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7. Explain why two fluorine atoms can form a covalent bond between themselves, while two neon atoms cannot form a covalent bond between themselves.

7. Explain why two fluorine atoms can form a covalent bond between themselves, while two neon atoms cannot form a covalent bond between themselves.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Please help answer question 7 and 8

**7. Explain why two fluorine atoms can form a covalent bond between themselves, while two neon atoms cannot form a covalent bond between themselves.** Fluorine atoms can form a covalent bond because each fluorine atom has seven electrons in its outer shell and needs one more to achieve a stable octet configuration, which they can achieve by sharing one electron with another fluorine atom. Neon atoms, on the other hand, already have a complete outer electron shell and do not need to share electrons, thus they do not form covalent bonds. **8. The curve below is the potential energy diagram as two H atoms approach each other. Does curve below look familiar and what new information can you glean from this curve?** *Potential Energy Diagram Description:* - The diagram is a graph that depicts the potential energy of two hydrogen atoms as a function of the distance between them. - The y-axis represents potential energy in kilojoules per mole (kJ/mol), and the x-axis represents the distance between the two hydrogen atoms (r). - As the hydrogen atoms approach each other, the potential energy decreases, reaching a minimum at the most stable state. This point is labeled as having a bond length of 74 pm and a potential energy of -436 kJ/mol, indicating the energy released when the bond is formed. - Before reaching the stable point, the curve is steep due to repulsive forces when the atoms are too close. - Past the optimal bond length, the potential energy rises as the attractive forces weaken. **Explanation of Curve:** When two hydrogen atoms come together, they experience both attractive and repulsive forces. Initially, as they approach from a distance, attractive forces dominate, lowering potential energy. However, if they come too close, repulsive forces from overlapping electron clouds increase, raising potential energy. The curve's minimum represents the most stable configuration, where the attractive forces are balanced by repulsive forces, resulting in bond formation.
Transcribed Image Text:**7. Explain why two fluorine atoms can form a covalent bond between themselves, while two neon atoms cannot form a covalent bond between themselves.** Fluorine atoms can form a covalent bond because each fluorine atom has seven electrons in its outer shell and needs one more to achieve a stable octet configuration, which they can achieve by sharing one electron with another fluorine atom. Neon atoms, on the other hand, already have a complete outer electron shell and do not need to share electrons, thus they do not form covalent bonds. **8. The curve below is the potential energy diagram as two H atoms approach each other. Does curve below look familiar and what new information can you glean from this curve?** *Potential Energy Diagram Description:* - The diagram is a graph that depicts the potential energy of two hydrogen atoms as a function of the distance between them. - The y-axis represents potential energy in kilojoules per mole (kJ/mol), and the x-axis represents the distance between the two hydrogen atoms (r). - As the hydrogen atoms approach each other, the potential energy decreases, reaching a minimum at the most stable state. This point is labeled as having a bond length of 74 pm and a potential energy of -436 kJ/mol, indicating the energy released when the bond is formed. - Before reaching the stable point, the curve is steep due to repulsive forces when the atoms are too close. - Past the optimal bond length, the potential energy rises as the attractive forces weaken. **Explanation of Curve:** When two hydrogen atoms come together, they experience both attractive and repulsive forces. Initially, as they approach from a distance, attractive forces dominate, lowering potential energy. However, if they come too close, repulsive forces from overlapping electron clouds increase, raising potential energy. The curve's minimum represents the most stable configuration, where the attractive forces are balanced by repulsive forces, resulting in bond formation.
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