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Chapter 4: Problem 32

What periodic trends exist for electronegativity? Explain the factors involved.

Short Answer

Expert verified
The periodic trends for electronegativity typically involve an increase in electronegativity as you move from left to right across a period due to an increasing nuclear charge. Electronegativity tends to decrease down a group due to increasing atomic size and electron shielding effect.

Step by step solution

01

- Understand Electronegativity

Before diving into the trends, it's important to understand that electronegativity is a measure of an atom's ability to attract a bonding pair of electrons. The greater the electronegativity, the greater its attractiveness for bonding electrons.
02

- Examine the trend across a period

As we move from left to right across a period of the periodic table, the electronegativity of the elements tends to increase. This is primarily due to the fact that the number of charges on the nucleus increases, which attracts electrons in a bond more strongly. Since the electrons are being added to the same energy level and the atom is getting smaller, the increased nuclear charge attracts electron more.
03

- Examine the trend down a group

As you go down a group, electronegativity decreases. Though the nuclear charge 'increases', the distance between the nucleus and the valence electrons also increases. Moreover, additional energy levels lead to electron shielding effect. Therefore, the pull felt towards the nucleus by the valence electrons (those involved in bonding) is less, causing a decrease in electronegativity.

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Most popular questions from this chapter

If an element breaks when it is struck with a hammer, could it be a metal? Explain.

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Consider two main-group elements, \(\mathrm{A}\) and B. Element A has an ionization energy of 419 \(\mathrm{kJ} / \mathrm{mol} .\) Element \(\mathrm{B}\) has an ionization energy of 1000 \(\mathrm{kJ} / \mathrm{mol} .\) Which element is more likely to form a cation?
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