Structure 2. Models of bonding and structure

Which equation represents lattice enthalpy?

A. NaCl (g) → Na⁺ (g) + Cl⁻ (g)

B. NaCl (s) → Na⁺ (g) + Cl⁻ (g)

C. NaCl (s) → Na⁺ (aq) + Cl⁻ (aq)

D. NaCl (s) → Na⁺ (s) + Cl⁻ (s)

The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.

State the types of bonding in magnesium, oxygen and magnesium oxide, and how the valence electrons produce these types of bonding.

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 is the formula of the compound formed from Ca²⁺ and PO₄³⁻?

A.  CaPO₄

B.  Ca₃(PO₄)₂

C.  Ca₂(PO₄)₃

D.  Ca(PO₄)₂

Outline the two distinct phases of this composite.

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.  $\text{NaOH}$

Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.

Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.

Outline the two distinct phases of this composite.

Which formula is correct?

A.  ${\mathrm{NH}}_4{\mathrm{PO}}_4$

B.  ${\left({\mathrm{NH}}_4\right)}_2{\mathrm{PO}}_4$

C.  ${\left({\mathrm{NH}}_4\right)}_3{\mathrm{PO}}_4$

D.  ${\left({\mathrm{NH}}_4\right)}_3{\left({\mathrm{PO}}_4\right)}_2$

Which substance has the highest lattice enthalpy?

A.  $\text{KCl}$

B.  ${\text{CaCl}}_2$

C.  $\text{KF}$

D.  ${\text{CaF}}_{\text{2}}$

Which equation represents lattice enthalpy?

A. NaCl (g) → Na⁺ (g) + Cl⁻ (g)

B. NaCl (s) → Na⁺ (g) + Cl⁻ (g)

C. NaCl (s) → Na⁺ (aq) + Cl⁻ (aq)

D. NaCl (s) → Na⁺ (s) + Cl⁻ (s)

The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.

State the types of bonding in magnesium, oxygen and magnesium oxide, and how the valence electrons produce these types of bonding.

The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.

State the types of bonding in magnesium, oxygen and magnesium oxide, and how the valence electrons produce these types of bonding.

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:

Identify the type of bonding in sodium hydrogencarbonate.

Between sodium and hydrogencarbonate:

Between hydrogen and oxygen in hydrogencarbonate:

What is the formula of the compound formed from Ca²⁺ and PO₄³⁻?

A.  CaPO₄

B.  Ca₃(PO₄)₂

C.  Ca₂(PO₄)₃

D.  Ca(PO₄)₂

Outline the two distinct phases of this composite.

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.  $\text{NaOH}$

Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.

Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.

Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.

Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.

Outline the two distinct phases of this composite.

Which formula is correct?

A.  ${\mathrm{NH}}_4{\mathrm{PO}}_4$

B.  ${\left({\mathrm{NH}}_4\right)}_2{\mathrm{PO}}_4$

C.  ${\left({\mathrm{NH}}_4\right)}_3{\mathrm{PO}}_4$

D.  ${\left({\mathrm{NH}}_4\right)}_3{\left({\mathrm{PO}}_4\right)}_2$

Which substance has the highest lattice enthalpy?

A.  $\text{KCl}$

B.  ${\text{CaCl}}_2$

C.  $\text{KF}$

D.  ${\text{CaF}}_{\text{2}}$

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.

State the types of bonding in magnesium, oxygen and magnesium oxide, and how the valence electrons produce these types of bonding.

Which statement best describes the intramolecular bonding in HCN (l)?

A. Electrostatic attractions between H⁺ and CN⁻ ions

B. Hydrogen bonding

C. Van der Waals forces and hydrogen bonding

D. Electrostatic attractions between pairs of electrons and positively charged nuclei

What is the main interaction between liquid CH₄ molecules?

A.  London (dispersion) forces

B.  Dipole–dipole forces

C.  Hydrogen bonding

D.  Covalent bonding

Sketch the Lewis (electron dot) structure of the P₄ molecule, containing only single bonds.

Identify the type of bonding in sodium hydrogencarbonate.

Between sodium and hydrogencarbonate:

Between hydrogen and oxygen in hydrogencarbonate:

The minor product, C₆H₅–CH₂–CH₂Br, can exist in different conformational forms (isomers).

Outline what this means.

Explain the electron domain geometry of SO₃.

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

Identify the number of sigma and pi bonds in HCN.

Suggest why hydrogen chloride, HCl, has a lower boiling point than hydrogen cyanide, HCN.

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

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

Draw the structure of one other isomer of xylene which retains the benzene ring.

Draw the structure of one other isomer of xylene which retains the benzene ring.

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

Identify the type of bonding in sodium hydrogencarbonate.

Between sodium and hydrogencarbonate:

Between hydrogen and oxygen in hydrogencarbonate:

The melting points of cocoa butter and coconut oil are 34 °C and 25 °C respectively.

Explain this in terms of their saturated fatty acid composition.

Lecithin aids the body’s absorption of vitamin E.

Suggest why vitamin E is fat-soluble.

The melting points of cocoa butter and coconut oil are 34 °C and 25 °C respectively.

Explain this in terms of their saturated fatty acid composition.

Draw a Lewis (electron dot) structure of chloramine.

Deduce the molecular geometry of chloramine and estimate its H–N–H bond angle.

Molecular geometry:

H–N–H bond angle:

Lecithin aids the body’s absorption of vitamin E.

Suggest why vitamin E is fat-soluble.

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

State, giving a reason, the shape of the dinitrogen monoxide molecule.

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

What is the order of increasing boiling point?

A. CH₃CH₂CH₂CH₃ < CH₃CH(OH)CH₃ < CH₃COCH₃ < CH₃CO₂H

B. CH₃CH₂CH₂CH₃ < CH₃COCH₃ < CH₃CH(OH)CH₃ < CH₃CO₂H

C. CH₃CO₂H < CH₃COCH₃ < CH₃CH(OH)CH₃ < CH₃CH₂CH₂CH₃

D. CH₃CH₂CH₂CH₃ < CH₃COCH₃ < CH₃CO₂H < CH₃CH(OH)CH₃

Which compound has the lowest boiling point?

A. CH₃CH₂CH₂CH₂CH₂CH₃

B. CH₃CH₂CH₂CH₂CH₃

C. CH₃CH(CH₃)CH₂CH₃

D. CH₃C(CH₃)₂CH₃

Which compound has the lowest boiling point?

A. CH₃CH₂CH₂CH₂CH₂CH₃

B. CH₃CH₂CH₂CH₂CH₃

C. CH₃CH(CH₃)CH₂CH₃

D. CH₃C(CH₃)₂CH₃

Ascorbic acid and retinol are two important vitamins.

Explain why ascorbic acid is soluble in water and retinol is not. Use section 35 of the data booklet.

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 order of increasing boiling point?

A. CH₃CH₂CH₂CH₃ < CH₃CH(OH)CH₃ < CH₃COCH₃ < CH₃CO₂H

B. CH₃CH₂CH₂CH₃ < CH₃COCH₃ < CH₃CH(OH)CH₃ < CH₃CO₂H

C. CH₃CO₂H < CH₃COCH₃ < CH₃CH(OH)CH₃ < CH₃CH₂CH₂CH₃

D. CH₃CH₂CH₂CH₃ < CH₃COCH₃ < CH₃CO₂H < CH₃CH(OH)CH₃

Draw a Lewis (electron dot) structure for ozone.

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

Draw the structure of the conjugate base of benzoic acid showing all the atoms and all the bonds.

The pH of an aqueous solution of benzoic acid at 298 K is 2.95. Determine the concentration of hydroxide ions in the solution, using section 2 of the data booklet.

Formulate the equation for the complete combustion of benzoic acid in oxygen using only integer coefficients.

Suggest how benzoic acid, M_r = 122.13, forms an apparent dimer, M_r = 244.26, when dissolved in a non-polar solvent such as hexane.

What is the structure and bonding in SiO₂(s)?

Deduce the Lewis (electron dot) structure and molecular geometry of sulfur dichloride, SCl₂.

Outline the two distinct phases of this composite.

Sketch the Lewis (electron dot) structure of the P₄ molecule, containing only single bonds.

Which compound has the shortest C to N bond?

A.  HCN

B.  CH₃CH₂NH₂

C.  CH₃CHNH

D.  (CH₃)₂NH

Draw the Lewis (electron dot) structure of hydrogen sulfide.

Which combination correctly describes the geometry of the carbonate ion, ${{\mathrm{CO}}_3}^{2-}$?

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 the two distinct phases of this composite.

Which molecule is most polar?

A.  ${\mathrm{CHF}}_3$

B.  ${\mathrm{CF}}_4$

C.  ${\mathrm{CClF}}_3$

D.  ${\mathrm{CCl}}_4$

Explain, with reference to intermolecular forces, why B is more volatile than A.

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

Which molecule is polar?

A.  BeH₂

B.  AlH₃

C.  PH₃

D.  SiH₄

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.

State the types of bonding in magnesium, oxygen and magnesium oxide, and how the valence electrons produce these types of bonding.

State the types of bonding in magnesium, oxygen and magnesium oxide, and how the valence electrons produce these types of bonding.

Which statement best describes the intramolecular bonding in HCN (l)?

A. Electrostatic attractions between H⁺ and CN⁻ ions

B. Hydrogen bonding

C. Van der Waals forces and hydrogen bonding

D. Electrostatic attractions between pairs of electrons and positively charged nuclei

What is the main interaction between liquid CH₄ molecules?

A.  London (dispersion) forces

B.  Dipole–dipole forces

C.  Hydrogen bonding

D.  Covalent bonding

Sketch the Lewis (electron dot) structure of the P₄ molecule, containing only single bonds.

Sketch the Lewis (electron dot) structure of the P₄ molecule, containing only single bonds.

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:

The minor product, C₆H₅–CH₂–CH₂Br, can exist in different conformational forms (isomers).

Outline what this means.

The minor product, C₆H₅–CH₂–CH₂Br, can exist in different conformational forms (isomers).

Outline what this means.

Explain the electron domain geometry of SO₃.

Explain the electron domain geometry of SO₃.

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

Identify the number of sigma and pi bonds in HCN.

Suggest why hydrogen chloride, HCl, has a lower boiling point than hydrogen cyanide, HCN.

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

Identify the number of sigma and pi bonds in HCN.

Suggest why hydrogen chloride, HCl, has a lower boiling point than hydrogen cyanide, HCN.

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

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

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

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

Draw the structure of one other isomer of xylene which retains the benzene ring.

Draw the structure of one other isomer of xylene which retains the benzene ring.

Draw the structure of one other isomer of xylene which retains the benzene ring.

Draw the structure of one other isomer of xylene which retains the benzene ring.

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

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:

The melting points of cocoa butter and coconut oil are 34 °C and 25 °C respectively.

Explain this in terms of their saturated fatty acid composition.

Lecithin aids the body’s absorption of vitamin E.

Suggest why vitamin E is fat-soluble.

The melting points of cocoa butter and coconut oil are 34 °C and 25 °C respectively.

Explain this in terms of their saturated fatty acid composition.

Draw a Lewis (electron dot) structure of chloramine.

Deduce the molecular geometry of chloramine and estimate its H–N–H bond angle.

Molecular geometry:

H–N–H bond angle:

Draw a Lewis (electron dot) structure of chloramine.

Deduce the molecular geometry of chloramine and estimate its H–N–H bond angle.

Molecular geometry:

H–N–H bond angle:

Lecithin aids the body’s absorption of vitamin E.

Suggest why vitamin E is fat-soluble.

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

State, giving a reason, the shape of the dinitrogen monoxide 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, giving a reason, the shape of the dinitrogen monoxide molecule.

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

What is the order of increasing boiling point?

A. CH₃CH₂CH₂CH₃ < CH₃CH(OH)CH₃ < CH₃COCH₃ < CH₃CO₂H

B. CH₃CH₂CH₂CH₃ < CH₃COCH₃ < CH₃CH(OH)CH₃ < CH₃CO₂H

C. CH₃CO₂H < CH₃COCH₃ < CH₃CH(OH)CH₃ < CH₃CH₂CH₂CH₃

D. CH₃CH₂CH₂CH₃ < CH₃COCH₃ < CH₃CO₂H < CH₃CH(OH)CH₃

Which compound has the lowest boiling point?

A. CH₃CH₂CH₂CH₂CH₂CH₃

B. CH₃CH₂CH₂CH₂CH₃

C. CH₃CH(CH₃)CH₂CH₃

D. CH₃C(CH₃)₂CH₃

Which compound has the lowest boiling point?

A. CH₃CH₂CH₂CH₂CH₂CH₃

B. CH₃CH₂CH₂CH₂CH₃

C. CH₃CH(CH₃)CH₂CH₃

D. CH₃C(CH₃)₂CH₃

Ascorbic acid and retinol are two important vitamins.

Explain why ascorbic acid is soluble in water and retinol is not. Use section 35 of the data booklet.

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 order of increasing boiling point?

A. CH₃CH₂CH₂CH₃ < CH₃CH(OH)CH₃ < CH₃COCH₃ < CH₃CO₂H

B. CH₃CH₂CH₂CH₃ < CH₃COCH₃ < CH₃CH(OH)CH₃ < CH₃CO₂H

C. CH₃CO₂H < CH₃COCH₃ < CH₃CH(OH)CH₃ < CH₃CH₂CH₂CH₃

D. CH₃CH₂CH₂CH₃ < CH₃COCH₃ < CH₃CO₂H < CH₃CH(OH)CH₃

Draw a Lewis (electron dot) structure for ozone.

Draw a Lewis (electron dot) structure for ozone.

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

Draw the structure of the conjugate base of benzoic acid showing all the atoms and all the bonds.

The pH of an aqueous solution of benzoic acid at 298 K is 2.95. Determine the concentration of hydroxide ions in the solution, using section 2 of the data booklet.

Formulate the equation for the complete combustion of benzoic acid in oxygen using only integer coefficients.

Suggest how benzoic acid, M_r = 122.13, forms an apparent dimer, M_r = 244.26, when dissolved in a non-polar solvent such as hexane.

Draw the structure of the conjugate base of benzoic acid showing all the atoms and all the bonds.

The pH of an aqueous solution of benzoic acid at 298 K is 2.95. Determine the concentration of hydroxide ions in the solution, using section 2 of the data booklet.

Formulate the equation for the complete combustion of benzoic acid in oxygen using only integer coefficients.

Suggest how benzoic acid, M_r = 122.13, forms an apparent dimer, M_r = 244.26, when dissolved in a non-polar solvent such as hexane.

What is the structure and bonding in SiO₂(s)?

Deduce the Lewis (electron dot) structure and molecular geometry of sulfur dichloride, SCl₂.

Deduce the Lewis (electron dot) structure and molecular geometry of sulfur dichloride, SCl₂.

Outline the two distinct phases of this composite.

Sketch the Lewis (electron dot) structure of the P₄ molecule, containing only single bonds.

Sketch the Lewis (electron dot) structure of the P₄ molecule, containing only single bonds.

Which compound has the shortest C to N bond?

A.  HCN

B.  CH₃CH₂NH₂

C.  CH₃CHNH

D.  (CH₃)₂NH

Draw the Lewis (electron dot) structure of hydrogen sulfide.

Draw the Lewis (electron dot) structure of hydrogen sulfide.

Which combination correctly describes the geometry of the carbonate ion, ${{\mathrm{CO}}_3}^{2-}$?

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 the two distinct phases of this composite.

Which molecule is most polar?

A.  ${\mathrm{CHF}}_3$

B.  ${\mathrm{CF}}_4$

C.  ${\mathrm{CClF}}_3$

D.  ${\mathrm{CCl}}_4$

Explain, with reference to intermolecular forces, why B is more volatile than A.

Explain, with reference to intermolecular forces, why B is more volatile than A.

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

Which molecule is polar?

A.  BeH₂

B.  AlH₃

C.  PH₃

D.  SiH₄

State the types of bonding in magnesium, oxygen and magnesium oxide, and how the valence electrons produce these types of bonding.

Describe the bonding in iron, Fe (s).

Determine the density of calcium, in g cm⁻³, using section 2 of the data booklet.

Ar = 40.08; metallic radius (r) = 1.97 × 10⁻¹⁰ m

Outline the two distinct phases of this composite.

Which series shows the correct order of metallic bond strength from strongest to weakest?

A.  $\mathrm{Na}>\mathrm{K}>\mathrm{Rb}>\mathrm{Mg}$

B.  $\mathrm{Mg}>\mathrm{Rb}>\mathrm{K}>\mathrm{Na}$

C.  $\mathrm{Rb}>\mathrm{K}>\mathrm{Na}>\mathrm{Mg}$

D.  $\mathrm{Mg}>\mathrm{Na}>\mathrm{K}>\mathrm{Rb}$

State the types of bonding in magnesium, oxygen and magnesium oxide, and how the valence electrons produce these types of bonding.

State the types of bonding in magnesium, oxygen and magnesium oxide, and how the valence electrons produce these types of bonding.

Describe the bonding in iron, Fe (s).

Describe the bonding in iron, Fe (s).

Determine the density of calcium, in g cm⁻³, using section 2 of the data booklet.

Ar = 40.08; metallic radius (r) = 1.97 × 10⁻¹⁰ m

Outline the two distinct phases of this composite.

Which series shows the correct order of metallic bond strength from strongest to weakest?

A.  $\mathrm{Na}>\mathrm{K}>\mathrm{Rb}>\mathrm{Mg}$

B.  $\mathrm{Mg}>\mathrm{Rb}>\mathrm{K}>\mathrm{Na}$

C.  $\mathrm{Rb}>\mathrm{K}>\mathrm{Na}>\mathrm{Mg}$

D.  $\mathrm{Mg}>\mathrm{Na}>\mathrm{K}>\mathrm{Rb}$

Deduce the products of the hydrolysis of a non-substituted phospholipid, where ${\mathrm{R}}^1$ and ${\mathrm{R}}^2$ represent long alkyl chains.

Draw the repeating unit of polyphenylethene.

Outline how alloys conduct electricity and why they are often harder than pure metals.

Conduct electricity:

Harder than pure metals:

Draw the structure of the repeating unit of starch and state the type of linkage formed between these units.

Type of linkage:

Formulate the equation for the complete hydrolysis of a starch molecule, (C₆H₁₀O₅)_n.

Draw the structure of the repeating unit of starch and state the type of linkage formed between these units.

Type of linkage:

Formulate the equation for the complete hydrolysis of a starch molecule, (C₆H₁₀O₅)_n.

Outline how alloys conduct electricity and why they are often harder than pure metals.

Conduct electricity:

Harder than pure metals:

Classify polybutadiene as either an addition or condensation polymer, giving a reason.

State one factor considered when making green chemistry polymers.

Which structure represents a repeating unit of a polymer formed from propene?

A.  –CH₂–CH(CH₃)–

B.  –CH₂–CH₂–CH₂–

C.  –CH(CH₃)–CH(CH₃)–

D.  –CH₂–CH₂–

Draw the structure of the monomers of Kevlar^® if the by-product of the condensation polymerization is hydrogen chloride.

Which monomer would produce the polymer shown?

A.  ${\text{CF}}_{\text{3}}{\text{CCl}}_{\text{2}}\text{F}$

B.  ${\text{CF}}_{\text{3}}\text{CClHF}$

C.  ${\text{CF}}_{\text{2}}\text{CClF}$

D.  ${\text{CF}}_{\text{2}}{\text{CF}}_{\text{2}}$

Which monomer forms the polymer shown?

A.  ${\text{CH(Cl)=CH(CH}}_{\text{3}}\text{)}$

B.  ${\text{CH}}_{\text{2}}{\text{=C(Cl)CH}}_{\text{3}}$

C.  ${\text{(CH}}_{\text{3}}{\text{)}}_{\text{2}}\text{CHCl}$

D.  ${\text{CH}}_{\text{2}}\text{=CHCl}$

Deduce the products of the hydrolysis of a non-substituted phospholipid, where ${\mathrm{R}}^1$ and ${\mathrm{R}}^2$ represent long alkyl chains.

Draw the repeating unit of polyphenylethene.

Draw the repeating unit of polyphenylethene.

Outline how alloys conduct electricity and why they are often harder than pure metals.

Conduct electricity:

Harder than pure metals:

Draw the structure of the repeating unit of starch and state the type of linkage formed between these units.

Type of linkage:

Formulate the equation for the complete hydrolysis of a starch molecule, (C₆H₁₀O₅)_n.

Draw the structure of the repeating unit of starch and state the type of linkage formed between these units.

Type of linkage:

Formulate the equation for the complete hydrolysis of a starch molecule, (C₆H₁₀O₅)_n.

Outline how alloys conduct electricity and why they are often harder than pure metals.

Conduct electricity:

Harder than pure metals:

Classify polybutadiene as either an addition or condensation polymer, giving a reason.

State one factor considered when making green chemistry polymers.

Which structure represents a repeating unit of a polymer formed from propene?

A.  –CH₂–CH(CH₃)–

B.  –CH₂–CH₂–CH₂–

C.  –CH(CH₃)–CH(CH₃)–

D.  –CH₂–CH₂–

Draw the structure of the monomers of Kevlar^® if the by-product of the condensation polymerization is hydrogen chloride.

Which monomer would produce the polymer shown?

A.  ${\text{CF}}_{\text{3}}{\text{CCl}}_{\text{2}}\text{F}$

B.  ${\text{CF}}_{\text{3}}\text{CClHF}$

C.  ${\text{CF}}_{\text{2}}\text{CClF}$

D.  ${\text{CF}}_{\text{2}}{\text{CF}}_{\text{2}}$

Which monomer forms the polymer shown?

A.  ${\text{CH(Cl)=CH(CH}}_{\text{3}}\text{)}$

B.  ${\text{CH}}_{\text{2}}{\text{=C(Cl)CH}}_{\text{3}}$

C.  ${\text{(CH}}_{\text{3}}{\text{)}}_{\text{2}}\text{CHCl}$

D.  ${\text{CH}}_{\text{2}}\text{=CHCl}$