Choose the correct condensed electronic configuration for Iodine with atomic number 53.[Kr] 4d10 5s2 5p5[Ar] 4d10 5s2 5p5[Kr] 5s2 5p5[Kr] 5d10 6s2 6p5

The correct condensed electronic configuration for Iodine (atomic number 53) is [Kr] 4d10 5s2 5p5.

Here's the step-by-step explanation:

1. The atomic number of Iodine is 53, which means it has 53 electrons in its neutral state.

2. The noble gas that precedes Iodine in the periodic table is Krypton (Kr), which has an atomic number of 36. So, the electron configuration of Iodine starts with [Kr].

3. After [Kr], the electrons fill up the 4d, 5s, and 5p orbitals.

4. The 4d orbital can hold up to 10 electrons, the 5s orbital can hold up to 2 electrons, and the 5p orbital can hold up to 6 electrons.

5. However, Iodine only has 17 more electrons to distribute after [Kr] (53 total electrons - 36 electrons already accounted for in [Kr] = 17 electrons left).

6. These 17 electrons fill up the 4d, 5s, and 5p orbitals in the following way: 10 go into the 4d orbital, 2 go into the 5s orbital, and the remaining 5 go into the 5p orbital.

So, the correct condensed electronic configuration for Iodine is [Kr] 4d10 5s2 5p5.