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Semester Two Presentation Problems Set Three Period 3-AP CHEM
Transcript of Semester Two Presentation Problems Set Three Period 3-AP CHEM
Set Three 1A 1B All of these compounds form Hydrogen bonds. These intermolecular forces form a strong barrier across a surface when these molecules bond to other molecules of the same kind. The strong H-bonds that form between these molecules enhance the strength of the surface tension. 2A 2B 282 torr x (1 atm/760 torr) = 0.371 atm Xe (s) must be more dense than Xe (l) because at low temperatures and high pressures, particles have less room to move around which leads to a higher amount of collisions and therefore a higher pressure in the solid, making it more dense. 2C 100 torr x (1 atm/760 torr) = 0.132 atm Xe (g) would undergo decomposition, because at 0.132 atm, the only phase change possible is from solid to gas. All temperatures past the triple point leave Xe in the gas phase, and all those before can either exist as a solid or gas, leaving decomposition as the phase change possible instead of condensation. Perovskite Chemical Formula: CaTiO3 Why?? There are 8 Ca, each with 1/8 of the atom touching another molecule, so really there is only one 1/8 Ca touching the same molecule, and there are 8 Ca in one unit cell, so there is one Ca per molecule. Then there are 6 O, each with 1/2 touching the adjacent molecules, so similarly, there are really only 3 O touching the same molecule. The Ti is exclusive to each molecule so there is just one per molecule. Thus, the chemical formula is CaTiO3 Compound
CH3CH2CH2OH Heat of Vaporization
47.3 4A As molar mass increases, ∆Hvap increases. This is because molecules with a higher molar mass contain more electrons and intermolecular forces. This requires more energy to break the bonds. CH3CH2CH3
MM: 44.08 g/mol
∆Hvap: 19.0 CH3CHBrCH3
MM: 122.97 g/mol
∆Hvap: 31.8 4B As the molecular structure becomes more complex, more bonds are created, requiring more energy to break them all.
CH3CH2CH2CH2CH3 <---- has more bonds to break than CH3CH2CH3 4C As molecules become more polar, the heat of vaporization increases. Dipole-Dipole forces are stronger than London Dispersion forces because they have stronger intermolecular forces. Therefore, polar molecules are stronger than non-polar molecules. Stronger bonds -> harder to break them -> high ∆Hvap CH3CH2CH2Br has strong Dipole-Dipole forces 4D Molecules that have hydrogen bonding have very strong intermolecular forces. This requires more energy to break the bond which increases the heat of vaporization. CH3CH2CH2OH <- has a strong O-H bond. Oxygen is highly electronegative and creates a highly polar covalent bond.