Examples of hybridization in the following topics:
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- In order to explain the bonding, the 2s orbital and two of the 2p orbitals (called sp2 hybrids) hybridize; one empty p-orbital remains.
- sp2 Hybridization in Ethene and the Formation of a Double Bond
- In this case, carbon will sp2 hybridize; in sp2 hybridization, the 2s orbital mixes with only two of the three available 2p orbitals, forming a total of three sp hybrid orbitals with one p-orbital remaining.
- The carbon atoms are sp2 hybridized.
- Recognize the role of sp2 hybridized atoms in sigma and pi bonding.
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- sp3 hybrid orbitals form when a single s and three p orbitals hybridize.
- In hybridization, carbon's 2s and three 2p orbitals combine into four identical orbitals, now called sp3 hybrids.
- For example, in the ammonia molecule, the fourth of the sp3 hybrid orbitals on the nitrogen contains the two remaining outer-shell electrons, which form a non-bonding lone pair.
- Ethane can form by replacing one of the hydrogen atoms in CH4 with another sp3 hybridized carbon fragment.
- Explain the process of hybridization as it applies to the formation of sp3 hybridized atoms.
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- In chemistry, hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals suitable for describing bonding properties.
- The hybrids are named for the atomic orbitals involved in the hybridization.
- For this molecule, carbon will sp2 hybridize.
- In this case, sp hybridization leads to two double bonds.
- Describe the role of hybridization in the formation of double and triple bonds.
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- In sp hybridization, the s orbital overlaps with only one p orbital.
- When atomic orbitals hybridize, the valence electrons occupy the newly created orbitals.
- The hybridization process involves mixing of the valence s orbital with one of the valence p orbitals to yield two equivalent sp hybrid orbitals that are oriented in a linear geometry.
- Hybridization of an s orbital and a p orbital of the same atom produces two sp hybrid orbitals.
- Each hybrid orbital is oriented primarily in just one direction.
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- These hybrid orbitals have a specific orientation, and the four are naturally oriented in a tetrahedral fashion.
- Click on the following link for a model of this hybridization (http://www2.chemistry.msu.edu/faculty/reusch/VirtTxtJml/Jmol-11.2/hyborbtl2.htm).
- A mixing of the 2s-orbital with two of the 2p orbitals gives three sp2 hybrid orbitals, leaving one of the p-orbitals unused.
- Two sp2 hybridized carbon atoms are then joined together by sigma and pi-bonds (a double bond), as shown in part B.
- Finally, in the case of carbon atoms with only two bonding partners only two hybrid orbitals are needed for the sigma bonds, and these sp hybrid orbitals are directed 180º from each other.
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- Double and triple bonds can be explained by orbital hybridization, or the 'mixing' of atomic orbitals to form new hybrid orbitals.
- Hybridization describes the bonding situation from a specific atom's point of view.
- A combination of s and p orbitals results in the formation of hybrid orbitals.
- From the perspective of the carbon atoms, each has three sp2 hybrid orbitals and one unhybridized p orbital.
- A schematic of the resulting orientation in space of sp3 hybrid orbitals.
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- Finally, Linus Pauling integrated Lewis' proposal and the Heitler-London theory to give rise to two additional key concepts in valence bond theory: resonance and orbital hybridization.
- We see the concept of orbital hybridization arise when bonding orbitals share the characteristics of several types of orbitals.
- When we apply valence bond theory to a coordination compound, the original electrons from the d orbital of the transition metal move into non-hybridized d orbitals.
- The electrons donated by the ligand move into hybridized orbitals of higher energy, which are then filled by electron pairs donated by the ligand.
- Calculate the theoretical hybridization of a metal in a coordination complex based on valence bond theory
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- This averaging of electron distribution over two or more hypothetical contributing structures (canonical forms) to produce a hybrid electronic structure is called resonance.
- Likewise, the structure of nitric acid is best described as a resonance hybrid of two structures, the double headed arrow being the unique symbol for resonance.
- The stability of a resonance hybrid is always greater than the stability of any canonical contributor.
- Consequently, if one canonical form has a much greater stability than all others, the hybrid will closely resemble it electronically and energetically.
- On the other hand, if two or more canonical forms have identical low energy structures, the resonance hybrid will have exceptional stabilization and unique properties.
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- Bond length between two atoms depends on factors such as the orbital hybridization and the electronic nature of the components.
- The actual distance between two atoms in a molecule depends on factors such as the orbital hybridization and the electronic nature of its components.
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- The sp-hybrid carbon atoms of the triple-bond render alkynes more electrophilic than similarly substituted alkenes.
- Isolated carbon double-bonds are not reduced by sodium in liquid ammonia, confirming the electronegativity difference between sp and sp2 hybridized carbons.