1. Ionization Energy PRactice

2. Which has a higher first IE?
Argon (Ar) or Krypton (Kr)? WHY?

3. Which has a higher first IE?
Argon (Ar)
Fewer energy levels – valence electrons are closer to the nucleus – more attracted – harder to remove

4. Which has a lower first IE?
Calcium (Ca) or Galium (Ga)? WHY?

5. Which has a lower first IE?
Galium (Ga)
EXCEPTION
First p electron is shielded (cannot penetrate nuclear region) – is less attracted to the nucleus, so is easier to remove

6. Which has the lowest first ionization energy?
Arsenic
Selenium
Silicon
Iodine

7. Which has the lowest first ionization energy?
Iodine
Most energy levels – valence electrons are greatest distance from the nucleus – least attracted, so easiest to remove

8. Which has a lower first IE
Arsenic (As) or Selenium (Se)? WHY?

9. Which has a lower first IE
Selenium (Se)
EXCEPTION
Repulsion caused by pairing of electrons makes 4th p electron easier to remove

10. Which has the highest first ionization energy?
Magnesium
Aluminum
Sulfur
Argon

11. Which has the highest first ionization energy?
Argon
All the same energy level, so look at Zeff – greatest core charge so valence electrons are most attracted to this nucleus – hardest to remove

12. Which has a lower first IE?
Sodium (Na) or Magnesium (Mg)? WHY?

13. Which has a lower first IE?
Sodium (Na)
Same energy level, so look at Zeff – weaker core charge, so valence electrons are less attracted to the nucleus – easier to remove