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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

For each of the following groups, place the atoms and/or ions in order of decreasing size. a. V,V2+,V3+,V5+ b. Na+,K+,Rb+,Cs+ c. Te2−,I−,Cs+,Ba2+ d. P,P−,P2−,P3− e. O2−,S2−,Se2−,Te2−

Consider the following reaction: A2+B2⟶2ABΔH=−285kJ The bond energy for A2 is one-half the amount of the AB bond energy. The bond energy of B2=432kJ/mol . What is the bond energy of A2 ?

Write the Lewis structure for O2F2(O2F2 exists as F−O−O−F). Assign oxidation states and formal charges to the atoms in O2F2. This compound is a vigorous and potent oxidizing and fluorinating agent. Are oxidation states or formal charges more useful in accounting for these properties of O2F2?

Draw a Lewis structure for the N,N -dimethylformamide molecule. The skeletal structure is Various types of evidence lead to the conclusion that there is some double bond character to the C-N bond. Draw one or more resonance structures that support this observation.

Identify the five compounds of H,N, and O described as follows. For each compound, write a Lewis structure that is consistent with the information given. a. All the compounds are electrolytes, although not all of them are strong electrolytes. Compounds C and D are ionic and compound B is covalent. b. Nitrogen occurs in its highest possible oxidation state in compounds A and C; nitrogen occurs in its lowest possible oxidation state in compounds C,D, and E. The formal charge on both nitrogens in compound C is +1; the formal charge on the only nitrogen in compound B is 0. c. Compounds A and E exist in solution. Both solutions give off gases. Commercially available concentrated solutions of compound A are normally 16M. The commercial, concentrated solution of compound E is 15M. d. Commercial solutions of compound E are labeled with a misnomer that implies that a binary, gaseous compound of nitrogen and hydrogen has reacted with water to produce ammonium ions and hydroxide ions. Actually, this reaction occurs to only a slight extent. e. Compound D is 43.7%N and 50.0% O by mass. If compound D were a gas at STP, it would have a density of 2.86 g/L. f. A formula unit of compound C has one more oxygen than a formula unit of compound D. Compounds C and A have one ion in common when compound A is acting as a strong electrolyte. g. Solutions of compound C are weakly acidic; solutions of compound A are strongly acidic; solutions of compounds B and E are basic. The titration of 0.726 g compound B requires 21.98 mL of 1.000 MHCl for complete neutralization.
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