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Chapter 9: Problem 58

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

Short Answer

Expert verified
A coordinate covalent bond is one in which both shared electrons come from the same atom, whereas in a normal covalent bond, each atom provides one electron for the bond. Thus, while they are both types of covalent bonds, the source of the shared electrons differs.

Step by step solution

01

Define a Coordinate Covalent Bond

A coordinate covalent bond, also known as a dative bond, is a type of covalent bond where the two electrons shared between two atoms are contributed by one of the bonding atoms. This generally happens when one atom (the donor) has a lone pair of electrons that could be potentially shared, and the other atom (the acceptor) has an empty orbital ready to accept the electrons.
02

Define a Covalent Bond

A normal covalent bond, on the other hand, is a type of chemical bond where two atoms share a pair of electrons with each other. This sharing generally occurs so that the atoms can have a full outermost electron shell and reach a more stable electronic configuration.
03

Highlight the Differences

The primary difference between the coordinate covalent bond and the normal covalent bond lies in the origin of the shared electrons. In a coordinate covalent bond, both shared electrons originate from the same atom, while in a covalent bond, one electron from each atom participates in forming the bond.

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Most popular questions from this chapter

The species \(\mathrm{H}_{3}^{+}\) is the simplest polyatomic ion. The geometry of the ion is that of an equilateral triangle. (a) Draw three resonance structures to represent the ion. (b) Given the following information and $$ \begin{aligned} 2 \mathrm{H}+\mathrm{H}^{+} \longrightarrow \mathrm{H}_{3}^{+} & \Delta H^{\circ}=-849 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{H}_{2} \longrightarrow 2 \mathrm{H} & \Delta H^{\circ}=436.4 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$ calculate \(\Delta H^{\circ}\) for the reaction $$ \mathrm{H}^{+}+\mathrm{H}_{2} \longrightarrow \mathrm{H}_{3}^{+} $$

What is a polar covalent bond? Name two compounds that contain one or more polar covalent bonds.

Draw Lewis structures of these organic molecules: (a) tetrafluoroethylene \(\left(\mathrm{C}_{2} \mathrm{~F}_{4}\right)\) (b) propane \(\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)\) (c) butadiene \(\left(\mathrm{CH}_{2} \mathrm{CHCHCH}_{2}\right.\) ), (d) propyne \(\left(\mathrm{CH}_{3} \mathrm{CCH}\right),\) (e) benzoic acid \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\right) .\) (Hint: To draw \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\), replace an \(\mathrm{H}\) atom in benzene with a COOH group.)

Of the noble gases, only \(\mathrm{Kr}, \mathrm{Xe},\) and \(\mathrm{Rn}\) are known to form a few compounds with \(\mathrm{O}\) and/or \(\mathrm{F}\). Write Lewis structures for these molecules: (a) \(\mathrm{XeF}_{2},\) (b) \(\mathrm{XeF}_{4}\) (c) \(\mathrm{XeF}_{6},\) (d) \(\mathrm{XeOF}_{4},\) (e) \(\mathrm{XeO}_{2} \mathrm{~F}_{2}\). In each case Xe is the central atom.

Because fluorine has seven valence electrons \(\left(2 s^{2} 2 p^{5}\right),\) seven covalent bonds in principle could form around the atom. Such a compound might be \(\mathrm{FH}_{7}\) or \(\mathrm{FCl}_{7}\). These compounds have never been prepared. Why?
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