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Which element in Period 2 has the highest second ionisation energy?


Which one of the following is the correct order of ionic radii?

Also the electron or multi-electron takes into account the number of shielding electrons that surrounds the nucleus and greater the effective nuclear charge smaller will be the ionic radius. Hence we can say that the correct order of ionic radii will be O2−>F−>Na+>Mg2+.

Which of the following order of ionic radii is correct?

Whereas the radius of anion is always greater than a cation due to decrease in effective nuclear charge. Hence the correct order is H->H>H+. the given species are isoelectronic and they are in contact with the same number of electrons.

Which of the following is correct for ionic size?

The radius of the ion is subject to the effective nuclear charge, more the effective nuclear charge, more strongly the electrons are attracted towards the nucleus and the size of the ion decreases. Therefore the ionic radius is inversely proportional to effective nuclear charge. So, the correct answer is “Option C”.

What is the period trend for electronegativity?

On the periodic table, electronegativity generally increases as you move from left to right across a period and decreases as you move down a group. As a result, the most electronegative elements are found on the top right of the periodic table, while the least electronegative elements are found on the bottom left.

What is the relationship between atomic radius and ionization energy and electron affinity?

Moving left to right within a period or upward within a group, the first ionization energy generally increases. As the atomic radius decreases, it becomes harder to remove an electron that is closer to a more positively charged nucleus.

What is the relationship between ionization and atomic radius?

Therefore the closer the electron to the nuclear the higher the attraction force, and thus the higher the energy required to overcome this attraction and remove the electron. Therefore the smaller the radius the higher the ionization energy, and the bigger the radius the lower the energy need.