1. Periodic Table Trends

2. Atomic Radius
Half the distance between the nuclei of two identical atoms bonded together

3. Atomic Radius

4. Atomic Radius Across a Period= DECREASES Down a Group=INCREASES
As you add more protons, the attractive force of the nucleus increases, pulling electrons in more closely
Down a Group=INCREASES
As you add more energy levels, the size of the electron cloud increases

5. Which of the elements would have the largest radius?
13-Aluminum
14-Silicon
17-Chlorine
12- Magnesium
16-Sulfur 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

6. Ionization Energy
The energy required to remove one electron from a neutral atom.
High I.E. – Harder to lose
electrons
Low I.E. –Easier to lose

7. Ionization Energy

8. Ionization Energy Across a Period=INCREASES Down a Group=DECREASES
Electrons are closer to nucleus, therefore harder to remove
Down a Group=DECREASES
Electrons are farther from the nucleus, therefore easier to remove

9. Which element would have the lowest ionization energy?
20- Calcium
56- Barium
4- Beryllium
38- Strontium
12-Magnesium 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

10. Electron Affinity
The energy released when a neutral atom acquires an electron.
Elements that really want another electron tend to release more energy (higher E.A.)
Across a period= INCREASES
Down a group= DECREASES

11. Electronegativity The ability of an atom to attract electrons
The most electronegative element is fluorine
Across a Period= INCREASES
Down a Group= DECREASES

12. Which of the elements would have the highest electronegativity?
13-Aluminum
14-Silicon
17-Chlorine
12- Magnesium
16-Sulfur 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

13. Ionic Radius Cations- Smaller than atomic radius
Anions- Larger than atomic radius

14. Which of the following would have the larger radius?
17-Chlorine
17-Chlorine Ion 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

15. Which of the following would have the larger radius?
11-Sodium
11-Sodium Ion 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

16. Which of the following would have the smaller radius?
3-Lithium
3-Lithium Ion 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

17. Fluorine Francium METALS vs NONMETALS NONMETALLIC CHARACTER
High I.E. (don’t want to lose e-)
High E.N. (tend to gain e-)
Dull (no luster)
Poor Conductors
Brittle as solids
MOST NONMETALLIC ELEMENT:
METALLIC CHARACTER
Lower I.E. (tend to lose e-)
Lower E.N. (don’t want e-)
High Luster (shiny!)
Good Conductors
Malleable and Ductile
MOST METALLIC ELEMENT:
Francium
Fluorine

19. Which of the elements would be the least reactive metal?
13-Aluminum
14-Silicon
17-Chlorine
12- Magnesium
16-Sulfur 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

20. Which of the elements would be the most reactive nonmetal?
13-Aluminum
14-Silicon
17-Chlorine
12- Magnesium
16-Sulfur 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

21. 37-Rubidium would have all of the following characteristics except?
High Conductivity
High Malleability
High Brittleness
Solid at Room Temperature
1 Valence Electron 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

22. 35-Bromine would have which one of the following characteristics?
High Conductivity
High Malleability
High Brittleness
Solid at Room Temperature
7 Valence Electrons 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30