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 5

Chapter 8, Problem 5

In the Lewis structure shown here, A, D, E, Q, X, and Z represent elements in the first two rows of the periodic table. Identify all six elements so that the formal charges of all atoms are zero.

Verified step by step guidance

Step 1: Understand the concept of formal charge. The formal charge is calculated using the formula: Formal Charge = (Valence Electrons) - (Non-bonding Electrons) - (Bonding Electrons/2).

Step 2: Recognize that the elements A, D, E, Q, X, and Z are from the first two rows of the periodic table, which include elements from Hydrogen to Neon.

Step 3: Consider the typical bonding patterns and valence electrons for these elements. For example, Carbon typically forms four bonds, Nitrogen three bonds with one lone pair, Oxygen two bonds with two lone pairs, etc.

Step 4: Assign possible elements to A, D, E, Q, X, and Z based on their ability to form bonds that result in a formal charge of zero. Ensure that the total number of valence electrons matches the number of electrons in the Lewis structure.

Step 5: Verify that each element's assigned bonding and lone pairs result in a formal charge of zero, adjusting assignments as necessary to achieve this condition for all elements involved.

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Key Concepts

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

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use dots to represent valence electrons and lines to represent bonds between atoms. Understanding how to draw and interpret Lewis structures is essential for visualizing molecular geometry and predicting the behavior of molecules.

Formal Charge

Formal charge is a concept used to determine the charge of an atom in a molecule based on its valence electrons, the number of bonds it forms, and the number of lone electrons it possesses. It is calculated using the formula: Formal Charge = Valence Electrons - (Non-bonding Electrons + 1/2 Bonding Electrons). Ensuring that the formal charges of all atoms are zero is crucial for achieving a stable and accurate representation of the molecule.

Periodic Table Trends

The periodic table organizes elements based on their atomic number and properties, revealing trends in reactivity, electronegativity, and atomic size. Elements in the first two rows include hydrogen, helium, lithium, beryllium, boron, carbon, nitrogen, oxygen, fluorine, and neon. Understanding these trends helps in predicting how elements will bond and interact, which is vital for constructing accurate Lewis structures.

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Periodic Trends

Related Practice

Textbook Question

The partial Lewis structure that follows is for a hydrocarbon molecule. In the full Lewis structure, each carbon atom satisfies the octet rule, and there are no unshared electron pairs in the molecule. The carbon—carbon bonds are labeled 1, 2, and 3. (c) Which carbon—carbon bond is the strongest one?

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Textbook Question

A portion of a two-dimensional 'slab' of NaCl(s) is shown here (see Figure 8.2) in which the ions are numbered. (a) Which colored balls must represent sodium ions?

A portion of a two-dimensional 'slab' of NaCl(s) is shown here (see Figure 8.2) in which the ions are numbered. (d) Consider ion 5. How many repulsive interactions are shown for it?

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Textbook Question

Illustrated are four ions — A, B, X, and Y— showing their relative ionic radii. The ions shown in red carry positive charges: a 2+ charge for A and a 1+ charge for B. Ions shown in blue carry negative charges: a 1- charge for X and a 2- charge for Y. (b) Among the combinations in part (a), which leads to the ionic compound having the largest lattice energy?

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