Elements

Electron configuration of Iodine (I)

Read the Iodine electron configuration, noble-gas shorthand, valence shell, orbital filling logic, and the mistakes to avoid when writing I.

Guide: Guía práctica Read: 5 min Updated: 2026-06-27

Element guide

Electron configuration of Iodine (I)

The electron configuration of Iodine is 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p5. In shorthand form it is written as [Kr] 4d10 5s2 5p5.

Use this page to connect the notation with atomic number 53, the p-block, and the valence pattern 5s2 5p5.

How to write the configuration

Configuration at a glance

Iodine has atomic number 53, so a neutral atom has 53 electrons. The configuration 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p5 records where those electrons sit by subshell.

The shorthand [Kr] 4d10 5s2 5p5 replaces the filled krypton core with the noble-gas symbol.

Step-by-step filling

After krypton (36 electrons), 17 more electrons need placement. These fill in this order: 5s2 (2), 4d10 (10), 5p5 (5). The 4d subshell fills completely before the 5p subshell begins. Iodine is one electron short of a full 5p6, making it a halogen.

Step-by-step filling walkthrough: 1. Start with atomic number 53. 2. Fill through krypton: up to 4p6 (36 electrons). 3. Fill 5s2 (38). 4. Fill 4d10 (48). 5. Fill 5p5 (53). 6. Verify: add every superscript and confirm the total equals 53.

Orbital diagram and valence meaning

An orbital diagram turns each subshell into boxes and arrows. Iodine has one unpaired electron in the 5p subshell. The valence clue for I is 5s2 5p5.

As a halogen (group 17), Iodine typically gains one electron to form I-, achieving the stable noble-gas configuration of Xenon. Iodine can also form positive oxidation states (+1, +3, +5, +7) in compounds with more electronegative elements.

Common mistakes

The first mistake is misplacing the 4d10 electrons. The sequence goes: 5s2, then 4d10, then 5p5. The second mistake is forgetting that Iodine has unpaired electrons. With 5p5, there is exactly one unpaired electron in the p subshell.

A third common error is writing the shorthand as [Kr] 5s2 5p5 without including 4d10. The shorthand [Kr] 4d10 5s2 5p5 is the correct and complete notation.

Iodine reference table

Item Value
Atomic number 53
Full configuration 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p5
Noble-gas notation [Kr] 4d10 5s2 5p5
Valence clue 5s2 5p5
Block p-block

Use the table as a learning reference, then verify advanced oxidation-state questions with your course material.

Before you submit an answer

  • The superscripts add up to 53 for a neutral Iodine atom.
  • The notation follows the filling order used in your course.
  • The last occupied subshell matches the periodic-table block.
  • Any transition-metal or actinide exception is checked against a reference.
  • The shorthand core is a noble gas, not a random previous element.

Common questions

What is the electron configuration of Iodine?

The neutral Iodine atom is written as 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p5. The shorthand form is [Kr] 4d10 5s2 5p5.

How many valence electrons does Iodine have?

Start from the outer-shell clue 5s2 5p5. For main-group elements this gives a direct valence count of 7 valence electrons.

Should I memorize this configuration?

Memorize the filling pattern first. Individual configurations become easier when you can rebuild them from atomic number, noble-gas cores, and periodic-table position.

Why does Iodine have unpaired electrons?

With five electrons in the 5p subshell, Hund's rule dictates that each of the three 5p orbitals gets one electron before pairing. This leaves exactly one unpaired electron in the 5p subshell.

Study notes and practice checks

From answer to understanding

Iodine is the heaviest stable halogen and an essential trace element for human health (thyroid function). Its electron configuration [Kr] 4d10 5s2 5p5 shows it is one electron short of a full p subshell.

Practice comparison

Compare Iodine (I) with Tellurium (Te) and Xenon (Xe). Te: [Kr] 4d10 5s2 5p4, I: [Kr] 4d10 5s2 5p5, Xe: [Kr] 4d10 5s2 5p6. The series shows the p subshell filling across period 5.

Teacher and self-study notes

Iodine is useful for teaching variable oxidation states. Unlike lighter halogens, Iodine can access +7 (e.g., in H5IO6 or IF7) because of available d orbitals for expanded octet bonding.

Elena Marquez

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Elena Marquez

Chemistry educator and study-guide editor

Elena explains electron configurations, orbital diagrams, and periodic trends for learners who need clear steps before memorization. Her guides focus on counting, notation, and common classroom mistakes.

Credenciales: Editorial specialization in introductory chemistry, periodic trends, and student reference material.

Experiencia: More than eight years preparing practical chemistry explainers, worksheets, and reference material for independent learners.

Actualizado: 2026-06-27 Politica editorial Correcciones

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