Answer is Both p oribitals are perpendicular to the F-Be-F bond axes . The elect

Question

Answer is Both p oribitals are perpendicular to the F-Be-F bond axes.

The electron configuration of Be = 1s22s2

Because it has no unpaired electrons, the Be atom in its ground state cannot bond with the fluorine atoms. The Be atom could form two bonds, however, by “promoting” one of the 2s electrons to a 2p orbital. So, Be will undergo sp hybridization.

The electrons in the sp hybrid orbitals can form bonds with the two fluorine atoms. Because the sp hybrid orbitals are equivalent but point in opposite directions, BeF2 has two identical bonds and a linear geometry. The remaining two 2p atomic orbitals of Be remain unhybridized and are vacant will be perpendicular to the Be-F bonds.

Explanation / Answer

Give It Some Thought 9.7 Part A What is the orientation of the two unhybridized p orbitals on Be with respect to the two Be Fbonds? Both p orbitals are perpendicular to the F - Be Fbond axes. Both p orbitals are parallel to the F Be F bond axes. O One p orbital is perpendicular to the F - Be F bond axis, the other is parallel. Submit My Answers Give Up

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