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Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Not the one you use?Change textbook
All textbooksTro 4th EditionCh.10 - Chemical Bonding II: Molecular Shapes & Valence Bond TheoryProblem 53b
Chapter 10, Problem 53b

The valence electron configurations of several atoms are shown here. How many bonds can each atom make without hybridization? b. P 3s23p3

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Identify the number of valence electrons for phosphorus (P) from its electron configuration.
The electron configuration for phosphorus is 3s^2 3p^3, indicating 5 valence electrons.
Determine the number of unpaired electrons in the valence shell, which are available for bonding.
In the 3p subshell, there are 3 electrons, which means there are 3 unpaired electrons.
Conclude that phosphorus can form 3 bonds without hybridization, as it has 3 unpaired electrons available for bonding.

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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 in determining how an atom can bond with others. The number of valence electrons influences the atom's ability to form bonds, as these electrons are involved in chemical reactions and bond formation.
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Bonding Capacity

The bonding capacity of an atom refers to the maximum number of bonds it can form with other atoms. This is determined by the number of unpaired valence electrons; for example, an atom with five valence electrons can typically form three bonds, as it can share its unpaired electrons with other atoms.
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Hybridization

Hybridization is a concept in chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals, which can influence the geometry and bonding properties of molecules. However, the question specifies 'without hybridization,' meaning we focus solely on the existing valence electron configuration to determine bonding capacity.
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