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Chapter 9: Problem 28

What is the difference between a Lewis dot symbol and a Lewis structure?

Short Answer

Expert verified
A Lewis dot symbol represents the valence electrons of a single atom while a Lewis structure uses these symbols to display the bonding between atoms in molecules and any lone pairs of electrons.

Step by step solution

01

Definition of Lewis Dot Symbol

A Lewis dot symbol is a simplified depiction of the valence electrons in an atom. It represents an element鈥檚 symbol surrounded by dots. Each dot represents a valence electron, that is, one of the electrons in the atom鈥檚 outermost shell.
02

Definition of Lewis Structure

A Lewis structure, also called a Lewis dot diagram, uses Lewis dot symbols to demonstrate the bonding between different atoms in a molecule and the lone pairs of electrons that may exist in the molecule. The dots in this case still represent valence electrons and the lines between the atoms represent shared pairs of electrons (covalent bonds). The entire structure indicates how the atoms in a molecule are connected and interact via chemical bonds.
03

Highlighting the Difference between Lewis Dot Symbol and Lewis Structure

The primary difference between a Lewis dot symbol and a Lewis structure is that the Lewis dot symbol illustrates the valence electrons of an atom of a particular element. On the other hand, a Lewis structure uses Lewis dot symbols to show how atoms bond within molecules and also indicates the presence of lone pairs of electrons.

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Most popular questions from this chapter

For each of the following pairs of elements, state whether the binary compound they form is likely to be ionic or covalent. Write the empirical formula and name of the compound: (a) I and \(\mathrm{Cl}\), (b) \(\mathrm{Mg}\) and \(\mathrm{F}\).

Draw reasonable resonance structures for these (a) \(\mathrm{HSO}_{4}^{-},(\mathrm{b}) \mathrm{SO}_{4}^{2-},(\mathrm{c}) \mathrm{HSO}_{3}^{-}\), sulfur-containing ions: (d) \(\mathrm{SO}_{3}^{2-}\).

What is a coordinate covalent bond? Is it different from a normal covalent bond?

Four atoms are arbitrarily labeled \(\mathrm{D}, \mathrm{E}, \mathrm{F},\) and \(\mathrm{G}\). Their electronegativities are: \(\mathrm{D}=3.8, \mathrm{E}=3.3, \mathrm{~F}=\) \(2.8,\) and \(\mathrm{G}=1.3\). If the atoms of these elements form the molecules DE, DG, EG, and DF, how would you arrange these molecules in order of increasing covalent bond character?

Write Lewis structures for these four isoelectronic species: (a) CO, (b) \(\mathrm{NO}^{+},\) (c) \(\mathrm{CN}^{-},\) (d) \(\mathrm{N}_{2}\). Show formal charges.
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