The atomic radius of elements decreases along the period but Argon has highest size among 4th period element. Why?How the IP and metallic character be correlated?
Answers
Explanation:
Atomic radius decreases from left to right and increases down the group in the periodic table. But the increase in atomic radius is more significant down the group because down the group number of shells increase in a consecutive element.
(b) The radius of an anion is larger than the parental atom. The anion is formed by a gain of electrons. The effective positive charge in the nucleus is less, so the less inward pull is experienced. Hence Br
−
has a large radius.
(c) In Na loss of the second electron takes place from a stable configuration, hence there is a huge difference between first and second ionization energies in sodium.
(d) Ionisation energy is largest for nitrogen because of its half-filled orbital and small in size.
(e) Because of the gain of more electrons, N
3−
has the largest size since gain of electrons led to decrease in effective nuclear charge.