Question

The seven diatomic elements (exist as two atoms bonded together in nature) are hydrogen (H2), Nitrogen (N2), Oxygen (O2), Fluorine (F2), Chlorine (C2), Iodine (I2) and Bromine (B2). Based on the position of the seven elements that are diatomic when pure in nature and the trends of the periodic table, which of the following characteristics would not describe them?

a) Smaller Atomic Radius
b) High Metallic Character
c) High Ionization Energy
d) High Electron Affinity

Answer 1

Smaller Atomic Radius, High Ionization Affinity, and High Electron Affinity

[Note: It is Br2, not B2, the bomber]

Step-by-step explanation:

a) Smaller Atomic Radius YES Each of these elements have a high number of electrons that nearly fill the lower energy orbitals, forcing the protons in the nucleus to cluster togeter more tightly.

b) High Metallic Character NO

c) High Ionization Energy YES - They want to keep their electrons, so the ionization energy is high.

d) High Electron Affinity YES They attract electons from anything that comes nearby.