Which of the following clusters of orbitals could form a shape similar to that shown here (Figure 3) in the valence shell of an isolated atom or one about to enter into bonding with other atoms?

A) five sp³d
B) three sp² and one p orbital

"three sp²" is the one cluster of orbitals among the following choices given in the question that could form a shape similar to that shown here (Figure 3) in the valence shell of an isolated atom or one about to enter into bonding with other atoms. The correct option among all the options given in the question is the second option.

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pstnonsonjoku pstnonsonjoku · Answer 2 · 2021-10-23T19:04:21+02:00

The cluster shown here is formed by five sp³d orbitals.

Hybridization is an idea put forward by Linus Pauling to explain the bonding in certain molecules. Hybridization has to do with the mixing of atomic orbitals. When atomic orbitals mix, equivalent hybrid orbitals suitable for bonding are formed.

The number of hybrid orbitals formed is equal to the number of atomic orbitals that were combined to form the hybrid orbitals. For sp³d hybrid orbitals; three p, one s and one d orbitals, a total of five atomic orbitals combine to form five equivalent sp³d hybrid orbitals.

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Which of the following clusters of orbitals could form a shape similar to that shown here (Figure 3) in the valence shell of an isolated atom or one about to enter into bonding with other atoms? A) five sp³d B) three sp² and one p orbital

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Which of the following clusters of orbitals could form a shape similar to that shown here (Figure 3) in the valence shell of an isolated atom or one about to enter into bonding with other atoms?

A) five sp³d
B) three sp² and one p orbital