notes/Bonding/Strength/Bond09.htm (320 words)

	HighBeam Encyclopedia - chemical bond
		There is a chemical bond between two atoms or groups of atoms when the forces acting between them are strong enough to lead to the formation of an aggregate with sufficient stability to be regarded as an independent species.
		The amount of energy required to break a bond and produce neutral atoms is called the bond energy.
		Covalent bonds are of particular importance in organic chemistry because of the ability of the carbon atom to form four covalent bonds.
	www.encyclopedia.com /html/c1/chem-bnd.asp (942 words)

	What is bond energy
		The next step enables you to draw an energy diagram representing the energy content of the species before, during and after the reaction.
		Bond energy is needed to break these strong bonds.
		Since bond making is the opposite of bond breaking, bond energy is released when bonds join individual atoms together to form molecules.
	www.matter.org.uk /schools/Content/Reactions/BondEnergy.html (143 words)

	Chemical Reactivity (Site not responding. Last check: 2007-10-26)
		Bond energy is the energy required to break a covalent bond homolytically (into neutral fragments).
		Bond energies are commonly given in units of kcal/mol or kJ/mol, and are generally called bond dissociation energies when given for specific bonds, or average bond energies when summarized for a given type of bond over many kinds of compounds.
		Energy is required to break bonds, and since the strengths of different kinds of bonds differ, there is often a significant overall energy change in the course of a reaction.
	www.cem.msu.edu /~reusch/VirtualText/react2.htm (2839 words)

	Bond Lengths and Energies
		The bond energy is essentially the average enthalpy change for a gas reaction to break all the similar bonds.
		Bond energy is a measure of the strength of a chemical bond.
		Bonds between the same type of atom are covalent bonds, and bonds between atoms when their electronegativity differs by a little (say 0.7) are also predominant covalent in character.
	www.science.uwaterloo.ca /~cchieh/cact/c120/bondel.html (854 words)

	Chemical Bonding
		Inversely, bond energy corresponds to the amount of energy that is required to break a bond.
		The energy term corresponds to the energy released, or bond energy.
		Bond Length is the average distance between the centers of two bonded atoms.
	www.bcpl.net /~kdrews/bonding/bonding.html (798 words)

	Chemical bonding: introduction
		A chemical bond is so often represented as a line drawn between atom symbols or a stick connecting two balls in a plastic molecular model that we sometimes tend to think of chemical bonds as “things”.
		Chemical bonding connotes the existence of an aggregate (assembly) of atoms that is sufficiently stable to possess a characteristic structure and composition.
		Bond lengths depend mainly on the sizes of the atoms, and secondarily on the bond strengths, the stronger bonds tending to be shorter.
	www.chem1.com /acad/webtext/chembond/cb01.html (2737 words)

	Bond Energies (Site not responding. Last check: 2007-10-26)
		Bond energies are a measure of the strength of a bond.
		If the energy given out when new bonds form is greater than the energy needed to break the original bonds, then the reaction is exothermic.
		If the energy given out when new bonds form is less than the energy needed to break the original bonds, then the reaction is endothermic.
	www.freewebtown.com /montfort/Chemistry/units/LR1404.html (634 words)

	GCSE Notes on Energy Changes in Chemistry at Doc Brown's Chemistry Clinic. revise revision revising website web sites ...
		The bond energy is the energy involved in making or breaking bonds and is usually quoted in kJ per mole of the particular bond involved.
		If more energy is needed to break the original existing bonds of the reactant molecules, than is given out when the new bonds are formed in the product molecules, the reaction is endothermic.
		If less energy is needed to break the original existing bonds of the reactant molecules, than is given out when the new bonds are formed in the product molecules, the reaction is exothermic.
	www.wpbschoolhouse.btinternet.co.uk /page03/3_51energy.htm (2245 words)

	Bond Energy
		The energies of bonds between atoms of substantially different electronegativities tend to be high, e.g., the 110 kcal of the H-O bond.
		Another important example is the bonds between oxygen and carbon atoms in carbon dioxide, CO The carbon atom shares two pairs of electrons with each of the oxygen atoms, and each of these double bonds has a bond energy of 187 kcal (or about 93 kcal for each shared pair of electrons).
		We should also note that the energy needed to break a particular bond, e.g., between carbon and oxygen, may also be influenced by the nature of the other atoms attached to the ones we are interested in.
	home.comcast.net /~john.kimball1/BiologyPages/B/BondEnergy.html (1332 words)

	General Chemistry Online: Glossary: Energy and chemical change
		Energy change per mole when a bond is broken in the gas phase for a particular substance.
		For example, when water evaporates, the internal energy of the water is dispersed with the water vapor produced, corresponding to an increase in entropy.
		Energy, enthalpy, temperature, volume, pressure, and temperature are examples of state functions; heat and work are examples of non-state functions.
	antoine.frostburg.edu /chem/senese/101/thermo/glossary.shtml (1938 words)

	Pauling on Electronegativity
		Independence of the bonds in a molecule would require that the total energy of formation of the molecule from separate atoms be expressible as the sum of constant energy terms characteristic of the various bonds.
		Inasmuch as the energy integral for any wave function for a system must be equal to or greater than the energy of the lowest state of the system, the energy of the actual bond between A and B must be at least as great as that for a normal covalent bond.
		I. Bond Energies and the Relative Electronegativity of Atoms.
	dbhs.wvusd.k12.ca.us /webdocs/Chem-History/Pauling-1932/Pauling-electroneg-1932.html (3217 words)

	Chemical bond energy example (Site not responding. Last check: 2007-10-26)
		In the chemical bonds of a molecule the attractive electrical forces cause bound states to exist.
		The balance of energy before and after the reaction can be illustrated schematically with the state in which all atoms are free taken as the reference for energy.
		The steps toward forming the NaCl ionic molecule could be seen as (1) providing the ionization energy of 5.14 eV to ionize Na, then (2) the recovery of -3.62 eV from the electron affinity of Cl, then the binding energy of the electric attractive forces based on the known bond length of 0.236 nm.
	hyperphysics.phy-astr.gsu.edu /hbase/molecule/boneng.html (322 words)

	Bond Energy and Stability (Site not responding. Last check: 2007-10-26)
		How does a h-cl bond with a bond energy of 431kj/mol have a greater stability than a h-h bond with a bond energy of 436kj/mol according to the text we are using.
		Bond dissociation energies are given for specific bonds, while average bond energies are given for the type of bond over many compounds (I think this is the one that may show up in textbooks.
		The thermodynamic stability (related to the potential energy) may be different from the chemical stability (the resistance of the compound to a chemical reaction--related to something called activation energy, which is a little extra bit of energy required to get a particular reaction going).
	www.newton.dep.anl.gov /askasci/chem00/chem00798.htm (307 words)

	Duran: Chapter Eleven Bond Energies / Metallic & Itermolecular Bonds (Site not responding. Last check: 2007-10-26)
		The bond energy is the amount of energy necessary to break one mole of covalent bonds into isolated gaseous species, it is sometimes called the bond dissociation energy or bond enthalpy.
		As the exact bond energy of a given bond varies somewhat with the species that are linked to the other side of the central atom, average bond energies are often quoted.
		The energy associated with the bonding process for a covalent bond between 2 H atoms is shown below
	www.chem.ufl.edu /~chm2040/Notes/Chapter_11/bond.html (175 words)

	Bond Energy (Site not responding. Last check: 2007-10-26)
		The optimum bond length between a pair of atoms is the distance at which there is a minimum energy value.
		The bond is most stable when the value displayed in red (labeled "bond energy") is at its lowest value (most negative).
		Find the bond length that results in the most stable bond between the two atoms in the Group V, VI, and VII homonuclear diatomic molecules in Period 2.
	www.bu.edu /smec/qsad/curriculum/text_modules/Bond_Energy.htm (436 words)

	General Chemistry Online: FAQ: Energy and chemical change: How can enthalpy changes for a reaction be estimated from ...
		The energy required to break the bonds is absorbed from the surroundings.
		If there was some way to figure out how much energy a single bond absorbed when broken, the enthalpy of reaction could be estimated by subtracting the bond energies for bonds formed from the total bond energies for bonds broken.
		Bond energies aren't appropriate for directly predicting enthalpies of reactions that occur in liquids, solutions, or solids, because they account only for bond breaking and making within molecules, and neglect attractions that are broken and formed between molecules.
	antoine.frostburg.edu /chem/senese/101/thermo/faq/enthalpy-from-bond-energies.shtml (584 words)

	Duran: Chapter Eleven Bond Energies / Metallic & Itermolecular Bonds (Site not responding. Last check: 2007-10-26)
		Ionic bonds have energies which can be quantified, energy is generally released when ionic bonds are formed
		Energy is released when isolated atoms form a covalent bond.
		Energy must be absorbed to break the bond apart.
	chem.ufl.edu /~chm2040/Notes/Chapter_11/bond.html (175 words)

	About Bond graphs - The System Modeling World (Site not responding. Last check: 2007-10-26)
		In bond graph terminology, an element that relates effort to the generalized displacement (or time integral of flow) is called a one port capacitor.
		The flows on the bonds attached to a 1-junction are equal and the algebraic sum of the efforts is zero.
		The bond number 4 in the figure is the pick-up bond where information of effort is masked and in bond number 5, which is the exciter bond, the flow is activated.
	www.bondgraphs.com /about.html (5796 words)

	General Chemistry Online: Companion Notes: Energy & change
		Use tables of bond energies to estimate the enthalpy of a reaction.
		Energy is required to break a chemical bond (just as energy is required to stretch a spring until it breaks).
		bond enthalpy: enthalpy change per mole when a bond is broken in the gas phase for a particular substance.
	antoine.frostburg.edu /chem/senese/101/thermo/index.shtml (992 words)

	Chemical Bond Energy
		Every chemical bond contains a definite amount of chemical energy, which can be large or small depending on the types of atoms in the bond.
		When you burn wood in a campfire, high-energy chemical bonds in the wood are broken and low-energy chemical bonds with oxygen (from the air) are formed.
		The net difference in chemical energy is the reason you built the campfire in the first place--it comes out as heat and light.
	www.cpast.org /Articles/fetch.adp?topicnum=6 (152 words)

	Homolytic Se-H Bond Energy and Ionization Energy of Benzeneselenol and the Acidity of the Corresponding Radical Cation (Site not responding. Last check: 2007-10-26)
		Homolytic Se-H Bond Energy and Ionization Energy of Benzeneselenol and the Acidity of the Corresponding Radical Cation
		The homolytic Se-H bond energy of benzeneselenol, a very efficient radical trap in solution and in the gas phase, was determined experimentally by using two independent approaches in a Fourier-transform ion cyclotron resonance mass spectrometer.
		An adiabatic ionization energy of 8.3 ± 0.1 eV was obtained by measurement of the efficiencies of various electron transfer reactions in the forward and reverse directions.
	pubs.acs.org /cgi-bin/abstract.cgi/jpchax/1996/100/i16/abs/jp953602r.html (258 words)

	Motion Planning for Proteins: Biophysics and Applications
		Interaction energy usually consists of the non-bonded terms found in the internal energy function, summed of all pairs of atoms (r,l), where r is an atom of the receptor and l is an atom of the ligand.
		The bond energy term corresponds to the stretching and compressing of the length of a bond.
		Hydrogen bonds (which are not true bonds in the strict, electron-sharing sense) are unusually strong electrostatic interactions, usually between a hydrogen atom and an electronegative atom such as oxygen or nitrogen.
	cnx.org /content/m11449/latest (5542 words)

	The Covalent Bond
		Ionic bonds are formed when there is a complete transfer of electrons from one atom to another, resulting in two ions, one positively charged and the other negatively charged.
		The energy of a typical single covalent bond is ~80 kilocalories per mole (kcal/mol).
		This is due to simple energetic considerations; the thermal energy of a molecule at room temperature (298 K) is only ~0.6 kcal/mol, much lower than the energy required to break a covalent bond.
	people.deas.harvard.edu /~jones/es154/lectures/lecture_2/covalent_bond/covalent_bond.html (350 words)

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