Electrons and the Periodic Table Name _________________
1. What is a valence electron?_______________________________________________
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? _______________________________________________________
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?
8. Why does ionization energy decrease as you go down the periodic table?
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: 6th 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