Questions: Which of the following elements would have a very different electron affinity value compared to the others? A Ne B Al C O D F E Na

Solution Steps

Electron affinity is the amount of energy released when an electron is added to a neutral atom in the gaseous state to form a negative ion. Elements with high electron affinity values release more energy when they gain an electron.

The elements given in the question are:

• Ne (Neon)
• Al (Aluminum)
• O (Oxygen)
• F (Fluorine)
• Na (Sodium)

• Neon (Ne): Neon is a noble gas with a complete valence shell, making it very stable and unlikely to gain an electron. Therefore, it has a very low (or even positive) electron affinity.
• Aluminum (Al): Aluminum has a moderate electron affinity as it is a metal and tends to lose electrons rather than gain them.
• Oxygen (O): Oxygen has a high electron affinity because it is a non-metal and tends to gain electrons to complete its valence shell.
• Fluorine (F): Fluorine has the highest electron affinity among the elements listed because it is highly electronegative and readily gains an electron to achieve a stable configuration.
• Sodium (Na): Sodium, like aluminum, is a metal and has a relatively low electron affinity as it tends to lose electrons.

Neon (Ne) is a noble gas and has a very different electron affinity value compared to the other elements, which are metals or non-metals with higher tendencies to gain electrons.

Final Answer