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Ch.8 - Basic Concepts of Chemical Bonding
All textbooksBrown 15th EditionCh.8 - Basic Concepts of Chemical BondingProblem 6
Chapter 8, Problem 6

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]

Verified step by step guidance
1
Identify the total number of valence electrons in the molecule C4H3NO. Carbon (C) has 4 valence electrons, hydrogen (H) has 1, nitrogen (N) has 5, and oxygen (O) has 6. Calculate the total by adding these up: 4(4) + 3(1) + 5 + 6.
Draw the skeletal structure of the molecule based on the given connectivity. Connect the atoms with single bonds initially, ensuring that each atom is connected as per the structure provided.
Distribute the remaining valence electrons to satisfy the octet rule for each atom, starting with the most electronegative atoms (usually oxygen and nitrogen).
Adjust the bonds (single, double, triple) as necessary to ensure that all atoms satisfy the octet rule, keeping in mind that hydrogen can only form single bonds.
Count the number of single bonds, double bonds, triple bonds, and nonbonding pairs of electrons in the completed Lewis structure.>

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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 help visualize how atoms are connected and the distribution of electrons, which is crucial for determining the number of single, double, and triple bonds, as well as nonbonding pairs.
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Lewis Dot Structures: Ions

Types of Chemical Bonds

Chemical bonds can be classified into single, double, and triple bonds based on the number of shared electron pairs between atoms. A single bond involves one pair of shared electrons, a double bond involves two pairs, and a triple bond involves three pairs. Understanding these types is essential for analyzing the connectivity in a molecule.
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Nonbonding Electron Pairs

Nonbonding electron pairs, also known as lone pairs, are pairs of valence electrons that are not involved in bonding. They play a significant role in determining the geometry and reactivity of a molecule. Identifying these pairs is important for accurately completing the Lewis structure and understanding the overall electron distribution.
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Related Practice
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. (d) Consider ion 5. How many repulsive interactions are shown for it?

Textbook Question

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

Textbook Question

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

Textbook Question

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.

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Textbook Question

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]