Electrons and the Periodic Table Name _________________

1. What is a valence electron?_______________________________________________

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2. How many energy levels do the atoms of each of the following elements have?

Li _______ Si 3 Au _______ Fr_______

Ca _______ Pm _______ U _______ He _______

3. How many valence electrons do each of the following atoms have?

Ca _______ Pb 4 Br _______ P _______

K _______ He _______ O _______ Al _______

4. Which element has atoms with...

seven valence electrons in the fourth energy level? Br

two valence electrons in the seventh energy level?__________

four valence electrons in the third energy level?___________

one valence electrons in the sixth energy level?___________

five valence electrons in the fourth energy level?__________

eight valence electrons in the fifth energy level?__________

5. What is ionization energy? _______________________________________________________

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6. In each of the following pairs tell which atom would be the hardest to remove an electron from:

Li or K ________ Mg or Cl Cl O or Cs ________

Sn or Te________ Ne or Rn________ S or K ________

7. Why does ionization energy increase as you go from left to right across the periodic table?

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8. Why does ionization energy decrease as you go down the periodic table?

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9. In each of the following pairs tell which atom would have the largest radius:

Li or K ________ Mg or Cl________ O or Cs ________ S or K ________

10. Why do atoms get bigger as you go down the periodic table?

Hint: what are you adding to the atoms with each row on the periodic table

11. Why do atoms get smaller as you go from left to right on the periodic table?

Hint: how does the nucleus change as you go across the periodic table?

Identify each of the following as either: alkali metal, alkaline earth metal, halogen, or noble gas

12. A colorful gas that burns your eyes and throat: ________________________

13. An atom with a valence configuration of s²:__________________________

14. A colorless gas that won’t corrode metal, or sting your eyes: _______________________

15. An element that has an unpaired s electron: _____________________

16. Has an s² p⁵ configuration: _______________________

Identify each of the following as a:

representative element, transition element, or an inner transition element

17. Iron: ______________________________

18. Sulfur: ______________________________

19. Uranium: ____________________________

20. An element with a partially filled f sublevel: ________________________

21. An element with a partially filled d sublevel: ________________________

Which element has the following electron configuration

22. [Ar] 4s² 3d⁷ _______ 23. [Rn] 7s² 5f⁶ _______ 24. [Xe] 6s² 4f¹⁴ 5d¹⁰ 6p¹ _______

For each of the following elements determine which ionization energy would be significantly higher than those preceding it. Example: element: Ca answer: third

25. As: 6^th because the first five electrons were removed from the valence level, but the sixth was removed from an inner energy level

26. S: ____________ 27. Al: ____________

28. How many valence electrons does each element have? A) _______ B) _______ C) ___4___

29. Which of the following elements might have the ionization energies listed for element A?

(circle one) Li Be B C N O F Ne

30. Which of the following elements might have the ionization energies listed for element C ?

(circle one) Na Mg Al Si P S Cl Ar

Si has four valence electrons and so does Element C