Day Zc

The combination of one s and two p orbitals will form a group of three hybrid orbitals. These hybrid orbitals adopt a(n) planar geometry and are at an angle of o to the remaining unhybridized p orbital.

-sp2-trigonal-90

Which of the following statements correctly describe the formation of sp2 hybrid orbitals? Select all that apply.

A group of sp2 hybrid orbitals assumes a trigonal planar geometry. The formation of sp2 hybrid orbitals leaves one unhybridized valence p orbital.

A central atom can be surrounded by five or six electron groups if orbitals are available for bonding. The appropriate number of equivalent bonding orbitals is formed by combining s orbital(s), p orbital(s), and one or two orbitals.

-d-one-three-d

Which of the following statements correctly describe a π bond? Select all that apply.

A π bond is formed by the side-to-side overlap of two p orbitals. A multiple bond always contains at least one π bond.

Which of the following options correctly describe the hybridization of s, p, and d orbitals? Select all that apply.

Only elements from Period 3 onward can use d orbitals for bonding. The hybridization of an atom surrounded by six electron pairs is sp3d2.

Which of the following options correctly describe sp hybrid orbitals? Select all that apply.

The energy of an sp hybrid orbital lies between the energies of the original s and p orbital that were mixed. Each sp hybrid orbital has one large and one small lobe.

A particular hybrid orbital is designated sp3d2. What information is provided by the superscripts in this designation?

The number of each type of atomic orbital combined to produce this type of hybrid orbital

A bond formed by sideways overlap of two p orbitals (one from each bonding atom) is called a(n) _____ bond. This type of bond has _____ regions of electron density.

pi; 2

Hybrid orbitals are designated by using a superscript to indicate the

number, one, two

A group of sp3 hybrid orbitals is formed by the hybridization of

one three shape

Valence bond theory describes a single covalent bond as the _____ of orbitals from two atoms to form a shared space, which is occupied by _____ electron(s).

overlap; two

Which of the following steps are necessary to determine the hybridization of the central atom? Select all that apply.

- Draw the Lewis structure of the molecule - Deduce the hybridization of the central atom based on the geometry of the molecule - Predict the geometry of the molecule using the VESPR model

sigma

Single bonds are σ bonds. A σ bond results from end-to-end overlap of two orbitals.