Periodic Trends Review Worksheet 1. Identify the following elements as metals, metalloids, or nonmetals. a) Ti b) Cl c) Ca d) Ge e) Eu

f) Ir

g) P

h) I

2. Give the name of the family that the following elements belong to: a) Rb b) O c) Kr d) Mg e) In

f) P

g) I

h) Th

i) Co

j) Ce

k) Al

l) Au

3. Why do elements in the same group/family generally have the same properties?

Atomic/Ionic Radius: 4. a) Define atomic radius.

b) What is meant by effective nuclear charge? How is it calculated? c) How does the effective nuclear charge experienced by the valence electrons in an atom vary in a period? d) How does the effective nuclear charge experienced by the valence electrons in an atom vary in a group?

e) What is its trend in a period and in a group? Explain.

f) How does the size of an atom change when it forms a cation? Explain why?

g) How does the size of an atom change when it forms an anion? Explain why?

h) What is the trend of the ionic radius in a period and in a group? Ionization Energy: 5. Define ionization energy. What is its trend in a period and group? Explain the reason for the trend.

6. Explain why the following is true. I1< I2
Electron Affinity: 7. Define Electron Affinity. What is its trend in a period and group? Explain the reason for the trend.

Electronegativity: 8. Define Electronegativity. What is its trend in a period and group? Explain the reason for the trend.

9. What is the difference between ionization energy and electron affinity?

10. What is the difference between electronegativity and electron affinity?

Reactivity: 11. How does the reactivity of metals vary in a period and in a group?

12. How does the reactivity of nonmetals vary in a period and in a group? Melting point: 13. How does the melting point of elements vary in a period and in a group?

14. Arrange the following elements and explain your answer: Ca, O, Bi, Ne, Be a. In decreasing atomic radius b. In decreasing ionization energy c. In increasing electron affinity d. In decreasing electronegativity

15. Sb, Rb, K, Ru, I a. Arrange the above elements in increasing order of atomic size. b. Arrange the above elements in increasing order of electron affinity. c. Arrange the above elements in decreasing order of ionization energy. Explain your answer in each case.

16. Explain why cesium is more reactive to water than lithium.

17. Explain why chlorine is more reactive to potassium metal than iodine.

18. Arrange the given elements in decreasing electronegativity. Explain your answer.

19. Arrange the given species in increasing size. Explain your answer.

20. Arrange the following in decreasing size. Explain your answer.

N, Cu, Bi, As, P

K , K+, Kr, Br

Te-2, S-2, Se-2, O-2

21. Explain why it is harder to remove an inner shell electron than a valence electron from an atom.

22. Explain why calcium forms a +2 ion (Ca+2) but Bromine forms a -1 ion (Br -).

23. Which element of the given elements has the largest jump in ionization energy between IE3 and IE4? Explain why? Rb, N, Be, V, Al

24. The first electron affinity value for the element X is - 142 kJ/mol and its second electron affinity value is + 844 kJ/mol. Explain what this means.

25. The first ionization energy of Xe and the electron affinity of Xe are both positive values. What does this positive value tell you in each case?