Question

Use ionization energies and electron affinities listed in the text to determine whether the following reaction is endothermic or exothermic. $$ \mathrm{Mg}(\mathrm{g})+2 \mathrm{F}(\mathrm{g}) \longrightarrow \mathrm{Mg}^{2+}(\mathrm{g})+2 \mathrm{F}^{-}(\mathrm{g}) $$

Short answer

The reaction is exothermic if the total energy change calculated in step 4 is negative, and endothermic if it's positive. The precise conclusion depends on the specific values of ionization energy for Mg and electron affinity for F.

Step-by-step solution

Understand What Ionization Energy and Electron Affinity Mean

Ionization energy is the energy required to remove the most loosely held electron from an atom in the gaseous state. On the other hand, electron affinity is the energy change of an atom in the gaseous state when it gains an electron.

Find Out The Values Of Ionization Energies and Electron Affinities

The ionization energy for Magnesium (Mg) is needed, along with the electron affinity for Fluorine (F). These values are available in textbooks or reliable online resources.

Calculate The Energy Changes For Each Part Of The Reaction

In the forward reaction, two electrons are removed from a single Mg atom, which equates to two times the ionization energy for Mg. When these two electrons are accepted by two F atoms, it releases energy equal to two times the electron affinity for F.

Calculate The Total Energy Change of The Reaction

The total energy change of the reaction can be calculated by subtracting the total energy released (2 times the electron affinity for F) from the total energy required (2 times the ionization energy of Mg).

Determine Whether The Reaction Is Endothermic Or Exothermic

If the total energy change is negative, it means the reaction releases energy and is hence exothermic. If the total energy change is positive, it means the reaction requires energy and is hence endothermic.

Key concepts

Electron Affinity

Electron affinity refers to the energy change that occurs when an atom in the gas phase accepts an additional electron and becomes negatively charged. It's a measure of how much an atom wants to gain an electron. This concept is crucial in understanding chemical reactions involving electron transfer.
Atoms with a high electron affinity release a significant amount of energy when they gain an electron. Fluorine is an example of an element with a high electron affinity, meaning it strongly attracts electrons. When fluorine atoms gain electrons, they release energy, contributing to the overall energy dynamics of a chemical reaction.
To determine how electron affinity affects a reaction, consider both the energy released during electron acquisition and the energy required for the initial ionization of another atom. Understanding this balance helps in predicting whether a reaction will be endothermic or exothermic.

Endothermic vs Exothermic Reactions

Chemical reactions can either absorb or release energy. These reactions are classified as endothermic or exothermic, respectively. Understanding the difference between these two types of reactions helps predict their outcome and their effect on the surroundings.

• Endothermic Reactions: These reactions absorb energy from their surroundings. They require an input of energy, usually in the form of heat. Consequently, the products have higher energy than the reactants. This makes the overall energy change of the reaction positive. An example includes photosynthesis, where energy from sunlight is absorbed to convert carbon dioxide and water into glucose and oxygen.
• Exothermic Reactions: In contrast, exothermic reactions release energy, typically as heat. The products are lower in energy compared to the reactants, leading to a negative overall energy change. Combustion of fuels is a prime example where the energy released is significant.

In the context of the original exercise, determining whether the magnesium and fluorine reaction is exothermic or endothermic requires calculating the net energy change using ionization energies and electron affinities.

Chemical Reactions

Chemical reactions involve the transformation of substances through the breaking and forming of chemical bonds. Understanding these changes is fundamental to mastering chemistry.
When a chemical reaction occurs, substances known as reactants are transformed into products. This transformation involves electrons; atoms may lose, gain, or share electrons to achieve more stable configurations. These changes should conserve mass and energy, as dictated by the laws of conservation.
Through reactions like the one involving magnesium and fluorine, you can see these principles in action. The atoms rearrange as electrons are transferred between them, leading to changes in chemical structure and energy. By calculating energy changes using ionization and electron affinities, we gain insights into the nature of these reactions, predicting whether they are efficient and spontaneous.