Chapter 13, Problem 1DQ

Explain the electronegativity trends across a row anddown a column of the periodic table. Compare thesetrends with those of ionization energy and atomic radii.How are they all related?

Interpretation Introduction

Interpretation:

The trend of electronegativity across a row and down a column of the periodic table should be explained. These trends should be compared with ionization energy and atomic radii. The relation between all these properties should be stated.

Concept Introduction:

The periodic table represents the arrangement of the elements in increasing order of their atomic number. The horizontal rows in the periodic table are known as periods while vertical columns are known as groups. There are 18 groups and 7 periods in a periodic table.

Answer to Problem 1DQ

The electronegativity across a row increases and down a column decreases. The atomic radius of an atom is inversely proportional to the electronegativity of an atom. The electronegativity and ionization energy are directly proportional to each other.

Explanation of Solution

The tendency of elements to attract shared pair of electrons towards itself is known as electronegativity. Ongoing from left to right in a period, the size of an atom decreases. The nuclear charge will increase and the tendency to attract the shared pair of electrons in a period will increase. Therefore, electronegativity along in a period increases.

On moving up to down in a group, the size of an atom increases. The nuclear charge will decrease and the tendency to attract the shared pair of electrons in a group will decrease. Therefore, electronegativity across in a group decreases.

Relation of electronegativity with atomic radii:

As the size of the atom decrease in a period, the atomic radii of an atom will also decrease. Hence, the tendency to attract the shared pair of electrons in a period will increase.Therefore, electronegativity increases.

Relation of electronegativity with ionization energy:

Ionization energy is the amount of energy required to remove an electron from the atom. As the size of the atom decreases, the atomic radii of an atom will also decrease and the electronegativity increases. Therefore, the high amount of energy required to remove an electron from the atom.

Conclusion

The electronegativity across a row increases and down a column decreases. The atomic radius of an atom is inversely proportional to the electronegativity of an atom. The electronegativity and ionization energy are directly proportional to each other.