(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 is the tendency of an atom to attract a bonding pair of electrons towards itself. As we move from left to right across a period in the periodic table, the number of protons in the nucleus increases, so the positive charge of the nucleus increases. Due to this increase in nuclear charge, the valence electrons are attracted more toward the nucleus and this leads to an increase in electronegativity. Hence, the trend in electronegativity from left to right in a row is that it increases.

When we go down a group or column in the periodic table, the number of electron shells increases. This results in an increased shielding effect, where the inner electron shells shield the outer valence electrons from the nucleus's positive charge. Due to this shielding effect, the attraction of valence electrons towards the nucleus decreases, and hence the electronegativity decreases. So, the electronegativity values generally decrease going down a column in the periodic table.

Ionization energy is the amount of energy required to remove an electron from a neutral atom in its gaseous state. An element with high ionization energy requires more energy to remove an electron, indicating that the electron is held more tightly by the atom, and hence the atom has a higher tendency to attract electrons. On the other hand, elements with lower ionization energy can easily lose electrons. Electronegativity is the ability of an atom to attract electrons towards itself in a chemical bond. Elements with high electronegativity have a stronger pull on electrons in a chemical bond due to their high effective nuclear charge. Statement (c) says: "The most easily ionizable elements are the most electronegative." This statement is false. Since elements with higher ionization energy have a stronger pull on electrons, they are more electronegative. In contrast, more easily ionizable elements, which have lower ionization energy, are less electronegative.