Question

State the forces operating between the units or molecule in the solid state of each of the following compounds and indicate how the forces are:

b. SiO₂

a. CO₂

c. NaCl

a. London dispersion forces
b. Covalent bonds
c. Ionic bonds
d. Hydrogen bonds

Answer 1

Solid CO₂ is held together by London dispersion forces, SiO₂ by strong covalent bonds in a network solid, and NaCl is an ionic solid held together by ionic bonds.

Step-by-step explanation:

The forces operating between the units or molecules in the solid state of CO₂ (carbon dioxide), SiO₂ (silicon dioxide), and NaCl (sodium chloride) vary due to their different structures and bonding types:

• CO₂ (carbon dioxide) in solid form, known as dry ice, is held together by London dispersion forces, which are weak intermolecular forces that arise from temporary fluctuations in electron distribution leading to temporary dipoles.
• SiO₂ (silicon dioxide) in the solid state is a network covalent solid where atoms are held together in a rigid lattice structure by strong covalent bonds. This gives SiO₂ very high melting and boiling points.
• NaCl (sodium chloride) is an ionic solid with a crystal lattice structure. The forces holding NaCl together are ionic bonds, which are strong electrostatic attractions between positively and negatively charged ions.