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Chapter 10: Problem 3

Write plausible Lewis structures for the following molecules that contain only single covalent bonds. (a) \(\mathrm{FCl} ;\) (b) \(\mathrm{I}_{2} ;\) (c) \(\mathrm{SF}_{2} ;\) (d) \(\mathrm{NF}_{3} ;\) (e) \(\mathrm{H}_{2} \mathrm{Te}\).

Short Answer

Expert verified
The plausible Lewis structures for the molecules with single covalent bonds are: F-Cl for FCl, I-I for I2, F-S-F for SF2, and H-Te-H for H2Te. The structure for NF3 is a bit more complicated: F is linked to N through a single bond, and this N is then linked to two other Fs through single bonds (forming a Y-like shape).

Step by step solution

01

Draw Lewis structure for FCl

F and Cl each has seven valence electrons. They can share one electron forming a single covalent bond. The remaining six electrons on each atom will be shown as lone pairs. The Lewis structure is: F-Cl.
02

Draw Lewis structure for I2

Both I atoms have seven valence electrons. They share a pair of electrons forming a single covalent bond with each other and the remaining six electrons on each atom are lone pairs. The Lewis structure is: I-I
03

Draw Lewis structure for SF2

S has six and each F has seven valence electrons. S shares one electron with each F atom forming single covalent bonds. The remaining four electrons on S are lone pairs and the six electrons on each F atom are lone pairs. The Lewis structure is: F-S-F
04

Draw Lewis structure for NF3

N has five and each F has seven valence electrons. N shares one electron with each F atom forming single covalent bonds. The remaining two electrons on N are a lone pair and the six electrons on each F atom are lone pairs. The Lewis structure is: F\n| \nN - F\n| \nF
05

Draw Lewis structure for H2Te

Each H has one and Te has six valence electrons. Te shares one electron with each H atom forming single covalent bonds. The remaining four electrons on Te are lone pairs. The Lewis structure is: H-Te-H

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Most popular questions from this chapter

The highest bond-dissociation energy is found in (a) \(\mathrm{O}_{2} ;\) (b) \(\mathrm{N}_{2} ;\) (c) \(\mathrm{Cl}_{2} ;\) (d) \(\mathrm{I}_{2}\).

The Lewis structure of nitric acid, \(\mathrm{HONO}_{2}\), is a resonance hybrid. How important do you think the contribution of the following structure is to the resonance hybrid? Explain.

The species \(\mathrm{PBr}_{4}^{-}\) has been synthesized and has been described as a tetrahedral anion. Comment on this description.

Draw Lewis structures for the following species, indicating formal charges and resonance where applicable: (a) \(\mathrm{HOSO}_{3}\) (b) \(\mathrm{H}_{2} \mathrm{NCN}\) (c) \(\mathrm{FCO}_{2}^{-}\) (d) \(\mathrm{S}_{2} \mathrm{N}_{2}\) (a cyclic structure with \(\mathrm{S}\) and \(\mathrm{N}\) alternating)

Draw Lewis structures for the following species, indicating formal charges and resonance where applicable: (a) \(\mathrm{HCO}_{2}=\) (b) \(\mathrm{HCO}_{3}^{-}\) (c) \(\mathrm{FSO}_{3}^{-}\) (d) \(\mathrm{N}_{2} \mathrm{O}_{3}^{2-}\) (the nitrogen atoms are joined centrally with one oxygen atom on one \(\mathrm{N}\) and two on the other)
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