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	Orbital hybridisation - Wikipedia, the free encyclopedia
		In chemistry, hybridisation or hybridization (see also spelling differences) is the concept of mixing atomic orbitals to form new hybrid orbitals suitable for the qualitative description of atomic bonding properties.
		Hydrogen orbitals are used as a basis for simple schemes of hybridisation because it is one of the few examples of orbitals for which an exact analytic solution to its Schrödinger equation is known.
		Hybridization theory is an integral part of organic chemistry and in general discussed together with molecular orbital theory in advanced organic chemistry textbooks although for different reasons.
	en.wikipedia.org /wiki/Orbital_hybridisation (1580 words)

	Organic Chemistry at Penn State: Quantum Primer - A Brief (Site not responding. Last check: 2007-10-21)
		Orbitals are volumes of space where electrons are allowed to spend their time.
		To the first approximation, the lowering of energy of the bonding orbital as compared to the constituent atomic orbitals is the same as the corresponding rise in energy of the antibonding orbital.
		All atoms in the molecule provide their atomic orbitals for construction of MO, but not all atomic orbitals must participate in all MO. The number of MO is equal to the number of atomic orbitals used to generate them.
	courses.chem.psu.edu /chem38/quantum/quantum-brief.html (1293 words)

	hybrid orbitals
		Both of these facts are difficult to immediately rationalize given the spatial arrangement of the valence orbitals in C (the 2s and the three 2p orbitals), and the fact that the 2s orbital is filled in the ground state of the carbon atom.
		The fundamental tenet of the HOM is that the atomic orbitals of differing energies will mix to form a new set of hybrid orbitals with energies determined by a weighted average of the atomic orbitals that combined.
		The hybrid orbital model is often used to explain the delocalized structures that arise when it is possible to draw multiple resonance structures for a molecule.
	www.wellesley.edu /Chemistry/chem120/hybrids.html (848 words)

	Part I of chapter 1
		orbitals with the analogous orbitals of adjacent atoms (e.g.
		The geometrical consequence of the sp hybridization is the linearity of the structure.
		Orbital hybridization gives instead four orbitals, one of which is filled (two electrons) and does not participate in bonding (two 2p nonbonding electrons frequently called a lone electon pair).
	tigger.uic.edu /~kbruzik/text/chapt1a.htm (900 words)

	Atomic Orbital Theory
		Hybridization is similar to the hybridizations that occur in the plant and animal kingdoms.
		The sp hybrid orbitals are oriented in a linear fashion with the hybrid orbitals 180 degrees separated.
		For the sp hybrid orbitals the percentage of s character is 50% (1/2 of the orbitals used in the hybridization process are s).
	members.aol.com /profchm/vb.html (2003 words)

	Lewis.dot.strucs (Site not responding. Last check: 2007-10-21)
		Enter hybridization theory proposed by Linus Pauling who showed mathematically how hybrid orbitals could be formed from s and p orbitals to give sp3, sp2 and sp hybrid orbitals.
		Stronger bonds are formed when hybridizaiton occurs and this follows directly from the fact that when hybrid orbitals are formed there is directionality to them because p orbitals have a subtractive and additive mode of combining with s orbitals (because of the sign of the orbitals).
		The sp hybrid orbitals form [[sigma]] bonds with the attached carbons and the p orbitals are orthogonal to one another and are empty.
	www.chem.tamu.edu /rgroup/romo/Chem227_502ontheWEB/hybridization.html (348 words)

	SparkNotes: Molecular Orbitals: Molecular Orbital Theory
		From the orbital correlation diagram above you should notice that the amount of stabilization due to bonding is equal to the amount of destabilization due to antibonding, because there are two electrons in the bonding orbital and two electrons in the antibonding orbital.
		Hybrid orbitals describe the bonding in polyatomic molecules one bond at a time.
		Each hybrid orbital is composed of a combination of an s and a p orbital on the central atom.
	www.sparknotes.com /chemistry/bonding/molecularorbital/section1.html (1814 words)

	Organic Chemistry at Penn State: Quantum Primer III (Site not responding. Last check: 2007-10-21)
		We have to use each atomic orbital completely, we have to generate normalized molecular orbitals (MOs), and the number of MOs must be equal to the number of atomic orbitals that we have started with.
		Predicting the ordering of the energy levels of the orbitals that are farther removed from the line dividing the occupied and unoccupied orbitals is more difficult, short of performing calculations.
		Since interaction between filled (occupied) orbitals does not result in net bonding (electron-electron repulsion), and interaction between empty (unoccupied) orbitals cannot contribute to bonding (no electrons to be shared) only the interaction between occupied and unoccupied will provide the initial impetus for the reorganization of existing bonding.
	courses.chem.psu.edu /chem38/quantum/quantum3.html (1337 words)

	Chemistry Lecture Notes
		The hybridized orbitals basically look like stretched-out balloons going to the other atoms (from C to the 2 Os, N to the three Hs, C to the four Hs, etc.).
		The yellow orbitals on the right are the H 1s orbitals, while the green ones are the Be sp orbitals.
		The bonding orbital is lower energy than the two atoms apart, and the antibonding orbital is higher energy.
	members.tripod.com /~Cat609/Chemistry/11-17-98.html (372 words)

	Molecular orbital (via CobWeb/3.1 planetlab1.tamu.edu) (Site not responding. Last check: 2007-10-21)
		Instead, one approximates the molecular orbitals as linear combinations of some basis for the electron's state space, usually what each atom's orbitals would be if it were on its own.
		To make up for this, we often take linear combinations of molecular orbitals so that electron density is localized around atoms, and between them (hybridized bonds), but it should be remembered that these are not stationary states, so although they are useful in treating electron density they have no real meaning in terms of energy.
		The linear combination of atomic orbitals approximation for molecular orbitals was introduced in 1929 by Sir John Lennard-Jones.
	molecular-orbital.iqnaut.net.cob-web.org:8888 (829 words)

	February 23, 1995
		The key feature of this diagram is that we started with two 2s atomic orbitals each with one electron and we end up with two molecular orbitals, one of which has a pair of electrons in a lower energy, more stable configuration.
		Clearly, you would have to know or accept the mathematics that we have now mixed two atomic orbitals, equal in energy, and producted two molecular orbitals, unequal in energy but one of which was more stable than the original atomic orbital.
		molecular orbital places the pair of electrons directly between the two nuclei, precisely the situation that we would expect if bonding were the outcome.
	www.uky.edu /Classes/BCH/401/Supplements/molecularorbitals.htm (965 words)

	Aromaticity: A Characteristic of Fluorescence Molecules (Site not responding. Last check: 2007-10-21)
		hybridization, which is a combination of one s-orbital combined with two p-orbital (of the three p-orbital) forming a planar orbital with 120º angles (planar hexagon ring).
		Another representation of an aromatic ring that illustrates the stability of aromatic compounds is the molecule orbital diagram.
		In molecule orbital diagram there are three portions to a molecule as illustrated in Figure 6a, b, and c.
	www.sas.upenn.edu /~jonessm/MCE507A/Aromaticity.htm (250 words)

	Method for forming a hard carbon thin film on article and applications thereof - Patent 4772513
		In this way, the deposited carbon layer is predominantly amorphous carbon of inclusion of hybridized orbital SP.sup.2 bond and hybridized orbital SP.sup.3 bond and crystalline carbon particles of hybridized orbital SP.sup.3 bond dispersed in said amorphous carbon, or an amorphous carbon of inclusion of hybridized orbital SP.sup.2 bond and hybridized orbital SP.sup.3 bond.
		Thus, it has been confirmed that the fine crystalline grains (crystalline particles of the diamond structure) of the SP.sup.3 bond were dispersed in the amorphous layer of the hybridized orbital SP.sup.2 bond and hybridized orbital SP.sup.3 bond, or that an amorphous carbon of the SP.sup.2 bond and SP.sup.3 bond was formed.
		Thus, it has been found due to the electron diffraction and ESCA spectrum that the hardness was within a range of HV 3,000 to 4,000 and the diamond particles having the hybridized orbital SP.sup.3 bond were dispersed in the carbon layer mainly having the hybridized orbital SP.sup.2 bond.
	www.freepatentsonline.com /4772513.html (4563 words)

	ORGANIC CHEMISTRY II PRACTICE PROBLEMS THURS. JAN. 16, 1997
		hybridized; one pair of electrons on the oxygen is in a p orbital that is part of the
		hybrid orbital, which is perpendicular to the p orbital, and thus cannot interact with the
		Instead, the nitrogen is sp3 hybridized as it would be in a regular amine.
	www.muhlberg.edu /depts/chemistry/chem202woh/PA011697.htm (526 words)

	Hybridization of Atomic Orbitals (Site not responding. Last check: 2007-10-21)
		Hybrid orbitals involving s and p atomic orbitals are explained in detail and three-dimensional models illustrate each type of hybrid set.
		Subsequently, hybrid orbitals involving the participation of d orbitals are described.
		After the student chooses the correct hybridization, the correct type and spatial orientation of a hybridized orbital must be selected for each bond in the molecule.
	www.cem.msu.edu /~gencem/hybrd (285 words)

	Experiment 12
		This modeling exercise will familiarize students with the carbon-chain nature of organic compounds, the types of hybridized orbitals and bonding between atoms in organic compounds, the general structures of characteristic functional groups, and types of structures necessary to form geometric isomers.
		The specific arrangement in space of atoms linked together is dependent on the type of hybridized orbital involved in the bond.
		Butane, CH is an example of a straight-chain hydrocarbon with each carbon having four sp3 hybrid orbitals and tetrahedral geometry.
	core.ecu.edu /chem/chemlab/exper12/objectives.htm (861 words)

	World of Carbon (Site not responding. Last check: 2007-10-21)
		A covalent chemical bond is formed between two atoms when their orbitals overlap and share a pair of electrons.
		hybridization to form sigma bonds with three nearest neighbors, separated by 1.4210 Angstroms, in the layer.
		The bond angles are all 109 degrees, typical of sp3 hybridization.
	invsee.asu.edu /nmodules/Carbonmod/bonding.html (725 words)

	Re: y electronegativity of carbon in methane is less than the carbon in ethene
		In an s atomic orbital, electrons are allowed to get much closer to the nucleus -- and are therefore more tightly held -- than in a p atomic orbital.
		As the p proportion of the mixture rises, the amount of "s-character" falls and the electrons in that orbital will be more loosely held by the central atom.
		When a C-H bond is deprotonated, the carbanion lone pair is held, according to the Pauling model, in a hybrid atomic orbital.
	www.madsci.org /posts/archives/sep2000/968887193.Ch.r.html (373 words)

	metallization
		The valence s-orbital of the metal adatom hybridizes most strongly with bands of surface states to produce a singly occupied orbital whose energy must consequently lie in the gap between the occupied and unoccupied surface bands of the silicon.
		The energy of the orbital is determined by the chemical bond formed between the metal and silicon, and this in turn fixes the exponent with which the orbital decays with distance outside the cell in which it is centered.
		It is this hybridized orbital of the isolated metal adatom which forms our basis for the electronic states of the metal overlayer, and because the spatial decay of the orbital outside its central cell is determined by the chemistry of the metal-silicon bond, we expect the different alkalis to behave similarly.
	darkwing.uoregon.edu /~msiuo/haydock/Numev.htm (3759 words)

	[No title]
		Overlap of silicon d-orbital with occupied hybridized and unhybridized N orbitals of trisilylamine, respectively.
		The molecular orbitals for the silyl fragments are calculated and presented in the Molecular Orbital diagram in Figure 4.
		The frontier orbitals of an N atom are familiar to you — the 2s and 2p orbitals.
	www.usm.maine.edu /~tracy/chy374/chy374labs/ModelingComputation.doc (2499 words)

	Nuclear Geometry: Rules (via CobWeb/3.1 planetlab1.tamu.edu) (Site not responding. Last check: 2007-10-21)
		A radical string pinned between quarks in adjacent nuclear shells may become a hybridized orbital from distortion of the radical string.
		They are more difficult to mensurate, without specific rules governing their amplitude, the particles containing them must have their loop values set on a sliding scale dependent on the length of the sinusoidal string, which may wander between physical amplitude limits imposed by the specific shell geometry.
		Hybridized orbitals of this nature should be abundant in metals, hybridization permits "daisy-chain" bonds utilizing a single interstitial electron between nuclei.
	www.stringtheory.com.cob-web.org:8888 /rules.htm (2584 words)

	Lesson plan (via CobWeb/3.1 planetlab1.tamu.edu) (Site not responding. Last check: 2007-10-21)
		The geometry of the SP hybridized orbital is tetrahedral with 109.5 angles with symmetry.
		These P orbitals overlap side by side forming pi bonds and the head -on overlap of SP orbitals form sigma bonds.
		The superscripts in hybrid orbitals refer to the number of orbitals of that particular type that are involved in the orbital blending.
	www.coe.drexel.edu.cob-web.org:8888 /ret/personalsites/2005/Weerasooriya/lesson.html (877 words)

	Metal Stannylene Complexes
		The hybridization of the central carbon atom is sp
		hybridized orbital is considerably lower in energy than the p-orbital and so the ground state structure of free stannylenes is always a singlet.
		hybridized orbital) which it could donate to the tungsten, formation of a bond between the tin and the tungsten centers will result in tungsten having 18 electrons surrounding it (5 from each of the Cp ligands, 6 from the W itself, and 2 from the stannylene ligand).
	web.grinnell.edu /individuals/mobleyt/sumres/metal_stannylene.htm (1700 words)

	Heavier Carbene Analogues
		This is because the tendency to form hybridized orbitals decreases on descending group 14...I accept this fact, but I don't fully understand it.
		In an sp2 orbital the highest electron density is farther away from the nucleus.
		Hybridisation in higher elements normally looks different because d-orbitals are also used.
	www.chemicalforums.com /index.php?topic=5914.0 (477 words)

	Bonding in Materials (Site not responding. Last check: 2007-10-21)
		Hybridization occurs by donation of one 2s shell electron from C into its 2p orbital.
		The shape of this hybridized orbital is tetrahedral with bond angles 109.5
		Because the hydrogens share one electron each with the central C atom, they do not bond to any other atoms, and the molecule is stable in this isolated form.
	www.mse.uiuc.edu /info/mse182/t86.html (99 words)

	General Chemistry, chem 1b, 2nd midterm exam, spring, 20000
		hybridized and the atoms attached to these carbons do not lie in a plane.
		The electrons belonging to the pi orbitals are delocalized, i.e.
		hybridized orbital AND a pi-type bond consisting of the overlap of a C unhybridized 2p orbital with an O unhybridized 2p orbital.
	pages.pomona.edu /~wes04747/ex_soln/exam_2b3.htm (772 words)

	HONORS ORGANIC I
		This means each atom in the ring has a p orbital, and there are a total of 6
		While it is cyclic, could be planar, and each atom in the ring has a p orbital, there are a total of 8
		hybridized (it makes 4 sigma bonds), so there is no way it can contribute a p orbital to the
	www.muhlenberg.edu /depts/chemistry/chem202woh/HOPA031402.html (435 words)

	C-C Bonds (Site not responding. Last check: 2007-10-21)
		A hybrid orbital always has higher energy than the lowest energy of its atomic components.
		In bonding with hybridized atomic orbitals there is overlap between the two sp orbitals centered in the atomic nuclei.
		The shape of a hybridized orbital is different than the pure atomic orbitals.OK? And it is very nice seeing a brazilian fellow around here...
	www.newton.dep.anl.gov /askasci/chem00/chem00343.htm (455 words)

	Glossary
		These orbitals are actually sharing a pinned string with the electrons (an Orphan string for the electrons, a Radical string for the nucleus).
		P.V.B's captured by a lower nuclear shell can sometimes be sandwiched between quarks in adjacent nuclear shells, resulting in a flattened lobe, providing a hybridized orbital (linearization) for metallic daisy-chain bonds requiring only a single interstitial electron nestled between nuclei.
		The pinned string is normally "blown" away from the surface of its host quark by charge currents, resulting in lobes, but in this situation the string is trapped between like charge mirrors, and an oblate (tangential) lobe is generated.
	www.stringtheory.com /gloss.htm (4090 words)

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