Trigonal planar geometry and sp hybridization

It goes from a trigonal planar geometry and sp hybridization to a tetrahedral... 

Characteristics Planar molecule with hexagonal C framework trigonal-planar geometry and sp hybridization at C atoms a framework has C-C and C-H single bonds 2p-orbitals (one from each C atom) overlap side-by-side form three rr-bonds six 7t-electrons) delocalized over the entire six C atom ring... 

Characteristics one C=C double bond (a plus 7t) other C-C bonds and all C-H bonds single (a) trigonal-planar geometry and sp hybridization at double-bonded C atoms tetrahedral geometry at other C (sp ) atoms rotation not allowed about double C=C bond rotation allowed about C-C single bonds... 

Trigonal-planar geometry with sp hybridization at C, 120 Z O-C-0 angles, and Csp -02p single bonds. Remaining C 2p-orbital can overlap with O 2p-orbitals to form a TT-bond in each of three ways corresponding to the resonance structures. Therefore, each carbon-oxygen bond can be viewed as one a-bond and one-third of a rr-bond. 

As the reaction takes place, the carbon atom undergoes a change from trigonal planar geometry and sfp hybridization to tetrahedral geometry and sp hybridization. 

Because the central carbon atom in allene has two charge clouds (two double bonds), it has a linear geometry and is sp-hybridized. Because the two terminal carbon atoms have three charge clouds each (one double bond and two C-H bonds), they have trigonal planar geometry and are sp2-hybridized. The central carbon uses its sp orbitals to form two cr bonds at 180° angles and uses its two unhybridized p orbitals to form... 

When there are three electron groups around the central atom, it is sp hybridized. AB molecules and ions with no lone pairs on the central atom have trigonal planar electronic geometry, trigonal planar molecular geometry and sp hybridization on the central atom. 

X-ray Crystallographic Analysis. The most important structural feature of a carbonyl compound is its trigonal planar geometry, which results from the sp -hybridized carbon. Since it has been revealed experimentally and theoretically that dimetallenes have a trans-bent structure in contrast to... 

The carbonyl carbon of an amide is sp hybridized and has trigonal planar geometry. A second resonance structure can be drawn that delocalizes the nonbonded electron pair on the N atom. Amides are more resonance stabilized than other acyl compounds, so the resonance structure having the C=N makes a significant contribution to the hybrid. 

The orbitals of carbocations are generally sp" hybridized to that the three full orbitals are arranged in a trigonal planar geometry about the carbon nucleus. The remaining p orbital is empty and will readily accept a pair of electrons from another atom. Because of the symmetry of this geometric arrangement, nucleophilic attack is equally favorable above or below the plane fonned by the full orbitals. 

Ethylene is a planar molecule, as the structural representations of Figure 1.24 indicate. Because sp hybridization is associated with a tetrahedral geometry at carbon, it is not appropriate for ethylene, which has a trigonal planar geometry at both of its carbons. The hybridization scheme is determined by the number of atoms to which the carbon is directly attached. In ethane, four atoms are attached to carbon by a bonds, and so four equivalent sp hybrid orbitals are required. In ethylene, three atoms are attached to each carbon, so three equivalent hybrid orbitals are required. As shown in Figure 1.25, these three orbitals are generated by mixing the carbon 2s orbital with two of the 2p orbitals and are called sp hybrid orbitals. One of the 2p orbitals is left unhybridized. 

Racemization is a common result in 8 1 reactions because the carbocation intermediate is sp hybridized and has trigonal planar geometry. However, many 8 1 reactions result in an excess of the product of inversion due to the formation of an ion-pair. 

Use valence shell electron pair repulsion (VSEPR) to predict geometry about any carbon or nitrogen atom. Count the number of other atoms attached to it and add to that the number of lone pair(s) it may contain. Two = linear and sp hybridized 3 = trigonal planar and sp2 hybridized 4 = tetrahedral and sp3. Not complicated. 

Each carbon is identical but now has three bonding electron domains that surroimd it. Therefore, the hybridization of each carbon atom is sp, and each carbon has local trigonal planar geometry with 120° angles. 

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