Chemistry, 26.01.2020 20:31 Loveraeee17

If all of the bonding electrons in a molecule are bonded in two hybrid sp orbitals, which shape does the molecule most likely have?

linear
tetrahedral
trigonal planar
trigonal pyramidal

Answers: 1

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Two hybrid sp bond , it will form Linear

the answer is linear !!
If all of the bonding electrons in a molecule are bonded in two hybrid sp orbitals, which shape does

If all of the bonding electrons in a molecule are bonded in two hybrid sp orbitals, which shape does

Answer from: ava5015

Option (a) is the correct answer.

Explanation:

Only sigma bonds involve bonding electrons in a molecule. Each sigma bond will have two electrons.

A sp hybrid orbital can only be formed when one s-orbital combines with one p-orbital.

For example, $BeF_{2}$ is sp hybridized because beryllium has 2 electrons for bonding whereas each fluorine atom has one electron for bonding. Thus, both beryllium and fluorine atoms will combine together to attain stability.

When fluorine atoms combine with beryllium then due to the electron-electron repulsion between each fluorine atom, they will move apart from each other forming an angle of 180 degrees. As a result, there will be less repulsion and hence the molecule will become more stable.

Thus, $BeF_{2}$ has linear geometry.

Hence, we can conclude that if all of the bonding electrons in a molecule are bonded in two hybrid sp orbitals, then the molecule will have linear shape.

Answer from: trapqueenriz12

Option (a) is the correct answer.

Explanation:

Only sigma bonds involve bonding electrons in a molecule. Each sigma bond will have two electrons.

A sp hybrid orbital can only be formed when one s-orbital combines with one p-orbital.

Thus, $BeF_{2}$ has linear geometry.

Hence, we can conclude that if all of the bonding electrons in a molecule are bonded in two hybrid sp orbitals, then the molecule will have linear shape.

Answer from: Quest

Cr(oh)3 -> cr(3+) + 3oh-

Answer from: Quest

by the combination of an unlimited number of elements

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