Question

missed this? read section 12.7. you can click on the review link to access the section in your etext

part a

identify each of the following solids as molecular, ionic, or atomic.
sort these solids into the proper categories.

co₂(s) ni(s) i₂(s) cacl₂(s)

molecular ionic atomic

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Explanation:

• Molecular solids: Composed of molecules held together by relatively weak intermolecular forces (such as London dispersion forces, dipole - dipole forces, or hydrogen bonds).
• $\ce{CO2(s)}$ (dry ice) is composed of $\ce{CO2}$ molecules. The solid is held together by London dispersion forces between the non - polar $\ce{CO2}$ molecules.
• $\ce{I2(s)}$ is composed of $\ce{I2}$ molecules. The solid iodine is held together by London dispersion forces between the non - polar $\ce{I2}$ molecules.
• Ionic solids: Composed of cations and anions held together by strong ionic bonds (electrostatic attractions between oppositely charged ions).
• $\ce{CaCl2(s)}$ is composed of $\ce{Ca^{2 + }}$ cations and $\ce{Cl^{-}}$ anions. The ions are held together by ionic bonds.
• Atomic solids: Composed of atoms held together by covalent bonds (in the case of network covalent solids like diamond) or metallic bonds (in the case of metals).
• $\ce{Ni(s)}$ is a metal. In solid nickel, the nickel atoms are held together by metallic bonds (a sea of delocalized electrons surrounding the metal cations).

Answer:

• Molecular: $\ce{CO2(s)}$, $\ce{I2(s)}$
• Ionic: $\ce{CaCl2(s)}$
• Atomic: $\ce{Ni(s)}$