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Chapter 8: Problem 23

What is the electronegativity trend? Where does hydrogen fit into the electronegativity trend for the other elements in the periodic table?

Short Answer

Expert verified
The electronegativity trend increases from left to right across a period and decreases from top to bottom within a group in the periodic table. Hydrogen, with an electronegativity value of 2.20 on the Pauling scale, is positioned around the middle of the trend, between metals and nonmetals, making it an exceptional case in the periodic table.

Step by step solution

01

Understand Electronegativity Trend

Electronegativity increases from left to right across a period and decreases from top to bottom within a group in the periodic table. This trend is attributable to two factors: increasing nuclear charge (i.e., more protons within the nucleus) as we move to the right across a period, and increasing the shielding effect of inner electrons as we move down a group.
02

Comparing Electronegativity of Elements

In general, nonmetals are more electronegative than metals. Halogens (Group 17 elements) are the most electronegative, with fluorine having the highest electronegativity value (3.98 on the Pauling scale). Alkali metals (Group 1 elements) are the least electronegative, followed by alkaline earth metals (Group 2 elements).
03

Hydrogen's Electronegativity

Hydrogen is a unique element since it is neither a metal nor a nonmetal. Its electronegativity on the Pauling scale is 2.20, which is quite close to the value of carbon (2.55) and higher than the values of alkali and alkaline earth metals. This places hydrogen around the middle electronegativity range for elements.
04

Position of Hydrogen in the Electronegativity Trend

Hydrogen can be placed somewhere between the metals and nonmetals in the periodic table in terms of electronegativity. Its electronegativity value is closer to nonmetals than metals, which makes it more likely to form covalent bonds with nonmetals. However, it is not as electronegative as most of the nonmetals on the right of the periodic table. In conclusion, the electronegativity trend increases across a period (left to right) and decreases down a group (top to bottom) in the periodic table. Hydrogen's electronegativity value of 2.20 positions it around the middle of the trend, between metals and nonmetals, making it an exceptional case in the periodic table.

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Most popular questions from this chapter

Which member of the following pairs would you expect to be more energetically stable? Justify each choice. a. \(\mathrm{NaBr}\) or \(\mathrm{NaBr}_{2}\) b. \(\mathrm{ClO}_{4}\) or \(\mathrm{ClO}_{4}^{-}\) c. \(\mathrm{SO}_{4}\) or \(\mathrm{XeO}_{4}\) d. \(\mathrm{OF}_{4}\) or \(\mathrm{SeF}_{4}\)

Benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) consists of a six- membered ring of carbon atoms with one hydrogen bonded to each carbon. Write Lewis structures for benzene, including resonance structures.

The standard enthalpy of formation for \(\mathrm{NO}(g)\) is \(90 . \mathrm{kJ} / \mathrm{mol}\) . Use this and the values for the O \(=\mathrm{O}\) and \(\mathrm{N} \equiv \mathrm{N}\) bond energies to estimate the bond strength in NO.

Although both \(\mathrm{Br}_{3}^{-}\) and \(\mathrm{I}_{3}^{-}\) ions are known, the \(\mathrm{F}_{3}-\) ion has not been observed. Explain.

When comparing the size of different ions, the general radii trend discussed in Chapter 7 is usually not very useful. What do you concentrate on when comparing sizes of ions to each other or when comparing the size of an ion to its neutral atom?
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