2.3 Structure of Ionic Solids

Open Ended

What's wrong with this students diagram?

Multiple Choice

Arrange the ionic compounds NaF, CsI, and CaO in order of increasing lattice energy.

• NaF>CaO>CsI

• NaF>CsI>CaO

• CaO>NaF>CsI

• CaO>CsI>NaF

Multiple Choice

Which of the images below best represents an ionic compound like NaCl dissolved in water?

• A

• B

• C

• D

Multiple Choice

Which of the following correctly indicates whether the solid represented by the particulate model shown to the left conducts electricity and explains why or why not?

• It conducts electricity because it is made of positive and negative ions.

• It conducts electricity because it is made of particles of different sizes.

• It does not conduct electricity because its ions cannot move freely within the solid.

• It does not conduct electricity because there are small spaces between the particles.

Multiple Choice

The particle-level diagram above represents the structure of solid  KF . Although the molar mass of  KCl  is greater than that of  KF , the density of  KCl  is actually less than that of  KF . Which of the following representations of the structure of  KCl  best helps to explain this phenomenon?

Multiple Choice

The energy required to dissociate an ionic solid into gaseous ions (lattice energy) for the compounds  NaF  and  MgF₂  is shown in the table above. On the basis of Coulomb’s law, which of the following best helps to explain the large difference between the lattice energies of  NaF  and  MgF₂  ?

• The solubility of  MgF₂ is less than that of  NaF .

• The electronegativity of  Mg  is greater than that of  Na.

• The mass of the  Mg  cation is greater than that of the  Na  cation.

• The charge of the  Mg  cation is larger than that of the  Na  cation.