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Chapter 5: Problem 64

Suppose one of the electrons from the covalent bond in \(\mathrm{H}_{2}\) suddenly vanished. Why would the bond between the atoms weaken?

Short Answer

Expert verified
In conclusion, if one of the electrons from the covalent bond in \(H_{2}\) suddenly vanished, the bond between the hydrogen atoms would weaken because the remaining shared electron wouldn't provide a strong enough electrostatic attraction to hold the two atoms together in a stable bond.

Step by step solution

01

Understand Covalent Bonding

A covalent bond is a type of chemical bond formed between two non-metal atoms when they share a pair of valence electrons. This sharing of electrons allows both atoms to achieve a stable electron configuration, typically with eight electrons in their outermost shell (octet rule). In the case of H₂, the covalent bond is formed between two hydrogen atoms, each contributing one electron to the shared pair of electrons.
02

Role of Shared Electrons in Bond Strength

The strength of a covalent bond largely depends on the shared electron pair, which maintains the electrostatic attraction between the positively charged nuclei of the bonded atoms and the negatively charged shared electrons. This electrostatic attraction, known as a bond, holds the atoms together and brings stability to the molecule.
03

Effect of Vanishing Electron on Covalent Bond

If one of the electrons from the covalent bond in H₂ were to suddenly vanish, the bond would be left with only one shared electron instead of the necessary pair. This would reduce the strength of the electrostatic attraction between the two hydrogen nuclei and the remaining shared electron. As a result, the bond between the atoms would weaken, making the molecule less stable and more prone to break apart. In conclusion, the bond between the hydrogen atoms in H₂ would weaken if one of the shared electrons suddenly vanished because the remaining shared electron wouldn't provide a strong enough electrostatic attraction to hold the two atoms together in a stable bond.

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Most popular questions from this chapter

Chlorine (Cl), neon (Ne), and helium (He) all exist as gases, but only one of them is diatomic. Which is it, and why is it diatomic while the others are monatomic?

The use of chlorofluorocarbons (CFCs) in airconditioning and refrigeration systems has been linked to depletion of the ozone layer of the atmosphere. One of the most widely used CFCs, freon-12, has the formula \(\mathrm{CF}_{2} \mathrm{Cl}_{2}\). It is now being replaced with a compound that has the formula \(\mathrm{CH}_{2} \mathrm{FCH}_{3}\). Draw the dot diagrams for \(\mathrm{CF}_{2} \mathrm{Cl}_{2}\) and \(\mathrm{C} \mathrm{H}_{2} \mathrm{FCH}_{3}\). (Hint: In \(\mathrm{CH}_{2} \mathrm{FCH}_{3}\), the carbons bond to each other, and one of them bonds to fluorine.)

Many acids can be thought of as anions that have an \(\mathrm{H}^{+}\) ion attached to them. Fill in the following table: \begin{tabular}{|l|l|l|l|} \hline Anion & Anion name & Acid formula & Acid name \\ \hline \(\mathrm{F}^{-}\) & & & \\ \hline \(\mathrm{NO}_{3}^{-}\) & & & \\ \hline \(\mathrm{Cl}^{-}\) & & & \\ \hline \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\) & & & \\ \hline \(\mathrm{NO}_{2}^{-}\) & & & \\ \hline \end{tabular}

Consider sulfur trioxide. (a) Draw a dot diagram that obeys the octet rule for all of the atoms. (b) Suppose the actual bond order for the \(\mathrm{S}-\mathrm{O}\) bonds was \(2 .\) Draw a dot diagram that explains this, using the concept of expanded octet. Also state whether expanding the octet as you have shown would be allowed, and why.

Chemists sometimes think of molecules with polar covalent bonds as being part covalent and part ionic. How can a bond be both covalent and ionic?
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