BL Ch 9 Molecular Shape and Bonding

Open Ended

Why is understanding molecular geometry important in the study of chemistry?

Multiple Choice

According to the Valence-Shell Electron-Pair Repulsion (VSEPR) model, what primarily determines the shape of a molecule?

• The number of protons in the nucleus

• The repulsion between electron pairs

• The mass of the atoms involved

• The temperature of the environment

Fill in the Blanks

The directions to which electrons point in a molecule are referred to as

domains.

Open Ended

Explain how the balloon analogy helps in understanding the arrangement of electron domains in the VSEPR model.

Multiple Select

Which of the following are electron-domain geometries for a central atom with four or more electron domains?

• Linear

• Tetrahedral

• Trigonal bipyramidal

• Octahedral

Fill in the Blanks

In the linear electron domain, the only possible molecular geometry is

.

Multiple Choice

Which molecular geometry results when all electron domains are bonding in a molecule with three electron domains?

• Trigonal planar

• Bent

• Tetrahedral

• Trigonal bipyramidal

Open Ended

Explain how the number of nonbonding pairs influences the molecular geometry of a molecule with a tetrahedral electron domain.

Multiple Choice

How does the presence of nonbonding pairs affect the bond angles in a molecule?

• They increase the bond angles.

• They have no effect on bond angles.

• They compress the bond angles.

• They make bond angles equal to 90°.

Fill in the Blanks

Double and triple bonds have larger electron domains than single bonds. This causes their bond angles to be

.

Multiple Choice

Which of the following statements about expanding beyond the octet rule is correct?

• Only elements with four or fewer electron domains can exist.

• Some elements can have more than four electron domains, resulting in trigonal bipyramidal or octahedral geometries.

• All elements must follow the octet rule strictly.

• Expanding beyond the octet rule leads to linear geometries only.

Multiple Select

Select all correct statements about the trigonal bipyramidal electron domain geometry.

• There are two distinct positions: axial and equatorial.

• Lone pairs occupy axial positions.

• Three equatorial positions form an equilateral triangle.

• Lone pairs occupy equatorial positions.

Multiple Choice

Which of the following is NOT a molecular geometry found in the trigonal bipyramidal electron domain?

• Trigonal bipyramidal

• Seesaw

• Square planar

• T-shaped

Open Ended

Compare the molecular geometries possible in the trigonal bipyramidal and octahedral electron domains. What is a key difference in the types of geometries found in each?

Open Ended

For larger molecules, why is it important to consider the geometry about each atom rather than the molecule as a whole?

Fill in the Blanks

Fill in the blank: If the average position of δ+ and δ– in a molecule coincide, the molecule is

Multiple Choice

Which of the following statements correctly describes the difference between a polar and a nonpolar molecule as shown in the comparison diagrams?

• A nonpolar molecule has equal and oppositely directed bond dipoles, resulting in no overall dipole moment.

• A polar molecule has equal and oppositely directed bond dipoles, resulting in no overall dipole moment.

• A nonpolar molecule has bond dipoles that do not cancel, resulting in an overall dipole moment.

• A polar molecule has no bond dipoles.

Multiple Select

Which of the following statements are correct about Valence-Bond Theory?

• Electrons of two atoms begin to occupy the same space.

• This is called 'overlap' of orbitals.

• The sharing of space between two electrons of opposite spin results in a covalent bond.

• Electrons of two atoms never share the same space.

Multiple Choice

What happens when the overlap between atomic orbitals increases during bond formation?

• The atoms move infinitely close together

• The potential energy increases without limit

• A balance is reached between repulsion and attraction

• Electrons are lost from the atoms

Open Ended

Why does the bond angle in H2O deviate from 90° to 104.5° according to VSEPR and orbital theory?

Fill in the Blanks

Hybrid orbitals are formed by the

of atomic orbitals to create new orbitals of equal energy.

Multiple Select

Which of the following statements about sp hybridization in beryllium compounds is/are correct?

• sp hybridization involves the mixing of one s and one p orbital

• Beryllium forms two bonds due to sp hybridization

• sp hybrid orbitals are always unpaired

• sp hybridization results in three hybrid orbitals

Open Ended

How do Lewis Structures help us determine the shapes of molecules, and what are some common shapes for molecules with two or three atoms connected to a central atom?

Open Ended

Describe the shape and characteristics of sp hybrid orbitals formed from s and p orbitals.

Fill in the Blanks

The two sp hybrid orbitals in BeF2 align themselves

degrees from each other, resulting in a linear geometry.