Ch.8 - Basic Concepts of Chemical Bonding

Brown - Chemistry: The Central Science 14th Edition

Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook

Brown 14th Edition

Ch.8 - Basic Concepts of Chemical Bonding

Problem 9b

Chapter 8, Problem 9b

(b) How many valence electrons does a nitrogen atom possess?

Verified step by step guidance

insert step 1> Determine the atomic number of nitrogen from the periodic table.

insert step 2> Recognize that the atomic number of nitrogen is 7, which means it has 7 electrons in total.

insert step 3> Understand that the electron configuration of nitrogen is 1s^2 2s^2 2p^3.

insert step 4> Identify the valence electrons, which are the electrons in the outermost shell. For nitrogen, these are the electrons in the 2s and 2p orbitals.

insert step 5> Count the valence electrons: 2 electrons from the 2s orbital and 3 electrons from the 2p orbital, totaling 5 valence electrons.

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Key Concepts

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

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial for determining how an atom interacts with others. They are involved in forming chemical bonds and influence the chemical properties of an element. The number of valence electrons can often be determined by an element's position in the periodic table.

Periodic Table

The periodic table organizes elements based on their atomic number and electron configuration. Elements in the same group (column) typically have the same number of valence electrons, which helps predict their chemical behavior. For nitrogen, which is in group 15, this organization aids in identifying its valence electrons.

Nitrogen Atom

A nitrogen atom has an atomic number of 7, meaning it has 7 protons and, in a neutral state, 7 electrons. The electron configuration of nitrogen is 1s² 2s² 2p³, indicating that it has 5 valence electrons in the second shell. Understanding the structure of nitrogen is essential for determining its reactivity and bonding capabilities.

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Textbook Question

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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?

Textbook Question

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;

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Textbook Question

(a) True or false: An element's number of valence electrons is the same as its atomic number.

Textbook Question

(a) True or false: The hydrogen atom is most stable when it has a full octet of electrons.

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Textbook Question

Ammonium chloride, NH₄Cl, is a very soluble salt in water. (b) Is there an N—Cl bond in solid ammonium chloride?