Ch.8 - Basic Concepts of Chemical Bonding

Brown - Chemistry: The Central Science 15th Edition

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Brown 15th Edition

Ch.8 - Basic Concepts of Chemical Bonding

Problema 7

Capitolo 8, Problema 7

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.

Guida verificata passo dopo passo

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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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.

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04:28

Lewis Dot Structures: Ions

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.

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01:53

Formal Charge

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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00:38

Periodic Trends

Pratica correlata

Domanda del libro di testo

The molecule shown here is styrene, C8H8, a benzene derivative that is used to make a number of polymers, including polystyrene. The shorthand notation for the benzene ring (described in Section 8.6) is used. Three of the carbon–carbon bonds are numbered in the structure.

a. Which of the three bonds is the strongest?

b. Which of the three bonds is the longest?

c. Which of the three bonds is best described as halfway between a single and a double bond? [Sections 8.6 and 8.8]

Domanda del libro di testo

The orbital diagram that follows shows the valence electrons for a 3+ ion of an element. (a) What is the element?

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Domanda del libro di testo

Which of the following charts shows the general periodic trends for the electronegativities of the representative elements? [Section 8.4]

Domanda del libro di testo

Consider the Lewis structure for the polyatomic oxyanion shown here, where X is an element from the third period (Na - Ar). By changing the overall charge, n, from 1- to 2- to 3- we get three different polyatomic ions. For each of these ions (b) determine the formal charge of the central atom, X;

887

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Domanda del libro di testo

A molecule with formula C4H3NO has the connectivity shown in the figure. After the Lewis structure of the molecule is completed, how many of each of the following are there in the molecule:

a. single bonds,

b. double bonds,

c. triple bonds,

d. nonbonding pairs? [Sections 8.3 and 8.5]

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