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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 53c
Chapter 10, Problem 53c

The valence electron configurations of several atoms are shown here. How many bonds can each atom make without hybridization? c. F 2s22p5

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Identify the number of valence electrons for the atom. Fluorine (F) has 7 valence electrons, as indicated by the configuration 2s^2 2p^5.
Determine the number of electrons needed to complete the octet. Fluorine needs 1 more electron to achieve a full octet (8 electrons).
Recognize that the number of bonds an atom can form is typically equal to the number of electrons it needs to complete its octet.
Since fluorine needs 1 more electron to complete its octet, it can form 1 bond.
Conclude that without hybridization, fluorine can form 1 single covalent bond.

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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 an atom's reactivity and the types of bonds it can form. For example, fluorine (F) has seven valence electrons, which allows it to form one bond to achieve a stable octet configuration.
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Bonding Capacity

Bonding capacity refers to the maximum number of bonds an atom can form based on its valence electron configuration. Atoms tend to form bonds to achieve a full outer shell, typically following the octet rule. In the case of fluorine, with its configuration of 2s²2p⁵, it can form one bond by sharing one of its unpaired electrons.
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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 of molecules. However, the question specifies 'without hybridization,' meaning we consider the atom's original atomic orbitals. For fluorine, without hybridization, it utilizes its existing p orbitals to form bonds.
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