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12 Jan 2021

Which of the following shows the orbital diagram of for two hybridized orbitals of carbon atoms bonding? Note that the orange nodes with a purple center are the hybrid orbitals and the blue and white nodes are the  orbitals.

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General Chemistry 1
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Apply Lewis, VSEPR, and Valence Bond Theory simultaneously
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Greg Montoya
Greg MontoyaLv10
12 Jan 2021

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Related questions

Which statement correctly correlates s or p bonding atoms and theirrespective bonding orbitals in formaldehyde?


A)The oxygen atom (with its 2s orbital) forms a s bond with one ofthe three sp2 hybrid orbitals of the carbon atom; the two hydrogenatoms (with their 1s orbitals) each form a s bond with one of thethree sp2 hybrid orbitals of the carbon atom.
B)The oxygen atom (with its 2p orbital) forms a p bond with one ofthe three sp2 hybrid orbitals of the carbon atom; the two hydrogenatoms (with their 1s orbitals) each form a s bond with one of thethree sp2 hybrid orbitals of the carbon atom.
C)The oxygen atom (with its 2p orbital) forms a p bond with the pzorbital of the carbon atom; the two hydrogen atoms (with their 1sorbitals) each form a s bond with one of the two sp2 hybridorbitals of the carbon atom.
D)The oxygen atom (with its 2p orbital) forms a s bond with one ofthe three sp2 hybrid orbitals of the carbon atom; the two hydrogenatoms (with their 1s orbitals) each form a s bond with one of thethree sp2 hybrid orbitals of the carbon atom. The oxygen atom alsoforms a p bond with carbon which involves the 2pz orbitals ofoxygen and carbon.

According to valence bond theory, which atomic orbitals of carbon may be hybridized to account for bonding? Why?

1s, 2s, and 2p orbitals all may hybridize; these orbitals are of the same phase.
Only 2p orbitals may hybridize; the 2p orbital is carbon’s highest-energy atomic orbital.
Only 1s and 2s orbitals of carbon may hybridize; each contains electrons to share in bonding.
Only 2s and 2p may hybridize; these orbitals contain valence electrons used in bonding.
Only 2s orbitals may hybridize; these orbitals contain valence electrons.

Use valence bond theory to describe the bonding and geometry in theSeF4 molecule.

A. The central atom is Se, which has five electron groups around it(four bonding pairs and one nonbonding/lone pair). Theelectron-group geometry is trigonal bipyramidal (and the moleculargeometry is see-saw). To facilitate this geometry, the Se atom'sorbitals are hybridized as sp3d orbitals. Four of these hybridorbitals contain one of Se's 6 valence electrons each, and thesehybrid orbitals overlap with unhybridized p orbitals of the four Fatoms. The fifth hybrid orbital of Se contains a lone pair ofelectrons. There are 4 sigma bonds and 0 pi bonds in thismolecule.
B. The central atom is Se, which has six electron groups around it.The electron-group geometry is octahedral. To facilitate thisgeometry, the Se atom's orbitals are hybridized as sp3d2 orbitals.Four of these hybrid orbitals contain one of Se's 6 valenceelectrons each, and these hybrid orbitals overlap with unhybridizedp orbitals of the four F atoms. The fifth and sixth hybrid orbitalsof Se contain lone pairs of electrons. There are 4 sigma bonds and0 pi bonds in this molecule.
C. The central atom is Se, which has four electron groups aroundit. The electron-group geometry is tetrahedral. To facilitate thisgeometry, the Se atom's orbitals are hybridized as sp3 orbitals.These hybrid orbitals overlap with unhybridized p orbitals of thefour F atoms. There are 4 sigma bonds and 0 pi bonds in thismolecule.
D. The central atom is Se, which has four electron groups aroundit, two single bonds and two double bonds. The electron-groupgeometry is tetrahedral. To facilitate this geometry, the Se atom'sorbitals are hybridized as sp3 orbitals. These hybrid orbitalscontain one electron each of Se's 6 valence electrons, and thesehybrid orbitals overlap with unhybridized p orbitals of the four Fatoms. The final 2 electrons of Se's 6 valence electrons reside inunhybridized p orbitals, which overlap with unhybridized p orbitalsof the F atoms. There are 4 sigma bonds and 2 pi bonds in thismolecule.

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