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Chapter 10: Q10.3CYL (page 528)

Ethane \(\left( {{\rm{C}}{{\rm{H}}_3}{\rm{C}}{{\rm{H}}_3}} \right)\) has a melting point of -1830C and a boiling point of -890C. Predict the melting and boiling points for methylamine \(\left( {{\rm{C}}{{\rm{H}}_3}{\rm{N}}{{\rm{H}}_2}} \right)\). Explain your reasoning.

Short Answer

Expert verified

Ethane is a non-polar molecule, therefore, only weak van der waals force of attraction are present.

Step by step solution

01

Define polarizability

A molecule that has a charge cloud that is easily distorted is said to be very polarizable and will have large dispersion forces; one with a charge cloud that is difficult to distort is not very polarizable and will have small dispersion forces.

02

 Identify the melting and boiling point of methylamine

Both the melting point and boiling point of methylamine will be more than that of ethane as hydrogen bonds are present in its molecules Therefore, more energy is required to break the bonds and hence, the melting and boiling point will be more. On the other hand, ethane is a non-polar molecule, therefore, only weak van der waals force of attraction are present.

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Most popular questions from this chapter

Which contains the compounds listed correctly in order of increasing boiling points

\(\begin{aligned}{\rm{(a)}}{{\rm{N}}_{\rm{2}}}{\rm{ < C}}{{\rm{S}}_{\rm{2}}}{\rm{ < }}{{\rm{H}}_{\rm{2}}}{\rm{O < KCl}}\\{\rm{(b)}}{{\rm{H}}_{\rm{2}}}{\rm{O < }}{{\rm{N}}_{\rm{2}}}{\rm{ < C}}{{\rm{S}}_{\rm{2}}}{\rm{ < KCl}}\\{\rm{(c)}}{{\rm{N}}_{\rm{2}}}{\rm{ < KCl < C}}{{\rm{S}}_{\rm{2}}}{\rm{ < }}{{\rm{H}}_{\rm{2}}}{\rm{O}}\\{\rm{(d)C}}{{\rm{S}}_{\rm{2}}}{\rm{ < }}{{\rm{N}}_{\rm{2}}}{\rm{ < KCl < }}{{\rm{H}}_{\rm{2}}}{\rm{O}}\\{\rm{(e)KCl < }}{{\rm{H}}_{\rm{2}}}{\rm{O < C}}{{\rm{S}}_{\rm{2}}}{\rm{ < }}{{\rm{N}}_{\rm{2}}}\end{aligned}\)

The surface tension and viscosity values for diethyl ether, acetone, ethanol, and ethylene glycol are shown here

(a) Explain their differences in viscosity in terms of the size and shape of their molecules and their IMFs.

(b) Explain their differences in surface tension in terms of the size and shape of their molecules and their IMFs:

For acetone (CH3)2CO, the normal boiling point is 56.5 °C and the enthalpy of vaporization is 31.3 kJ/mol.What is the vapor pressure of acetone at 25.0°C?

Substance B is hard, does not conduct electricity, and melts at\({\rm{1200 ^\circ C}}\). Substance B is likely a(n): (a) ionic solid (b) metallic solid (c) molecular solid (d) covalent network solid

Open the PhET States of Matter Simulation (http://openstaxcollege.org/l/16phetvisual) to answer the following questions:

(a) Select the Solid, Liquid, Gas tab. Explore by selecting different substances, heating and cooling the systems, and changing the state. What similarities do you notice between the four substances for each phase (solid, liquid, gas)? What differences do you notice?

(b) For each substance, select each of the states and record the given temperatures. How do the given temperatures for each state correlate with the strengths of their intermolecular attractions? Explain.

(c) Select the Interaction Potential tab, and use the default neon atoms. Move the Ne atom to the right and observe how the potential energy changes. Select the Total Force button, and move the Ne atom as before. When is the total force on each atom attractive and large enough to matter? Then select the Component Forces button, and move the Ne atom. When do the attractive (van der Waals) and repulsive (electron overlap) forces balance? How does this relate to the potential energy versus the distance between atoms graph? Explain.
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