Chem Learnsmart chapter 11.

Which partial orbital diagram correctly shows the hybrid orbitals and electron distribution of the O atom in the molecule OF2?

B

Which of the following statements correctly defines hybrid orbitals?

Orbitals used for bonding that are formed by mixing atomic orbitals from the same atom

When should the VSEPR model and hybridization theory be applied to describe bonding?

Whenever an observed molecular shape needs to be rationalized in terms of atomic orbitals

The hybridization model of VSEPR and VB theories is relied upon to explain ______.

observed molecular shape

According to valence bond theory, a(n) _____ bond is formed by the overlap of orbitals from two atoms. In order to explain the observed bond angles in many species, it is proposed that the atomic orbitals first form _____ orbitals, which differ from the orbitals of the isolated atoms.

covalent; hybrid

Recent quantum-mechanical calculations have indicated that ______ do not hybridize effectively with other orbitals of a given n value. However, we continue to use them in hybridization models since VB theory does successfully explain the molecular geometries of central atoms with expanded octets.

d orbitals

Match each type of orbital hybridization with the corresponding electron-group arrangement.

sp matches Choice, Linear Linear sp2 matches Choice, Trigonal planar Trigonal planar sp3 matches Choice, Tetrahedral Tetrahedral sp3d matches Choice, Trigonal bipyramidal Trigonal bipyramidal sp3d2 matches Choice, Octahedral Octahedral

Match each type of orbital hybridization with the corresponding configuration?

sp matches Choice, Two p orbitals Two p orbitals sp3d matches Choice, Four d orbitals Four d orbitals sp2 matches Choice, One p orbital One p orbital sp3 matches Choice, None None sp3d2 matches Choice, Three d orbitals Three d orbitals

Arrange the steps for determining the hybridization of an atom in the correct order. Start with the first step at the top of the list

1. Draw a lewis structure 2.count the number 3. the number 4. build

Which of the following statements correctly describe valence bond theory? Select all that apply

A shared electron pair has the highest probability of being located between the nuclei of the bonded atoms. The space formed by overlapping orbitals can accommodate a maximum of two electrons. The extent of orbital overlap depends on the shape and direction of the orbitals involved.

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 VSEPR model.

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

The shape and orientation of a hybrid orbital allow maximum overlap with an orbital from another atom to form a bond. The type of hybrid orbital formed varies depending on the specific combination of atomic orbitals. The spatial orientations of the hybrid orbitals match observed molecular shapes.

Which of the following statements correctly describes how Pauling's hybridization model explains differences between the geometry of atomic orbitals and observed bond angles?

Valence orbitals of the atoms mix to become new hybrid orbitals in the molecule. The spatial orientations of hybrid orbitals match the observed molecular shapes.

Hybrid orbitals are designated by using a superscript to indicate the -------- of each type of orbital used to form them. For example, the designation sp2 indicates that ----- s and ----- p orbital(s) were combined to form this orbital type.

Blank 1: number, amount, #, or quantity Blank 2: one or 1 Blank 3: two or 2

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.

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.

Blank 1: sp2 or sp^2 Blank 2: trigonal Blank 3: 90

Match each structure shown with the correct hybridization for the central atom.

A Choice, sp3d2 sp3d2 B matches Choice, sp3 sp3 C matches Choice, sp sp D matches Choice, sp2 sp2

In the structure shown, the carbon atom marked "1" is _____ hybridized while the oxygen atom marked "2" is _____ hybridized.

sp2; sp3

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 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.

Which of the following statements correctly describe sp3 hybrid orbitals? Select all that apply.

An sp3 hybrid orbital is unsymmetrical in shape, having one small and one large lobe. The four sp3 hybrid orbitals of a group are equivalent in shape and energy.

Hybrid orbitals are formed by the combination or "mixing" of -----orbitals from a specific atom. The number of hybrid orbitals formed is----- to/than the number of orbitals mixed, and the ------ of hybrid orbital varies according to the specific orbitals mixed.

Blank 1: atomic or valence atomic Blank 2: equal or equivalent Blank 3: type, shape, energy, or number

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.

Blank 1: d Blank 2: 1 or one Blank 3: three or 3 Blank 4: d

Valence bond theory proposes that before a covalent bond forms, atomic orbitals from a given atom can combine to form new atomic orbitals. This process is called ------ of orbitals, and the new atomic orbitals are referred to as -------- orbitals.

Blank 1: hybridization Blank 2: hybrid

A group of sp3 hybrid orbitals is formed by the hybridization of ------ s and ------- p orbital(s) from the valence shell of an atom. These hybrid orbitals have the same -------- and energy.

Blank 1: one or 1 Blank 2: three or 3 Blank 3: shape, size, geometry, structure, or form

The boron atom in the structure shown requires 3 equivalent bonding orbitals, which are formed by combining ------ s and ------ p orbital(s) from the boron atom to form 3 equivalent ------ hybrid orbitals. There is(are) ----- unhybridized p orbital(s) on the boron atom, which contain(s) no electrons.

Blank 1: one or 1 Blank 2: two or 2 Blank 3: sp2 or sp^2 Blank 4: 1 or one

The hybridization of one s and one p orbital will result in the formation of two ----- hybrid orbitals. This will leave ----- unhybridized valence p orbital(s), lying at right angles to the hybrid orbitals.

Blank 1: sp Blank 2: two, 2, two empty, or 2 empty

Which partial orbital diagram correctly shows the hybrid orbitals and electron distribution of the N atom in the molecule NBr3?

C

The Lewis structure for the molecule NF3 is shown. Which of the following statements correctly describe the bonding in this molecule? Select all that apply.

The N uses one sp3 hybrid orbital to form each N-F bond. The bond angles for this molecule are slightly less than 109.5o.

Which of the following statements correctly describe a covalent bond in terms of valence bond theory? Select all that apply.

The electrons of a shared pair must have opposite spins. The greater the overlapped area, the stronger the bond. A covalent bond is formed by the overlap of an orbital from each of the bonding atoms.

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

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

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

Why is the hybridization model necessary to explain the bonding in a molecule such as CH4? Select all that apply.

The observed bond angles cannot be explained with reference to unhybridized orbitals. The atomic electron configuration of carbon cannot account for four equivalent bonds.

Hybridization is less useful as a bonding model when describing the bonding in _______. Select all that apply.

large nonmetal hydrides structures with expanded valence shells