Chapter 22, Problem 22.19CP

Interpretation Introduction

(a)

Interpretation:

The element with lowest ionization energy should be located on the periodic table.

Concept introduction:

The ionization energy is defined as the minimum energy required to remove the loosely bound valence electron of a neutral gaseous atom.

Interpretation Introduction

(b)

Interpretation:

Most electronegative element should be located on the periodic table.

Concept introduction:

Electronegativity is the tendency of an atom to attract a shared pair of electrons towards itself.

Interpretation Introduction

(c)

Interpretation:

Group 4A elements with the largest atomic radius should be located on the periodic table.

Concept introduction:

Atomic radius is the distance between the center of the nucleus to the outer most shell filled with electrons. Down an element group, atomic radius tends to increase because more electrons shells are added down the group.

Interpretation Introduction

(d)

Interpretation:

Group 6A element with smallest atomic radius should be located on the periodic table.

Concept introduction:

Atomic radius is the distance between the center of the nucleus to the outer most shell filled with electrons. Down an element group, atomic radius tends to increase because more electrons shells are added down the group.

Interpretation Introduction

(e)

Interpretation:

Group 3A element that is a semiconductor should be located on the periodic table.

Concept introduction:

Semiconductors are crystalline solids which conduct electricity between a conductor and an insulator. Semiconductors are used in manufacturing diodes, transistors and ICs.

Interpretation Introduction

(f)

Interpretation:

Group 5A element that forms the strongest p bonds should be located on the periodic table.

Concept introduction:

Pi bonds are formed when two lobes of an orbital on one atom laterally overlap with two lobes of an orbital of another atom.