Chapter 4, Problem 4.129CQ

Interpretation Introduction

Interpretation:

“Consider three elements with the following abbreviated electron configuration:

$X=[Ar]4s^2$ $Y=[Ne]3s^{2}3p^4$

$Z=[Ar]4s^{2}3d^{10}4s^4$

a. Identity each element as a metal, a non-metal or a metalloid.

b. Which element ha the largest atomic size.

c. Which elements have similar properties?

d. Which element has the highest ionization energy?

e. Which element has the smallest atomic size? should be explained

Concept introduction:

► The arrangement of electrons in an atom by a superscript, in each sublevel is known as electron configuration. For example the d block elements have $(n-1)d^{1-10}n{s}^{0-2}$ electronic configuration.

► Ionization energy is the energy required to remove an electron from a gaseous atom or ion. Generally as we go across a period from left to right, the first ionization energy increases, on the other hand first ionization energy decrease in going down a group.

► Atomic radius decreases in going from left to right across a period. This decrease can be explained in term of the increasing effective nuclear charge in going from left to right. This means that the valence electrons are closer to the nucleus, decreasing the size of atom. Atomic radius increases down a group, because of the increases in the orbital sizes in successive principal quantum levels.