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Chapter 37: Problem 3

Ionic bonds clearly result from electrostatic attraction between ions. In what way do covalent bonds also involve electrostatic attraction?

Short Answer

Expert verified
Covalent bonds involve electrostatic attraction between the positively charged atomic nuclei and the negatively charged shared electrons.

Step by step solution

01

Understanding Covalent Bonds

A covalent bond is a chemical bond that involves the sharing of electron pairs between atoms. These shared electrons are known as bonding pairs.
02

Electrostatic Attraction in Covalent Bonds

Although in covalent bonds, electrons are shared between atoms instead of transferred from one atom to another (as in ionic bonds), there is still the presence of electrostatic forces. The positively charged nuclei of the bonded atoms are attracted to the shared (negatively charged) electron pair, thus creating an electrostatic attraction.
03

Clarification of Electrostatic Attraction in Covalent Bonds

In essence, while ionic bonds involve electrostatic attraction between oppositely charged ions, covalent bonds involve electrostatic attraction between the positively charged atomic nuclei and the negatively charged shared electrons.

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Most popular questions from this chapter

Name some technological innovations that might result from a room-temperature superconductor.

The lower-energy states in a covalently bound diatomic molecule can be found approximately from the so-called Morse potential \(U(r)=U_{0}\left(e^{2\left(r-r_{0}\right) / a}-e^{-2\left(r-r_{0}\right) / a}\right),\) where \(r\) is the atomic separation and \(U_{0}, r_{0},\) and \(a\) are constants determined from experimental data. Calculate \(d U / d r\) and \(d^{2} U / d r^{2}\) to show that \(U\) has a minimum, and find expressions for (a) \(U_{\min }\) and (b) the separation \(r_{\min }\) at the minimum energy.

Suppose a room-temperature superconductor were discovered. but it had a very low critical field. In what way would this limit its practical applicability?

Why is the exclusion principle crucial to the existence of stable molecules?

Would you expect solid hydrogen to conduct electricity? Why or why not?
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