Decide what kind of crystalline solid each element or compound in the table forms, and what kind of force holds the solid together. Then, rank the solids in order of decreasing melting point. That is, select "1" next to the solid with the highest melting point, "2" next to the solid with the next highest melting point, and so on. (You may need to use the scrollbar to see all the choices.) element or compound CH₂ C1 Zn Kr type of solid force holding the solid formed together molecular ionic molecular dipole hydrogen-bonding ✓ dispersion X melting point of solid 2 3 (lowest) 1 (highest)

2.The heat of sublimation for carbon dioxide is 32.3 kJ/mol. Calculate the mass of solid dry ice (CO2) that would be sublimed with 200kJ of heat?    A) 128.6 g B) 184.7g C) 235.8g D) 272.4g

Match each term to the correct example. Quartz (silicon dioxide) v [Choose ] Molecular solid lonic solid Sulfur (S8) Network covalent solid Metallic solid Amorphous solid Cesium bromide salt Nonbonding atomic solid Copper [Choose ] Solid helium [Choose ]

Consider two ionic compounds containing the same anion but different cations: Compound 1 has a melting point of 801 °C, and Compound 2 has a melting point of 770 °C. Which of the following choices best predicts the likely identities of the cations in these compounds and explains the physical reason for their difference in melting point? Ion 1 Ion 2 Reasoning A) K+ Na+Potassium is larger than sodium, so the London Dispersion Forces (LDFs) in Compound 1 are stronger than they are in Compound 2. This means that more energy is required to break the LDFs, resulting in a higher melting point. B) K+ Na+Potassium is more massive than sodium, so the gravitational forces holding Compound 1 together are stronger than in Compound 2. Thus, more energy is required to break the gravitational forces, resulting in a higher melting point. C) Na+ K+Sodium is more electronegative than potassium, so the dipole-dipole forces in Compound 1 are stronger than they are in Compound 2. This means that more energy…