Question

Describe the trends in properties for the elements belonging to Group VI A in the periodic table. How do the following properties vary down the group?

a. Atomic Radius

b. 1st Ionization Energy

c. Electron Affinity

d. Oxidation number

e. Electronic Configuration starting from the preceding noble gas configuration

Answer 1

a) the atomic radius is increased for elements in down the VI A group (with increasing atomic weight) O: 140, S: 184, Se:198, Te:221

b) & c) 1st ionization energy and Electron affinity is decreases for elements in down the VI A group (with increasing atomic weight) Ionization Energy of O: 1314, S: 1000, Se: 941, Te: 869, Po: 812.

oxidation state (oxidation number) is incraeses or elements in down the VI A group (Oxygen: -2, sulfur: +4 and +6 Se, Te, and Po: +2, +4, and +6)

MW Electron Configuration

4             Helium: 2s² 2p⁶

16          Oxygen: 1s² 2s² 2p⁴

32           Sulfur: 1s² 2s²p⁶ 3s²p⁴

78           Selenium: 1s² 2s²p⁶ 3s²p⁶d¹⁰ 4s²p⁴

128         Tellurium: 1s² 2s²p⁶ 3s²p⁶d¹⁰ 4s²p⁶d¹⁰ 5s²p⁴

210         Polonium: 1s² 2s²p⁶ 3s²p⁶d¹⁰ 4s²p⁶d¹⁰f¹⁴ 5s²p⁶d¹⁰ 6s²p⁴