(a) What is the trend in electronegativity going from left to right in a row of the periodic table? (b) How do electronegativity values generally vary going down a column in the periodic table? (c) True or false: The most easily ionizable elements are the most electronegative.

Electronegativity generally increases as we move from left to right across a period in the periodic table. This is because the number of protons in the nucleus increases, leading to a stronger positive charge which attracts the electrons more strongly. Additionally, the atomic radius decreases as we move across a period, causing the electrons to be closer to the nucleus. The overall effect is an increase in the tendency to attract a bonding pair of electrons, resulting in a higher electronegativity value.

As we move down a column or group in the periodic table, electronegativity generally decreases. This occurs because the atomic radius increases as more energy levels are added to the electron configuration. With larger atomic radii, the electrons are farther away from the nucleus and less attracted by the positive charge of the protons. Consequently, the tendency of an atom to attract a bonding pair of electrons is weaker, leading to lower electronegativity values.

The statement "The most easily ionizable elements are the most electronegative" is false. In fact, it's quite the opposite. The most easily ionizable elements are those with low electronegativity. When an element is easily ionizable, it means that it has a low ionization energy and can readily lose electrons to form a positive ion (cation). On the other hand, highly electronegative elements have a greater tendency to attract electrons and generally do not lose electrons easily. To further support this claim, consider that the most easily ionizable elements are usually found in Group 1 (alkali metals) of the periodic table, while the most electronegative elements are found in Group 17 (halogens). So, the statement is incorrect.