The Ionic Model

9.Of the four compounds listed below, which one has the greatest ionic character?

10.What is the correct formula for aluminium sulfate?

11.Which of the following statements about ions and ionic compounds are true? (select all that apply)

12.Lattice enthalpy is always endothermic because energy is required to break the bonds between the ions in the lattice.

13.A sodium ion has the same electronic configuration as an argon atom.

14.Match each polyatomic ion to its correct formula and charge.

15.Place the following ionic compounds in order of increasing melting point, from lowest to highest.

16.An ionic compound has the empirical formula H₄N₂O₃. Which pair of ions is present in this compound?

17.Aluminium iodide vapour can exist as an AlI₃ molecule. How many valence electrons are in one AlI₃ molecule?

18.What are the correct formulas for the phosphate, ammonium, ethanoate and nitrate ions?

19.Which physical property of an ionic compound is correctly described?

20.Which of the following statements about ionic lattices and lattice enthalpy are correct? (select all that apply)

21.Ionic compounds are generally soluble in water because polar water molecules form ion–dipole interactions with the ions.

22.Ionic compounds conduct electricity in the solid state because the ions can move within the lattice.

23.Match each structure type to its electrical conductivity behaviour.

24.Arrange the following ionic compounds in order of increasing lattice enthalpy, from lowest to highest.

25.Which of the following is the correct name for the compound formed between copper with a 2+ charge and oxygen?

26.Metals lose electrons from their valence shell to form positively charged cations.

27.Which of the following are properties of giant ionic lattice structures? (select all that apply)

28.Place the following ionic compounds in order of increasing lattice enthalpy, from lowest to highest.

29.Which statement about the formation of ions is correct?

30.An ionic compound has the empirical formula H4N2O3. Which pair of ions is present in this compound?

31.Aluminium iodide vapour can exist as an AlI3 molecule. How many valence electrons are in one AlI3 molecule?

32.A student is given four unknown solids and records the following results. Which solid is most likely to be a giant ionic lattice?

33.The lattice dissociation enthalpy of NaCl is +790 kJ mol⁻¹. What is the enthalpy change when 3.0 moles of NaCl are completely broken down into gaseous ions?

34.A compound has the empirical formula H₄N₂O₃. Which pair of ions is present in this compound?

35.The lattice dissociation enthalpies of three compounds are: MgO +3795 kJ mol⁻¹, Na₂O +2481 kJ mol⁻¹, K₂O +2230 kJ mol⁻¹. Which statement best explains the trend?

36.Which of the following statements about ionic lattices are correct? (select all that apply)

37.A student heats a white crystalline solid. It melts at 1074 K. The molten liquid conducts electricity, but the solid does not. The solid is soluble in water, and the aqueous solution also conducts electricity. What is the most likely structure of the solid?

38.Which of the following statements about the electrical conductivity of ionic compounds are correct? (select all that apply)

39.Lattice dissociation enthalpy is defined as the enthalpy change when one mole of a solid ionic lattice is formed from its gaseous ions.

40.Match each observation with the correct conclusion about the type of structure or bonding.

41.Complete the names of the binary ionic compounds formed from the following pairs of elements.

42.The lattice dissociation enthalpy of NaCl is +790 kJ mol⁻¹. How much energy, in kJ, is required to completely break down 2 moles of NaCl into gaseous ions?

43.State the term for an ion made up of more than one type of atom, such as the ammonium ion.

44.Complete the definition of ionic bonding.

45.Complete the sentences about the properties of ionic compounds.

46.In the reaction NaCl(s) → Na⁺(g) + Cl⁻(g), the enthalpy change is +790 kJ mol⁻¹. Calculate the enthalpy change, in kJ, when 0.5 moles of NaCl are converted into gaseous ions.

47.Give the name of the binary ionic compound formed when calcium reacts with nitrogen.

48.State the noble gas that has the same electronic structure as the Mg²⁺ ion.

49.Complete the definition of lattice enthalpy.

50.Complete the naming rules for binary ionic compounds.

51.State the type of bonding in potassium chloride, which melts at 1043 K.

52.The lattice dissociation enthalpy of NaCl is +790 kJ mol⁻¹. Calculate the energy, in kJ, required to break down 2.5 moles of NaCl into gaseous ions.

53.Define ionic bonding.

54.Describe the structure and bonding in solid magnesium oxide.

55.Explain why solid magnesium chloride does not conduct electricity, but molten magnesium chloride does.

56.Explain why lattice enthalpy is always endothermic.

57.Lithium bromide dissolves in organic solvents, whereas potassium fluoride is insoluble in organic solvents. Suggest a reason for the difference in solubility.

58.The lattice dissociation enthalpy of NaCl is +790 kJ mol⁻¹. How much energy, in kJ, is required to completely break down 2 moles of NaCl into gaseous ions?

59.In the reaction NaCl(s) → Na⁺(g) + Cl⁻(g), the enthalpy change is +790 kJ mol⁻¹. Calculate the enthalpy change, in kJ, when 0.5 moles of NaCl are converted into gaseous ions.

60.The lattice dissociation enthalpy of NaCl is +790 kJ mol⁻¹. Calculate the energy, in kJ, required to break down 2.5 moles of NaCl into gaseous ions.