19 ccc stability and change predict whether or not the substances in the table will sublime at stp. base your predictions only on the type of bond or intermolecular force holding the solid together. will it sublime? compound type of bond or intermolecular force sublime at stp? carbon dioxide (co₂) hydrogen fluoride (hf) calcium chloride (cacl₂) naphthalene (c₁₀h₈) iodine (i₂) sodium chloride (nacl) water (h₂o)

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# Brief Explanations:
- **Carbon dioxide ($\ce{CO2}$)**:
  - Type of bond or intermolecular force: London dispersion forces (non - polar covalent molecule).
  - Sublime at STP: Yes. The weak London dispersion forces mean it can go from solid to gas at STP.
- **Hydrogen fluoride ($\ce{HF}$)**:
  - Type of bond or intermolecular force: Hydrogen bonding (polar covalent molecule).
  - Sublime at STP: No. Hydrogen bonds are stronger than London dispersion forces (but weaker than ionic or covalent bonds in solids like $CaCl_2$ and $NaCl$). At STP, it does not sublime as the hydrogen - bonded solid structure is more stable than a gaseous state at STP.
- **Calcium chloride ($\ce{CaCl2}$)**:
  - Type of bond or intermolecular force: Ionic bonds.
  - Sublime at STP: No. Ionic bonds are very strong. Ionic solids like $CaCl_2$ have high melting and boiling points. At STP,  the ionic lattice structure is too stable to convert directly to gas.
- **Naphthalene ($\ce{C10H8}$)**:
  - Type of bond or intermolecular force: London dispersion forces (non - polar covalent molecule).
  - Sublime at STP: Yes. Weak London dispersion forces allow it to sublime at STP (it is known to sublime, for example, mothballs which contain naphthalene slowly disappear as they sublime).
- **Iodine ($\ce{I2}$)**:
  - Type of bond or intermolecular force: London dispersion forces (non - polar covalent molecule).
  - Sublime at STP: Yes. The large $I_2$ molecules have enough energy at STP (due to weak London dispersion forces between non - polar $I_2$ molecules) to go from solid to gas.
- **Sodium chloride ($\ce{NaCl}$)**:
  - Type of bond or intermolecular force: Ionic bonds.
  - Sublime at STP: No. Ionic bonds are extremely strong. The ionic lattice of $NaCl$ is very stable at STP, and it will not convert directly to gas.
- **Water ($\ce{H2O}$)**:
  - Type of bond or intermolecular force: Hydrogen bonding (polar covalent molecule).
  - Sublime at STP: No. At STP ($0^{\circ}C$ and 1 atm),  ice (solid water) melts to liquid water rather than subliming. The hydrogen - bonded structure of ice is such that at STP, the solid - liquid transition (melting) is more favorable than solid - gas (sublimation) transition.

# Answer:
| Compound | Type of Bond or Intermolecular Force | Sublime at STP? |
|---|---|---|
| Carbon dioxide ($\ce{CO2}$) | London dispersion forces | Yes |
| Hydrogen fluoride ($\ce{HF}$) | Hydrogen bonding | No |
| Calcium chloride ($\ce{CaCl2}$) | Ionic bonds | No |
| Naphthalene ($\ce{C10H8}$) | London dispersion forces | Yes |
| Iodine ($\ce{I2}$) | London dispersion forces | Yes |
| Sodium chloride ($\ce{NaCl}$) | Ionic bonds | No |
| Water ($\ce{H2O}$) | Hydrogen bonding | No |

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Answer:

Compound	Type of Bond or Intermolecular Force	Sublime at STP?
Hydrogen fluoride (\(\ce{HF}\))	Hydrogen bonding	No
Calcium chloride (\(\ce{CaCl2}\))	Ionic bonds	No
Naphthalene (\(\ce{C10H8}\))	London dispersion forces	Yes
Iodine (\(\ce{I2}\))	London dispersion forces	Yes
Sodium chloride (\(\ce{NaCl}\))	Ionic bonds	No
Water (\(\ce{H2O}\))	Hydrogen bonding	No