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Chapter 8 - Periodic Trends - Part 2 Electron Affinity The electron affinity (EA) of an atom is the energy change associated with the gaining of an electron by the atom in the gaseous state. Cl(g) + 1 e? ? Cl?(g) E A= -349 kJ/mol 1. The electron affinity of an atom is usually negative (but not always). Does the atom absorb or release energy when it gains an electron? 2. Which atom is more likely to gain an electron, Li or F? Why? 3. Which atom would have a larger (i.e. more negative) electron affinity, Li or F? Why? Periodic Trends in Electron Affinity 4. What is the trend in electron affinity as you move from left to right along a given period? 5. Which group on the periodic table has the most negative electron affinities? Explain why (in terms of electron configurations). 6. Why do you think the noble gases have a positive electron affinity? (hint: think about the electron configurations of the noble gases) 7. Why do you think Nitrogen has a positive electron affinity? (hint: think about the electron configuration of nitrogen)

          Chapter 8 - Periodic Trends - Part 2

Electron Affinity

The electron affinity (EA) of an atom is the energy change associated with the gaining of an electron by the atom in the gaseous state.

Cl(g) + 1 e? ? Cl?(g) E A= -349 kJ/mol

1. The electron affinity of an atom is usually negative (but not always). Does the atom absorb or release energy when it gains an electron?

2. Which atom is more likely to gain an electron, Li or F? Why?

3. Which atom would have a larger (i.e. more negative) electron affinity, Li or F? Why?

Periodic Trends in Electron Affinity

4. What is the trend in electron affinity as you move from left to right along a given period?

5. Which group on the periodic table has the most negative electron affinities? Explain why (in terms of electron configurations).

6. Why do you think the noble gases have a positive electron affinity? (hint: think about the electron configurations of the noble gases)

7. Why do you think Nitrogen has a positive electron affinity? (hint: think about the electron configuration of nitrogen)

Chapter 8 - Periodic Trends - Part 2

Electron Affinity

The electron affinity (EA) of an atom is the energy change associated with the gaining of an electron by the atom in the gaseous state.

Cl(g) + 1 e? ? Cl?(g) E A= -349 kJ/mol

1. The electron affinity of an atom is usually negative (but not always). Does the atom absorb or release energy when it gains an electron?

2. Which atom is more likely to gain an electron, Li or F? Why?

3. Which atom would have a larger (i.e. more negative) electron affinity, Li or F? Why?

Periodic Trends in Electron Affinity

4. What is the trend in electron affinity as you move from left to right along a given period?

5. Which group on the periodic table has the most negative electron affinities? Explain why (in terms of electron configurations).

6. Why do you think the noble gases have a positive electron affinity? (hint: think about the electron configurations of the noble gases)

7. Why do you think Nitrogen has a positive electron affinity? (hint: think about the electron configuration of nitrogen)

Added by Eric H.

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