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Why axial bonds are longer than equatoria bonds in PF5 bonds in space geometry?
Wiki User
∙ 11y ago
The axial bond is 158 pm and the equatorial is 152 pm.
One explanation is that the hybridisation of the equatorial bonds is sp2 and the hybridisation of the equatorial is pd, the greater s character of the equatorial making the bond shorter. (taken from text book Inorganic chemistry by House)
I know of no theretical study that backs this up.
Most text books duck this ,e.g Greenwood and Wiberg.
Wiki User
∙ 11y ago
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Why PCl5 is reactive but SF6 is stable?
PCL5 is formed two types of P-CL bond, equitorial and axial bonds. The axial bonds suffer more repulsion than the equitorial bonds, and they can easily break, which makes PCL5 unstable. SF6 is largely inert due to steric hindrance.
What molecular geometry exists when a central carbon atom bonds to four other atoms?
tetrahedral
Why PCl5 is used in organic rections than NCl5?
The fact that NCl5 does not exist might come into play. Think about it. NCl5 does not exist
Why are carbon hydrogen bonds longer than hydrogen hydrogen bonds?
due to the property of catenation
Are all single bonds sigma bonds why?
A sigma bond is defined as bond with axial symmetry- where the axis runs between the two atoms being bonded. The bond is formed by overlap of atomic orbitals that point along the axis (these can be s orbitals, p d or hybrid orbitals.) In practise the majority of single bonds encountered are sigma bonds, this is particularly true in organic chemistry. However there is no logical reason why thereall single bonds (sharing of a par of electrons) have to be sigma bonds. One example is the bonding in Zeise's salt where a filled d- orbital on the metal atom bonds to an alkene by overlap with a pi antibonding orbital- thisbond has pi symmetry and does not have axial symmetry and there is only one pair of electrons.
Why axial bonds are larger than equatorial bonds?
axial bonds are longer than equatorial bonds becz axial bond contain very less "s" character as compare to equatorial bond, hence probability of finding it near nucleus is less hence force of attraction by nucleus is less as compare to to equatorial bonds
Why PCl5 is reactive but SF6 is stable?
PCL5 is formed two types of P-CL bond, equitorial and axial bonds. The axial bonds suffer more repulsion than the equitorial bonds, and they can easily break, which makes PCL5 unstable. SF6 is largely inert due to steric hindrance.
What is the electronic geometry of methane?
All of the hydrogens on methane are evenly spaced apart at 109.5 degree bonds. This makes the geometry tetrahedral.
The electron geometry of the bonds and lone pairs around the oxygen is water is?
tetrahederal.
What is the molecular geometry for CH3I?
Since there is 4 electron domains which are all single bonds without any lone pairs, the molecular geometry is tetrahedral.
Describe the role of each of the following in predicting molecular geometries a unshared electron pairs by double bonds?
Lone electron pairs give the geometry a triangular base, while double bonds make the molecular geometry bent or angular.
What molecular geometry exists when a central carbon atom bonds to four other atoms?
tetrahedral
Why PCl5 is used in organic rections than NCl5?
The fact that NCl5 does not exist might come into play. Think about it. NCl5 does not exist
Does PCl4 have resonance structures?
I would imagine it has a tetrahedral geometry since the Cl atoms are quite large in size, thus electron replusion is high, so adopts a geometry that gives the largest angle between the C-Cl bonds.
What is the molecular geometry if you have 3 single bonds and 1 lone pair around the central atom?
Trigonal Pyramidal
Why are carbon hydrogen bonds longer than hydrogen hydrogen bonds?
due to the property of catenation
Are all single bonds sigma bonds why?
A sigma bond is defined as bond with axial symmetry- where the axis runs between the two atoms being bonded. The bond is formed by overlap of atomic orbitals that point along the axis (these can be s orbitals, p d or hybrid orbitals.) In practise the majority of single bonds encountered are sigma bonds, this is particularly true in organic chemistry. However there is no logical reason why thereall single bonds (sharing of a par of electrons) have to be sigma bonds. One example is the bonding in Zeise's salt where a filled d- orbital on the metal atom bonds to an alkene by overlap with a pi antibonding orbital- thisbond has pi symmetry and does not have axial symmetry and there is only one pair of electrons.
