Question

which of the following statements summarizing valence bond theory is correct? group of answer choices a bond is formed only by the overlap of two hybrid orbitals or two atomic orbitals. a chemical bond forms only when occupied orbitals are involved. the only orbitals used in bond formation are atomic orbitals (s, p, d, and f). the geometry of the molecule is determined by the geometry of the orbitals used.

Answer 1

In valence bond theory, a covalent bond forms from the overlap of half-filled atomic or hybrid orbitals, creating a shared pair of electrons, and this overlap dictates the geometry of the molecule.

Step-by-step explanation:

According to valence bond theory, there are a few key points to understand:

• A covalent bond is described as the overlap of half-filled atomic orbitals, each containing a single electron, from two different atoms.
• The overlap of these orbitals creates a shared pair of electrons, thereby forming a bond.
• Hybrid orbitals can also be formed when atomic orbitals of similar energy on the same atom mix to create new, equivalent orbitals that are optimally oriented for bonding.
• The molecular geometry is indeed influenced by the geometry of the overlapping orbitals or the hybrid orbitals if they are used.

So, to answer the question, the correct statement summarizing valence bond theory is that a bond is formed by the overlap of two hybrid orbitals or two atomic orbitals, and the geometry of the molecule is determined by the geometry of the orbitals used.

Answer 2

Valence bond theory explains that chemical bonds are the results of overlaps between atomic orbitals, which can be either pure or hybridized orbitals, leading to the shared electron pairs that form bonds.

Step-by-step explanation:

According to valence bond theory, a correct statement summarizing its principles would be that a chemical bond forms as a consequence of the overlap of two separate atomic orbitals on different atoms, which creates a region with a pair of electrons shared between those atoms. The bonds can form via the overlap of purely atomic orbitals or through hybrid orbitals, which are combinations of two or more atomic orbitals from the same atom, allowing for different molecular geometries. Hybridization helps explain molecules with geometries that cannot be accounted for by the use of unhybridized atomic orbitals alone, as seen in water (H2O), where the bond angle is not the predicted 90 degrees from p orbital overlap but rather an observed 104.5 degrees.