Question 1

Which figure best illustrates the hybrid orbitals on phosphorous in PH₃?

Accepted Answer

The hybridization of phosphorous in PH₃ is sp3, which means that we expect four hybrid orbitals. Choice B shows four lobes pointing towards the corners of a tetrahedron, which is the expected geometry for sp3 hybrid orbitals. Choices A, C, D, and E do not match this geometry.

Question 2

Consider the species F₂⁺, F₂, and F₂^-. Which of these species will be paramagnetic?

Accepted Answer

F₂⁺ and F₂^- are paramagnetic because they have unpaired electrons in their molecular orbital configurations.

Question 3

For a polyatomic ion having the general formula AB₃ⁿ^±, where A is an atom from Group 6A, B is an atom from Group 7A, and the ionic charge is n±, what charge must the ion have in order to yield a molecular geometry that is trigonal pyramidal?

Accepted Answer

In order to have a trigonal pyramidal molecular geometry, the polyatomic ion must have a central atom with four electron groups, three of which are bonding and one of which is a lone pair. This means that the central atom must have a tetrahedral electron geometry. Group 6A elements have 6 valence electrons, and Group 7A elements have 7 valence electrons. Therefore, if we use one atom from each group in the ion, we have a total of 26 valence electrons (6 from A, 7 from B, and 1 from the single negative charge). To achieve a tetrahedral electron geometry with this number of electrons, the central atom must have one lone pair. Looking at the formula given, there is only one atom that could be the central atom with one lone pair, and that is the A atom. Therefore, the ion must be in the form A1B3S1 with one negative charge, giving a total of 26 valence electrons. In order to achieve a trigonal pyramidal molecular geometry, the ion must have a total of four electron groups around the central A atom, which means that there must be three bonding groups (corresponding to the three B atoms) and one lone pair. This requires that the ion have an overall charge of 1+, so that the central A atom can have a lone pair of electrons. Therefore, the correct answer is C) 1+.

Question 4

Which figure best illustrates the hybrid orbitals on carbon in benzene, C₆H₆?

Accepted Answer

The answer of Which figure best illustrates the hybrid orbitals...

Question 5

The nitrosonium ion, NO⁺, forms a number of interesting complexes with nickel, cobalt, and iron. According to molecular orbital theory, which statement about NO⁺is correct?

Accepted Answer

NO⁺ has a bond order of 3 and is diamagnetic because it has no unpaired electrons.

Question 6

Consider the species N₂^-, N₂, and N₂⁺. Which of these species will be paramagnetic?

Accepted Answer

To determine if a species is paramagnetic or diamagnetic, we need to look at the electronic configuration and the presence of unpaired electrons. N₂ has a closed-shell electronic configuration, meaning all the electrons are paired. Therefore, it is diamagnetic. N₂^- has one more electron than N₂, and the additional electron is in the singly occupied P orbital, which is unpaired. Therefore, this species has an unpaired electron and is paramagnetic. N₂⁺ has one less electron than N₂^-, and the electron that is removed is in the singly occupied P orbital. This removal of an electron does not change the pairing of the remaining electrons, so this species is diamagnetic. Therefore, the only species that is paramagnetic is N₂^-. The correct answer is choice C.

Question 7

According to molecular orbital theory, what is the bond order in the O₂⁺ion?

Accepted Answer

The bond order can be calculated by subtracting the number of antibonding electrons from the number of bonding electrons and dividing the result by 2. The molecular orbital diagram of the given ion shows that there are 16 bonding electrons and 10 antibonding electrons. Therefore, the bond order is (16-10)/2 = 3, which corresponds to a triple bond. However, there are also two lone pairs on the central S atom, which are not included in the bond order calculation. Taking these into account, the effective bond order becomes (3+2)/2 = 2.5. Therefore, the correct answer is D.

Question 8

For a homonuclear diatomic molecule, which molecular orbital is the lowest in energy?

Accepted Answer

The answer of For a homonuclear diatomic molecule, which molecular...

Question 9

Which molecular formula corresponds to a structural formula with carbon atoms having hybridizations of sp, sp², and sp³?

Accepted Answer

The answer of Which molecular formula corresponds to a structural...

Question 10

According to molecular orbital theory, what is the bond order in the O₂^-ion?

Accepted Answer

The bond order can be calculated by subtracting the number of antibonding electrons from the number of bonding electrons and dividing the result by 2. The molecular orbital diagram of the given ion shows that there are 16 bonding electrons and 10 antibonding electrons. Therefore, the bond order is (16-10)/2 = 3, which corresponds to a triple bond. However, there are also two lone pairs on the central S atom, which are not included in the bond order calculation. Taking these into account, the effective bond order becomes (3+2)/2 = 2.5. Therefore, the correct answer is D.

Question 11

According to molecular orbital (MO) theory, the twelve valence electrons in the O₂ molecule are distributed as follows:

Accepted Answer

According to MO theory, the 12 valence electrons in the O₂ molecule will fill the molecular orbitals in order of increasing energy. There are six molecular orbitals available, three bonding and three antibonding. The first six electrons will fill the bonding molecular orbitals, while the remaining six electrons will fill the antibonding molecular orbitals. Therefore, there will be 8 electrons in bonding MOs and 4 electrons in antibonding MOs.Choice D is the only option that fits this description.

Question 12

Which figure best illustrates the hybrid orbitals on iodine in ICl₂^-?

Accepted Answer

The answer of Which figure best illustrates the hybrid orbitals...

Question 13

Allene, C₃H₄ (shown below), is one component of gas used for high-temperature welding. According to the valence bond model, which is a proper description of the bonding on the central carbon atom in allene?

Accepted Answer

The answer of Allene, C₃H₄ (shown below), is one component...

Question 14

The electrons in the delocalized π molecular orbitals of benzene (C₆H₆)

Accepted Answer

The delocalized π molecular orbitals of benzene are spread out over the entire six-membered ring, making the electrons free to move around the ring. This is what gives benzene its unique stability and aromatic character. Therefore, choice B is the best choice. Choices A, C, D, and E do not accurately describe the nature of the delocalized π electrons in benzene.

Question 15

Hyposulfite, SO₂^2-, is a polyatomic ion that has not yet been definitively confirmed to exist. However, the VSEPR model may still be applied to yield a prediction on its molecular geometry. What is the most reasonable estimate for the O-S-O bond angle in hyposulfite?

Accepted Answer

Based on the VSEPR model, hyposulfite has a trigonal pyramidal shape, with the sulfur atom at the apex of the pyramid and the three oxygen atoms forming a triangular base. This arrangement leads to a bond angle of approximately 106° between the oxygen atoms.

Question 16

According to molecular orbital theory, what is the bond order of the hypofluorite ion, OF^-?

Accepted Answer

To determine the bond order using molecular orbital theory, we need to first draw the molecular orbital diagram for the hypofluorite ion. This is a complex process that involves calculating the number of valence electrons, determining the symmetries of the atomic orbitals, and calculating the overlap integrals between them.

The end result is a diagram that shows the energies and symmetries of the molecular orbitals formed from the atomic orbitals. In this case, we would expect to see three occupied molecular orbitals (OMOs) and two unoccupied molecular orbitals (UMOs).

The bond order is given by the difference between the number of electrons in the bonding OMOs and the number of electrons in the antibonding OMOs, divided by 2. In the case of hypofluorite ion, we have:

Bonding OMOs: sigma bond between oxygen and sulfur, sigma bond between sulfur and fluorine, pi bond between sulfur and fluorine (3 electrons total)
Antibonding OMOs: sigma* bond between oxygen and sulfur, sigma* bond between sulfur and fluorine (2 electrons total)

Therefore, the bond order is:

(3 - 2)/2 = 0.5

However, we need to take into account the fact that the hypofluorite ion is a radical species, meaning it has an unpaired electron. This unpaired electron will occupy the pi* antibonding orbital, resulting in a bond order of:

(3 - 3)/2 = 0

This means that there is no net bond between the oxygen and sulfur atoms in the hypofluorite ion, and the answer is:

Answer: C (0)

Question 17

Which is the correct hybrid orbital diagram representing the hybridization of iodine in ICl₅?

Accepted Answer

The answer of Which is the correct hybrid orbital diagram...

Question 18

For a homonuclear diatomic molecule, which molecular orbital is the highest in energy?

Accepted Answer

The answer of For a homonuclear diatomic molecule, which molecular...

Question 19

The number of π bonds in phosgene, COCl₂, is

Accepted Answer

Phosgene (COCl₂) has a structure where the carbon atom is double-bonded to the oxygen atom, which accounts for one π bond. The carbon-chlorine bonds are single bonds and do not contribute any π bonds.

Question 20

Rank the following molecules in order of increasing dipole moment.

Accepted Answer

The answer of Rank the following molecules in order of...

Quiz 9: Chemical Bonding II: Molecular Geometry and Bonding Theories

Which figure best illustrates the hybrid orbitals on phosphorous in PH₃?

Consider the species F₂⁺, F₂, and F₂^-. Which of these species will be paramagnetic?

For a polyatomic ion having the general formula AB₃ⁿ^±, where A is an atom from Group 6A, B is an atom from Group 7A, and the ionic charge is n±, what charge must the ion have in order to yield a molecular geometry that is trigonal pyramidal?

Which figure best illustrates the hybrid orbitals on carbon in benzene, C₆H₆?

The nitrosonium ion, NO⁺, forms a number of interesting complexes with nickel, cobalt, and iron. According to molecular orbital theory, which statement about NO⁺is correct?

Consider the species N₂^-, N₂, and N₂⁺. Which of these species will be paramagnetic?

According to molecular orbital theory, what is the bond order in the O₂⁺ion?

For a homonuclear diatomic molecule, which molecular orbital is the lowest in energy?

Which molecular formula corresponds to a structural formula with carbon atoms having hybridizations of sp, sp², and sp³?

According to molecular orbital theory, what is the bond order in the O₂^-ion?

According to molecular orbital (MO) theory, the twelve valence electrons in the O₂ molecule are distributed as follows:

Which figure best illustrates the hybrid orbitals on iodine in ICl₂^-?

Allene, C₃H₄ (shown below) , is one component of gas used for high-temperature welding. According to the valence bond model, which is a proper description of the bonding on the central carbon atom in allene?

The electrons in the delocalized π molecular orbitals of benzene (C₆H₆)

Hyposulfite, SO₂^2-, is a polyatomic ion that has not yet been definitively confirmed to exist. However, the VSEPR model may still be applied to yield a prediction on its molecular geometry. What is the most reasonable estimate for the O-S-O bond angle in hyposulfite?

According to molecular orbital theory, what is the bond order of the hypofluorite ion, OF^-?

Which is the correct hybrid orbital diagram representing the hybridization of iodine in ICl₅?

For a homonuclear diatomic molecule, which molecular orbital is the highest in energy?

The number of π bonds in phosgene, COCl₂, is

Rank the following molecules in order of increasing dipole moment.

Quiz 9: Chemical Bonding II: Molecular Geometry and Bonding Theories

Which figure best illustrates the hybrid orbitals on phosphorous in PH3?

Consider the species F2+, F2, and F2-. Which of these species will be paramagnetic?

For a polyatomic ion having the general formula AB3n±, where A is an atom from Group 6A, B is an atom from Group 7A, and the ionic charge is n±, what charge must the ion have in order to yield a molecular geometry that is trigonal pyramidal?

Which figure best illustrates the hybrid orbitals on carbon in benzene, C6H6?

The nitrosonium ion, NO+, forms a number of interesting complexes with nickel, cobalt, and iron. According to molecular orbital theory, which statement about NO+ is correct?

Consider the species N2-, N2, and N2+. Which of these species will be paramagnetic?

According to molecular orbital theory, what is the bond order in the O2+ ion?

For a homonuclear diatomic molecule, which molecular orbital is the lowest in energy?

Which molecular formula corresponds to a structural formula with carbon atoms having hybridizations of sp, sp2, and sp3?

According to molecular orbital theory, what is the bond order in the O2- ion?

According to molecular orbital (MO) theory, the twelve valence electrons in the O2 molecule are distributed as follows:

Which figure best illustrates the hybrid orbitals on iodine in ICl2-?

Allene, C3H4 (shown below) , is one component of gas used for high-temperature welding. According to the valence bond model, which is a proper description of the bonding on the central carbon atom in allene?

The electrons in the delocalized π molecular orbitals of benzene (C6H6)

Hyposulfite, SO22-, is a polyatomic ion that has not yet been definitively confirmed to exist. However, the VSEPR model may still be applied to yield a prediction on its molecular geometry. What is the most reasonable estimate for the O-S-O bond angle in hyposulfite?

According to molecular orbital theory, what is the bond order of the hypofluorite ion, OF-?

Which is the correct hybrid orbital diagram representing the hybridization of iodine in ICl5?

For a homonuclear diatomic molecule, which molecular orbital is the highest in energy?

The number of π bonds in phosgene, COCl2, is

Rank the following molecules in order of increasing dipole moment.

Which figure best illustrates the hybrid orbitals on phosphorous in PH₃?

Consider the species F₂⁺, F₂, and F₂^-. Which of these species will be paramagnetic?

For a polyatomic ion having the general formula AB₃ⁿ^±, where A is an atom from Group 6A, B is an atom from Group 7A, and the ionic charge is n±, what charge must the ion have in order to yield a molecular geometry that is trigonal pyramidal?

Which figure best illustrates the hybrid orbitals on carbon in benzene, C₆H₆?

The nitrosonium ion, NO⁺, forms a number of interesting complexes with nickel, cobalt, and iron. According to molecular orbital theory, which statement about NO⁺is correct?

Consider the species N₂^-, N₂, and N₂⁺. Which of these species will be paramagnetic?

According to molecular orbital theory, what is the bond order in the O₂⁺ion?

Which molecular formula corresponds to a structural formula with carbon atoms having hybridizations of sp, sp², and sp³?

According to molecular orbital theory, what is the bond order in the O₂^-ion?

According to molecular orbital (MO) theory, the twelve valence electrons in the O₂ molecule are distributed as follows:

Which figure best illustrates the hybrid orbitals on iodine in ICl₂^-?

Allene, C₃H₄ (shown below) , is one component of gas used for high-temperature welding. According to the valence bond model, which is a proper description of the bonding on the central carbon atom in allene?

The electrons in the delocalized π molecular orbitals of benzene (C₆H₆)

Hyposulfite, SO₂^2-, is a polyatomic ion that has not yet been definitively confirmed to exist. However, the VSEPR model may still be applied to yield a prediction on its molecular geometry. What is the most reasonable estimate for the O-S-O bond angle in hyposulfite?

According to molecular orbital theory, what is the bond order of the hypofluorite ion, OF^-?

Which is the correct hybrid orbital diagram representing the hybridization of iodine in ICl₅?

The number of π bonds in phosgene, COCl₂, is