Nomen:____________________________________________________
IB Chemistry Year 1 HL – Unit 4 Bonding (Topic 4 and 14)
Dies:________________
Problem Set
Directions: Please put all answers to the multiple choice question on a scantron
sheet (available in Ms. Capasso’s room). Use pencil and do not bend scantron sheet.
Each multiple choice question is worth 1 point. For all short answer questions,
answer them directly on this paper. If you need additional room, staple loose-leaf to
the end of this problem set. All question values are given.
Multiple Choice
1. What are the correct formulas for magnesium sulfate and aluminium phosphide?
A. Mg(SO4)2 and AlPO4
B. MgSO4 and AlPO4
C. Mg(SO4)2 and AlP
D. MgSO4 and AlP
2. Which is the correct formula for iron(III) hydroxide?
A. Fe2(OH)3
B. Fe3OH
C. Fe(OH)3
D. Fe3(OH
3. Which describes ionic bonding best?
A. The electrostatic attraction between nuclei and pairs of electrons
B. The electrostatic attraction between positive ions and negative ions
C. The electrostatic attraction between a positive ion and an electron
D. The electrostatic attraction between protons and electrons
4. Which are the correct formulas for their respective ions?
5. Metal M shows only one oxidation state when it forms compounds. The formula of
the oxide of M is M2O3? Which is the correct formula for another of the compounds
M forms?
A. M3P2
B. MP
C. M2P
D. M2P3
Nomen:____________________________________________________
IB Chemistry Year 1 HL – Unit 4 Bonding (Topic 4 and 14)
Dies:________________
Problem Set
6. What is the correct formula for an ionic compound formed between a Group 2
element, A, and a Group 16 element, B.
A. AB
B. A2B6
C. AB3
D. A3B
7. Which molecule or ion contains a dative (coordinate) covalent bond?
A. CO2
B. C2H4
C. OHD. NH4+
8. Which substance contains both ionic and covalent bonds?
A. HCN
B. NaNO3
C. MgO
D. HCOOH
9. Which is the best description of the bonding present in ice?
A. Each oxygen atom is covalently bonded to four hydrogen atoms.
B. Each oxygen atom is attracted to four hydrogen atoms by hydrogen
bonding.
C. Each oxygen atom is covalently bonded to two hydrogen atoms and
attracted to two other hydrogen atoms by hydrogen bonding.
D. Each oxygen atom is covalently bonded to two hydrogen atoms and
attracted to two other hydrogen atoms by dative bonding.
10. Which is the correct order when the molecules ethane, ethene and ethyne are
arranged in order of decreasing carbon to carbon bond length?
A. C2H6 > C2H4 > C2H2
B. C2H2 > C2H4 > C2H6
C. C2H6 > C2H2 > C2H4
D C2H2 > C2H6 > C2H4
11. Which is a correct statement about the bond lengths in ethanoic acid, CH3COOH?
A. The carbon to oxygen bond length for the C-OH bond is the same as the
carbon to oxygen bond length for the C=O bond.
B. The carbon to oxygen bond length for the C-OH bond is shorter than the
carbon to oxygen bond length for the C=O bond.
C. The carbon to oxygen bond length for the C-OH bond is longer than the
carbon to oxygen bond length for the C=O bond.
D. The carbon to carbon bond length for the C-CH3 bond is the same as the
carbon to oxygen bond length for the C=O bond.
Nomen:____________________________________________________
IB Chemistry Year 1 HL – Unit 4 Bonding (Topic 4 and 14)
Dies:________________
Problem Set
12. Which molecules or ion contain a bond angle less than 109o?
I. NH3
II. CCl4
III. H3O+
A. I and II only
B. I and III only
C. II and III only
D. I, II and III
13. Which is correct when the species NH2-, NH3 and NH4+ are arranged in order of
increasing H-N-H bond angle?
A. NH3 < NH4+ < NH2B. NH4+ < NH3 < NH2-
C. NH2- < NH4+ < NH3
D. NH2- < NH3 < NH4+
14. Which molecule has a linear shape?
A. HCN
B. SO2
C. H2S
D. SiO2
15. What intermolecular forces are present in fluorine gas?
A. Dipole-dipole attractions
B. London (dispersion) forces
C. Covalent bonds
D. Hydrogen bonds
16. Which is a non-polar molecule?
A. CCl4
B. HCN
C. H2S
D. SO2
17. What is the high electrical conductivity of metals due to?
A. Delocalized atoms
B. Delocalized negative ions
C. Delocalized positive ions
D. Delocalized outer electrons
18. Why is the boiling point of HCl lower than the boiling point of HF?
A. The H-Cl bond is weaker than the H-F bond.
B. Van der Waals’ forces are weaker in HCl than in HF.
C. HF is polar whereas HCl is non-polar.
D. HF contains hydrogen bonding whereas HCl does not.
19. Which compound dissolves in water to form a solution that conducts electricity?
A. C2H5OH
B. CH3COCH3
C. CH3COOH
D. CH3COOCH3
Nomen:____________________________________________________
IB Chemistry Year 1 HL – Unit 4 Bonding (Topic 4 and 14)
Dies:________________
Problem Set
20. Which statements accurately describe the structure of solid sodium chloride?
I. It is an ionic lattice
II. Each sodium ion is surrounded by six chloride ions
III. The sodium ions are arranged octahedrally around each chloride
ion
A. I and II only
B. I and III only
C. II and III only
D. I, II and III
21. Which statement best describes the intramolecular bonding in ammonia?
A. Van der Waals’ forces and hydrogen bonding
B. Electrostatic attraction between nuclei and shared pairs of electrons
C. London dispersion forces only
D. Hydrogen bonding only
22. Which statements are correct about carbon to oxygen bond lengths?
I. The C to O bond lengths are equal in CH3COOH.
II. The C to O bond length in carbon monoxide is shorter than the C to
O bond length in carbon dioxide.
III. The C to O bond lengths in the ethanoate ion, CH3COO- , are equal.
A. I and II only
B. I and III only
C. II and III only
D. I, II and III
23. What is VSEPR (Valence Shell Electron Pair Repulsion theory) used for?
A. To predict the Lewis structure of a molecule
B. To show the arrangement of energy levels in a particular atom
C. To deduce the shape of a molecule or simple ion
D. To deduce the type of bonding in a compound
24. What is the O-N-O bond angle in the NO3- ion?
A. 109.5o
C. between 100o and 109o
B. 120o
D. 90o
Nomen:____________________________________________________
IB Chemistry Year 1 HL – Unit 4 Bonding (Topic 4 and 14)
Dies:________________
Problem Set
25. How many bonding pairs and non-bonding pairs of electrons are around the
sulfur atom in a molecule of SCl4?
A
4
0
B
4
1
C
4
2
D
8
0
26. Which molecules or ion contain a bond angle less than 109o?
I. NH3
II. CCl4
III. H3O+
A. I and II only
B. I and III only
C. II and III only
D. I, II and III
27. Which shows the increasing order of oxygen to oxygen bond lengths in oxygen,
ozone and hydrogen peroxide?
A. O2 < O3 < H2O2
B. O3 < O2 < H2O2
C. H2O2 < O2 < O3
D. O3 < H2O2 < O2
28. What is the shape of the ICl4- ion?
A. Tetrahedral
B. Square pyramidal
C. Octahedral
D. Square planar
29. Which combination shows the number of non-bonded electron pairs in the
Lewis structure, the shape of the molecule and the type of hybridization present in a
molecule of dichloromethane, CH2Cl2?
30. Which is a correct statement about the NO2- ion?
A. The N atom is sp2 hybridized
B. The ion has a linear shape
C. There are two non-bonded pairs of electrons on the N atom
D. There are double bonds between the N atom and the two O atoms
Nomen:____________________________________________________
IB Chemistry Year 1 HL – Unit 4 Bonding (Topic 4 and 14)
Dies:________________
Problem Set
31. What is the geometry of the bonds around an atom that is sp hybridized?
A. 4 bonds at 90o
B. 4 bonds at 109.5o
C. 3 bonds at 120o
D. 2 bonds at 180o
32. Which types of hybridization are shown by the carbon atoms in propene?
I. sp3
II. sp2
III. sp
A. I and II only
B. I and III only
C. II and III only
D. I, II and III
33. Which contain delocalized electrons?
I. CO
II. O3
III. CH3COOA. I and II only
B. I and III only
C. II and III only
D. I, II and III
34. Which types of hybridization are present in but-1-yne, CH3CH2CCH?
A. sp, sp2 and sp3
B. sp and sp3 only
C. sp2 and sp3 only
D. sp and sp2 only
35. Which will not conduct electricity?
A. Hg(l)
B. NaCl(s)
C. PbBr2(l)
D. HCl(aq)
36. Which is most likely to result in the formation of an ionic bond?
A. When two highly electronegative elements react together.
B. When a highly electronegative element reacts with a group 2 element.
C. When a group 16 element reacts with a group 17 element.
D. When hydrogen reacts with a group 17 element.
37. What is the shape of PCl5?
A. Square planar
B. Trigonal pyramidal
C. Trigonal bipyramidal
D. Pentahedral
Nomen:____________________________________________________
IB Chemistry Year 1 HL – Unit 4 Bonding (Topic 4 and 14)
Dies:________________
Problem Set
38. Which molecule or ion has the same shape as XeF4?
A. ICl4B. SiCl4
C. SCl4
D. PH4+
39. Which is the smallest bond angle in the PF6- ion?
A. 180o
B. 120o
C. 109.5o
D. 90o
40. What is the shape of the H3O+ ion and its approximate bond angle?
A. Tetrahedral, 104o
B. Tetrahedral 109o
C. Trigonal pyramidal, 104o
D. Trigonal planar, 120o
41. What are the molecular geometry and the F-Br-F bond angle in the BrF3
molecule?
A. Trigonal pyramid, 107o
B. Trigonal planar, 109.5o
C. Trigonal planar, 120o
D. T-shaped, 86o
42. Which is correct when the species NH2-, NH3 and NH4+ are arranged in order of
increasing H-N-H bond angle?
A. NH3 < NH4+ < NH2B. NH4+ < NH3 < NH2-
C. NH2- < NH4+ < NH3
D. NH2- < NH3 < NH4
43. Which is the best description of how π bonds are formed?
A. The axial overlap of an s and a p orbital
B. The sideways overlap of parallel p orbitals
C. The axial overlap of two p orbitals
D. The sideways overlap of an s and a p orbital
44. Which is correct concerning the bonding between two carbon atoms?
A. Double bonds are formed when the two carbon atoms are sp3 hybridized.
B. Double bonds are caused by the overlap of two π bonds.
C. π bonds are weaker than σ bonds.
D. Triple bonds are made up of two σ bonds and one π bond.
45. What is the hybridization of the N atom in NO3– and NH3 respectively?
A. sp3 and sp3
B. sp2 and sp2
C. sp and sp3
D. sp2 and sp3
Nomen:____________________________________________________
IB Chemistry Year 1 HL – Unit 4 Bonding (Topic 4 and 14)
Dies:________________
Problem Set
46. Which types of hybridization are shown by the carbon atoms in ethyl ethanoate,
CH3COOC2H5?
I. sp3
II. sp2
III. sp
A. I and II only
B. I and III only
C. II and III only
D. I, II and III
47. Which substance does not contain delocalized electrons?
A. Sodium metal
B. Sodium carbonate
C. Sodium iodide
D. Sodium ethanoate
48. Which changes take place when water freezes?
I. The spacing between the molecules increases
II. The density decreases
III. The average kinetic energy of the molecules increases
A. I and II only
B. I and III only
49. Which substance is the most volatile?
A. Bromine
B. Iodine
C. II and III only
D. I, II and III
C. Lithium bromide
D. Lithium iodide
50. Which describes metallic bonding best?
A. Positively charged metal ions are attracted to negatively charged ions.
B. Negatively charged metal ions are attracted to positive ions.
C. Negatively charged metal ions are attracted to delocalized electrons.
D. Positively charged metal ions are attracted to delocalized electrons.
Nomen:____________________________________________________
IB Chemistry Year 1 HL – Unit 4 Bonding (Topic 4 and 14)
Dies:________________
Problem Set
Short Answer
51. (a) For each of the species PBr3 and SF6:
(i) Deduce the Lewis (electron dot) structure (ii) Predict the shape and bond angle. (iii) Predict and explain the molecular polarity.
(b)
(8) (i) Compare the formation of sigma (σ) and pi (π) bonds between the carbon
atoms in a molecule of ethyne (C2H2).
(2)
(ii) Identify the number of sigma and pi bonds present in trans-but-2-ene1,4-dioic acid.
(1)
Nomen:____________________________________________________
IB Chemistry Year 1 HL – Unit 4 Bonding (Topic 4 and 14)
Dies:________________
Problem Set
(iii) Explain why the melting point of trans-but-2-ene-1,4-dioic acid is higher
than that of cis-but-2-ene-1,4-dioic acid.
(1)
(iv) Explain why cis-but-2-ene-1,4-dioic acid forms cis-but-2-ene-1,4-dioic
anhydride when heated, whereas no cyclic anhydride forms when trans-but2-ene-1,4-dioic acid is heated.
(1)
c) Deduce the hybridization of each oxygen atom in cis-but-2-ene-1,4-dioic acid.
(1)
(Total 14 marks)
52. Carbon and silicon belong to the same group of the periodic table.
(a) Describe and compare three features of the structure and bonding in the
three allotropes of carbon: diamond, graphite, and C60 fullerene.
(6) Nomen:____________________________________________________
IB Chemistry Year 1 HL – Unit 4 Bonding (Topic 4 and 14)
Dies:________________
Problem Set
(b) Both silicon and carbon form oxides. (i) Describe the structure and bonding in SiO2.
(2)
(ii) Explain why silicon dioxide is a solid and carbon dioxide is a gas at room
temperature.
(c) Describe the bonding within the carbon monoxide molecule.
(2)
(2)
(d) Describe the delocalization of pi (π) electrons and explain how this can account
for the structure and stability of the carbonate ion, CO32–.
(3) Nomen:____________________________________________________
IB Chemistry Year 1 HL – Unit 4 Bonding (Topic 4 and 14)
Dies:________________
Problem Set
(e) Explain the meaning of the term hybridization. State the type of hybridization
shown by the carbon atoms in carbon dioxide, diamond, graphite, and the
carbonate ion.
(5) (Total 20 marks)
53. Methoxymethane, CH3OCH3, and ethanol, C2H5OH, have the same relative
molecular mass. Explain why methoxymethane has a much lower boiling point than
ethanol.
(Total 3 marks)
Nomen:____________________________________________________
IB Chemistry Year 1 HL – Unit 4 Bonding (Topic 4 and 14)
Dies:________________
Problem Set
54. But-2-ene is a straight-chain alkene with formula C4H8. The molecule contains
both sigma and pi bonds.
(a) Explain the formation of the pi bond.
(b) For each of the carbon atoms, C1 and C2, C4 identify the type of hybridization
shown.
(2)
(1)
(Total 3 marks)
Nomen:____________________________________________________
IB Chemistry Year 1 HL – Unit 4 Bonding (Topic 4 and 14)
Dies:________________
Problem Set
55. SF2, SF4 and SF6 have different shapes. Draw their Lewis (electron dot)
structures and use the VSEPR theory to predict the name of the shape of each
molecule.
(Total 6 marks) 56. (a) Draw the Lewis (electron dot) structures, state the shape, and predict the
bond angles for the following species. (i) PCl3
(ii) NH2–
(iii) XeF4
(3)
(3)
(3) Nomen:____________________________________________________
IB Chemistry Year 1 HL – Unit 4 Bonding (Topic 4 and 14)
Dies:________________
Problem Set
(b) (i) Compare the formation of a sigma (σ) and a pi (π) bond between two carbon
atoms
in a molecule.
(ii) Identify how many sigma and pi bonds are present in propene, C3H6.
(iii) Deduce all the bond angles present in propene.
(2)
(2)
(2) (iv) Explain how the concept of hybridization can be used to explain the bonding in
the triple bond present in propyne.
(3)
(Total 18 marks)
Nomen:____________________________________________________
IB Chemistry Year 1 HL – Unit 4 Bonding (Topic 4 and 14)
Dies:________________
Problem Set
57. (a) Draw the Lewis (electron dot) structures, state the shapes, and predict the
bond angles for the following species.
(i) SiF62–
(3)
(ii)
NO2+
(b) Explain, using diagrams, why NO2 is a polar molecule but CO2 is a non-polar
molecule.
(3)
(3)
(c) Describe the structure and bonding in silicon dioxide.
(2)
Nomen:____________________________________________________
IB Chemistry Year 1 HL – Unit 4 Bonding (Topic 4 and 14)
Dies:________________
Problem Set
(d) Consider the molecule HCONH2.
(i) State the name of the compound and draw its structural formula, showing
all the bonds present.
(2) (ii) Explain the term hybridization.
(1) (iii) Describe how sigma and pi bonds form.
(iv) State the type of hybridization of the carbon and nitrogen atoms in
HCONH2.
(2) (2) (Total 18 marks)