Element guide
Electron configuration of Nickel (Ni)
The electron configuration of Nickel is 1s2 2s2 2p6 3s2 3p6 3d8 4s2. In shorthand form it is written as [Ar] 3d8 4s2.
Use this page to connect the notation with atomic number 28, the d-block, and the valence pattern 4s2.
How to write the configuration
Configuration at a glance
Nickel has atomic number 28, so a neutral atom has 28 electrons. The configuration 1s2 2s2 2p6 3s2 3p6 3d8 4s2 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 [Ar] 3d8 4s2 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.
Nickel follows the standard filling order
Nickel is a period 4 transition metal that follows the standard Aufbau sequence: 1s2 2s2 2p6 3s2 3p6 4s2 3d8. Note that 4s fills before 3d, but when nickel forms ions, the 4s electrons are lost first.
Step-by-step filling walkthrough: 1. Start with atomic number 28. 2. Follow the Aufbau sequence: fill 1s, 2s, 2p, 3s, 3p, then continue through 4s, 3d, 4p in order. 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 28.
Near the end of the 3d series
Nickel sits near the end of the first transition series, with only Copper (Z=29) and Zinc (Z=30) having more d-electrons. The 3d8 configuration means there are two unpaired electrons, making nickel magnetic. However, nickel's magnetism is weaker than iron's because the d-subshell is nearly full.
Real-world applications
- Nickel is a key component in stainless steel, improving corrosion resistance and strength.
- Nickel-metal hydride (NiMH) batteries use nickel's redox chemistry for rechargeable power.
- Nickel catalysts are used in hydrogenation reactions in the food and chemical industries.
- Nickel is used in coins, electroplating, and superalloys for jet engines.
Common ions: Ni2+ ([Ar] 3d8) is the most stable oxidation state. Ni3+ ([Ar] 3d7) is less common but exists in some battery materials.
Nickel reference table
| Item | Value |
|---|---|
| Atomic number | 28 |
| Full configuration | 1s2 2s2 2p6 3s2 3p6 3d8 4s2 |
| Noble-gas notation | [Ar] 3d8 4s2 |
| Valence clue | 4s2 |
| 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 28 for a neutral Nickel 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 Nickel?
The neutral Nickel atom is written as 1s2 2s2 2p6 3s2 3p6 3d8 4s2. The shorthand form is [Ar] 3d8 4s2.
How many valence electrons does Nickel have?
Start from the outer-shell clue 4s2. For transition metals, inspect both s and d electrons since both can contribute to bonding in different oxidation states.
What is the most stable oxidation state of Nickel?
Ni2+ is the most common and stable oxidation state. The configuration loses the two 4s electrons to give [Ar] 3d8.
Is Nickel magnetic?
Yes, nickel is ferromagnetic, though less strongly than iron. The two unpaired electrons in the 3d8 subshell give it magnetic properties used in alloys and electronics.
Practice nearby concepts
Study notes and practice checks
Element-specific practice problems
Problem 1: Write the full electron configuration for neutral Nickel and verify the electron count against 28.
Problem 2: Convert the full configuration to noble-gas shorthand notation.
Problem 3: Compare the configuration of Nickel (Z=28) with Cobalt (Z=27) and Copper (Z=29). How does the d-electron count change across these three neighbours?
Problem 4: Predict the electron configuration of Ni2+ and explain why Ni3+ is less stable.
Problem 5: Nickel is used as a hydrogenation catalyst. How might its electron configuration contribute to its ability to adsorb hydrogen molecules?
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