Ch.8 - Basic Concepts of Chemical Bonding

Brown - Chemistry: The Central Science 14th Edition

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Brown 14th Edition

Ch.8 - Basic Concepts of Chemical Bonding

Problem 40d

Chapter 8, Problem 40d

By referring only to the periodic table, select (d) the element in the group K, C, Zn, F that is most likely to form an ionic compound with Ba.

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Identify the group of each element: K (Potassium) is in Group 1, C (Carbon) is in Group 14, Zn (Zinc) is in Group 12, and F (Fluorine) is in Group 17.

Recall that ionic compounds are typically formed between metals and nonmetals, where metals lose electrons and nonmetals gain electrons.

Recognize that Ba (Barium) is an alkaline earth metal in Group 2, which tends to form +2 cations.

Determine which element among K, C, Zn, and F is a nonmetal and can gain electrons to form an anion.

Conclude that the element most likely to form an ionic compound with Ba is the nonmetal that can accept electrons from Ba to form a stable ionic bond.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Ionic Compounds

Ionic compounds are formed when atoms transfer electrons, resulting in the formation of positively and negatively charged ions. Typically, this occurs between metals, which lose electrons, and nonmetals, which gain electrons. The electrostatic attraction between these oppositely charged ions leads to the formation of a stable ionic lattice structure.

Periodic Table Groups

Elements in the periodic table are organized into groups based on their similar chemical properties. Group K (alkali metals) and Group F (halogens) are particularly relevant here, as alkali metals tend to lose one electron to form cations, while halogens typically gain one electron to form anions. Understanding the behavior of these groups helps predict how elements will interact with each other.

Barium's Reactivity

Barium (Ba) is an alkaline earth metal that readily forms ionic compounds, typically by losing two electrons to form a Ba²⁺ ion. When considering potential ionic compounds with other elements, it is essential to identify which element can effectively gain or lose electrons to balance the charge. In this case, the most suitable partner for Ba would be an element that can form a stable ionic bond by achieving a full outer electron shell.

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Using only the periodic table as your guide, select the most electronegative atom in each of the following sets: (a) Se, Te, Br, I; (b) Be, Mg, C, Si (c) Al, Si, P, S (d) Zn, Ge, Ga, As.

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Arrange the bonds in each of the following sets in order of increasing polarity: (c) C—S, B—F, N—O.

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Textbook Question

(a) From the data in Table 8.2, calculate the effective charges on the H atom of the HBr molecule in units of the electronic charge, e.

Arrange the bonds in each of the following sets in order of increasing polarity: (a) C—F, O—F, Be—F (b) O—Cl,S—Br, C—P

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Textbook Question

By referring only to the periodic table, select (a) the most electronegative element in group 13; (b) the least electronegative element in the group As, Se and Br;