Writing Lewis structures Give the Lewis structure for each of the following. [latex] a. HF b. N_{2} c. NH_{3} d. CH_{4} e. CF_{4} f. NO^{+}[/latex]

In each case we apply the three rules for writing Lewis structures. Recall that lines are used to indicate shared electron pairs and that dots are used to indicate nonbonding pairs (lone pairs). We have the following tabulated results: Total Valence Electrons Draw Single Bonds Calculate Number of Electrons Remaining Use Remaining Electrons to Achieve Noble Gas Configurations a. HF 1 + 7 = 8 H—F 6 [latex] b. N_{2}[/latex] 5 + 5 = 10 N—N 8 [latex] c. NH_{3} [/latex] 5 + 3 (1) = 8 2 [latex]d. CH_{4} [/latex] 4 + 4 (1) = 8 0 [latex]e. CF_{4} [/latex] 4 + 4 (7) = 32 24 [latex] f. NO^{+}[/latex] 5 + 6 -1 = 10 N—O 8 When writing Lewis structures, don’t worry about which electrons came from which atoms. The best way to look at a molecule is to regard it as a new entity that uses all of the available valence electrons of the atoms to achieve the lowest possible energy.* The valence electrons belong to the molecule rather than to the individual atoms. Simply distribute all valence electrons so that the various rules are satisfied, without regard to the origin of each particular electron.

Question 13.6: Writing Lewis structures Give the Lewis structure for each o...

Chemical Principles

Writing Lewis structures
Give the Lewis structure for each of the following.

a.  HF          b.  N_{2}            c.  NH_{3}           d.  CH_{4}          e.  CF_{4}            f.  NO^{+}

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In each case we apply the three rules for writing Lewis structures. Recall that lines are used to indicate shared electron pairs and that dots are used to indicate nonbonding pairs (lone pairs). We have the following tabulated results:

	Total Valence Electrons	Draw Single Bonds	Calculate Number of Electrons Remaining	Use Remaining Electrons to Achieve Noble Gas Configurations
a. HF	1 + 7 = 8	H—F	6
$b. N_{2}$	5 + 5 = 10	N—N	8
$c. NH_{3}$	5 + 3 (1) = 8		2
$d. CH_{4}$	4 + 4 (1) = 8		0
$e. CF_{4}$	4 + 4 (7) = 32		24
$f. NO^{+}$	5 + 6 -1 = 10	N—O	8

When writing Lewis structures, don’t worry about which electrons came from which atoms. The best way to look at a molecule is to regard it as a new entity that uses all of the available valence electrons of the atoms to achieve the lowest possible energy.* The valence electrons belong to the molecule rather than to the individual atoms. Simply distribute all valence electrons so that the various rules are satisfied, without regard to the origin of each particular electron.