Boiling points periodic trends

Periodic trends in the boiling points of binary hydrogen compounds. Notice that H2O L HF, and NH3 are exceptions to the trends. 

Research one of the most recently discovered elements. New elements are created in particle accelerators and tend to be very unstable. Because of this, many of the properties of a new element cannot be determined. Using periodic group trends in melting and boiling point, predict whether the new element you selected is likely to be a solid, liquid, or gas. 

Use the data from Table 15.7 to plot the normal boiling points of the hydrogen halides against the period number of the halogens. Account for the trend revealed by the graph. 

Examine the trends for boiling points, atomic radii, and ionization energies using the Interactive Periodic Table (eChapter 20.2). Explain the factors that account for each of these trends. 

For example, hydrogen chloride, also known as hydrochloric acid, has a low melting point and a low boiling point. (It is a gas at room temperature.) These properties might lead you to believe that hydrogen chloride is a covalent compound. Hydrogen chloride, however, is extremely soluble in water, and the water solution conducts electricity. These properties are characteristic of an ionic compound. Is there a clear, theoretical way to decide whether the bond between hydrogen and chlorine is ionic or covalent The answer lies in a periodic trend. 

Describe periodic trends in ionic size, electron affinity, and melting and boiling points, and relate them to the atomic structures of the elements. 

As you move across Period 6, the periodic trend for melting and boiling points goes through two cycles of first increasing, reaching a peak, and then decreasing. 

Explain how the trends in melting and boiling points differ from the other periodic trends. 

Classify the solid states in terms of crystal types of the elements in the third period of the periodic table. Predict the trends in their melting points and boiling points. 

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