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 a molecular solid. Carbon dioxide molecules ($\ce{CO2}$) are held together by London dispersion forces in the solid state.
• $\ce{I2(s)}$: Iodine molecules ($\ce{I2}$) are non - polar, and the solid is held together by London dispersion forces, so it is a molecular solid.
• Ionic solids: Composed of cations and anions held together by strong electrostatic (ionic) forces.
• $\ce{CaCl2(s)}$: It is composed of $\ce{Ca^{2 + }}$ cations and $\ce{Cl^{-}}$ anions. The electrostatic attraction between these ions forms the ionic lattice, so it is an ionic solid.
• Atomic solids: Composed of atoms held together by covalent bonds (in the case of covalent atomic solids like diamond) or metallic bonds (in the case of metallic atomic solids).
• $\ce{Ni(s)}$: Nickel is a metal. In solid nickel, atoms are held together by metallic bonds (a sea of delocalized electrons surrounding metal cations), so it is an atomic (metallic) solid.

Answer:

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