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    Colligative Properties/Phase Diagrams/Intermolecular Forces

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    Diagram and explain the H-Bonds if they exist for the following molecules:
    (a.)H2S, (b.)CH4, (c.)H2SO3, and (d) PH3.

    Give reasons for the fact that ionic solids as NaCl have high melting points and dissolve readily in water, whereas network solids such as diamond have very high melting points and do not dissolve in water.

    Determine the Osmotic Pressure for the following aqueous solutions @ 25 degrees Celsius. (a.) 1.0. M Glucose, and (b.)1.0 M NaCl. Explain which solution has the greater osmotic pressure if any and why.

    Determine the effect on the freezing point and boiling point of the solvent for both solutions described in question number three above.

    Describe what happens, draw a phase diagram, energy diagram, and give the energy for each change and the total energy s Carbon Dioxide is transformed from 2 atm. and a temperature of -155 degrees celsius to 1.0 atm. and a temperature of 45 degrees celsius.

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    https://brainmass.com/chemistry/physical-chemistry/colligative-properties-phase-diagrams-intermolecular-forces-148646

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    Diagram and explain the H-Bonds if they exist for the following molecules:
    (a)H2S, (b)CH4, (c)H2SO3, and (d) PH3.

    Hydrogen bonds form only when there are O-H, N-H or F-H bonds present. This kind of bond is just a special case of dipole-dipole interaction, but the high electronegativity of O, N and F make these bonds more polar, which makes the interactions stronger. The only one capable of hydrogen bonding is (c). None of the others contain O-H, N-H or F-H bonds.

    In the diagram above, the + and - represent "partial charges". These are formed due to the polarity of the bond. As a general rule, place the - on the more electronegative of the two atoms in the bond. This is an indication that the electron density in the bond is pulled closer to the electronegative atom. Note how the hydrogen bonding interaction can occur with single-bond-O and double-bond-O.

    Give reasons for the fact that ionic solids as NaCl have high melting points and dissolve readily in water, whereas network solids such as diamond have very high melting points and do not dissolve in water.

    NaCl is an ionic compound. It can be written as Na+Cl-. It actually exists in a lattice with each atom being ...

    Solution Summary

    The expert examines colligative properties, phase diagrams and intermolcular forces.

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