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Chapter 9: Problem 83

A rule for drawing plausible Lewis structures is that the central atom is invariably less electronegative than the surrounding atoms. Explain why this is so.

Short Answer

Expert verified
The central atom is less electronegative in Lewis structures because it needs to share more electrons to complete its octet. This sharing allows for better electron distribution and overall stability in the molecule.

Step by step solution

01

Understanding Electronegativity

Electronegativity refers to the ability of an atom to attract shared electrons in a bond towards itself. The more electronegative an atom is, the more it will tend to attract electrons.
02

Understanding Lewis Structures

In a Lewis structure, atoms share electrons to achieve a full octet (8 valence electrons), leading to more stability. The atom at the center is usually the one that needs the most electrons to complete its octet.
03

Analysis of Electronegativity and Lewis Structures

In a Lewis structure, the less electronegative atom is usually placed in the center because it can better 'handle' shared electrons. If the more electronegative atom were in the center, it would tend to pull the shared electrons closer to itself, resulting in an unbalanced electron distribution and a less stable molecule.

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Most popular questions from this chapter

Use Lewis dot symbols to show the transfer of electrons between the following atoms to form cations and anions: (a) \(\mathrm{Na}\) and \(\mathrm{F},\) (b) \(\mathrm{K}\) and \(\mathrm{S},\) (c) \(\mathrm{Ba}\) and \(\mathrm{O}\), (d) \(\mathrm{Al}\) and \(\mathrm{N}\).

Draw Lewis structures for these chlorofluorocarbons (CFCs), which are partly responsible for the depletion of ozone in the stratosphere: \(\mathrm{CFCl}_{3}, \mathrm{CF}_{2} \mathrm{Cl}_{2}\), \(\mathrm{CHF}_{2} \mathrm{Cl}, \mathrm{CF}_{3} \mathrm{CHF}_{2}\).

Without referring to Figure 9.1 , write Lewis dot symbols for atoms of the following elements: (a) Be, (b) \(\mathrm{K},\) (c) \(\mathrm{Ca},\) (d) \(\mathrm{Ga},\) (e) \(\mathrm{O},\) (f) \(\mathrm{Br},(\mathrm{g}) \mathrm{N},(\mathrm{h}) \mathrm{I},\) (i) \(\mathrm{As}\), (j) F.

Write three reasonable resonance structures of the azide ion \(\mathrm{N}_{3}^{-}\) in which the atoms are arranged as NNN. Show formal charges.

Explain what an ionic bond is.
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