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Chapter 8: Problem 1

Explain the electronegativity trends across a row and down a column of the periodic table. Compare these trends with those of ionization energies and atomic radii. How are they related?

Short Answer

Expert verified
Electronegativity increases across a period (row) and decreases down a group (column) in the periodic table, similar to ionization energy trends. Conversely, atomic radii decrease across a period and increase down a group. The increase in electronegativity and ionization energy across a period is due to decreasing atomic radii and higher effective nuclear charge experienced by the outer electrons. The trends show the interdependent relationships between electronegativity, ionization energy, and atomic radii in the periodic table.

Step by step solution

01

Electronegativity Trends

Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. As we move across a period (row) from left to right in the periodic table, the electronegativity generally increases. On the other hand, as we move down a group (column), the electronegativity decreases.
02

Ionization Energy Trends

Ionization energy is the energy required to remove an electron from an atom to form a positive ion. Similar to electronegativity, ionization energy also increases across a period and decreases down a group. This is because as we move across a period, the atomic radii decrease, making it more difficult to remove an electron, and so the ionization energy increases. In contrast, as we move down a group, the atomic radii increase, making it easier to remove an electron, and thus causing the ionization energy to decrease.
03

Atomic Radii Trends

Atomic radii refer to the sizes of the atoms. Going across a period, atomic radii decrease due to the increase in the effective nuclear charge experienced by the outer electrons, caused by the increased number of protons and similar shielding by inner electrons. Moving down a group in the periodic table, atomic radii increase due to the addition of electron shells, which cause the increase in atomic size.
04

Relationship Between Electronegativity, Ionization Energy, and Atomic Radii

Electronegativity trends and ionization energy trends are positively correlated across a period and down a group in the periodic table. As atomic radii decrease across a period, the effective nuclear charge increases, making the atom more likely to gain electrons (higher electronegativity) and harder to remove an electron (higher ionization energy). Similarly, as atomic radii increase down a group, it is easier for the atom to lose an electron (lower ionization energy) and less likely to gain an electron (lower electronegativity). In summary, electronegativity and ionization energy both increase when moving across a period and decrease when moving down a group due to the changes in atomic radii. These trends show the interdependent relationships between electronegativity, ionization energy, and atomic radii in the periodic table.

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Most popular questions from this chapter

Without using Fig. \(8.3\), predict the order of increasing electronegativity in each of the following groups of elements. a. \(\mathrm{C}, \mathrm{N}, \mathrm{O}\) c. \(\mathrm{Si}, \mathrm{Ge}, \mathrm{Sn}\) b. \(\mathrm{S}, \mathrm{Se}, \mathrm{Cl}\) d. Tl, S, Ge

Identify the five compounds of \(\mathrm{H}, \mathrm{N}\), and \(\mathrm{O}\) described below. 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 \(\mathrm{C}\) and \(\mathrm{D}\) are ionic and compound \(\mathrm{B}\) is covalent. b. Nitrogen occurs in its highest possible oxidation state in compounds \(\mathrm{A}\) and \(\mathrm{C}\); nitrogen occurs in its lowest possible oxidation state in compounds \(\mathrm{C}, \mathrm{D}\), and \(\mathrm{E}\). The formal charge on both nitrogens in compound \(\mathrm{C}\) is \(+1\); the formal charge on the only nitrogen in compound \(\mathrm{B}\) is \(0 .\) c. Compounds A and E exist in solution. Both solutions give off gases. Commercially available concentrated solutions of compound \(\mathrm{A}\) are normally \(16 M .\) The commercial, concentrated solution of compound \(\mathrm{E}\) is \(15 M\). d. Commercial solutions of compound \(\mathrm{E}\) 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 \(\mathrm{D}\) is \(43.7 \% \mathrm{~N}\) and \(50.0 \% \mathrm{O}\) by mass. If compound D were a gas at STP, it would have a density of \(2.86 \mathrm{~g} / \mathrm{L}\). f. A formula unit of compound \(\mathrm{C}\) has one more oxygen than a formula unit of compound D. Compounds \(\mathrm{C}\) and \(\mathrm{A}\) have one ion in common when compound \(\mathrm{A}\) is acting as a strong electrolyte. g. Solutions of compound \(\mathrm{C}\) are weakly acidic; solutions of compound \(\mathrm{A}\) are strongly acidic; solutions of compounds \(\mathrm{B}\) and \(\mathrm{E}\) are basic. The titration of \(0.726 \mathrm{~g}\) compound \(\mathrm{B}\) requires \(21.98 \mathrm{~mL}\) of \(1.000 M \mathrm{HCl}\) for complete neutralization.

What do each of the following sets of compounds/ions have in common with each other? See your Lewis structures for Exercises 107 through 110 . a. \(\mathrm{XeCl}_{4}, \mathrm{XeCl}_{2}\) b. \(\mathrm{ICl}_{5}, \mathrm{TeF}_{4}, \mathrm{ICl}_{3}, \mathrm{PCl}_{3}, \mathrm{SCl}_{2}, \mathrm{SeO}_{2}\)

Think of forming an ionic compound as three steps (this is a simplification, as with all models): (1) removing an electron from the metal; (2) adding an electron to the nonmetal; and (3) allowing the metal cation and nonmetal anion to come together. a. What is the sign of the energy change for each of these three processes? b. In general, what is the sign of the sum of the first two processes? Use examples to support your answer. c. What must be the sign of the sum of the three processes? d. Given your answer to part \(\mathrm{c}\), why do ionic bonds occur? e. Given your above explanations, why is NaCl stable but not \(\mathrm{Na}_{2} \mathrm{Cl} ? \mathrm{NaCl}_{2} ?\) What about \(\mathrm{MgO}\) compared to \(\mathrm{MgO}_{2} ?\) \(\mathrm{Mg}_{2} \mathrm{O} ?\)

Write Lewis structures and predict whether each of the following is polar or nonpolar. a. HOCN (exists as \(\mathrm{HO}-\mathrm{CN}\) ) b. \(\operatorname{COS}\) c. \(\mathrm{XeF}_{2}\) d. \(\mathrm{CF}_{2} \mathrm{Cl}_{2}\) e. \(\mathrm{SeF}_{6}\) f. \(\mathrm{H}_{2} \mathrm{CO}(\mathrm{C}\) is the central atom. \()\)
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