Question

b. why is it still beneficial for chemists to understand as many periodic trends as they can?

c. propose an explanation for one of the exceptions you identified in part a. use your knowledge of atomic structure and coulombic attraction in your hypothesis.

1. rank the following elements from smallest to largest electronegativity based on the trends you have discovered thus far in the periodic table: barium (atomic number 56), bromine (atomic number 35), and iron (atomic number 26). explain your reasoning.

Explanation:

b.

Understanding periodic trends helps chemists predict chemical properties and re - activity of elements. It aids in the design of new compounds, understanding chemical reactions, and in material science for developing new materials with desired properties.

For example, in the case of electron affinity, some exceptions occur due to the stability of half - filled or fully - filled sub - shells. When adding an electron disrupts this stability, the electron affinity may be lower than expected. The Coulombic attraction between the nucleus and the incoming electron is also affected by the shielding effect of inner - shell electrons. If the shielding is not as expected based on the general trend, it can lead to exceptions.

Electronegativity increases across a period and decreases down a group. Barium is in Group 2 and Period 6, iron is in Group 8 and Period 4, and bromine is in Group 17 and Period 4. Barium is a metal with low electronegativity as metals tend to lose electrons. Iron has a moderate electronegativity. Bromine is a non - metal and has a high electronegativity.

Answer:

It helps in prediction of element properties, reaction understanding, and new - compound design.

c.