is a chemical bond an example of potential energy?
827189
Yes. Check out this website for more information.  \n\nhttp://chemed.chem.purdue.edu/genchem/\n\nHope that helps.
1064705
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.
970781
Potential of Hydrogen.
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I think so.\nFor calculating the forces between atoms in molecules, you can solve this problem now, for small molecules using the law of physics.\nHowever for large molecules it is not the case and you must use approximations
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ONE THING IT MUST HAVE POTENTIAL ENERGY BUT FOR YOUR CONVENIENCE I ASSUME IT HAS 0 KE & PE\nTHE TOTAL ENERGY OF A SYSTEM REMAINS CONSTANT SO IT MUST HAVE "ZERO" END ENERGY
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There are fundamentally many ways to answer this question; and I will address three.\n\nIn nuclear chemistry, there are four fundamental interactions of matter that can be termed energy:\n\n1. Strong interaction, or strong force. This is the force which holds together quarks and other subnuclear particles into discreet protons, neutrons, and electrons. This is the energy that is released in a nuclear reaction.\n\n2. Weak interaction, or weak force. This is the force which holds protons and neutrons together in the nucleus of an atom. This is the energy that is released in radioactive decay.\n\n3. Electromagnetism. This is the attractive or repulsive force caused by the positive or negative charge of atomic particles and the electromagnetic field of photons. This force is the most wide in function, and is present in practically every conventional phenomenon. The electromagnetic force is responsible for electron orbitals, for chemical bonds and reactions, for electromagnetic radiation, and fundamentally for traditional force.\n\n4. Gravity. This is the tendency of objects with mass to accelerate toward each other. This is the weakest force, but can act over an almost unlimited distance.\n\nOR ....\n\nIn classic chemistry, a molecule can have three kinds of energy:\n\n1. Transitional energy, or the energy relative to motion.\n\n2. Chemical energy, or the energy inherent to electrochemical bonds.\n\n3. Vibrational energy, or energy relative to the vibration or oscillation of individual molecules.\n\nOR ...\n\nIn physics, we categorize all energy in the universe into two sets:\n\n1. Potential energy. This is the energy inherent in position or interaction with another body.\n\n2. Kinetic energy. This is the energy a mass possesses relative to its motion, whether it be classic velocity or vibration. This is sometimes termed work, though this is technically incorrect; both kinetic and potential energy are work, in different forms.\n\nAnd there you have it.
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To put it very simply,\nin a covalent bond, the atoms share electrons,\nin an ionic bond, electrons from one atoms are totally removed and added to the other atom, forming ions.\n\nBut in all bonds, there is some degree of sharing, even ionic.  Atoms of different elements "pull" on electrons with different strengths, the stronger the pull (larger electron negativity), the more time the electron will be found around that atom as opposed to the other.\n\nHydrogen gas (H2) is a good example of a covalent bond between two of the same elements, in this case, they share the electrons perfectly since they both have the same electron negativity.\n\nHF, or Hydrogen Floride is an example of a very ionic bond, with an electronegativity difference of 2.0 (4.1 - 2.1).  In this case, the electrons being shared spend almost all of thier time around the Floride ion, making that side develop a negative charge whereas the Hydrogen develops a positive charge.
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thermodynamic factors as well as the orientation and relative energies of the pi molecular orbitals involved.
200870
Any two elements from different sides of the periodic table. More specifically, one from the metal category and one from the nonmetal category.\n\nEDIT: brwneyes, sodium chloride is one example of an ionic bond, not the only kind of ionic bond.
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ya because the intramolecular force of attraction is not compatible. Hence hydrogen bonds are not able to be form.\n\nspecial case where force of attraction are not compatibl but compound can combine with H2O: ionic compound and H2O (ion dipole interaction)
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There is potential energy and kinetic energy.  Kinetic energy is the energy that something has from motion.  It's equation is E=1/2*m*v(squared) where m=mass and v=velocity.  For potential energy there are many forms.  Gravity E=mass*height*gravity, Electric and magnetic fields are potential energy.  And nuclear energy E=m*c(squared) which is the rest potential energy that anything with mass will have.  There is also energy from light E=h*nu, nu=frequency h=planck's constant.  There is also chemical potential energy which is the energy contained within molecules.
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No - methanol, ammonium\nYes - formic acid, sulfur troxide\nKinda - carbonate, nitrate, chlorate (all can be drawn as resonance structures, so the bonds aren't quite single and aren't quite double)
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B and C.  Molecules with H bonded to N, O, or F can form hydrogen bonds.  Others cannot.  In molecules A and D, all the H's are bonded to C's, so they are not capable of hydrogen bonding.  In molecules B and C, there is an O-H bond, so they are capable of hydrogen bonding.\n\nAlthough all four structural formulas have H written next to O, that doesn't necessarily indicate that there is an O-H bond.\n\nMolecule A is an ether, so the oxygen is between two carbons.  Specifically, it's dimethyl ether, so there's a methyl group (CH3) on each side of the oxygen.  You can find a picture of it here: http://en.wikipedia.org/wiki/Dimethyl_ether\nThe oxygen in an ether doesn't allow for hydrogen bonding because none of the hydrogens are attached to it.\n\nMolecule B a carboxylic acid.  Specifically, it's acetic acid.  It consists of a methyl group attached to a carboxyl group, which is a carbon double bonded to an oxygen and also single bonded to an OH group.  The O-H bond in the carboxyl group allows the molecule to form hydrogen bonds.\nYou can find a picture of its structure here:\nhttp://en.wikipedia.org/wiki/Acetic_acid\n\nMolecule C is ethanol.  It consists of a methyl group, a methylene group (CH2), and an OH groupl.  Like with carboxylic acid, the O-H bond is capable of hydrogen bonding.\nHere's it's structure:\nhttp://en.wikipedia.org/wiki/Ethanol\n\nMolecule D might be a bit misleading at first glance, but it's actually an aldehyde, specifically acetaldehyde.  It consists of a methyl group bonded to a second carbon that is bonded to a hydrogen and double-bonded to an oxygen.  That last hydrogen is attached to the carbon, rather than the oxygen, so it can't do hydrogen bonding.  Here's a picture of it's structure:\nhttp://en.wikipedia.org/wiki/Acetylaldehyde
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B\n\nStrong bonds requires more energy to break and therefore releases more energy when formed.\n\nSo when enthalpy(heat) is lowered you need something that eats more energy than it creates.
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Potential, kinetic, chemical, electrical, and thermal.
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Force holding atoms in a molecule together as a specific, separate entity (as opposed to, e.g., colloidal aggregates; see bonding).\n\nIn covalent bonds, two atoms share one or more pairs of valence electrons to give each atom the stability found in a noble gas. In single bonds (e.g., H-H in molecular hydrogen), one electron pair is shared; in double bonds (e.g., O=O in molecular oxygen or H2C=CH2 in ethylene), two; in triple bonds (e.g., HCºCH in acetylene), three. In coordinate covalent bonds, additional electron pairs are shared with another atom, usually forming a functional group, such as sulfate (SO4) or phosphate (PO4). The number of bonds and the atoms participating in each (including any additional paired electrons) give molecules their configuration; the slight negative and positive charges at the opposite ends of a covalent bond are the reason most molecules have some polarity (see electrophile; nucleophile). Carbon in organic compounds can have as many as four single bonds, each pointing to one vertex of a tetrahedron; as a result, certain molecules exist in mirror-image forms (see optical activity). Double bonds are rigid, leading to the possibility of geometric isomers (see isomerism). Some types of bonds, such as the amide linkages that join the amino acids in peptides and proteins (peptide bonds), are apparently single but have some double-bond characteristics because of the electronic structure of the participating atoms. The configurations of enzymes and their substrates, determined by their covalent bonds (particularly the peptide bonds) and hydrogen bonds, are crucial to the reactions they participate in, which are fundamental to all life
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The potential energy of a system is the energy which was spent to constitute the system from bringing its constituents closer\nto each other against the forces among them and this energy is stored in the syetem. The same way the interatomic energy is \nthe enrgy which was spent to bring the atoms closer against the vanderwaal forces.