Question

Be sure to answer all parts. Dichlorine heptaoxide, Cl2O7, can be viewed as two ClO4 groups sharing an O atom. Draw a Lewis structure for Cl2O7 with the lowest formal charges and predict any deviation from the ideal for the Cl―O―Cl bond angle. Be sure to include lone-pair electrons.

Answer 1

Explanation:

Dichlorine heptaoxide ($Cl_{2}O_{7}$) can also be written as $OCl_{2}O_{6}$ as one oxygen atom will be at the center and there will be two terminal $ClO_{3}$ groups.

This dichlorine heptaoxide is electrically neutral as there is no charge on this compound.

Number of valence electrons in an oxygen atom are 6, valence electrons in a chlorine atom are 7.

Hence, total number of valence electrons in $OCl_{2}O_{6}$ will be as follows.

       Total valence electrons = $(1 \times 6) + (2 \times 7) + (1 \times 6)$

                                                = 56

Lewis structure of $Cl_{2}O_{7}$ will have one oxygen atom at the center and two terminal $ClO_{3}$ groups. Each oxygen atom in will have 2 lone pair of electrons and oxygen atoms of $ClO_{3}$ groups will be attached to chlorine atoms through double bonds.

Answer 2

The Lewis structure shows the arrangement of valence electrons in atoms in a molecule.

The Lewis structure of a molecule is a diagram that shows the valence electrons in a molecule as dots. A Lewis structure shows the symbol of an element and the valence electrons that surround it as well as any formal charges present.

The Lewis structure of Cl2O7 is shown in which the formal charges on each atom is zero. The bond angle of the central Cl-O-Cl bond is 119° while the bond angle of the Cl-O-Cl where there is a C=O double bond is 115°. The central chlorine atoms are sp3 hybridized.

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