Chapter U1.24, Problem 3E

Interpretation Introduction

Interpretation:

The relation between the arrangements of electrons in an atom with the location of the atom on the periodic table is to be described.

Concept introduction:

A periodic table can be divided into four zones, s block, p block, d block and f block. The element belonging to a particular block will have its outermost electron in that particular subshell. For example, in the case of s block elements, the outermost electrons will occupy the subshell. Elements in p block will have its outermost electrons in p subshell.

Explanation of Solution

Electrons revolve around the nucleus in orbits. These orbits are called shells. The shells are numbered as n = 1, 2, 3, 4, and so on. In an atom, the number of shells depends on the period number in the periodic table. A periodic table can be divided into four zones, s block, p block, d block and f block. Elements belong to one of these four zones.

Any element located in the s block will have its outermost electron(s) in s subshell. On moving across the periodic table from one element to the next, one additional proton and one additional electron are added, along with one or more neutrons. Each additional electron goes into a specific subshell. If an atom is located in the p block of the table, the last electron is placed into a p subshell. If an atom is located in the d block of the table, the last electron is placed into a d subshell and so on.

The element belonging to a particular block will have its outermost electron in that particular subshell.

The elements in each block have related properties. The elements in the s-block are reactive metals. The elements in the d-block tend to form colorful compounds that are used as pigments. The elements in the p-block form colorless compounds.

Conclusion

By knowing the position of an element on a periodic table, one can predict the arrangement of electrons. The periodic table provides the information needed to write electronic configurations.