Web viewIB Chemistry Year 1 HL – Unit 4 Bonding (Topic 4 and 14) Problem Set. Directions:...

Nomen:____________________________________________________ Dies:________________IB Chemistry Year 1 HL – Unit 4 Bonding (Topic 4 and 14) 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 AlPD. MgSO4 and AlP

2. Which is the correct formula for iron(III) hydroxide?

A. Fe2(OH)3

B. Fe3OHC. Fe(OH)3

D. Fe3(OH

3. Which describes ionic bonding best?

A. The electrostatic attraction between nuclei and pairs of electronsB. The electrostatic attraction between positive ions and negative ionsC. The electrostatic attraction between a positive ion and an electronD. 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. MPC. M2PD. M2P3


6. What is the correct formula for an ionic compound formed between a Group 2 element, A, and a Group 16 element, B.

A. ABB. A2B6

C. AB3

D. A3B

7. Which molecule or ion contains a dative (coordinate) covalent bond?

A. CO2

B. C2H4

C. OH-

D. NH4+

8. Which substance contains both ionic and covalent bonds?

A. HCNB. NaNO3

C. MgOD. 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 arearranged 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.


12. Which molecules or ion contain a bond angle less than 109o?I. NH3

II. CCl4

III. H3O+

A. I and II onlyB. I and III only

C. II and III onlyD. I, II and III

13. Which is correct when the species NH2-, NH3 and NH4

+ are arranged in order ofincreasing H-N-H bond angle?

A. NH3 < NH4+ < NH2

-

B. NH4+ < NH3 < NH2

-C. NH2

- < NH4+ < NH3

D. NH2- < NH3 < NH4

+

14. Which molecule has a linear shape?

A. HCNB. SO2

C. H2SD. SiO2

15. What intermolecular forces are present in fluorine gas?

A. Dipole-dipole attractionsB. London (dispersion) forces

C. Covalent bondsD. Hydrogen bonds

16. Which is a non-polar molecule?

A. CCl4

B. HCNC. H2SD. SO2

17. What is the high electrical conductivity of metals due to?

A. Delocalized atomsB. Delocalized negative ions

C. Delocalized positive ionsD. 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. C2H5OHB. CH3COCH3

C. CH3COOHD. CH3COOCH3


20. Which statements accurately describe the structure of solid sodium chloride?I. It is an ionic latticeII. Each sodium ion is surrounded by six chloride ionsIII. The sodium ions are arranged octahedrally around each chloride ion



21. Which statement best describes the intramolecular bonding in ammonia?

A. Van der Waals’ forces and hydrogen bondingB. Electrostatic attraction between nuclei and shared pairs of electronsC. London dispersion forces onlyD. 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 onlyB. I and III onlyC. II and III onlyD. I, II and III

23. What is VSEPR (Valence Shell Electron Pair Repulsion theory) used for?

A. To predict the Lewis structure of a moleculeB. To show the arrangement of energy levels in a particular atomC. To deduce the shape of a molecule or simple ionD. 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

B. 120o

C. between 100o and 109o

D. 90o


25. How many bonding pairs and non-bonding pairs of electrons are around the sulfur atom in a molecule of SCl4?A 4 0B 4 1C 4 2D 8 0

26. Which molecules or ion contain a bond angle less than 109o?I. NH3

II. CCl4

III. H3O+



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. TetrahedralB. Square pyramidal

C. OctahedralD. 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 hybridizedB. The ion has a linear shapeC. There are two non-bonded pairs of electrons on the N atomD. There are double bonds between the N atom and the two O atoms


31. What is the geometry of the bonds around an atom that is sp hybridized?

A. 4 bonds at 90o

B. 4 bonds at 109.5oC. 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



33. Which contain delocalized electrons?I. COII. O3

III. CH3COO-



34. Which types of hybridization are present in but-1-yne, CH3CH2CCH?

A. sp, sp2 and sp3B. sp and sp3 only

C. sp2 and sp3 onlyD. 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 planarB. Trigonal pyramidal

C. Trigonal bipyramidalD. Pentahedral


38. Which molecule or ion has the same shape as XeF4?

A. ICl4-

B. SiCl4

C. SCl4

D. PH4+

39. Which is the smallest bond angle in the PF6- ion?

A. 180o

B. 120oC. 109.5o

D. 90o

40. What is the shape of the H3O+ ion and its approximate bond angle?

A. Tetrahedral, 104o

B. Tetrahedral 109oC. 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, 109.5oC. 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+ < NH2

-

B. NH4+ < NH3 < NH2

-C. NH2

- < NH4+ < NH3

D. NH2- < NH3 < NH4

43. Which is the best description of how bonds are formed?π

A. The axial overlap of an s and a p orbitalB. The sideways overlap of parallel p orbitalsC. The axial overlap of two p orbitalsD. 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 bonds.πC. bonds are weaker than bonds.π σD. Triple bonds are made up of two bonds and one bond.σ π

45. What is the hybridization of the N atom in NO3– and NH3 respectively?

A. sp3 and sp3B. sp2 and sp2

C. sp and sp3D. sp2 and sp3


46. Which types of hybridization are shown by the carbon atoms in ethyl ethanoate, CH3COOC2H5?

I. sp3II. sp2III. sp



47. Which substance does not contain delocalized electrons?

A. Sodium metalB. Sodium carbonate

C. Sodium iodideD. Sodium ethanoate

48. Which changes take place when water freezes?

I. The spacing between the molecules increasesII. The density decreasesIII. The average kinetic energy of the molecules increases



49. Which substance is the most volatile?A. BromineB. Iodine

C. Lithium bromideD. 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.


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.

(8) (b) (i) Compare the formation of sigma ( ) and pi ( ) bonds between the carbon σ π

atoms in a molecule of ethyne (C2H2).

(2)(ii) Identify the number of sigma and pi bonds present in trans-but-2-ene-1,4-dioic acid.

(1)


(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-but-2-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)


(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.

(2) (c) Describe the bonding within the carbon monoxide molecule.

(2) (d) Describe the delocalization of pi ( ) electrons and explain how this can account πfor the structure and stability of the carbonate ion, CO3

2–.

(3)


(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)


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.

(2) (b) For each of the carbon atoms, C1 and C2, C4 identify the type of hybridization shown.

(1) (Total 3 marks)


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

(3) (ii) NH2

–

(3) (iii) XeF4

(3)


(b) (i) Compare the formation of a sigma ( ) and a pi ( ) bond between two carbon σ πatomsin a molecule.

(2) (ii) Identify how many sigma and pi bonds are present in propene, C3H6.

(2) (iii) Deduce all the bond angles present in propene.

(2) (iv) Explain how the concept of hybridization can be used to explain the bonding in the triple bond present in propyne.



57. (a) Draw the Lewis (electron dot) structures, state the shapes, and predict the bond angles for the following species. (i) SiF6

2–

(3) (ii) NO2

+

(3) (b) Explain, using diagrams, why NO2 is a polar molecule but CO2 is a non-polar molecule.

(3) (c) Describe the structure and bonding in silicon dioxide.

(2)


(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.

(2) (iv) State the type of hybridization of the carbon and nitrogen atoms in HCONH2.


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