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Electron configuration of Ruthenium (Ru)

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

Guide: Guía práctica Read: 7 min Updated: 2026-06-19
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Element guide

Electron configuration of Ruthenium (Ru)

The electron configuration of Ruthenium is 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d7 5s1. In shorthand form it is written as [Kr] 4d7 5s1.

Use this page to connect the notation with atomic number 44, the d-block, and the valence pattern 5s1.

How to write the configuration

Configuration at a glance

Ruthenium has atomic number 44, so a neutral atom has 44 electrons. The configuration 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d7 5s1 is a compact record of where those electrons sit by subshell. The number before each letter is the principal energy level, the letter names the subshell, and the superscript tells you how many electrons are assigned there.

The shorthand [Kr] 4d7 5s1 replaces the filled inner core with the previous noble gas. That notation keeps attention on the electrons that usually explain bonding, ions, and periodic trends.

Ruthenium's electron configuration

Ruthenium is a transition metal in group 8, period 5. Its ground-state configuration is [Kr] 4d7 5s1, which is an exception to the simple Aufbau expectation of [Kr] 4d6 5s2. The stability gained from having the 4d subshell one electron closer to half-filled causes one 5s electron to move into 4d.

For Ruthenium: the Aufbau sequence through krypton gives [Kr], then fill 5s2 4d6. However, the measured ground state promotes one 5s electron to 4d, resulting in 4d7 5s1.

Step-by-step filling walkthrough: 1. Start with atomic number 44. 2. Follow the Aufbau sequence: fill 1s, 2s, 2p, 3s, 3p, then continue through 4s, 3d, 4p in order (or 5s, 4d, 5p for period 5). 3. Keep a running total of electrons after each subshell. 4. Write the noble-gas shorthand by replacing the filled core with the previous noble gas in brackets. 5. Verify: add every superscript and confirm the total equals 44.

Real-world applications

Ruthenium's configuration with a partially filled 4d subshell (4d7) gives it useful catalytic and electronic properties: - Hard disk drive read heads (giant magnetoresistance layers) - Electrical contacts and thick-film resistors - Catalysts for ammonia synthesis and hydrogenation - Platinum-group metal alloys for corrosion-resistant equipment - Ruthenium-based chemotherapy drugs

Common oxidation states: Ru3+ ([Kr] 4d5) and Ru4+ ([Kr] 4d4). The 4d electrons are progressively removed. Ruthenium can reach Ru8+ in ruthenium tetroxide (RuO4), unusual for a d-block element.

Common exam questions

- Q: What is the electron configuration of ruthenium? A: Full: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d7 5s1. Shorthand: [Kr] 4d7 5s1.

- Q: Why is ruthenium's configuration [Kr] 4d7 5s1 instead of [Kr] 4d6 5s2? A: Moving one 5s electron into 4d gives a configuration closer to half-filled (4d7 versus 4d6).

- Q: Is ruthenium paramagnetic? A: Yes. The 4d7 subshell has unpaired electrons (Hund's rule: five d orbitals get one electron each first, then pairing begins).

How to read the subshells

Read the configuration in filling-order language first, not as a simple shell list. For transition metals, the s subshell of the outermost shell fills before the d subshell of the previous shell, but ions always lose the outer s electrons first. Keeping these two ideas separate prevents many wrong answers on ion configuration questions.

For Ruthenium, the valence clue is 5s1. The element sits in period 4 and belongs to the d-block.

Orbital diagram

An orbital diagram turns each subshell into boxes and arrows. Each orbital receives one electron before pairing when several equal-energy orbitals are available (Hund's rule).

For Ruthenium, draw the diagram by filling each subshell in Aufbau order and applying Hund's rule within p and d subshells. Count the unpaired electrons — this determines magnetic properties and influences common oxidation states.

Common mistakes

The first mistake is counting the superscripts incorrectly. Add every superscript and confirm the total equals the atomic number for a neutral atom. The second mistake is writing orbitals in shell order (e.g., 3d before 4s) and ignoring the filling sequence. The third mistake is forgetting that when writing ion configurations, the outer s electrons are removed before the inner d electrons, even though the s subshell filled first.

Ruthenium reference table

Item Value
Atomic number 44
Full configuration 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d7 5s1
Noble-gas notation [Kr] 4d7 5s1
Valence clue 5s1
Block d-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 44 for a neutral Ruthenium 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 Ruthenium?

The neutral Ruthenium atom is written as 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d7 5s1. The shorthand form is [Kr] 4d7 5s1.

How many valence electrons does Ruthenium have?

Start from the outer-shell clue 5s1. For main-group elements this usually gives a direct valence count; for transition metals, inspect both s and d electrons carefully.

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.

What are the common oxidation states of Ruthenium?

The d-block position and outer-shell configuration 5s1 determine the most stable ions. Check the periodic group and compare with neighboring elements.

Practice nearby concepts

Elements hub Start from the periodic-table families and move to individual configurations. Electron configuration calculator Check a classroom configuration and see the shell-by-shell reading. Orbital diagram guide Translate a configuration into boxes, arrows, and paired electrons. Valence electrons guide Use the outer shell to predict bonding patterns and common ions.

Study notes and practice checks

Element-specific practice problems

Problem 1: Write the full electron configuration for neutral Ruthenium and verify the electron count against 44.

Problem 2: Convert the full configuration to noble-gas shorthand notation.

Problem 3: Consider the trend in group 8: Fe [Ar] 3d6 4s2, Ru [Kr] 4d7 5s1, Os [Xe] 4f14 5d6 6s2. Explain why ruthenium is the only group 8 element with an s/d exception.

Problem 4: Predict the configuration of Ru3+. Which electrons are removed first?

Problem 5: Compare ruthenium with technetium (Z=43, [Kr] 4d5 5s2) and rhodium (Z=45, [Kr] 4d8 5s1). How does the electron count explain the trend in exceptions?

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Elena Marquez

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Elena Marquez

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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.

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Elements

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Electron configuration of Tungsten (W) Read the Tungsten electron configuration, noble-gas shorthand, valence shell, orbital filling logic, and the mistakes to avoid when writing W. Electron configuration of Uranium (U) Read the Uranium electron configuration, noble-gas shorthand, valence shell, orbital filling logic, and the mistakes to avoid when writing U. Electron configuration of Vanadium (V) Read the Vanadium electron configuration, noble-gas shorthand, valence shell, orbital filling logic, and the mistakes to avoid when writing V. Electron configuration of Xenon (Xe) Read the Xenon electron configuration, noble-gas shorthand, valence shell, orbital filling logic, and the mistakes to avoid when writing Xe. Electron configuration of Ytterbium (Yb) Read the Ytterbium electron configuration, noble-gas shorthand, valence shell, orbital filling logic, and the mistakes to avoid when writing Yb. Electron configuration of Yttrium (Y) Read the Yttrium electron configuration, noble-gas shorthand, valence shell, orbital filling logic, and the mistakes to avoid when writing Y. Electron configuration of Zinc (Zn) Read the Zinc electron configuration, noble-gas shorthand, valence shell, orbital filling logic, and the mistakes to avoid when writing Zn. Electron configuration of Zirconium (Zr) Read the Zirconium electron configuration, noble-gas shorthand, valence shell, orbital filling logic, and the mistakes to avoid when writing Zr.

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