Ch.10 - Chemical Bonding I: The Lewis Model

Tro - Chemistry: A Molecular Approach 5th Edition

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Tro 5th Edition

Ch.10 - Chemical Bonding I: The Lewis Model

Problem 42

Chapter 10, Problem 42

Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. a. Ca and N b. Mg and I c. Ca and S d. Cs and F

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Identify the valence electrons for each element using the periodic table.

Use Lewis symbols to represent the valence electrons for each element.

Determine how many electrons each element needs to gain or lose to achieve a full outer shell (octet rule).

Pair the elements such that the total number of electrons lost by the metal equals the total number of electrons gained by the non-metal.

Write the chemical formula by balancing the charges to ensure the compound is neutral.

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Key Concepts

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

Lewis Symbols

Lewis symbols represent the valence electrons of an atom as dots around the element's symbol. This visual representation helps in understanding how atoms bond with each other by either sharing or transferring electrons. For example, the Lewis symbol for calcium (Ca) shows two dots, indicating its two valence electrons, which are crucial for forming ionic or covalent bonds.

Ionic Bonding

Ionic bonding occurs when one atom donates electrons to another, resulting in the formation of charged ions. This typically happens between metals, which lose electrons, and nonmetals, which gain electrons. For instance, in the case of calcium (Ca) and nitrogen (N), calcium loses two electrons to form Ca²⁺, while nitrogen gains three electrons to form N³⁻, leading to the compound Ca₃N₂.

Covalent Bonding

Covalent bonding involves the sharing of electron pairs between atoms, usually between nonmetals. This type of bond is characterized by the formation of molecules where the shared electrons allow each atom to achieve a stable electron configuration. For example, when magnesium (Mg) bonds with iodine (I), they share electrons to form MgI₂, illustrating the concept of covalent bonding in molecular compounds.

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Use the Born–Haber cycle and data from Appendix IIB, Chapter 9 and this chapter to calculate the lattice energy of KCl. (ΔHsub for potassium is 89.0 kJ>mol.)

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Use the Born–Haber cycle and data from Appendix IIB and Table 10.3 to calculate the lattice energy of CaO. (ΔHsub for calcium is 178 kJ>mol; IE1 and IE2 for calcium are 590 kJ>mol and 1145 kJ>mol, respectively; EA1 and EA2 for O are -141 kJ>mol and 744 kJ>mol, respectively.)

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Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. a. Sr and Se b. Ba and Cl c. Na and S d. Al and O

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