Textbook Question
(a) True or false: The hydrogen atom is most stable when it has a full octet of electrons.
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Ch.8 - Basic Concepts of Chemical Bonding
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 8, Problem 11c
(c) An atom has the electron configuration 1s22s22p63s23p2. How many valence electrons does the atom have?
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Identify the highest principal quantum number (n) in the given electron configuration. This number indicates the outermost shell of the atom.
Locate the subshells (s, p, d, f) associated with the highest principal quantum number. In this case, look at the electrons in the 3s and 3p subshells.
Count the total number of electrons in these subshells. The number of electrons in these subshells represents the number of valence electrons.
Sum the electrons in the 3s and 3p subshells to find the total number of valence electrons.
The total number of electrons in the 3s and 3p subshells is the number of valence electrons the atom has.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Electron Configuration
Electron configuration describes the distribution of electrons in an atom's orbitals. It is represented by a series of numbers and letters indicating the energy levels and types of orbitals occupied by electrons. Understanding electron configuration is essential for determining the chemical properties of an element, including its reactivity and bonding behavior.
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Electron Configuration Example
Valence Electrons
Valence electrons are the electrons in the outermost shell of an atom that are involved in chemical bonding. They determine how an atom interacts with other atoms and are crucial for understanding an element's reactivity. The number of valence electrons can be deduced from the electron configuration, particularly from the highest principal energy level.
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Principal Energy Levels
Principal energy levels are the layers of electrons surrounding the nucleus of an atom, denoted by the principal quantum number (n). Each level can hold a specific number of electrons, and the outermost level contains the valence electrons. Identifying the principal energy levels helps in understanding the structure of the atom and predicting its chemical behavior.
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Related Practice
Textbook Question
(a) Write the electron configuration for the element titanium, Ti. How many valence electrons does this atom possess?
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Textbook Question
(b) How many valence electrons does a nitrogen atom possess?
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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
Consider the element silicon, Si. (c) Which subshells hold the valence electrons?
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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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