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Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory
All textbooksMcMurry 8th EditionCh.6 - Ionic Compounds: Periodic Trends and Bonding TheoryProblem 78d
Chapter 6, Problem 78d

Element X reacts with element Y to give a product containing X3+ ions and Y2-ions. (d) In what groups of the periodic table are elements X and Y likely to be found?

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Identify the charges of the ions formed by elements X and Y. Element X forms X3+ ions, indicating it loses three electrons. Element Y forms Y2- ions, indicating it gains two electrons.
Recall that elements that lose electrons are metals and are typically found on the left side of the periodic table. The ability to lose three electrons suggests that element X is likely a metal in groups 1, 2, or 13-16, as these groups contain elements capable of forming +3 ions.
Consider that elements that gain electrons are nonmetals or metalloids and are typically found on the right side of the periodic table. The ability to gain two electrons suggests that element Y is likely a nonmetal in groups 16 or 17, as these groups contain elements capable of forming -2 ions.
Narrow down the groups by focusing on common oxidation states. Metals in group 13 frequently form +3 ions, making it a likely group for element X. Nonmetals in group 16 commonly form -2 ions, making it a likely group for element Y.
Conclude that element X is likely found in group 13 of the periodic table, and element Y is likely found in group 16 of the periodic table.

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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 elements transfer electrons, resulting in the formation of positively charged cations and negatively charged anions. In this case, X3+ indicates that element X has lost three electrons, while Y2- shows that element Y has gained two electrons. Understanding the formation of these ions is crucial for identifying the elements involved.
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Ionic Compounds Naming

Periodic Table Groups

Elements in the periodic table are organized into groups based on their similar properties and electron configurations. Group 13 elements typically form +3 cations, while Group 16 elements commonly form -2 anions. Recognizing the groups helps in predicting the likely identities of elements X and Y based on their ionic charges.
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Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. The tendency of elements to lose or gain electrons to achieve a stable electron configuration, often resembling that of noble gases, is fundamental in determining their reactivity. This concept aids in understanding why element X forms a +3 ion and element Y forms a -2 ion.
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Related Practice
Textbook Question

Element X reacts with element Y to give a product containing X3+ ions and Y2-ions. (a) Is element X likely to be a metal or a nonmetal? Explain.

Textbook Question

Element X reacts with element Y to give a product containing X3+ ions and Y2-ions. (b) Is element Y likely to be a metal or a nonmetal? Explain.

Textbook Question

Element X reacts with element Y to give a product containing X3+ ions and Y2- ions. (c) What is the formula of the product?

Textbook Question
Cesium has the smallest ionization energy of all elements (376 kJ/mol), and chlorine has the most negative electron affinity 1-349 kJ/mol2. Will a cesium atom transfer an electron to a chlorine atom to form isolated Cs+1g2 and Cl-1g2 ions? Explain.
Textbook Question
How does electron shielding in multielectron atoms give rise to energy differences among 3s, 3p, and 3d orbitals?
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