EVERYDAY SCIENCE

Detailed explanation-1: -On the periodic table, first ionization energy generally increases as you move left to right across a period. This is due to increasing nuclear charge, which results in the outermost electron being more strongly bound to the nucleus.

Detailed explanation-2: -The ionization energy decreases from top to bottom in groups, and increases from left to right across a period.

Detailed explanation-3: -Ionization energy increases left to right across a period. WHY? As you go down a group, the valence electrons are farther away from the nucleus, and so it takes less energy to pull them away from the atom. The more electrons in the outside energy level, the less eager an atom will be to lose an electron.

Detailed explanation-4: -On the periodic table, first ionization energy generally decreases as you move down a group. This is because the outermost electron is, on average, farther from the nucleus, meaning it is held less tightly and requires less energy to remove.

Detailed explanation-5: -As the effective nuclear charge increases the electrons are strongly attracted and hence more energy is needed to remove them, hence IE is higher. Thus answer is option D.