DP Chemistry Questionbank

• Syllabus

Topic 4: Chemical bonding and structure

Sub sections and their related questions

4.1 Ionic bonding and structure

• 15M.1.hl.TZ1.11: Which substance has the following properties? •     Low melting point •     Very soluble in...
• 15M.2.hl.TZ1.2b.i: Explain why the melting point of phosphorus(V) oxide is lower than that of sodium oxide in terms...
• 15M.2.hl.TZ1.2b.ii: Predict whether phosphorus(V) oxide and sodium oxide conduct electricity in their solid and...
• 15M.2.hl.TZ2.8b.ii: Describe the ionic bonding present in...
• 15M.2.hl.TZ2.8b.iii: Suggest why solid \({\text{C}}{{\text{r}}_{\text{2}}}{{\text{O}}_{\text{3}}}\) does not conduct...
• 15M.2.hl.TZ2.9a.i: State and explain the electrical conductivities of these two chloride compounds in their liquid...
• 15M.3.hl.TZ1.17b.i: Phosphate ions can be removed from a solution by adding calcium ions. State the ionic equation...
• 15M.1.sl.TZ2.9: The formula of gallium phosphate is \({\text{GaP}}{{\text{O}}_{\text{4}}}\). What is the correct...
• 15M.2.sl.TZ1.6f.i: Describe the bonding and structure of sodium chloride.
• 15M.2.sl.TZ1.6f.ii: State the formula of the compounds formed between the elements below.   Sodium and...
• 15M.2.sl.TZ2.3b: Outline why solid magnesium chloride does not conduct electricity.
• 15M.2.sl.TZ2.6b.iv: Describe the ionic bonding present in potassium chloride and how the ions are formed.
• 14M.1.hl.TZ1.11: A solid has a melting point of 1582 °C and does not dissolve in water. It does not conduct...
• 14M.2.hl.TZ1.5a: (i)     State the changes in the acid-base nature of the oxides across period 3 (from...
• 14M.1.sl.TZ2.9: What is the formula of calcium phosphide? A.    ...
• 14M.1.sl.TZ2.10: Which properties do typical ionic compounds have?
• 14N.2.hl.TZ0.8c: (i)     Magnesium reacts with oxygen to form an ionic compound, magnesium oxide. Describe how the...
• 13N.1.hl.TZ0.9: What is the formula of calcium nitride? A.    ...
• 13N.1.hl.TZ0.10: Which compounds have an ionic lattice structure in the solid state? I.     Silicon dioxide II....
• 13N.2.hl.TZ0.3a.i: State the formula of both ions present and the nature of the force between these...
• 13N.1.sl.TZ0.10: What is the formula of calcium nitride? A.    ...
• 13N.1.sl.TZ0.11: Which compounds have an ionic lattice structure in the solid state? I.     Silicon dioxide II. ...
• 13N.2.sl.TZ0.3a.i: State the formula of both ions present and the nature of the force between these...
• 13M.1.sl.TZ1.10: Which statement best describes ionic bonding? A.     It is the electrostatic attraction between...
• 13M.1.sl.TZ1.11: What are the correct formulas of the following ions?
• 13M.1.sl.TZ1.12: Which statements concerning the sodium chloride ionic lattice are correct? I.     Sodium ions...
• 13M.1.sl.TZ1.13: Which combination best describes the type of bonding present and the melting point of silicon and...
• 13M.2.sl.TZ1.3a: Compare how electric current passes through sodium and sodium chloride by completing the table...
• 13M.2.sl.TZ2.5a.i: Ionic bonding occurs in sodium chloride. Describe what is meant by the term ionic bonding.
• 13M.2.sl.TZ2.5a.ii: Sodium chloride has a lattice structure. Describe the lattice structure of sodium chloride...
• 13M.2.sl.TZ2.5a.iii: Ammonium phosphate is also an ionic compound, used in the manufacture of fertilizers. State the...
• 13M.2.sl.TZ2.5c: Using electronegativity values from Table 7 of the Data Booklet, state and explain which of the...
• 12N.1.sl.TZ0.10: What is the formula of the ionic compound formed when calcium and nitrogen react together? A.  ...
• 12N.1.sl.TZ0.13: Which statement about the physical properties of substances is correct? A.     The only solids...
• 12N.2.sl.TZ0.4c: (i)     Explain why metals are good conductors of electricity and why they are malleable. (ii)  ...
• 12N.2.sl.TZ0.5b.vii: One common nitrogen-containing fertilizer is ammonium sulfate. State its chemical formula.
• 09N.1.sl.TZ0.10: What compound is formed when lithium reacts with selenium? A.     LiSe B.    ...
• 09N.1.sl.TZ0.14: Which substance does not conduct electricity? A.     Solid zinc B.     Molten zinc C.   ...
• 10M.1.sl.TZ2.10: What is the formula of magnesium fluoride? A.    ...
• 09M.1.sl.TZ1.11: What are the correct formulas of the following ions?
• 09M.1.sl.TZ1.13: Which is the best description of ionic bonding? A.     The electrostatic attraction between...
• 09M.2.sl.TZ1.3a: Explain why solid sodium oxide is a non-conductor of electricity.
• 09M.1.sl.TZ2.10: Which statement best describes the intramolecular bonding in HCN(l)? A.     Electrostatic...
• 09M.1.sl.TZ2.12: Metal M has only one oxidation number and forms a compound with the formula...
• 09M.2.sl.TZ2.5b.iii: Explain why solid sodium chloride does not conduct electricity but molten sodium chloride does.
• 11M.2.hl.TZ1.6f.i: Explain the electrical conductivity of molten sodium oxide and liquid sulfur trioxide.
• 11M.1.sl.TZ1.12: Which combination of the characteristics of element X, a metal, and element Y, a non metal, is...
• 11M.1.sl.TZ1.13: Which particles are responsible for electrical conductivity in metals? A.     Anions B.   ...
• 11M.1.sl.TZ2.12: The number of electrons in the valence shell of elements A and B, are 6 and 7 respectively. What...
• 11M.1.sl.TZ2.14: Which particles are responsible for the conduction of electricity in molten aluminium? A.    ...
• 12M.2.hl.TZ2.7c.i: Aluminium chloride, \({\text{A}}{{\text{l}}_{\text{2}}}{\text{C}}{{\text{l}}_{\text{6}}}\), does...
• 12M.1.sl.TZ2.10: What is the formula of magnesium nitride? A.    ...
• 11N.2.hl.TZ0.6b.i: State and explain the difference in the electrical conductivity in the liquid state of the two...
• 11N.1.sl.TZ0.9: What are the correct formulas of the following ions?
• 11N.1.sl.TZ0.10: Which row correctly describes the bonding type and melting point of carbon and carbon dioxide?
• 11N.2.sl.TZ0.1a: Sodium azide involves ionic bonding, and metallic bonding is present in sodium. Describe ionic...
• 11N.2.sl.TZ0.3b: Explain why solid sodium chloride does not conduct electricity.
• 11N.2.sl.TZ0.5d.i: State the name of A.
• 16M.1.sl.TZ0.10: Which compound contains both ionic and covalent bonds? A.  SIH4 B. NaNO3 C. H2CO D. Na2S
• 16N.2.sl.TZ0.4f: Describe the structure and bonding in solid magnesium oxide.
• 16N.3.hl.TZ0.22c: (i) Uranium hexafluoride, UF6, is used in the uranium enrichment process that produces fuel for...
• 17M.1.sl.TZ1.9: A substance has the following properties: What is the most probable structure of this...
• 17M.2.sl.TZ1.2e.i: State the type of bonding in potassium chloride which melts at 1043 K.
• 17M.3.sl.TZ1.6b: Lanthanum has a similar electronegativity to group 2 metals. Explain, in terms of bonding and...
• 17M.1.sl.TZ2.10: Which bonds cause the boiling point of water to be significantly greater than that of...
• 17M.1.sl.TZ2.19: Which of the following does not react with dilute HCl(aq)? A.     Na2CO3 B.     Cu C.    ...
• 17M.2.sl.TZ2.1c.ii: Explain the electrical conductivity of molten Na2O and P4O10.
• 18M.2.hl.TZ1.2a: Describe the nature of ionic bonding.
• 18M.1.sl.TZ1.9: What is the formula of ammonium phosphate? A.     (NH3)3PO4 B.     (NH4)3PO4 C.   ...
• 18M.2.sl.TZ1.2a: Describe the nature of ionic bonding.
• 18M.1.sl.TZ2.9: What is the formula of magnesium nitride? A.     MgN B.     Mg2N3 C.     Mg3N D.     Mg3N2

4.2 Covalent bonding

• 15M.1.hl.TZ1.11: Which substance has the following properties? •     Low melting point •     Very soluble in...
• 15M.2.hl.TZ1.1e: Predict and explain the difference in carbon-oxygen bond lengths in ethanedioic acid and its...
• 15M.2.hl.TZ1.2b.i: Explain why the melting point of phosphorus(V) oxide is lower than that of sodium oxide in terms...
• 15M.2.hl.TZ1.2b.ii: Predict whether phosphorus(V) oxide and sodium oxide conduct electricity in their solid and...
• 15M.2.hl.TZ2.9a.i: State and explain the electrical conductivities of these two chloride compounds in their liquid...
• 15M.2.hl.TZ2.9d.i: Describe the covalent bond between carbon and hydrogen in the molecule above and how it is formed.
• 15M.1.sl.TZ2.12: Which statement is correct about carbon-oxygen bond lengths? A.     The C–O bond lengths are...
• 15M.2.sl.TZ2.6b.iii: Describe the covalent bond present in the chlorine molecule and how it is formed.
• 14M.1.hl.TZ1.11: A solid has a melting point of 1582 °C and does not dissolve in water. It does not conduct...
• 14M.1.hl.TZ2.10: What is the difference between the strength and the length of the carbon-oxygen bond in butanal...
• 14M.1.sl.TZ1.10: Which combination of length and strength of the carbon‒to‒carbon bonds in...
• 14M.1.sl.TZ2.11: Which compounds contain both ionic and covalent bonding? I.    ...
• 14M.2.sl.TZ2.2d: (i)     State the formula of the compound that boron forms with fluorine.   (ii)     Explain...
• 14N.1.hl.TZ0.10: Which sequence has the molecules in order of increasing nitrogen-nitrogen bond length? A.    ...
• 14N.2.hl.TZ0.8c: (i)     Magnesium reacts with oxygen to form an ionic compound, magnesium oxide. Describe how the...
• 14N.2.hl.TZ0.8d: (i)     Predict the type of hybridization of the carbon and oxygen atoms in...
• 14N.1.sl.TZ0.10: Which diatomic molecule has the strongest bonding between its atoms? A.    ...
• 14N.1.sl.TZ0.11: Which molecule is non-polar? A.     \({\text{CC}}{{\text{l}}_{\text{4}}}\) B.    ...
• 14N.2.sl.TZ0.6e: (i)     Deduce the Lewis structure of \({\text{PH}}_4^ + \).   (ii)     Predict, giving a...
• 13N.2.hl.TZ0.3a.ii: State which atoms are covalently bonded.
• 13N.2.hl.TZ0.5g: Outline how the length of the N–N bond in trinitramide compares with the N–N bond in nitrogen...
• 13N.2.hl.TZ0.6f.i: Describe the differences in the hybridization of these group 4 elements and the precise nature of...
• 13N.2.hl.TZ0.7c.i: The strength of the hydrogen–halogen bond.
• 13N.2.sl.TZ0.3a.ii: State which atoms are covalently bonded.
• 13N.2.sl.TZ0.4d: Outline how the length of the N–N bond in trinitramide compares with the N–N bond in nitrogen...
• 13M.2.sl.TZ1.6c.ii: Describe how covalent bonds are formed.
• 13M.1.sl.TZ2.12: Which statements are correct for the bonds between two carbon atoms? I.     Single bonds are...
• 13M.2.sl.TZ2.5c: Using electronegativity values from Table 7 of the Data Booklet, state and explain which of the...
• 12N.1.sl.TZ0.11: Which bond is the least polar? A.     C–H B.     F–H C.     O–H D.     N–H
• 12N.1.sl.TZ0.13: Which statement about the physical properties of substances is correct? A.     The only solids...
• 10N.2.hl.TZ0.7a: (i)     Draw the Lewis (electron dot) structure for N2H4 showing all valence electrons. (ii)    ...
• 10N.2.sl.TZ0.4a: (i)     Draw Lewis (electron dot) structures for...
• 09M.2.sl.TZ1.6a.i: Draw the Lewis structures for carbon monoxide, CO, carbon dioxide,...
• 09M.2.sl.TZ1.6a.ii: List, with an explanation, the three compounds in order of increasing carbon to oxygen bond...
• 09M.2.hl.TZ2.5d: Explain, using diagrams, why \({\text{N}}{{\text{O}}_{\text{2}}}\) is a polar molecule but...
• 09M.1.sl.TZ2.10: Which statement best describes the intramolecular bonding in HCN(l)? A.     Electrostatic...
• 09M.1.sl.TZ2.13: Which molecule has the shortest bond between carbon atoms? A.    ...
• 09M.2.sl.TZ2.1b.vi: The following is a three-dimensional computer-generated representation of aspirin. A third...
• 09M.2.sl.TZ2.7c: Explain, using diagrams, why CO and \({\text{N}}{{\text{O}}_{\text{2}}}\) are polar molecules but...
• 11M.2.sl.TZ1.7e: Describe the bonding within the carbon monoxide molecule.
• 11M.1.sl.TZ2.11: When \({{\text{C}}_{\text{2}}}{{\text{H}}_{\text{2}}}\),...
• 11M.1.sl.TZ2.12: The number of electrons in the valence shell of elements A and B, are 6 and 7 respectively. What...
• 12M.2.hl.TZ2.7c.i: Aluminium chloride, \({\text{A}}{{\text{l}}_{\text{2}}}{\text{C}}{{\text{l}}_{\text{6}}}\), does...
• 12M.1.sl.TZ2.11: Which single covalent bond is the most polar, given the following electronegativity...
• 12M.2.sl.TZ2.5a: (i)     Distinguish between the terms empirical formula and molecular formula. Empirical...
• 11N.1.sl.TZ0.13: Which bonds are arranged in order of increasing polarity? A.     H–F \( < \) H–Cl \( < \)...
• 16M.1.sl.TZ0.9: Which molecule is non-polar? A.  OF2 B.  NH3 C.  BF3 D.  SO2
• 16M.1.sl.TZ0.10: Which compound contains both ionic and covalent bonds? A.  SIH4 B. NaNO3 C. H2CO D. Na2S
• 16M.2.sl.TZ0.1a: (i) Draw a Lewis (electron dot) structure of phosphine. (ii) Outline whether you expect the...
• 16M.2.hl.TZ0.1a: (i) Draw a Lewis (electron dot) structure of phosphine. (ii) State the hybridization of the...
• 16N.1.hl.TZ0.11: How many electrons form the carbon–oxygen bond in methanal, HCHO? A. 2 B. 4 C. 8 D. 12
• 16N.3.sl.TZ0.3b: Predict the predominant type of bonding for a binary compound AB in which the electronegativity...
• 16N.3.sl.TZ0.6c: (i) Suggest why incomplete combustion of plastic, such as polyvinyl chloride, is common in...
• 17M.1.sl.TZ1.10: Which two atoms form the most polar bond? A.     C and F B.     C and Cl C.     Si and F D.  ...
• 17M.2.sl.TZ1.2e.ii: A chloride of titanium, TiCl4, melts at 248 K. Suggest why the melting point is so much lower...
• 17M.3.sl.TZ1.6a: Determine the type of bond present in SbBr3, showing your method. Use sections 8 and 29 of the...
• 17M.1.sl.TZ2.9: How many bonding electrons are there in the urea molecule? A.     8 B.     16 C.     20 D....
• 17M.1.sl.TZ2.10: Which bonds cause the boiling point of water to be significantly greater than that of...
• 17M.2.sl.TZ2.4a.i: State and explain the difference in bond strength between the nitrogen atoms in a hydrazine and...
• 17N.1.sl.TZ0.9: The electronegativity values of four elements are given. What is the order of increasing...
• 17N.1.sl.TZ0.10: Which compound has the shortest C–N bond? A. CH3NH2 B. (CH3)3CNH2 C. CH3CN D. CH3CHNH
• 18M.1.sl.TZ2.10: Which species has the longest carbon to oxygen bond length? A.     CO B.     CH3OH C.   ...
• 18M.1.sl.TZ2.11: What are the predicted electron domain geometries around the carbon and both nitrogen atoms in...
• 18M.2.sl.TZ2.6a.i: Explain why the hydrides of group 16 elements (H2O, H2S, H2Se and H2Te) are polar molecules.
• 18M.2.sl.TZ2.6a.ii: The graph shows the boiling points of the hydrides of group 16 elements. Explain the increase...

4.3 Covalent structures

• 15M.1.hl.TZ1.11: Which substance has the following properties? •     Low melting point •     Very soluble in...
• 15M.1.hl.TZ2.10: Which diagrams can be used to represent the Lewis (electron dot) structure of boron...
• 15M.2.hl.TZ1.1d: Deduce the Lewis (electron dot) structure of ethanedioic acid, \({\text{HOOC–COOH}}\).
• 15M.2.hl.TZ1.2b.i: Explain why the melting point of phosphorus(V) oxide is lower than that of sodium oxide in terms...
• 15M.2.hl.TZ1.2b.ii: Predict whether phosphorus(V) oxide and sodium oxide conduct electricity in their solid and...
• 15M.2.hl.TZ1.5g: Identify three allotropes of carbon and describe their structures.
• 15M.1.sl.TZ1.9: What describes the structure of silicon and silicon dioxide?
• 15M.1.sl.TZ1.10: Which molecules react to form a dative covalent (coordinate) bond? A.    ...
• 15M.1.sl.TZ1.11: What describes the relationship between diamond, graphite and \({{\text{C}}_{{\text{60}}}}\)...
• 15M.1.sl.TZ2.10: Which species contain a dative covalent (coordination or coordinate) bond? I.     Carbon...
• 15M.1.sl.TZ2.11: Which combination of shape and bond angle best describes a molecule of sulfur dioxide,...
• 15M.2.sl.TZ1.1e: Deduce the Lewis (electron dot) structure of ethanedioic acid, HOOC−COOH.
• 15M.2.sl.TZ1.6g: Covalent bonds form when phosphorus reacts with chlorine to form...
• 15M.2.sl.TZ2.6a.i: Draw the Lewis (electron dot) structure of chloromethane.
• 15M.2.sl.TZ2.6a.ii: Predict the shape of the chloromethane molecule and the H–C–H bond angle.   Shape:     Bond...
• 15M.2.sl.TZ2.6a.iii: Explain why chloromethane is a polar molecule.
• 14M.1.hl.TZ1.11: A solid has a melting point of 1582 °C and does not dissolve in water. It does not conduct...
• 14M.2.hl.TZ1.1d: Magnesium sulfate is one of the products formed when acid rain reacts with dolomitic limestone....
• 14M.2.hl.TZ1.5a: (i)     State the changes in the acid-base nature of the oxides across period 3 (from...
• 14M.2.hl.TZ2.4b: State the shape of the ozone molecule and estimate the bond angle.   Shape:   Bond angle:
• 14M.1.sl.TZ1.11: What is the shape and the bond angle of the molecule \({\text{B}}{{\text{F}}_{\text{3}}}\)?
• 14M.1.sl.TZ2.12: Which pair has the same bond angles? A.    ...
• 14M.1.sl.TZ2.13: Which diagram represents the bonding in \({\text{Si}}{{\text{O}}_{\text{2}}}\)?
• 14M.2.sl.TZ1.1e: (i)     State the equation for the reaction of sulfuric acid with magnesium...
• 14M.2.sl.TZ2.4c.v: Draw the Lewis (electron dot) structure of chloric(I) acid.
• 14M.2.sl.TZ2.4c.vi: Predict the H–O–Cl bond angle in this molecule and explain this in terms of the valence shell...
• 14M.3.sl.TZ1.24d: State the formula and deduce the shape of the positive ion (cation) formed when triethylamine,...
• 14N.1.hl.TZ0.13: Which group of ions and molecules has delocalized electrons in all the species? A.    ...
• 14N.2.hl.TZ0.5a: Identify the type of attraction represented by the dotted lines shown between the layers.
• 14N.2.hl.TZ0.5b: Graphite is used as a lubricant. Discuss two other uses of graphite with reference to its layered...
• 14N.1.sl.TZ0.9: Which species contains a dative covalent (coordinate) bond? A.     HCN B.    ...
• 14N.1.sl.TZ0.13: Which species contains a bond angle of approximately 107°? A.    ...
• 14N.2.sl.TZ0.3a: Explain why the distance between adjacent carbon atoms within a layer is shorter than the...
• 14N.2.sl.TZ0.3b: Graphite is used as a lubricant. Discuss two other uses of graphite with reference to its layered...
• 14N.2.sl.TZ0.6e: (i)     Deduce the Lewis structure of \({\text{PH}}_4^ + \).   (ii)     Predict, giving a...
• 13N.2.hl.TZ0.4b: State the name given to species that bond to a central metal ion, and identify the type of bond...
• 13N.2.hl.TZ0.5h: Deduce the N–N–N bond angle in trinitramide and explain your reasoning.
• 13N.2.hl.TZ0.5i: Predict, with an explanation, the polarity of the trinitramide molecule.
• 13N.2.hl.TZ0.6e.i: Compare the properties of the three oxides by completing the table below.
• 13N.2.hl.TZ0.6e.iii: As well as the oxide above, sodium forms a peroxide that contains the peroxide ion,...
• 13N.1.sl.TZ0.12: The Lewis (electron dot) structure of aspirin is represented below. What are the approximate...
• 13N.2.sl.TZ0.4e: Deduce the N–N–N bond angle in trinitramide and explain your reasoning.
• 13N.2.sl.TZ0.4f: Predict, with an explanation, the polarity of the trinitramide molecule.
• 13M.2.hl.TZ1.6c.v: Compare the melting points of \({\text{PC}}{{\text{l}}_{\text{3}}}\) and...
• 13M.1.sl.TZ1.13: Which combination best describes the type of bonding present and the melting point of silicon and...
• 13M.2.sl.TZ1.6c.i: Deduce the Lewis structures of \({\text{N}}{{\text{H}}_{\text{3}}}\) and...
• 13M.2.sl.TZ1.6c.iii: Compare the shapes of the two molecules and explain the difference using valence shell electron...
• 13M.2.sl.TZ1.6c.iv: Predict and explain whether the molecules \({\text{N}}{{\text{H}}_{\text{3}}}\) and...
• 13M.2.hl.TZ2.3b: State the type of bonding between platinum and nitrogen in carboplatin.
• 13M.2.hl.TZ2.5b.ii: State and explain the Cl–P–Cl bond angle in PCl3.
• 13M.1.sl.TZ2.11: Which statements about graphite are correct? I.     Carbon atoms are held in layers with weak...
• 13M.1.sl.TZ2.13: Which statements about the structure and bonding of silicon dioxide are correct?
• 13M.2.sl.TZ2.5b.i: Deduce the Lewis (electron dot) structure and predict the shape of each molecule, using the...
• 13M.2.sl.TZ2.5b.ii: State and explain the F–S–F bond angle in SF2.
• 13M.2.sl.TZ2.5b.iii: Deduce whether each of the three molecules is polar or non-polar, giving your reason in each...
• 12N.1.sl.TZ0.12: Diamond, C60 fullerene and graphite are allotropes of carbon. Which statements are correct about...
• 12N.1.sl.TZ0.13: Which statement about the physical properties of substances is correct? A.     The only solids...
• 12N.2.sl.TZ0.2b: (i)     Determine \(\Delta H\), the enthalpy change of the reaction, in...
• 12N.2.sl.TZ0.5b.ii: The Lewis (electron dot) structure of nitrous acid is given below. Identify which...
• 12N.2.sl.TZ0.5b.iii: Deduce the approximate value of the hydrogen-oxygen-nitrogen bond angle in nitrous acid and...
• 12N.2.sl.TZ0.5b.v: Ammonia, NH3, is a weak base. Deduce the Lewis (electron dot) structure of NH3. State the name of...
• 10N.1.hl.TZ0.12: Which molecule has an octahedral shape? A.     SF6 B.     PCl5 C.     XeF4 D.     BF3
• 10N.2.hl.TZ0.7d: The reaction between \({{\text{N}}_{\text{2}}}{{\text{H}}_{\text{4}}}{\text{(aq)}}\) and HCl(aq)...
• 10N.1.sl.TZ0.11: Which species contain a dative covalent bond? I.     HCHO II.     CO III.    ...
• 10N.2.sl.TZ0.4f: (i)     Identify the type of reaction that occurs. (ii)     Predict the value of the H–N–H bond...
• 09N.1.hl.TZ0.11: What is the bond angle in the \({{\text{H}}_{\text{3}}}{{\text{O}}^ + }\) ion? A.     104° B.  ...
• 09N.1.hl.TZ0.13: How many atoms is each carbon directly bonded to in its allotropes?
• 09N.1.sl.TZ0.11: How many non-bonding pairs of electrons are there in a nitrogen molecule? A.     0 B.   ...
• 09N.1.sl.TZ0.12: Which molecule contains a bond angle of approximately 120°? A.    ...
• 09N.2.sl.TZ0.2: PF3, SF2 and SiF4 have different shapes. Draw their Lewis structures and use the VSEPR theory to...
• 10M.2.sl.TZ1.3a.i: Draw the Lewis structure for chloroethene and predict the H–C–Cl bond angle.
• 10M.1.sl.TZ2.11: What is the shape of the ammonia molecule, \({\text{N}}{{\text{H}}_{\text{3}}}\)? A.    ...
• 10M.1.sl.TZ2.12: Which molecule is polar? A.    ...
• 10M.1.sl.TZ2.14: Which compound has a covalent macromolecular (giant covalent) structure? A.     MgO(s) B.    ...
• 10M.2.sl.TZ2.7a.ii: Deduce the Lewis structure of chloroethene and identify the formula of the repeating unit of the...
• 09M.1.hl.TZ1.11: Which molecule contains a dative covalent (coordinate) bond? A.     HCN B.    ...
• 09M.2.hl.TZ1.6c.iii: Deduce all the bond angles present in propene.
• 09M.1.sl.TZ1.14: Which is the best description of the bonding present in silicon dioxide,...
• 09M.2.sl.TZ1.6b.i: \({\text{C}}{{\text{O}}_{\text{2}}}\)
• 09M.2.sl.TZ1.6b.ii: \({\text{CO}}_3^{2 - }\)
• 09M.2.sl.TZ1.6b.iii: \({\text{BF}}_4^ - \)
• 09M.2.hl.TZ2.5b.ii: \({\text{NO}}_2^ + \)
• 09M.2.sl.TZ2.7a.iii: Describe the structure and bonding in silicon dioxide and carbon dioxide.
• 09M.2.sl.TZ2.7b.i: Draw the Lewis structure of NH3, state its shape and deduce and explain the H–N–H bond angle in...
• 11M.1.hl.TZ1.14: The Lewis structure of \({\text{S}}{{\text{O}}_{\text{2}}}\) is given below. What is the shape...
• 11M.2.hl.TZ1.6f.i: Explain the electrical conductivity of molten sodium oxide and liquid sulfur trioxide.
• 11M.1.sl.TZ1.9: What is the correct Lewis structure for hypochlorous acid, a compound containing chlorine,...
• 11M.1.sl.TZ1.11: How do the bond angles in \({\text{C}}{{\text{H}}_{\text{4}}}\),...
• 11M.2.sl.TZ1.5b.ii: sodium oxide has a higher melting point than sulfur trioxide.
• 11M.2.sl.TZ1.7c: Describe and compare three features of the structure and bonding in the three allotropes of...
• 11M.2.sl.TZ1.7d.i: Draw the Lewis structure of \({\text{C}}{{\text{O}}_{\text{2}}}\) and predict its shape and bond...
• 11M.2.sl.TZ1.7d.ii: Describe the structure and bonding in \({\text{Si}}{{\text{O}}_{\text{2}}}\).
• 11M.2.sl.TZ1.7d.iii: Explain why silicon dioxide is a solid and carbon dioxide is a gas at room temperature.
• 11M.1.sl.TZ2.10: Which molecule has a non-bonding (lone) pair of electrons on the central atom? A.    ...
• 11M.1.sl.TZ2.13: Lewis structures are represented in different ways in different parts of the world. Two ways of...
• 12M.1.hl.TZ2.9: Which species contain dative covalent bonds? I.     CO II.    ...
• 12M.1.sl.TZ2.12: The Lewis (electron dot) structure of paracetamol (acetaminophen) is: What are the approximate...
• 12M.1.sl.TZ2.13: \({{\text{C}}_{{\text{60}}}}\) fullerene consists of a simple molecular structure. Silicon...
• 12M.2.sl.TZ2.5c: Graphite is used as a lubricant and is an electrical conductor. Diamond is hard and does not...
• 12M.2.sl.TZ2.6c: (i)     When ammonium chloride, \({\text{N}}{{\text{H}}_{\text{4}}}{\text{Cl(aq)}}\), is added to...
• 11N.2.hl.TZ0.6b.i: State and explain the difference in the electrical conductivity in the liquid state of the two...
• 11N.2.hl.TZ0.8e.i: Identify the type of bond present between \({\text{B}}{{\text{F}}_{\text{3}}}\) and...
• 11N.1.sl.TZ0.10: Which row correctly describes the bonding type and melting point of carbon and carbon dioxide?
• 11N.1.sl.TZ0.12: Which is the correct Lewis structure for ethene?
• 11N.2.sl.TZ0.1c.ii: The metal oxides from the second reaction then react with silicon dioxide to form a silicate in...
• 11N.2.sl.TZ0.5c.i: For each of the species \({\text{PB}}{{\text{r}}_{\text{3}}}\) and HCHO: •     deduce the Lewis...
• 11N.2.sl.TZ0.5c.ii: Explain why \({\text{PB}}{{\text{r}}_{\text{3}}}\) is a polar molecule.
• 16M.1.sl.TZ0.11: Which compound has resonance structures? A.  C6H12 B.  CH3CHO C.  NaBr D.  Na2CO3
• 16M.2.sl.TZ0.1a: (i) Draw a Lewis (electron dot) structure of phosphine. (ii) Outline whether you expect the...
• 16M.2.sl.TZ0.1b: Phosphine is usually prepared by heating white phosphorus, one of the allotropes of phosphorus,...
• 16M.2.hl.TZ0.1a: (i) Draw a Lewis (electron dot) structure of phosphine. (ii) State the hybridization of the...
• 16M.2.hl.TZ0.3c: One of the intermediates in the reaction between nitrogen monoxide and hydrogen is dinitrogen...
• 16N.1.sl.TZ0.9: Which pair of molecules has the same bond angles?  A. PCl3 and BCl3  B. SO2 and CO2  C. H2O...
• 16N.1.sl.TZ0.12: Which substance has a giant covalent structure?
• 16N.2.sl.TZ0.2d: The Lewis (electron dot) structure of the ethanedioate ion is shown below. Outline why all the...
• 16N.2.hl.TZ0.2d: Draw the Lewis (electron dot) structure of the ethanedioate ion, –OOCCOO–.
• 16N.2.hl.TZ0.2e: Outline why all the C–O bond lengths in the ethanedioate ion are the same length and suggest a...
• 16N.3.sl.TZ0.6c: (i) Suggest why incomplete combustion of plastic, such as polyvinyl chloride, is common in...
• 17M.1.sl.TZ1.9: A substance has the following properties: What is the most probable structure of this...
• 17M.1.sl.TZ1.11: Which combination describes the sulfate(IV) ion, SO32– (also known as sulfite ion)?
• 17M.1.sl.TZ1.12: Which correctly states the strongest intermolecular forces in the compounds below?
• 17M.1.hl.TZ1.12: Which combination describes the bonding and structure in benzoic acid, C6H5COOH?
• 17M.2.sl.TZ1.4a: Estimate the H−N−H bond angle in methanamine using VSEPR theory.
• 17M.2.hl.TZ1.5b: State the electron domain geometry around the nitrogen atom and its hybridization in methanamine.  
• 17M.1.sl.TZ2.11: What are the approximate bond angles and structure of crystalline SiO2?
• 17M.2.sl.TZ2.3b: Deduce the Lewis (electron dot) structure and molecular geometry of PCl3.
• 17M.2.sl.TZ2.4b: Deduce the Lewis (electron dot) structures of ozone.
• 17M.2.hl.TZ2.4b.ii: Deduce one resonance structure of ozone and the corresponding formal charges on each oxygen atom.
• 17M.2.hl.TZ1.5a: Estimate the H−N−H bond angle in methanamine using VSEPR theory.
• 17M.2.hl.TZ1.5c: Ammonia reacts reversibly with...
• 17N.2.sl.TZ0.3a: Draw the Lewis (electron dot) structures of PF3 and PF4+ and use the VSEPR theory to deduce the...
• 17N.2.sl.TZ0.3b: Predict with a reason, whether the molecule PF3 is polar or non-polar.
• 17N.2.hl.TZ0.4a: Draw the Lewis (electron dot) structures of PF3 and PF5 and use the VSEPR theory to deduce the...
• 17N.2.hl.TZ0.4b: Predict whether the molecules PF3 and PF5 are polar or non-polar.
• 18M.2.hl.TZ1.1b: The structural formula of urea is shown. Predict the electron domain and molecular geometries...
• 18M.2.hl.TZ2.7e: Carbon and silicon are elements in group 14. Explain why CO2 is a gas but SiO2 is a solid at...
• 18M.1.sl.TZ1.10: Which form of carbon is the poorest electrical conductor? A.     Graphite B.     Graphene C. ...
• 18M.1.sl.TZ1.11: What is the molecular geometry and bond angle in the molecular ion NO3−?
• 18M.2.sl.TZ1.1b: The structural formula of urea is shown. Predict the electron domain and molecular geometries...
• 18M.1.sl.TZ2.10: Which species has the longest carbon to oxygen bond length? A.     CO B.     CH3OH C.   ...
• 18M.1.sl.TZ2.11: What are the predicted electron domain geometries around the carbon and both nitrogen atoms in...
• 18M.2.sl.TZ2.6b: Lewis structures show electron domains and are used to predict molecular geometry. Deduce the...
• 18M.3.sl.TZ2.1a.i: Graphene is two-dimensional, rather than three-dimensional, material. Justify this by using the...
• 18M.3.sl.TZ2.1a.ii: Show that graphene is over 1600 times stronger than graphite.
• 18M.3.sl.TZ2.1a.iii: Identify a value from the table which can be used to support the information about graphene given...
• 18M.3.sl.TZ2.1b: Diamond, graphene, and graphite are all network solids. Suggest, giving a reason, the electron...
• 18M.3.sl.TZ2.1c: The melting point of diamond at 1 × 106 kPa is 4200 K (in the absence of oxygen). Suggest, based...

4.4 Intermolecular forces

• 15M.1.hl.TZ2.11: Which correctly lists butane \({\text{(}}{M_{\text{r}}} = {\text{58)}}\), propanone...
• 15M.2.hl.TZ1.1c: Identify the strongest intermolecular force in solid ethanedioic acid.
• 15M.2.hl.TZ1.2b.i: Explain why the melting point of phosphorus(V) oxide is lower than that of sodium oxide in terms...
• 15M.2.hl.TZ1.2b.ii: Predict whether phosphorus(V) oxide and sodium oxide conduct electricity in their solid and...
• 15M.2.hl.TZ2.10f: Explain why but-2-ene is more volatile than compound C.
• 15M.3.hl.TZ2.28b.iii: Deduce, giving a reason, whether carotenoids are water-soluble or fat-soluble.
• 15M.1.sl.TZ1.12: Which forces are present between molecules of carbon dioxide in the solid state? A.   ...
• 15M.1.sl.TZ1.13: The following compounds have similar molar...
• 15M.2.sl.TZ1.1d: Identify the strongest intermolecular force in solid ethanedioic acid.
• 15M.2.sl.TZ1.7b: \({{\text{C}}_{\text{5}}}{{\text{H}}_{{\text{12}}}}\) exists as three isomers. Identify the...
• 15M.2.sl.TZ2.6a.iv: Methanol has a lower molar mass than chloromethane. Explain why the boiling point of methanol is...
• 15M.2.sl.TZ2.7f: Explain why but-2-ene is more volatile than compound C,...
• 14M.1.hl.TZ2.24: Which combination of properties is correct?
• 14M.2.hl.TZ1.5c: (i)     Explain why the boiling point of HF is much higher than the boiling points of the other...
• 14M.2.hl.TZ1.7b: (i)     Compare the two liquids in terms of their boiling points, enthalpies of vaporization and...
• 14M.2.hl.TZ2.1g: Propanone is used as the solvent because one compound involved in the equilibrium is insoluble in...
• 14M.2.hl.TZ2.1h: Suggest one other reason why using water as a solvent would make the experiment less successful.
• 14M.2.hl.TZ2.5b.i: Chloric(I) acid is a weak acid, but hydrochloric acid is a strong acid. Outline how this is...
• 14M.2.hl.TZ2.5b.ii: State a balanced equation for the reaction of chloric(I) acid with water.
• 14M.2.hl.TZ2.5b.iii: Outline, in terms of the equilibrium in aqueous chlorine, why it is dangerous to use an acidic...
• 14M.2.hl.TZ2.5b.iv: Suggest why a covalent molecule, such as chloric(I) acid, is readily soluble in water.
• 14M.1.sl.TZ1.12: What is the correct order of increasing boiling point? A.    ...
• 14M.2.sl.TZ1.4a: Deduce the order of increasing solubility in water of the three compounds.
• 14M.2.sl.TZ1.4b: Explain your reasoning.
• 14M.2.sl.TZ1.5c: (i)     Explain why the boiling point of HF is much higher than the boiling points of the other...
• 14M.2.sl.TZ2.1j: Propanone is used as the solvent because one compound involved in the equilibrium is insoluble in...
• 14M.2.sl.TZ2.1k: Suggest one other reason why using water as a solvent would make the experiment less successful.
• 14M.2.sl.TZ2.4c.i: Chloric(I) acid is a weak acid, but hydrochloric acid is a strong acid. Outline how this is...
• 14M.2.sl.TZ2.4c.ii: State a balanced equation for the reaction of chloric(I) acid with water.
• 14M.2.sl.TZ2.4c.iii: Outline, in terms of the equilibrium above, why it is dangerous to use an acidic toilet cleaner...
• 14M.2.sl.TZ2.4c.iv: Suggest why a covalent molecule, such as chloric(I) acid, is readily soluble in water.
• 14M.3.sl.TZ1.18c: Explain why the triglyceride formed from linoleic acid and glycerol is a liquid and not a solid...
• 14N.2.hl.TZ0.3a: A liquid boils when its vapour pressure equals atmospheric pressure. Determine the boiling point...
• 14N.2.hl.TZ0.3b: Sketch another curve on the axes above to show how the vapour pressure of a liquid that has...
• 14N.2.hl.TZ0.10b: The oxygen in half-equation 2 is atmospheric oxygen that is found dissolved in water in very...
• 14N.1.sl.TZ0.12: Which process involves the breaking of hydrogen bonds? A.    ...
• 14N.2.sl.TZ0.8b: The oxygen in half-equation 2 is atmospheric oxygen that is found dissolved in water in very...
• 13N.2.hl.TZ0.7c.ii: The interaction between an undissociated hydrogen halide molecule and a water molecule.
• 13N.2.hl.TZ0.8d: Explain why 2-methylbut-2-ene is less soluble in water than 2-methylbutan-2-ol.
• 13N.1.sl.TZ0.14: Which compound has the highest boiling point? A.    ...
• 13N.2.sl.TZ0.6d: Explain why 2-methylbut-2-ene is less soluble in water than 2-methylbutan-2-ol.
• 13M.1.sl.TZ1.14: Which statements are correct about hydrogen bonding? I.     It is an electrostatic attraction...
• 13M.1.sl.TZ2.14: Which series shows increasing boiling points? A.  ...
• 13M.2.sl.TZ2.4a: Identify the intermolecular forces present in hydrogen iodide in the liquid state, HI(l).
• 13M.2.sl.TZ2.4b.ii: State and explain which compound can form hydrogen bonds with water.
• 13M.2.sl.TZ2.4b.iii: Draw a diagram showing the resulting hydrogen bonds between water and the compound chosen in (ii).
• 13M.2.sl.TZ2.6c.v: Suggest why monomers are often gases or volatile liquids whereas polymers are solids.
• 12N.2.sl.TZ0.1b: Although the molar masses of ICl and \({\rm{B}}{{\rm{r}}_2}\) are very similar, the boiling point...
• 12N.2.sl.TZ0.4c: (i)     Explain why metals are good conductors of electricity and why they are malleable. (ii)  ...
• 10N.2.hl.TZ0.2d: (i)     Outline two reasons why the polymers of the alkenes are of economic importance. (ii)    ...
• 10N.2.hl.TZ0.7b: Hydrazine and ethene, C2H4, are hydrides of adjacent elements in the periodic table. The boiling...
• 10N.1.sl.TZ0.13: Which order is correct when the following compounds are arranged in order of increasing melting...
• 10N.2.sl.TZ0.2c: (i)     Outline two reasons why the polymers of the alkenes are of economic importance. (ii)    ...
• 10N.2.sl.TZ0.4c: The boiling point of hydrazine is much higher than that of ethene. Explain this difference in...
• 10N.2.sl.TZ0.5f: (i)     Deduce the structural formula of each isomer. (ii)     Identify the isomer from part (f)...
• 10N.3.sl.TZ0.B2c: The formula of stearic acid is also given in Table 22 of the Data Booklet. Explain why linoleic...
• 09N.1.hl.TZ0.10: What is the correct order if the compounds are arranged in order of increasing boiling point? A....
• 09N.1.sl.TZ0.13: Which compound does not form hydrogen bonds between its molecules? A.    ...
• 09N.2.sl.TZ0.4a.i: Identify the boiling points for each of the isomers A, B and C and state a reason for your answer.
• 10M.1.sl.TZ2.13: Which substance can form intermolecular hydrogen bonds in the liquid state? A.    ...
• 09M.2.sl.TZ1.1d: The reactants had to be stirred vigorously because they formed two distinct layers in the...
• 09M.2.sl.TZ1.7a.i: List the three compounds in order of increasing boiling point (lowest first) and explain the...
• 09M.2.sl.TZ1.7a.ii: Predict, with an explanation, which of the three compounds is least soluble or miscible in water.
• 09M.3.sl.TZ1.B2c.iii: Determine whether cholesterol or lecithin is more soluble in water.
• 09M.1.sl.TZ2.10: Which statement best describes the intramolecular bonding in HCN(l)? A.     Electrostatic...
• 09M.2.sl.TZ2.6a.v: Deduce and explain whether ethanol or A has the higher boiling point.
• 09M.2.sl.TZ2.7b.ii: The graph below shows the boiling points of the hydrides of group 5. Discuss the variation in the...
• 11M.1.sl.TZ1.10: Which compound forms hydrogen bonds in the liquid state? A.    ...
• 11M.2.sl.TZ1.5b.ii: sodium oxide has a higher melting point than sulfur trioxide.
• 11M.2.sl.TZ1.6a: State and explain the trend of the boiling points of the first five members of the alkene...
• 11M.2.sl.TZ1.7d.iii: Explain why silicon dioxide is a solid and carbon dioxide is a gas at room temperature.
• 11M.2.hl.TZ2.8b.iv: Explain whether the boiling point of 1-bromopentane will be higher, lower or the same as that of...
• 11M.1.sl.TZ2.8: Which change explains why the boiling points of the halogens increase as their molecular masses...
• 11M.2.sl.TZ2.4: Methoxymethane, \({\text{C}}{{\text{H}}_{\text{3}}}{\text{OC}}{{\text{H}}_{\text{3}}}\), and...
• 11M.2.sl.TZ2.5a.i: Draw the Lewis structure of ammonia and state the shape of the molecule and its bond angles.
• 11M.2.sl.TZ2.5a.ii: The conjugate acid of ammonia is the ammonium ion, \({\text{NH}}_4^ + \). Draw the Lewis...
• 12M.1.sl.TZ2.28: Which compound has the lowest boiling point? A.    ...
• 12M.2.sl.TZ2.5b: (i)     State and explain which of propan-1-ol,...
• 11N.1.hl.TZ0.24: Four identical sealed containers are prepared each containing...
• 11N.2.hl.TZ0.9b.iv: Discuss the volatility of E compared to F.
• 11N.1.sl.TZ0.11: What is the correct order of increasing boiling points? A.    ...
• 11N.2.sl.TZ0.4d: Based on the types of intermolecular force present, explain why butan-1-ol has a higher boiling...
• 11N.2.sl.TZ0.7b.iv: Discuss the volatility of Y compared to Z.
• 16M.1.sl.TZ0.12: Which of the following are van der Waals’ forces? I.  Dipole-dipole forcesII.  Hydrogen...
• 16M.2.sl.TZ0.1a: (i) Draw a Lewis (electron dot) structure of phosphine. (ii) Outline whether you expect the...
• 16M.2.hl.TZ0.1a: (i) Draw a Lewis (electron dot) structure of phosphine. (ii) State the hybridization of the...
• 16N.1.sl.TZ0.11: Between which pair of molecules can hydrogen bonding occur?  A. CH4 and H2OB. CH3OCH3 and CF4 C....
• 16N.2.sl.TZ0.1c: Explain why the boiling point of ethane-1,2-diol is significantly greater than that of ethene.
• 16N.3.sl.TZ0.8b: The table below shows average figures for the percentage fatty acid composition of some common...
• 16N.3.sl.TZ0.18b: Suggest why isolation of the crude product involved the addition of ice-cold water.
• 16N.3.sl.TZ0.18c: Justify the conclusion that recrystallization increased the purity of the product, by reference...
• 16N.3.hl.TZ0.22c: (i) Uranium hexafluoride, UF6, is used in the uranium enrichment process that produces fuel for...
• 17M.1.sl.TZ1.9: A substance has the following properties: What is the most probable structure of this...
• 17M.1.sl.TZ1.12: Which correctly states the strongest intermolecular forces in the compounds below?
• 17M.1.sl.TZ1.24: What is the order of increasing boiling point? A.     C4H10 < CH3COOH < CH3CH2CHO <...
• 17M.2.sl.TZ1.2e.ii: A chloride of titanium, TiCl4, melts at 248 K. Suggest why the melting point is so much lower...
• 17M.3.sl.TZ1.10b.ii: Explain why the difference in their structures affects their melting points.
• 17M.3.sl.TZ1.11b.i: The drain pipe of a kitchen sink can become clogged by fatty acids, such as linoleic acid,...
• 17M.3.sl.TZ1.13d: The solubility of a vitamin depends on its structure. Identify the vitamin given in section 35...
• 17M.3.sl.TZ1.19a: Suggest why aspirin is slightly soluble in water. Refer to section 37 of the data booklet.
• 17M.1.sl.TZ2.10: Which bonds cause the boiling point of water to be significantly greater than that of...
• 17M.2.sl.TZ2.4a.ii: State why hydrazine has a higher boiling point than dinitrogen tetraoxide.
• 17M.3.sl.TZ2.8a: Explain which one of these fatty acids has the highest boiling point.
• 17M.3.sl.TZ2.11: Suggest, in terms of its structure, why vitamin D is fat-soluble using section 35 of the data...
• 17M.3.sl.TZ2.16a: Explain why diamorphine passes more readily than morphine through the blood-brain barrier.
• 17N.1.sl.TZ0.11: Which of the following series shows increasing hydrogen bonding with water? A. Propane <...
• 17N.2.sl.TZ0.2b: Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group.
• 17N.2.hl.TZ0.3b: Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group whereas...
• 17N.3.sl.TZ0.7b.i: Describe how the structures of LDPE and HDPE affect one mechanical property of the plastics.
• 17N.3.sl.TZ0.9c: Explain how the inclusion of carbohydrates in plastics makes them biodegradable.
• 17N.3.sl.TZ0.10a: Explain, at the molecular level, why vitamin D is soluble in fats. Use section 35 of the data...
• 17N.3.hl.TZ0.7c: Identify the type of intermolecular bonding that is responsible for Kevlar®’s strength.
• 18M.2.hl.TZ1.1e.i: Suggest one reason why urea is a solid and ammonia a gas at room temperature.
• 18M.2.hl.TZ1.1e.ii: Sketch two different hydrogen bonding interactions between ammonia and water.
• 18M.2.hl.TZ2.7e: Carbon and silicon are elements in group 14. Explain why CO2 is a gas but SiO2 is a solid at...
• 18M.1.sl.TZ1.12: What are the strongest intermolecular forces between molecules of propanone, CH3COCH3, in the...
• 18M.2.sl.TZ1.1e.i: Suggest one reason why urea is a solid and ammonia a gas at room temperature.
• 18M.2.sl.TZ1.1e.ii: Sketch two different hydrogen bonding interactions between ammonia and water.
• 18M.3.sl.TZ1.1a.i: Part of this molecule is hydrophilic (bonds readily to water) and part hydrophobic (does not bond...
• 18M.3.sl.TZ1.1a.ii: When a small amount of palmitic acid is placed in water it disperses to form a layer on the...
• 18M.1.sl.TZ2.12: The compounds shown below have similar relative molecular masses. What is the correct order of...

4.5 Metallic bonding

• 15M.2.hl.TZ1.4c: Describe the bonding in solid copper.
• 15M.2.hl.TZ2.8a.ii: Outline the nature of the metallic bonding present in chromium.
• 15M.2.hl.TZ2.8a.iii: Explain why chromium metal is malleable.
• 15M.2.sl.TZ1.4d: Suggest two properties of copper that make it useful and economically important.
• 15M.2.sl.TZ1.4c: Describe the bonding in solid copper.
• 15M.2.sl.TZ2.6b.ii: Outline the nature of the metallic bonding present in potassium.
• 14M.1.hl.TZ1.11: A solid has a melting point of 1582 °C and does not dissolve in water. It does not conduct...
• 14M.2.hl.TZ2.8f: (i)     Describe the bonding present in magnesium metal.       (ii)     Suggest why magnesium...
• 14M.1.sl.TZ1.13: Which particles are present in the lattice of a metal? A.     Negative ions B.     Positive and...
• 14N.2.sl.TZ0.6b: Describe the bonding in magnesium.
• 13M.2.hl.TZ1.7b.i: Describe the bonding in metals and explain their malleability.
• 13M.2.sl.TZ1.3a: Compare how electric current passes through sodium and sodium chloride by completing the table...
• 13M.1.sl.TZ2.10: Which is the best description of a metallic bond? A.     Electrostatic attraction between...
• 12N.2.hl.TZ0.2b: (ii)     Cobalt is a transition metal. One common ion of cobalt is...
• 12N.1.sl.TZ0.13: Which statement about the physical properties of substances is correct? A.     The only solids...
• 10N.1.sl.TZ0.12: Which substance is made up of a lattice of positive ions and free moving electrons? A.   ...
• 10N.2.sl.TZ0.3d: Describe the bonding in iron and explain the electrical conductivity and malleability of the metal.
• 09N.1.sl.TZ0.14: Which substance does not conduct electricity? A.     Solid zinc B.     Molten zinc C.   ...
• 10M.2.sl.TZ1.1: (a)     (i)     Deduce the change in the oxidation numbers of copper and nitrogen in step...
• 09M.1.sl.TZ2.11: Which statement best describes metallic bonding? A.     Electrostatic attractions between...
• 11M.1.sl.TZ1.13: Which particles are responsible for electrical conductivity in metals? A.     Anions B.   ...
• 11M.2.sl.TZ1.5b.i: calcium has a higher melting point than potassium.
• 11M.1.sl.TZ2.14: Which particles are responsible for the conduction of electricity in molten aluminium? A.    ...
• 12M.3.sl.TZ1.C1c: Almost all iron is used in the form of an alloy. State the name of the most common type of iron...
• 12M.3.sl.TZ1.C1d: An early alloy of aluminium was Duralumin which contained small quantities of copper and...
• 12M.1.hl.TZ2.14: Zinc metal contains metallic bonding. Which is the best description of a metallic bond? A.   ...
• 12M.3.sl.TZ2.C1b: Steel is an alloy of iron, carbon and other metallic and non-metallic elements. Stainless steel...
• 11N.2.sl.TZ0.1a: Sodium azide involves ionic bonding, and metallic bonding is present in sodium. Describe ionic...
• 17M.1.sl.TZ1.9: A substance has the following properties: What is the most probable structure of this...
• 17M.2.sl.TZ1.2a: Describe the bonding in metals.
• 17M.2.sl.TZ1.2d.ii: Explain why an aluminium-titanium alloy is harder than pure aluminium.
• 17M.2.hl.TZ1.2d.ii: Suggest why the melting point of vanadium is higher than that of titanium.
• 17M.1.sl.TZ2.12: Which metal has the strongest metallic bond? A.     Li B.     Na C.     K D.     Rb
• 17N.2.sl.TZ0.2b: Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group.
• 17N.2.hl.TZ0.3b: Explain why the melting points of the group 1 metals (Li → Cs) decrease down the group whereas...
• 18M.1.hl.TZ1.11: Which metal has the strongest metallic bonding? A.     Na B.     Mg C.     Al D.     Ca
• 18M.2.hl.TZ1.2d.ii: Outline why solid calcium is a good conductor of electricity.
• 18M.2.sl.TZ1.2d.ii: Outline why solid calcium is a good conductor of electricity.