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Topic: Bonding electron

	Chemical bond - Wikipedia, the free encyclopedia
		Electrons in non-bonding orbitals tend to be in deep orbitals (nearly atomic orbitals) associated almost entirely with one nucleus or the other, and thus they spend equal time between nuclei or not.
		The type of strong bond depends on the difference in electronegativity and the distribution of the electron orbital paths available to the atoms that are bonded.
		The Banana bond is a kind of bonding in which the bond bends, often due to the presence of an influencing atom in the middle of another covalent bond.
	en.wikipedia.org /wiki/Chemical_bond (2637 words)

	curvedarrows.html (Site not responding. Last check: 2007-11-02)
		Electrons never flow from atoms which are electron-poor to atoms which are electron-rich, so a curved arrow will never point from an atom with a positive charge to an atom with a negative charge.
		The curved arrow on the left indicates the electron pair that was the O-H bond becomes a lone pair on the oxygen of the hydroxide ion.
		The curved arrow on the right indicates that the electron pair of the bromine-bromine bond is shifting to reside solely on the bromine on the right, resulting in rupture of the bond and formation of bromine with four lone pairs and a negative charge.
	web.chem.ucla.edu /~harding/tutorials/curvedarrows/curvedarrows.html (1233 words)

	CHEMystery: Atomic Structure and Bonding: Electron Configurations
		The distributions of electrons among the orbitals of an atom is the atom's electronic structure or electron configuration.
		In a neutral atom, the number of electrons equals the number of protons of the atom.
		The core electrons are the rest of the electrons, and they are buried deep within the atom and usually do not play a role in chemical reactions.
	library.thinkquest.org /3659/structures/electronconfig.html (740 words)

	Molecular Structure & Bonding
		A wedge shaped bond is directed in front of this plane (thick end toward the viewer), as shown by the bond to substituent B; and a hatched bond is directed in back of the plane (away from the viewer), as shown by the bond to substituent D.
		Of course, it is the configuration of atoms (not electrons) that defines the the shape of a molecule, and in this sense ammonia is said to be pyramidal (not tetrahedral).
		The bonding MO is occupied by two electrons of opposite spin, the result being a covalent bond.
	www.cem.msu.edu /~reusch/VirtualText/intro3.htm#strc4 (3290 words)

	Chapter 9: Animations (Site not responding. Last check: 2007-11-02)
		In ionic bonding, an electron is transferred from one atom to the another.
		Electrons in covalent bonds tend to be localized, meaning they are generally associated with two particular atoms that are bonded to each other.
		Electrons in ionic bonds are generally bound to only one atom, which carries a net charge.
	www.dac.neu.edu /physics/b.maheswaran/phy1121/data/ch09/anim/anim0904.htm (254 words)

	Davidson College - CHE 115 - VSEPR Model (Site not responding. Last check: 2007-11-02)
		For this reason, these electrons are oriented away from the region immediately around the center atom and thus do not contribute significantly to the repulsions between nonbonding and sigma bonding electron pairs.
		The ideal bond angles are the bond angles are the angles one would expect if each bond and each nonbonding electron pair occupied the same amount of space and exerted the same repulsive force.
		(The bonding interaction tends to draw the electron pair into the region immediately between the two atoms, thereby reducing the size of the orbital.) Consequently, the real bond angles (i.e., those measured experimentally) will differ from the ideal bond angles unless the symmetry of the molecule is very high.
	www.chm.davidson.edu /vsepr/model.html (345 words)

	CB11 - Chemical Bonding
		The twenty lessons in the Chemical Bonding set cover most of the aspects of this subject that are usually taught in first-year college and university Chemistry courses.
		An important theme that runs through all of these lessons is that our working theories of chemical bonding are based on models which have varying degrees of applicability to different kinds of systems.
		Bond polarity and dipole moments in CO2, H2O and CH4.
	www.chem1.com /chem1/lessondesc/CB11.html (736 words)

	Electron Configurations & The Periodic Table
		Transfer of the lone 3s electron of a sodium atom to the half-filled 3p orbital of a chlorine atom generates a sodium cation (neon valence shell) and a chloride anion (argon valence shell).
		These electron sharing diagrams (Lewis formulas) are a useful first step in understanding covalent bonding, but it is quicker and easier to draw Kekulé formulas in which each shared electron pair is represented by a line between the atom symbols.
		For bonds to hydrogen, acidity is one criterion.
	www.cem.msu.edu /~reusch/VirtTxtJml/intro2.htm (2092 words)

	Introduction to Bonding (Site not responding. Last check: 2007-11-02)
		A single bond between two atoms may be formed by the two atoms donating electrons equally, i.e., each atom contributes one electron to the bond.
		Bond polarity: We noted above that when two atoms donate one electron each to a bond, that this bond is a covalent bond.
		Bonds are more polar the greater the difference is in the electronegativities of the two atoms involved in the bond.
	www.owlnet.rice.edu /~chem151/lecture/Handouts/bonding/bondsum.html (7562 words)

	GCSE Revision notes Ionic, Covalent, Polymer and Metallic Bonding at Doc Brown's Chemistry Clinc. btbnwpb wpbchemhelp
		The covalent bonding is caused by the mutual electrical attraction between the two positive nuclei of the two atoms of the bond, and the electrons between them.
		One single covalent bond is a sharing of 1 pair of electrons, two pairs of shared electrons between the same two atoms gives a double bond and it is possible for two atoms to share 3 pairs of electrons and give a triple bond.
		The electrons are shown as dots and crosses to indicate which atom the electrons come from, though all electrons are the same.
	www.wpbschoolhouse.btinternet.co.uk /page04/4_72bond.htm (4285 words)

	H2hybridization (Site not responding. Last check: 2007-11-02)
		The bond energy is the smallish difference between the substantial stabilizing energy of the isolated atoms (vs. separated electrons and protons) and the energy of the molecule.
		Naturally the approximation does a better job on the total energy (93%) than on the small bonding energy, since most of the energy, like most of the electron density is just that of the two separate atoms.
		Of course one cannot hybridize much without spoiling the description of the electron distribution in the vicinity of the nuclei, since for the atom the 2s and 2p orbitals are much higher in energy than the 1s orbital.
	www.chem.yale.edu /~chem125/125/quantum/Hybridoverlap/H2hybridization.html (700 words)

	Chapter 9, Section 2 (Site not responding. Last check: 2007-11-02)
		Because of resonance, the bonds between the central O atom and the outer O atoms are of equal length.
		F bonds are slightly bent back away from the nonbonding electron pair, suggesting that they are pushed by the nonbonding electron pair, which has a greater repulsive effect.
		Thus the electron-pair geometry is trigonal planar, and the bond angle is approximately 120°.
	cwx.prenhall.com /bookbind/pubbooks/blb/chapter9/medialib/blb0902.html (2094 words)

	Ch109_Lec_Bonding Supplement
		Note that the inner, "core" electrons for both atoms are shown as yellow dots, while the valence electrons for both atoms are shown as green.
		In the middle figure the upper diagram is a plot of the electron density in the x-y plane.
		In the simplest case, that of hydrogen, the resulting bond and molecule are cylindrically symmetrical, as seen in the figure and QuickTime movie of hydrogen.
	www.humboldt.edu /~chem_dpt/resources/C109_BndSup.htm (686 words)

	Bonding (Site not responding. Last check: 2007-11-02)
		Ionic bonds are bonds between ions and are always formed as the result of a gain and loss of electrons.
		Those electrons in the atom which have low ionization potentials are considered to be free to move through the lattice, giving metals the ability to conduct heat and electricity.
		However the bond between two atoms in the metal is still electrostatic, between the positive nuclei and the loosely held negative electrons.
	www.chemistrycoach.com /bonding.htm (1405 words)

	chap09 (Site not responding. Last check: 2007-11-02)
		This atom also has a double bond; this must contain a single (bonding) electron in a hybrid orbital (this would be for the sigma bond in the double bond), and another single electron in a p orbital (for the pi bond in the double bond).
		This atom has a single bond to a hydrogen atom, therefore there must be a single electron in a hybrid orbital.
		This must contain a single (bonding) electron in a hybrid orbital (this would be for the sigma bond in the double bond), and another single electron in a p orbital (for the pi bond in the double bond).
	wine1.sb.fsu.edu /chm1045/faq/chap09/chap09.htm (560 words)

	The electron-tunneling model of chemical bonding
		As the electron gets closer to the nucleus, the nuclear charge confines the electron to such a tiny volume of space that its energy rises, allowing it to "float" slightly away from the nucleus without ever falling into it.
		But the electron fluid is able to tunnel through the potential energy barrier separating the two wells; like any liquid, it will seek a common level in the two sides of the container.
		If the two electrons have opposite spins, the two fluids are able to interpenetrate each other, very much as two gases are able to occupy the same container.
	www.cartage.org.lb /en/themes/Sciences/Chemistry/Inorganicchemistry/Informationbonding/Electrontunneling/electrontunneling.htm (801 words)

	Covalent Bond (Site not responding. Last check: 2007-11-02)
		Covalent bonds are formed as a result of the sharing of one or more pairs of bonding electrons.
		This sharing of electrons is as a result of the electronegativity(electron attracting ability) of the two bonded atoms are either equal or the difference is no greater than 1.7.
		The dash is symbolic of the bonding pair.
	members.aol.com /profchm/covalent.html (421 words)

	ChemTeam: VSEPR - Odd Electron Molecules (Site not responding. Last check: 2007-11-02)
		Since there are three electron domains, this is a trigonal planar arrangement, but it is signified AX e, to signal the single electron domain, also called a half-filled orbital.
		The bond angles are not 120°, since the repulsive power of the single electron is less tha if there were two.
		The substance has 19 electrons to place and is a tetrahedral family member.
	dbhs.wvusd.k12.ca.us /webdocs/VSEPR/Odd-Electron-Molecules.html (239 words)

	Nonfatal Attractions: CHM 1311 Lecture 20 June 2000
		Bonding with another atom allows the valence electrons of both to taste the attraction of not one but two positive nuclei.
		The electrons might begin to avoid the space between the nuclei; an example would be if the two electrons were the same spin.
		But while Li H (a legitimate molecule, by the way), does aptly connote the electrons spending more of their time between the nuclei than before to constitute the bond, the structure is more often displayed as Li-H. That dash will mean bonding pair, and is always read as two electrons.
	www.utdallas.edu /~parr/chm1311/13110714.html (2020 words)

	VSEPR: Trigonal Bipyramidal Electronic Symmetry
		A premise of VSEPR theory is that groups of electrons surrounding a central atom repel one another and try to get as far away from one another as possible.
		However, electrons participating in a covalent atom-atom bond and non-bonding electrons (lone-pair electrons) do not repel one another with the same strength.
		The repulsion between two groups of non-bonding electrons, for example, is greater than the repulsion between two groups of bonding electrons.
	chemlabs.uoregon.edu /GeneralResources/models/AB5.html (195 words)

	[No title]
		This theory predicts that bonding (sigma bonds only) and non-bonding electron pairs in a molecule will adopt a geometry in which the distance between the electron pairs is maximized from one another in order to minimize the repulsions.
		Then we count how many pairs of electrons (triple bonds are counted as one pair) are around the central atom.
		Depending upon the number of non-bonding electron pairs, the shape of the molecule not counting non-bonding electron pairs can be: a) tetrahedral (no non-bonding pairs); b) trigonal pyramidal (one non-bonding pair); or c) "bent" or "V" (two non-bonding pairs).
	www.uwosh.edu /faculty_staff/xie/tutorial/vsepr.htm (361 words)

	Class Notes 09 CHM-121 EMU
		This number is obtained by adding the number of bonding and non-bonding electron pairs in the Lewis Structure
		It is the same as the electron-pair geometry only if all the electron pairs are equivalent, otherwise the molecular geometry is a distorted electron pair geometry.
		Based on the polarity of individual polar bonds and the molecular geometry a molecular polarity can be reasoned.
	www.emunix.emich.edu /~vites/121/notesc09.htm (100 words)

	Chemistry Tutorial
		If atoms are sharing electrons, then the bond between them is covalent.
		Oxygen and hydrogen form a highly polar bond because of the much stronger affinity for electrons by O. Insulin is a complicated molecule called a protein.
		Hydrogen bonds-result from electrostatic attraction between an electronegative atom (O or N) and a hydrogen atom that is bonded covalently to a second electronegative atom.
	www.biology.arizona.edu /biochemistry/tutorials/chemistry/page2.html (348 words)

	CHM 1341 Lecture Notes 18 June 1996
		That VSEPR speaks of pairs and not individual electrons is because it, like Lewis, considers the electrons shared in bonds to be part of an atom's valence shell.
		Carbon is the architect of so much interesting geometry because its four bonds, in methane say, array themselves to the corners of a perfect tetrahedron (all the hydrogens are equidistant from carbon and from one another), the most elementary of the Platonic solids.
		When it bonds, as ammonia say, there will be a total of four electron pairs again surrounding the central bonding atom (N), 3 are bonding and one non-bonding.
	www.utdallas.edu /~parr/chm1341/13410618.html (1345 words)

	[No title]
		bond to pairs, of nearby carbon atoms, in ethane gas molecules.
		that has,two electron orbitals,just inside,the outer bonding orbitals.
		Repels the nearby, inner orbital's electron, to the atom's opposite side.
	www.chem-data.com /orbital_drawings_m.htm (523 words)

	One Non-Bonding Electron Pair (Site not responding. Last check: 2007-11-02)
		This would force the three pairs of bonding electrons away from that non-bonding pair.
		This would force the bonding pairs to form a tri-pod arrangement which is referred to as a Trigonal Pyramidal geometry with a 107 degree separation of the bonding pairs from one another..
		One could place four of the bonding pairs in the same plane forming a square and the fifth bonding pair would be either above or below that plane.
	members.aol.com /profchm/one_nb.html (350 words)

	Diffusion Bonding and Electron Beam Diffusion Bonding of Titanium and Titanium Alloys
		Titanium is the easiest of al common engineering materials to join by diffusion bonding, due to its ability to dissolve its own oxide at bonding temperatures.
		This process is a variant of diffusion bonding in which only the interface region is heated, resulting in a considerable energy saving.
		The heating source is an electron beam which is swept over the area of the joint at such a speed that fusion of the titanium alloy is prevented.
	www.azom.com /details.asp?ArticleID=2545 (323 words)

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