Chapter 8: Problem 66

Consider the ionic bonds between \(\mathrm{Na}^{+}\) ions and \(\underline{\mathrm{Cl}}^{-}\) ions in \(\mathrm{NaCl}(\mathrm{s}) .\) Why must energy be added to break these bonds (in other words, what is the added energy used for)?

Short Answer

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In summary, to break the ionic bonds between Na+ and Cl- ions in NaCl, energy must be added to overcome the strong electrostatic attractive forces between these oppositely charged ions. This energy input is needed to separate the ions, allowing them to move more freely and potentially form new bonds or exist as individual ions. The bond-breaking process is endothermic, meaning it absorbs energy, in contrast to the exothermic bond formation process, which releases energy.

Step by step solution

Understanding the ionic bond and its stability

Ionic bond is an electrostatic attraction between oppositely charged ions. In NaCl, Na+ and Cl- ions are held together through ionic bonding. This bond is formed when one or more electrons are transferred from one atom (Na) to another (Cl). The ionic bond is stable because there's a balance of attractive forces between the positive (cation) and negative (anion) ions and repulsive forces between ions of the same charge.

Energy changes in bond formation and breaking

In order to form an ionic bond, energy is released as the ions come together and become attracted to each other. This energy release is called the lattice energy. The bond formation process is exothermic, meaning it releases energy. On the other hand, breaking an ionic bond requires adding energy to the system. This is necessary to overcome the attractive forces between the ions. The process of breaking a bond is endothermic, meaning it absorbs energy.

Explaining the need for added energy to break ionic bonds

To break the ionic bonds between Na+ and Cl- ions in NaCl, energy must be added to counteract the attractive forces between the ions. The added energy is used to overcome these attractive forces and separate the ions. Once the ions are separated, they can move more freely and potentially form new bonds or exist as individual ions. In conclusion, energy must be added to break the ionic bonds between Na+ and Cl- ions in NaCl because this energy is required to overcome the attractive forces holding the ions together in the stable, bonded state.

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Consider the ionic bonds between \(\mathrm{Na}^{+}\) ions and \(\underline{\mathrm{Cl}}^{-}\) ions in \(\mathrm{NaCl}(\mathrm{s}) .\) Why must energy be added to break these bonds (in other words, what is the added energy used for)?

Short Answer

Step by step solution

Understanding the ionic bond and its stability

Energy changes in bond formation and breaking

Explaining the need for added energy to break ionic bonds

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