Chemistry 101

Chapter 9: Ionic and Covalent Bonding

1. Which of the following molecules has no net dipole moment (non-polar) ?

2. Which one of the following molecules is non-polar?

3. The electron configuration of a ground state Vanadium (V)

4. The element whose 2+ ion has a configuration of [Ar] is :

5. In which of the following bonds would P have a partial negative charge?

6. Which of the following ionic compounds does not exist?

7. How can Br acquire a noble gas electron configuration?

8. Which of the following N-bonds is most polar?

9. Which of the following atoms is smallest in size?

10. How many electrons are there in the valence shell of Br in BrO4- ?

11. Which one of the following electron configurations is considered a pseudo-noble gas configuration?

12. Which combination below will have the most negative lattice energy?

A) Low charge ions separated by large distances

B) Low charge ions separated by small distances

C) High charge ions separated by large distance

D) High charge ions separated by small distances

13. Assuming that the separation between cation and anions the lattice in nearly identical, which species would have the greatest lattice energy ?

14. Which of the following atoms or ions are isoelectronic?

15. Which of the following has the largest radius?

16. Given the following set of data:&nbsp;
Sublimation energy of Li=155 KJ/mol
first ionization energy of Li=521 KJ/mol
F-F bond dissociation energy =158 KJ/mol
Electron affinity for F=328 KJ/mol (F(g) +e —&gt; F- (g))
For the change : Li+ (g)+F- (g) —&gt; LiF (I)
ΔH= 1034KJ
Calculate ΔHf for LiF(I) (in KJ/mol )

17. Which species is more likely covalently bonded ?

Which one of the following electron configurations of Mn+2 ion?

19) Which of the following arrangement is in order of increasing size?

A) S-2 &lt; Cl- &lt; K+ &lt; Ca+2 &lt; Ga+3

B) Ga+3 &lt; Ca+2 &lt; K+ &lt;Cl- &lt; S-2

C) Ga+3 &lt; S-2 &lt; Ca+2 &lt; Cl- &lt; K+

D) Ga+3 &lt; Ca+2 &lt; S-2 &lt; Cl- &lt; K+

E) Ga+3 &lt; Ca+2 &lt; S-2 &lt; K+ &lt; Cl-

20. Among the following atoms : N,Na,P,O,S in order of increasing electronegativity

21) The polar molecule among the following is:

22. Which one of the following ions has greatest lattice
energy?

23. One of these molecules is polar :

24. Which two ions from the following have the electron configuration: [Ar]3d6
A) Ti+2 and V+3
B) Fe+2 and Co+3
C) Fe+3 and Mn+2
D) Mn+3 and Cr+2
E) Cr+3 and V+2

25. What is the standard enthalpy change for the following reaction?
3CH4(g) +403(g) → 3C02(g) + 6H20(g)
CH4(g) △H°f (KJ/mol) -74.87
03(g) △H°f (KJ/mol) +142.7
CO2(g) △H°f (KJ/mol) -393.5
H20(g) △H°f (KJ/mOl) -241.8

26. Which of the following is the best explanation for a covalent bond?

A) Positive ion attracting negative ions

B) An interaction between outer electrons

C) Electrons simultaneously attracted by more than one nucleus

D) The overlapping of two electron-filled orbitals having different energies

E) The overlapping of unoccupied orbitals of two or more atoms

28. Which of the following statements concerning lattice energy is false?

A) MgO has a larger lattice energy than NaF

B) MgO has a larger lattice energy than LiF

C) Lattice energy is often defined as the change in energy that occurs when an ionic solid is separated into isolate ions in the gas phase

D) The lattice energy for a solid with 2+ and 2- ions should be two times that for a solid with 1+ and 1- ions

29. Which of the following compounds has the most ionic bonding has the highest percentage of ionic character?

30. In which of the series of elements listed below would the elements have most nearly the same atomic radius?

31. Which pair of elements would form a covalent bond that is the least polar?

A) The triple bond in N2 has a smaller bond order and a smaller bond length than the single bond in F2

B) The triple bond in N2 has a larger bond order and a larger bond length than the single bond in a F2

C) The triple bond in N2 has larger bond order and a smaller bond length than th e single bond in F2

D) The triple bond in N2 and the single bond in F2 have the same bond order and same bond length

E) The triple bond in N2 has a smaller bond order and a larger length than single bond in F2

33. Which of the following has the shortest bond distance?

35. Which of the following represent the Lewis structure for N?
<img src="https://gateway.medhemmeh.com/downloads/66f5b13f84b3ad83e8f3d529/fns2xq4jv1"/>

35. Which of the following represent the Lewis structure for S2-?
<img src="https://gateway.medhemmeh.com/downloads/66f5b13f84b3ad83e8f3d529/vpponz1e0y"/>

36. Use Lewis theory to determine the chemical formula for the compound formed between Rb and S

37. Use Lewis theory to determine the chemical formula for the compound formed between Al and O

38. Which of the following reactions is associated with the lattice energy of CaS (ΔH°latt)?

C) Ca2⁺(aq) + S2⁻(aq) → CaS(s)

D) Ca2⁺(g) + S2⁻(g) → CaS(s)

E) CaS(s) → Ca2⁺(aq) + S2⁻(aq)

39. Place the following in order of increasing magnitude of lattice energy.
CaO &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;MgO &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;SrS

40. Place the following in order of decreasing magnitude of lattice energy.
KF &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;MgS &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;RbI

41. Choose the compound below that should have the highest melting point according to the ionic bonding model.

42. Choose the compound below that should have the lowest melting point according to the ionic bonding model.

43. In the Lewis structure of CH3OH, how many lone pairs of electrons are there?

44. In the Lewis structure of CH3OH, how many bonding pairs of electrons are there?

45. Place the following elements in order of decreasing electronegativity.
S &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;Cl &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;Se

46. Place the following elements in order of increasing electronegativity.
Sr &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;N &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;Na

47. Choose the bond below that is most polar.

48. Choose the bond below that is least polar.

49. Using periodic trends, place the following bonds in order of increasing ionic character.
S-F &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;Se-F &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;O-F

50. Using periodic trends, place the following bonds in order of decreasing ionic character.
Sb-Cl &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;P-Cl &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;As-Cl

51. Choose the best Lewis structure for CH2Cl2.
<img src="https://gateway.medhemmeh.com/downloads/66f5b13f84b3ad83e8f3d529/2gfwsklt5f"/>

52. Choose the best Lewis structure for SF4.
<img src="https://gateway.medhemmeh.com/downloads/66f5b13f84b3ad83e8f3d529/ddvq7xkdb2"/>

53. Choose the best Lewis structure for SO42⁻
<img src="https://gateway.medhemmeh.com/downloads/66f5b13f84b3ad83e8f3d529/fzyf1oxwhl"/>

54. Draw the Lewis structure for SO4 2-.How many equivalent resonance structures can be drawn?

55. Draw the best Lewis structure for CH3+1. What is the formal charge on the C?

56. How many of the following elements can form compounds with an expanded octet?
Pb &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;Kr &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;Si &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;B

57. Place the following in order of increasing bond length.
NO2⁻ &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;NO3⁻ &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;NO

58. Which of the following processes are endothermic?

E) None of the above are endothermic.

59. Use the bond energies provided to estimate ΔH°rxn for the reaction below.
XeF2 + 2 F2 → XeF6 ΔH°rxn = ?
Bond Bond Energy (kJ/mol)
Xe-F &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;147
F-F &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;159

60. Which of the following elements can form compounds with an expanded octet?

E) None of the above can form compounds with an expanded octet.