Chapter 16: Problem 6

Considering the valence shell for these atoms, explain why \(\mathrm{C}, \mathrm{N}, \mathrm{O}\) and \(\mathrm{F}\) can accommodate only eight electrons (sum of the bonding and lone-pair electrons) in Lewis structures.

Short Answer

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The atoms of C, N, O, and F can accommodate only eight electrons (sum of the bonding and lone-pair electrons) in Lewis structures due to the octet rule, which postulates that atoms are stable when their outermost (valence) shell is full, typically with eight electrons. In this light, C needs 4 more electrons, N needs 3, O needs 2, and F needs 1 to fulfill the octet rule.

Step by step solution

Understanding Atomic Structure

Atoms consist of a nucleus, a dense core of protons and neutrons, surrounded by a much larger region of electron cloud. The electrons exist in different energy levels also known as shells. The outermost shell is referred to as the valence shell and the electrons in this shell are called valence electrons.

Recognizing the Octet Rule

The octet rule is a chemical rule of thumb that reflects the theory that atoms are stable when their outermost shell is full, normally with eight electrons. Therefore, in the process of chemical bonding, atoms tend to gain, lose or share electrons to achieve a full valence shell of eight electrons.

Understanding Valence Electrons

Valence electrons participate in the formation of chemical bonds. In the Lewis structure, dots are used to represent the valence electrons. A single line or a pair of dots represents a single bond or a pair of electrons respectively.

Applying Octet Rule to C, N, O, and F

Applying the octet rule to these atoms: C has 4 valence electrons and requires 4 more to complete its octet, N has 5 and needs 3 more, O has 6 and needs 2 more, and F has 7 and needs 1 more to fulfill the octet rule. Therefore, all of these atoms can accommodate only eight electrons in their Lewis structures.

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Considering the valence shell for these atoms, explain why \(\mathrm{C}, \mathrm{N}, \mathrm{O}\) and \(\mathrm{F}\) can accommodate only eight electrons (sum of the bonding and lone-pair electrons) in Lewis structures.

Short Answer

Step by step solution

Understanding Atomic Structure

Recognizing the Octet Rule

Understanding Valence Electrons

Applying Octet Rule to C, N, O, and F

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