4.2 Covalent bonding

Which compound has the shortest C–N bond?

A. CH₃NH₂

B. (CH₃)₃CNH₂

C. CH₃CN

D. CH₃CHNH

Which compound has the shortest C–N bond?

A. CH₃NH₂

B. (CH₃)₃CNH₂

C. CH₃CN

D. CH₃CHNH

Which compound contains both ionic and covalent bonds?

A.  $\text{MgO}$

B.  ${\text{CH}}_{\text{2}}{\text{Cl}}_{\text{2}}$

C.  ${\text{CH}}_{\text{3}}\text{COOH}$

D.  $\text{NaOH}$

Which compound contains both ionic and covalent bonds?

A.  $\text{MgO}$

B.  ${\text{CH}}_{\text{2}}{\text{Cl}}_{\text{2}}$

C.  ${\text{CH}}_{\text{3}}\text{COOH}$

D.  $\text{NaOH}$

Which compound has the shortest C to N bond?

A.  HCN

B.  CH₃CH₂NH₂

C.  CH₃CHNH

D.  (CH₃)₂NH

Which compound has the shortest C to N bond?

A.  HCN

B.  CH₃CH₂NH₂

C.  CH₃CHNH

D.  (CH₃)₂NH

The graph shows the boiling points of the hydrides of group 16 elements.

Explain the increase in the boiling point from H₂S to H₂Te.

The graph shows the boiling points of the hydrides of group 16 elements.

Explain the increase in the boiling point from H₂S to H₂Te.

The graph shows the boiling points of the hydrides of group 16 elements.

Explain the increase in the boiling point from H₂S to H₂Te.

Compare, giving a reason, the length of the bond between the carbon atoms in ethyne with that in ethane, C₂H₆.

Compare, giving a reason, the length of the bond between the carbon atoms in ethyne with that in ethane, C₂H₆.

Compare, giving a reason, the length of the bond between the carbon atoms in ethyne with that in ethane, C₂H₆.

Identify the type of bonding in sodium hydrogencarbonate.

Between sodium and hydrogencarbonate:

Between hydrogen and oxygen in hydrogencarbonate:

Identify the type of bonding in sodium hydrogencarbonate.

Between sodium and hydrogencarbonate:

Between hydrogen and oxygen in hydrogencarbonate:

Identify the type of bonding in sodium hydrogencarbonate.

Between sodium and hydrogencarbonate:

Between hydrogen and oxygen in hydrogencarbonate:

What are the predicted electron domain geometries around the carbon and both nitrogen atoms in urea, (NH₂)₂CO, applying VSEPR theory?

What are the predicted electron domain geometries around the carbon and both nitrogen atoms in urea, (NH₂)₂CO, applying VSEPR theory?

Explain why the hydrides of group 16 elements (H₂O, H₂S, H₂Se and H₂Te) are polar molecules.

Explain why the hydrides of group 16 elements (H₂O, H₂S, H₂Se and H₂Te) are polar molecules.

Explain why the hydrides of group 16 elements (H₂O, H₂S, H₂Se and H₂Te) are polar molecules.

Compare, giving a reason, the length of the bond between the carbon atoms in ethyne with that in ethane, C₂H₆.

Compare, giving a reason, the length of the bond between the carbon atoms in ethyne with that in ethane, C₂H₆.

Compare, giving a reason, the length of the bond between the carbon atoms in ethyne with that in ethane, C₂H₆.

Identify the type of bonding in sodium hydrogencarbonate.

Between sodium and hydrogencarbonate:

Between hydrogen and oxygen in hydrogencarbonate:

Identify the type of bonding in sodium hydrogencarbonate.

Between sodium and hydrogencarbonate:

Between hydrogen and oxygen in hydrogencarbonate:

Identify the type of bonding in sodium hydrogencarbonate.

Between sodium and hydrogencarbonate:

Between hydrogen and oxygen in hydrogencarbonate:

Determine the percentage of ionic bonding in alumina using sections 8 and 29 of the data booklet.

Determine the percentage of ionic bonding in alumina using sections 8 and 29 of the data booklet.

Determine the percentage of ionic bonding in alumina using sections 8 and 29 of the data booklet.

Which of these species contains the shortest carbon to oxygen bond length?

A.  ${\mathrm{CH}}_3{\mathrm{CH}}_2{\mathrm{O}}^{-}$

B.  ${\mathrm{CH}}_3{\mathrm{CH}}_2\mathrm{OH}$

C.  ${\mathrm{CH}}_3{\mathrm{COO}}^{-}$

D.  ${\mathrm{CH}}_3\mathrm{COOH}$

Which of these species contains the shortest carbon to oxygen bond length?

A.  ${\mathrm{CH}}_3{\mathrm{CH}}_2{\mathrm{O}}^{-}$

B.  ${\mathrm{CH}}_3{\mathrm{CH}}_2\mathrm{OH}$

C.  ${\mathrm{CH}}_3{\mathrm{COO}}^{-}$

D.  ${\mathrm{CH}}_3\mathrm{COOH}$

Outline two differences between the bonding of carbon atoms in C₆₀ and diamond.

Outline two differences between the bonding of carbon atoms in C₆₀ and diamond.

Outline two differences between the bonding of carbon atoms in C₆₀ and diamond.

Explain why C₆₀ and diamond sublime at different temperatures and pressures.

Explain why C₆₀ and diamond sublime at different temperatures and pressures.

Explain why C₆₀ and diamond sublime at different temperatures and pressures.

Chlorofluorocarbons (CFCs) contain bonds of the following lengths:

C—C = 1.54 × 10⁻¹⁰ m

C—F = 1.38 × 10⁻¹⁰ m

C—Cl = 1.77 × 10⁻¹⁰ m

What is the order of increasing bond strength in the CFC molecule?

A.   C—C  <  C—F  <  C—Cl

B.   C—C  <  C—Cl <  C—F

C.   C—Cl <  C—C  <  C—F

D.   C—F  <  C—C  <  C—Cl

Chlorofluorocarbons (CFCs) contain bonds of the following lengths:

C—C = 1.54 × 10⁻¹⁰ m

C—F = 1.38 × 10⁻¹⁰ m

C—Cl = 1.77 × 10⁻¹⁰ m

What is the order of increasing bond strength in the CFC molecule?

A.   C—C  <  C—F  <  C—Cl

B.   C—C  <  C—Cl <  C—F

C.   C—Cl <  C—C  <  C—F

D.   C—F  <  C—C  <  C—Cl

Nitrogen (IV) oxide exists in equilibrium with dinitrogen tetroxide, N₂O₄(g), which is colourless.

2NO₂ (g) ⇌ N₂O₄ (g)

Nitrogen (IV) oxide exists in equilibrium with dinitrogen tetroxide, N₂O₄(g), which is colourless.

2NO₂ (g) ⇌ N₂O₄ (g)

Nitrogen (IV) oxide exists in equilibrium with dinitrogen tetroxide, N₂O₄(g), which is colourless.

2NO₂ (g) ⇌ N₂O₄ (g)

Nitrogen (IV) oxide exists in equilibrium with dinitrogen tetroxide, N₂O₄(g), which is colourless.

2NO₂ (g) ⇌ N₂O₄ (g)

Nitrogen (IV) oxide exists in equilibrium with dinitrogen tetroxide, N₂O₄(g), which is colourless.

2NO₂ (g) ⇌ N₂O₄ (g)

Nitrogen (IV) oxide exists in equilibrium with dinitrogen tetroxide, N₂O₄(g), which is colourless.

2NO₂ (g) ⇌ N₂O₄ (g)

Determine the standard enthalpy of reaction ($\text{Δ}{H}_{\text{r}}^{⦵}$), in kJ mol⁻¹, for the oxidation of SO₂ to SO₃.

Determine the standard enthalpy of reaction ($\text{Δ}{H}_{\text{r}}^{⦵}$), in kJ mol⁻¹, for the oxidation of SO₂ to SO₃.

Determine the standard enthalpy of reaction ($\text{Δ}{H}_{\text{r}}^{⦵}$), in kJ mol⁻¹, for the oxidation of SO₂ to SO₃.