13 Prelab Questions: Molecular Geometry 1. Complete the follow ing Table by fill
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13 Prelab Questions: Molecular Geometry 1. Complete the follow ing Table by filling in all the missing informatiom: or om Electron-pair Molecular or lon llybridization of CH H2O CO BFs NH, CIF SF XeF: SF. GeometryCentral Atom letrahedral bent sp tetrahedral T-shaped trigonal bipyramidal Based on VSEPR, explain why BeCl; is a linear molecule, but H:0 is a bent molecule. 2. 3. The H-CHH bond angle in CH, is 109.5. the H-N-H bond angle in NH, is 107. and the H-0-H bond angle in H:O is 104. Explain the trend and why, since the central atom is sp' hybridized, the angles in ammonia and water are not the ideal 109.5° of the tetrahedron. 65Explanation / Answer
The electron-pair geometry of methane is tetrahedral and so is its molecular geometry. The central atom carbon possesses a sp3 hybridisation.
Water has O with two bond pairs and 2 lone pairs arising from its 2s and 2p orbitals having sp3 hybridisation and giving a tetrahedral electron-pair geometry but a bent molecular geometry.
Carbon dioxide has no lone pairs in its central C atom and has two sigma and two pi-bonds. Since only two sigma bonds are formed, only one s and one p electrons are involved giving it a sp hybridisation and linear electronic and molecular grometry.
Boron trifluoride is sp2 hybridised and has all three F atoms lying on a plane 60 degrees to each other, giving the molecule a trigonal planar geometry. The absence of lone pairs in the B atom gives the electronic structure to also be trigonal planar.
In ammonia, the N atom is sp3 hybridised and due to its electronic configuration in the valence shell, it has one lone pair. This gives the molecule trigonal pyramidal geometry and a tetrahedral electronic geometry.
In chlorine triflouride, there exists 5 electron pairs around the central chlorine atom, giving it an electronic geometry of trigonal bipyramidal. But due to two of the electron pairs being non-bonding, the molecule becomes T-shaped. Due to three F atoms approaching for sigma bonding situations, the p5 chlorine atom, with its lone pairs has sp3 hybridisation in chlorine trifluoride.
Sulphur tetrafluoride is a hypervalent molecule. In it, the s,p and d electrons of S atom are involved in forming the molecule's 4 bond pairs along with 1 lone pair. This gives the molecule a trigonal bipyramidal electronic geometry, sp3d hybridisation and a see-saw molecular geometry.
Xenon difluoride has Xe in sp3d hybridisation as its 8 valence electrons form 2 bond-pairs and three lone pairs. This gives the molecule a linear geometry and a trigonal bipyramidal electronic geometry.
Sulphur hexafluoride is a hypervalent molecule in which all 6 valence electrons of sulphur are involved. This gives S a sp3d2 hybridisation and an octahedral electronic and molecular geometry.
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