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Chapter 4: Problem 9

Fill in the blanks. In the long form of the periodic table, ___ group elements can release maximum amount of energy by the addition of electron into its valence shell.

Short Answer

Expert verified
Answer: Group 17

Step by step solution

01

Understanding the Periodic Table

The periodic table is divided into several groups (columns) and periods (rows), where elements with similar properties are organized. There are two main categories of elements: metals and non-metals. Metals are located on the left and center of the table, while non-metals are located on the right.
02

Electron Affinity

Electron affinity is the amount of energy released when an electron is added to an atom, forming a negative ion. The greater the electron affinity, the more energy is released when an electron is added to the atom. In general, electron affinity increases from left to right across a period and decreases down a group in the periodic table.
03

Finding the Group with Maximum Electron Affinity

As we move across a period from left to right, the electron affinity increases. Therefore, we should look for elements on the right side of the periodic table. Among non-metals, Group 17 elements, called halogens, have the highest electron affinity. This is because halogens have seven valence electrons, and adding one more electron to the valence shell results in a full outer shell, which is energetically favorable.
04

Answering the Question

Based on our understanding of electron affinity and the periodic table, we can conclude that the group with the maximum energy release upon electron addition is Group 17 or halogens. The answer for the exercise is: In the long form of the periodic table, _Group 17_ group elements can release the maximum amount of energy by the addition of an electron into its valence shell.

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Most popular questions from this chapter

An element with atomic number " \(32 "\) "belongs to (a) \(4^{\text {th }}\) period, VIA group or \(16^{\text {th }}\) group (b) \(3^{\text {rd }}\) period, IVA group or \(14^{\text {th }}\) group (c) \(4^{\text {th }}\) period, IVA group or \(14^{\text {th }}\) group (d) \(5^{\text {th }}\) period, VA group or \(15^{\text {th }}\) group

In a period, from the left to right the electron affinity increases, but alkaline earth metals have lower electron affinity than alkali metals because (a) alkaline earth metals have lesser atomic radius than alkali metals. (b) alkaline earth have higher electronegativity than alkali metals. (c) alkaline earth metals have completely filled "s-" orbitals. (d) alkaline earth metals have lesser electronegativity than alkali metals.

Fill in the blanks. The total number of inner transition elements present in the 7 th period are ____.

In the sixth period, the orbitals which are completely filled are (a) \(6 \mathrm{~s}, 6 \mathrm{p}, 5 \mathrm{~d}, 5 \mathrm{f}\) (b) \(6 s, 6 p, 6 d, 6 f\) (c) \(6 \mathrm{~s}, 5 \mathrm{f}, 6 \mathrm{~d}, 6 \mathrm{p}\) (d) \(6 s, 4 f, 5 d, 6 p\)

The first ionization energies of \(\mathrm{Li}, \mathrm{Be}, \mathrm{B}\) and \(\mathrm{C}\) are in the order: (a) \(\mathrm{Li}>\mathrm{Be}<\mathrm{B}<\mathrm{C}\) (b) \(\mathrm{Li}<\mathrm{Be}>\mathrm{B}<\mathrm{C}\) (c) \(\mathrm{Li}>\mathrm{Be}>\mathrm{B}>\mathrm{C}\) (d) \(\mathrm{Li}<\mathrm{Be}>\mathrm{B}>\mathrm{C}\)
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