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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

Write Lewis structures that obey the octet rule (duet rule for H) for each of the following molecules. Carbon is the central atom in \(\mathrm{CH}_{4}\) , nitrogen is the central atom in \(\mathrm{NH}_{3},\) and oxygen is the central atom in \(\mathrm{H}_{2} \mathrm{O}\) . a. \(\mathrm{F}_{2} \quad\) e. \(\mathrm{NH}_{3}\) b. \(\mathrm{O}_{2} \quad\) f. \(\mathrm{H}_{2} \mathrm{O}\) c. \(\mathrm{CO} \quad\) g. \(\mathrm{HF}\) d. \(\mathrm{CH}_{4}\)

Which of the following incorrectly shows the bond polarity? Show the correct bond polarity for those that are incorrect. a. \(^{\delta+} \mathrm{H}-\mathrm{F}^{\delta-} \quad\) d. $\delta^{+} \mathrm{Br}-\mathrm{Br}^{\delta-}$ b. \(^{\delta+} \mathrm{Cl}-\mathrm{I}^{\delta-} \qquad\) e. \(\quad\) e. $\quad ^{\delta+}\mathrm{O}-\mathrm{P}^{\delta-}$ c. \(\quad \delta+\mathrm{Si}-\mathrm{S}^{\delta-}\)

The most common type of exception to the octet rule are compounds or ions with central atoms having more than eight electrons around them. PF_. \(\mathrm{PF}_{5}, \mathrm{SF}_{4}, \mathrm{ClF}_{3}\) and \(\mathrm{Br}_{3}^{-}\) are examples of this type of exception. Draw the Lewis structure for these compounds or ions. Which elements, when they have to, can have more than eight electrons around them? How is this rationalized?

List the bonds $\mathrm{P}-\mathrm{Cl}, \mathrm{P}-\mathrm{F}, \mathrm{O}-\mathrm{F},\( and \)\mathrm{Si}-\mathrm{F}$ from least polar to most polar.

Hydrogen has an electronegativity value between boron and carbon and identical to phosphorus. With this in mind, rank the following bonds in order of decreasing polarity: \(\mathrm{P}-\mathrm{H}\) , $\mathrm{O}-\mathrm{H}, \mathrm{N}-\mathrm{H}, \mathrm{F}-\mathrm{H}, \mathrm{C}-\mathrm{H} .$
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