In its neutral state, a single iodine (I) atom has seven valence electrons. The electron configuration of iodine is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁵.
To determine the number of bonds and lone pairs in a single iodine atom, we need to consider its tendency to gain or share electrons to achieve a stable electron configuration. Iodine belongs to Group 17 (Group 7A), also known as the halogens, which typically have seven valence electrons and tend to form one covalent bond to complete their octet.
In the case of iodine, it has one unpaired electron in its outermost shell (5p⁵). Therefore, an iodine atom can form one covalent bond by sharing this unpaired electron with another atom. This bond would be represented as I·, where the dot represents the unpaired electron.
So, in summary:
- Number of bonds: 1
- Number of lone pairs: 6 (since iodine has a total of seven valence electrons, and one electron is involved in the bond, there are six remaining electrons that are not involved in bonding and thus considered lone pairs).
Keep in mind that this description is for a single iodine atom. In compounds, iodine can form multiple bonds and can have different arrangements of lone pairs depending on the specific molecule or ion it is part of.