Topic 14: Chemical bonding and structure

Which combination correctly describes the geometry of ${{\mathrm{BrF}}_4}^{-}$?

Which combination correctly describes the geometry of ${{\mathrm{BrF}}_4}^{-}$?

State the number of sigma ($\mathrm{\sigma }$) and pi ($\mathrm{\pi }$) bonds around the central carbon atom in molecule B.

State the number of sigma ($\mathrm{\sigma }$) and pi ($\mathrm{\pi }$) bonds around the central carbon atom in molecule B.

State the number of sigma ($\mathrm{\sigma }$) and pi ($\mathrm{\pi }$) bonds around the central carbon atom in molecule B.

State the type of hybridization shown by the central carbon atom in molecule B.

State the type of hybridization shown by the central carbon atom in molecule B.

State the type of hybridization shown by the central carbon atom in molecule B.

Draw the Lewis (electron dot) structures of PF₃ and PF₅ and use the VSEPR theory to deduce the molecular geometry of each species including bond angles.

Draw the Lewis (electron dot) structures of PF₃ and PF₅ and use the VSEPR theory to deduce the molecular geometry of each species including bond angles.

Draw the Lewis (electron dot) structures of PF₃ and PF₅ and use the VSEPR theory to deduce the molecular geometry of each species including bond angles.

Draw diagrams to show how sigma (σ) and pi (π) bonds are formed between atoms.

Draw diagrams to show how sigma (σ) and pi (π) bonds are formed between atoms.

Draw diagrams to show how sigma (σ) and pi (π) bonds are formed between atoms.

Describe how sigma (σ) and pi ($\pi$) bonds are formed.

Describe how sigma (σ) and pi ($\pi$) bonds are formed.

Describe how sigma (σ) and pi ($\pi$) bonds are formed.

Which overlap of atomic orbitals leads to the formation of only a sigma (σ) bond?

       I.     s − p

       II.     p − p

       III.     s − s

A.     I and II only

B.     I and III only

C.     II and III only

D.     I, II and III

Which overlap of atomic orbitals leads to the formation of only a sigma (σ) bond?

       I.     s − p

       II.     p − p

       III.     s − s

A.     I and II only

B.     I and III only

C.     II and III only

D.     I, II and III

The C–N bonds in urea are shorter than might be expected for a single C–N bond. Suggest, in terms of electrons, how this could occur.

The C–N bonds in urea are shorter than might be expected for a single C–N bond. Suggest, in terms of electrons, how this could occur.

The C–N bonds in urea are shorter than might be expected for a single C–N bond. Suggest, in terms of electrons, how this could occur.

Deduce the number of σ and $\pi$ bonds in a molecule of ethyne.

Deduce the number of σ and $\pi$ bonds in a molecule of ethyne.

Deduce the number of σ and $\pi$ bonds in a molecule of ethyne.

Absorption of UV light in the ozone layer causes the dissociation of oxygen and ozone.

Identify, in terms of bonding, the molecule that requires a longer wavelength to dissociate.

Absorption of UV light in the ozone layer causes the dissociation of oxygen and ozone.

Identify, in terms of bonding, the molecule that requires a longer wavelength to dissociate.

Absorption of UV light in the ozone layer causes the dissociation of oxygen and ozone.

Identify, in terms of bonding, the molecule that requires a longer wavelength to dissociate.

Carbon dioxide can be represented by at least two resonance structures, I and II.

Calculate the formal charge on each oxygen atom in the two structures.

Carbon dioxide can be represented by at least two resonance structures, I and II.

Calculate the formal charge on each oxygen atom in the two structures.

Carbon dioxide can be represented by at least two resonance structures, I and II.

Calculate the formal charge on each oxygen atom in the two structures.

Deduce, giving a reason, the more likely structure.

Deduce, giving a reason, the more likely structure.

Deduce, giving a reason, the more likely structure.

Which molecules contain two pi ($\mathrm{\pi }$) bonds?

I.   HCN
II.  H₂CO₃
III. H₂C₂O₄

A.  I and II only

B.  I and III only

C.  II and III only

D.  I, II and III

Which molecules contain two pi ($\mathrm{\pi }$) bonds?

I.   HCN
II.  H₂CO₃
III. H₂C₂O₄

A.  I and II only

B.  I and III only

C.  II and III only

D.  I, II and III

What is the number of sigma (σ) and pi (π) bonds in the molecule (NC)₂C=C(CN)₂?

What is the number of sigma (σ) and pi (π) bonds in the molecule (NC)₂C=C(CN)₂?

Draw two Lewis (electron dot) structures for BrO₃⁻.

Draw two Lewis (electron dot) structures for BrO₃⁻.

Draw two Lewis (electron dot) structures for BrO₃⁻.

What is the formal charge of the oxygen atom in H₃O⁺?

A.  −2

B.  −1

C.  0

D.  +1

What is the formal charge of the oxygen atom in H₃O⁺?

A.  −2

B.  −1

C.  0

D.  +1

Explain the relative lengths of the three bonds between N and O in nitric acid.

Explain the relative lengths of the three bonds between N and O in nitric acid.

Explain the relative lengths of the three bonds between N and O in nitric acid.

Identify the number of sigma and pi bonds in HCN.

Identify the number of sigma and pi bonds in HCN.

Identify the number of sigma and pi bonds in HCN.

Sketch the shape of one sigma ($\text{σ}$) and one pi ($\mathrm{\pi }$) bond.

Sketch the shape of one sigma ($\text{σ}$) and one pi ($\mathrm{\pi }$) bond.

Sketch the shape of one sigma ($\text{σ}$) and one pi ($\mathrm{\pi }$) bond.

Outline why both C to O bonds in the conjugate base are the same length and suggest a value for them. Use section 10 of the data booklet.

Outline why both C to O bonds in the conjugate base are the same length and suggest a value for them. Use section 10 of the data booklet.

Outline why both C to O bonds in the conjugate base are the same length and suggest a value for them. Use section 10 of the data booklet.

State the hybridization of the nitrogen atom in chloramine.

State the hybridization of the nitrogen atom in chloramine.

State the hybridization of the nitrogen atom in chloramine.

Dinitrogen monoxide in the stratosphere is converted to nitrogen monoxide, NO (g).

Write two equations to show how NO (g) catalyses the decomposition of ozone.

Dinitrogen monoxide in the stratosphere is converted to nitrogen monoxide, NO (g).

Write two equations to show how NO (g) catalyses the decomposition of ozone.

Dinitrogen monoxide in the stratosphere is converted to nitrogen monoxide, NO (g).

Write two equations to show how NO (g) catalyses the decomposition of ozone.

Deduce the hybridization of the central nitrogen atom in the molecule.

Deduce the hybridization of the central nitrogen atom in the molecule.

Deduce the hybridization of the central nitrogen atom in the molecule.

State what the presence of alternative Lewis structures shows about the nature of the bonding in the molecule.

State what the presence of alternative Lewis structures shows about the nature of the bonding in the molecule.

State what the presence of alternative Lewis structures shows about the nature of the bonding in the molecule.

When excess ammonia is added to copper(II) chloride solution, the dark blue complex ion, [Cu(NH₃)₄(H₂O)₂]²⁺, forms.

State the molecular geometry of this complex ion, and the bond angles within it.

Molecular geometry:

Bond angles: 

When excess ammonia is added to copper(II) chloride solution, the dark blue complex ion, [Cu(NH₃)₄(H₂O)₂]²⁺, forms.

State the molecular geometry of this complex ion, and the bond angles within it.

Molecular geometry:

Bond angles: 

When excess ammonia is added to copper(II) chloride solution, the dark blue complex ion, [Cu(NH₃)₄(H₂O)₂]²⁺, forms.

State the molecular geometry of this complex ion, and the bond angles within it.

Molecular geometry:

Bond angles: 

Deduce the Lewis (electron dot) structure, including formal charges, and shape for dinitrogen monoxide showing nitrogen as the central atom.

Deduce the Lewis (electron dot) structure, including formal charges, and shape for dinitrogen monoxide showing nitrogen as the central atom.

Deduce the Lewis (electron dot) structure, including formal charges, and shape for dinitrogen monoxide showing nitrogen as the central atom.

Deduce the Lewis (electron dot) structure for sulfur dioxide.

Deduce the Lewis (electron dot) structure for sulfur dioxide.

Deduce the Lewis (electron dot) structure for sulfur dioxide.

How many sigma (σ) and pi (π) bonds are present in this molecule?

How many sigma (σ) and pi (π) bonds are present in this molecule?

How many sigma (σ) and pi (π) bonds are present in hydrogen cyanide, HCN?

How many sigma (σ) and pi (π) bonds are present in hydrogen cyanide, HCN?

$\mathrm{CFC}$s produce chlorine radicals. Write two successive propagation steps to show how chlorine radicals catalyse the depletion of ozone.

$\mathrm{CFC}$s produce chlorine radicals. Write two successive propagation steps to show how chlorine radicals catalyse the depletion of ozone.

$\mathrm{CFC}$s produce chlorine radicals. Write two successive propagation steps to show how chlorine radicals catalyse the depletion of ozone.

Distinguish between a sigma and pi bond.

Distinguish between a sigma and pi bond.

Distinguish between a sigma and pi bond.

State the number of $\text{σ}$ (sigma) and $\mathrm{\pi }$ (pi) bonds in Compound A.

State the number of $\text{σ}$ (sigma) and $\mathrm{\pi }$ (pi) bonds in Compound A.

State the number of $\text{σ}$ (sigma) and $\mathrm{\pi }$ (pi) bonds in Compound A.

Deduce a Lewis (electron dot) structure of the nitric acid molecule, HNO₃, that obeys the octet rule, showing any non-zero formal charges on the atoms.

Deduce a Lewis (electron dot) structure of the nitric acid molecule, HNO₃, that obeys the octet rule, showing any non-zero formal charges on the atoms.

Deduce a Lewis (electron dot) structure of the nitric acid molecule, HNO₃, that obeys the octet rule, showing any non-zero formal charges on the atoms.

Which molecule produces this ¹H-NMR spectrum?

_{[Source: SDBS, National Institute of Advanced Industrial Science and Technology.]}

A.  CH₃COOCH₃

B.  CH₃COCH₃

C.  CH₃CHO

D.  CH₃CH₂CH₃

Which molecule produces this ¹H-NMR spectrum?

_{[Source: SDBS, National Institute of Advanced Industrial Science and Technology.]}

A.  CH₃COOCH₃

B.  CH₃COCH₃

C.  CH₃CHO

D.  CH₃CH₂CH₃

An electrolytic cell was set up using inert electrodes and a dilute aqueous solution of magnesium chloride, MgCl₂ (aq).

An electrolytic cell was set up using inert electrodes and a dilute aqueous solution of magnesium chloride, MgCl₂ (aq).

An electrolytic cell was set up using inert electrodes and a dilute aqueous solution of magnesium chloride, MgCl₂ (aq).