Answer
See explanation
Work Step by Step
To prove mathematically that it is more energetically favorable for a fluorine atom to take an electron from a sodium atom than from another fluorine atom, we would compare the energy released when fluorine gains an electron to form F- with the energy required to remove an electron from another fluorine atom to form F+. The difference in energy, known as the electron affinity, should be negative for the formation of F- (energy is released), indicating that fluorine readily gains an electron. For F+, the electron affinity would be positive, indicating that it requires energy to remove an electron from fluorine, making it less favorable compared to gaining an electron from sodium.
