Practice Exam Problems: Periodic Trends
Periodic Trends Review
1. Rank the following in order of increasing ionization energy: S, F, Rb, Zn,
2. Fill in the table below. (Isoelectronic – equal number of electrons.)
|Ground state electron configuration |Neutral atom |Isoelectronic |Isoelectronic |Isoelectronic |Isoelectronic |
| | |2+ ion |3- ion |1+ ion |1- ion |
| |Ne | | | | |
| | |Ba2+ | | | |
| | | |P3- | | |
3. Name an element that requires more energy to ionize than Rb. ___________________________________
4. Name an element that requires less energy to ionize than Rb. ___________________________________
5. Why does removing a second electron from Cs require significantly more energy than removing the first?
6. Circle the atom of each pair with the greater electronegativity.
Na or Rb Al or F Ge or Ba
7. Using your knowledge of atomic structure and attraction, explain the following statements.
a. Potassium has a lower first-ionization energy than lithium.
b. A calcium atom is larger than a zinc atom
c. The radius of N3- is larger than the radius of N.
d. Fluorine is more electronegative than iodine.
e. O2- is smaller than N3-
8. The ionization energies (kJ/mol) for three third period elements are given in the table below. Identify each of the elements.
| |IE1 |IE2 |IE3 |IE4 |IE5 |IE6 |Element? |
|A |1,012 |1,903 |2,912 |4,957 |6,274 |21,269 | |
|B |496 |4,562 |6,912 |9,544 |13,353 |16,610 | |
|C |578 |1,817 |2,745 |11,578 |14,831 |23,295 | |
9. Would you expect the ions, Li+, Na+, ...Cs+ to be smaller or larger than the neutral atoms? Explain.
10. Sodium atoms are larger than fluorine atoms, but sodium ions are smaller than fluorine ions. Offer an explanation.
11. Four elements of atomic numbers 17, 18, 19, and 20 have first ionization energies of 1500, 600, 400 and 1300 kJ/mol (listed in random order) Which ionization energy belongs to which element?
12. Based on their positions in the periodic table, predict which atom of the following pairs will have the larger radius:
a. O, Ne b. Mg, Sr c. K, Cr d. Br, Sb e. Ga, Ge
13. Decide if the following atoms would be paramagnetic or diamagnetic based on their position on the periodic table.
a. Ca
b. Zn
c. Mn
d. P
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