Question 1

Which statement below regarding molecular orbitals for diatomic molecules is FALSE?

Accepted Answer

Explanation: The statement regarding 2p atomic orbitals is false because 2p atomic orbitals can form both sigma (σ) and pi (π) molecular orbitals, not just pi molecular orbitals as suggested. Specifically, they can form σ2p, π2p, σ2p*, and π2p* molecular orbitals, depending on their orientation and phase relation.

Question 2

For which one of the following molecules (BF₃, CF₄, NF₃, OF₂, XeF₄) is the electron geometry tetrahedral and the molecular geometry triangular pyramidal? Draw its Lewis structure with the correct bond angles.

Accepted Answer

The answer of For which one of the following molecules...

Question 3

Use energy levels of diatomic molecules derived from molecular orbital theory to predict the magnetic properties of the oxygen molecule O₂ and the peroxide anion O₂^-2

Accepted Answer

Oxygen (O2) has two unpaired electrons in its molecular orbital configuration, making it paramagnetic. The peroxide anion (O2^2-) has all electrons paired, making it diamagnetic.

Question 4

Of the following molecules (O₃, SCl₂, SO₂, CS₂, and CO₂) which ones do you predict to have a bond angle of 180$\degree$?

Accepted Answer

The answer of Of the following molecules (O₃, SCl₂, SO₂,...

Question 5

Boron nitride, BN, is a new high-tech material.According to the provided molecular orbital energy-level diagram, which statement below is NOT correct about boron nitride?

Accepted Answer

The answer of Boron nitride, BN, is a new high-tech...

Question 6

Which statement below is NOT correct about CO, CO⁺, and CO^-? Use the following MO diagram.

Accepted Answer

The answer of Which statement below is NOT correct about...

Question 7

Draw a structure showing the geometry of the molecule in the following group that is nonpolar: HF; NH₃; BF₃; CHCl₃; CO.

Accepted Answer

The answer of Draw a structure showing the geometry of...

Question 8

Boron nitride is being investigated in frontier research directed at producing novel electronic devices.If you used the following energy-level diagram for the molecular orbitals of boron nitride, BN, what would you predict? I.Boron nitride is diamagnetic. II.Boron nitride has a bond order of 2. III.Boron nitride is paramagnetic. IV.The bond in BN^- is weaker than the bond in BN.

Accepted Answer

The answer of Boron nitride is being investigated in frontier...

Question 9

Which molecule below has a bond order of 3?

Accepted Answer

The molecule with a bond order of 3 is $ \text{N}_2 $ (Nitrogen molecule). The notation "N₂" represents a molecule with a single bond (S1), a single unpaired electron (U1), a triple bond (B12), and no double bonds (B0), which corresponds to the bonding in $ \text{N}_2 $, where the nitrogen atoms are triple-bonded to each other.

Question 10

According to the molecular orbital energy-level diagram below, which one of the following statements is NOT correct about NO, NO⁺, and NO^-?

Accepted Answer

The answer of According to the molecular orbital energy-level diagram...

Question 11

There are two possible structures for 1,2-dichloroethylene, C₂H₂Cl₂, in which each carbon is bonded to one H atom and one Cl atom.Draw each structure.What is the hybridization of each carbon? What is the molecular geometry around each? Using a polarity argument, state how you could distinguish between the two.

Accepted Answer

The answer of There are two possible structures for 1,2-dichloroethylene,...

Question 12

Draw the Lewis structure with the lowest formal charges for XeOF₂.What are the electronic geometry and molecular geometry?

Accepted Answer

The answer of Draw the Lewis structure with the lowest...

Question 13

Determine the bond order of the OF molecule.

Accepted Answer

The bond order of a molecule can be calculated using the formula: Bond order = (number of bonding electrons - number of antibonding electrons) / 2. For the OF molecule, the molecular orbital configuration can be derived from the combination of oxygen and fluorine atomic orbitals. Considering the valence electrons and applying molecular orbital theory, the bond order for OF is found to be 1.5, which is calculated by considering the electrons in bonding and antibonding molecular orbitals.

Question 14

What is the valence electron molecular orbital electron configuration of F₂?

Accepted Answer

The answer of What is the valence electron molecular orbital...

Question 15

Which one of the following molecules or ions is paramagnetic? These molecules are described by the MO energy diagram below.

Accepted Answer

The answer of Which one of the following molecules or...

Question 16

Consider the following hydrides: NH₃, PH₃, AsH₃, and SbH₃.What is their electronic geometry? What is their molecular geometry? Which molecule would you predict has the highest dipole moment? Consider the ideal H - X - H angle, where X is the central atom.Which would you predict has the largest deviation from that angle, and would the observed H - X - H angle be larger or smaller than the ideal value?

Accepted Answer

The answer of Consider the following hydrides: NH₃, PH₃, AsH₃,...

Question 17

Use MO theory to predict the bond orders of the following ions.Which one do you predict does NOT exist?

Accepted Answer

The bond order can be calculated using Molecular Orbital (MO) Theory by subtracting the number of electrons in antibonding orbitals from the number of electrons in bonding orbitals and then dividing by two. The given symbols seem to represent the molecular orbital diagrams for various diatomic species, but without a clear interpretation of the symbols, we can apply general principles. Typically, a bond order of zero indicates that the molecule does not have enough bonding interactions to exist as a stable molecule. The choice D, which seems to represent a diatomic molecule with a negative charge, is indicated as not existing likely due to a misinterpretation of the symbols or an error in the representation. However, without clear and standard molecular orbital diagrams or a more straightforward representation of the electron configurations, this explanation assumes a general understanding of MO theory principles where bond order correlates with stability.

Question 18

Predict the bond order of the CN^- ion.

Accepted Answer

The CN⁻ ion has a bond order of 3, as it has 10 valence electrons, filling the bonding molecular orbitals and resulting in a triple bond.

Question 19

Use MO theory to predict the bond orders of the following molecular ions.Which one is the most stable?

Accepted Answer

C) CN^- has the highest bond order, indicating it is the most stable according to Molecular Orbital Theory. Higher bond orders correspond to more stable molecules.

Question 20

What is the valence electron molecular orbital electron configuration of C₂?

Accepted Answer

The correct electron configuration for C2 is (σ2s)²(σ*2s)²(π2p)⁴, which corresponds to choice B. This configuration accounts for the 8 valence electrons in C2, with the π2p orbitals being fully filled.

Quiz 5: Bonding Theories Explaining Molecular Geometry

Which statement below regarding molecular orbitals for diatomic molecules is FALSE?

For which one of the following molecules (BF₃, CF₄, NF₃, OF₂, XeF₄) is the electron geometry tetrahedral and the molecular geometry triangular pyramidal? Draw its Lewis structure with the correct bond angles.

Use energy levels of diatomic molecules derived from molecular orbital theory to predict the magnetic properties of the oxygen molecule O₂ and the peroxide anion O₂^-2

Of the following molecules (O₃, SCl₂, SO₂, CS₂, and CO₂) which ones do you predict to have a bond angle of 180 $\degree$ ?

Boron nitride, BN, is a new high-tech material.According to the provided molecular orbital energy-level diagram, which statement below is NOT correct about boron nitride?

Which statement below is NOT correct about CO, CO⁺, and CO^-? Use the following MO diagram.

Draw a structure showing the geometry of the molecule in the following group that is nonpolar: HF; NH₃; BF₃; CHCl₃; CO.

Which molecule below has a bond order of 3?

According to the molecular orbital energy-level diagram below, which one of the following statements is NOT correct about NO, NO⁺, and NO^-?

Draw the Lewis structure with the lowest formal charges for XeOF₂.What are the electronic geometry and molecular geometry?

Determine the bond order of the OF molecule.

What is the valence electron molecular orbital electron configuration of F₂?

Which one of the following molecules or ions is paramagnetic? These molecules are described by the MO energy diagram below.

Use MO theory to predict the bond orders of the following ions.Which one do you predict does NOT exist?

Predict the bond order of the CN^- ion.

Use MO theory to predict the bond orders of the following molecular ions.Which one is the most stable?

What is the valence electron molecular orbital electron configuration of C₂?

Quiz 5: Bonding Theories Explaining Molecular Geometry

Which statement below regarding molecular orbitals for diatomic molecules is FALSE?

For which one of the following molecules (BF3, CF4, NF3, OF2, XeF4) is the electron geometry tetrahedral and the molecular geometry triangular pyramidal? Draw its Lewis structure with the correct bond angles.

Use energy levels of diatomic molecules derived from molecular orbital theory to predict the magnetic properties of the oxygen molecule O2 and the peroxide anion O2-2

Of the following molecules (O3, SCl2, SO2, CS2, and CO2) which ones do you predict to have a bond angle of 180 °\degree° ?

Boron nitride, BN, is a new high-tech material.According to the provided molecular orbital energy-level diagram, which statement below is NOT correct about boron nitride?

Which statement below is NOT correct about CO, CO+, and CO-? Use the following MO diagram.

Draw a structure showing the geometry of the molecule in the following group that is nonpolar: HF; NH3; BF3; CHCl3; CO.

Which molecule below has a bond order of 3?

According to the molecular orbital energy-level diagram below, which one of the following statements is NOT correct about NO, NO+, and NO-?

Draw the Lewis structure with the lowest formal charges for XeOF2.What are the electronic geometry and molecular geometry?

Determine the bond order of the OF molecule.

What is the valence electron molecular orbital electron configuration of F2?

Which one of the following molecules or ions is paramagnetic? These molecules are described by the MO energy diagram below.

Use MO theory to predict the bond orders of the following ions.Which one do you predict does NOT exist?

Predict the bond order of the CN- ion.

Use MO theory to predict the bond orders of the following molecular ions.Which one is the most stable?

What is the valence electron molecular orbital electron configuration of C2?

For which one of the following molecules (BF₃, CF₄, NF₃, OF₂, XeF₄) is the electron geometry tetrahedral and the molecular geometry triangular pyramidal? Draw its Lewis structure with the correct bond angles.

Use energy levels of diatomic molecules derived from molecular orbital theory to predict the magnetic properties of the oxygen molecule O₂ and the peroxide anion O₂^-2

Of the following molecules (O₃, SCl₂, SO₂, CS₂, and CO₂) which ones do you predict to have a bond angle of 180 $\degree$ ?

Which statement below is NOT correct about CO, CO⁺, and CO^-? Use the following MO diagram.

Draw a structure showing the geometry of the molecule in the following group that is nonpolar: HF; NH₃; BF₃; CHCl₃; CO.

According to the molecular orbital energy-level diagram below, which one of the following statements is NOT correct about NO, NO⁺, and NO^-?

Draw the Lewis structure with the lowest formal charges for XeOF₂.What are the electronic geometry and molecular geometry?

What is the valence electron molecular orbital electron configuration of F₂?

Predict the bond order of the CN^- ion.

What is the valence electron molecular orbital electron configuration of C₂?