Element guide
Electron configuration of Titanium (Ti)
The electron configuration of Titanium is 1s2 2s2 2p6 3s2 3p6 3d2 4s2. In shorthand form it is written as [Ar] 3d2 4s2.
Use this page to connect the notation with atomic number 22, the d-block, and the valence pattern 3d2 4s2.
How to write the configuration
Configuration at a glance
Titanium has atomic number 22, so a neutral atom has 22 electrons. The configuration 1s2 2s2 2p6 3s2 3p6 3d2 4s2 is a compact record of where those electrons sit by subshell.
The shorthand [Ar] 3d2 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.
Step-by-step filling
After the argon core (18 electrons), 4 more electrons need placement. The 4s subshell receives 2 electrons (4s2) before the 3d subshell starts filling. The remaining 2 electrons go into separate 3d orbitals following Hund's rule.
Step-by-step filling walkthrough: 1. Start with atomic number 22. 2. Fill through argon: 1s2 2s2 2p6 3s2 3p6 (18 electrons). 3. Fill 4s2 (20 electrons total). 4. Place 2 electrons in 3d (22 electrons total). 5. These two 3d electrons occupy different d orbitals (Hund's rule), giving Ti two unpaired electrons.
Orbital diagram and valence meaning
An orbital diagram turns each subshell into boxes and arrows. Ti has two unpaired electrons in the 3d subshell, which contributes to its common +4 and +3 oxidation states. The valence clue for Ti is 3d2 4s2.
For transition metals, both the 4s and 3d electrons participate in bonding. Ti commonly forms Ti4+ (losing all 4 valence electrons) or Ti3+ (losing 4s2 and one 3d electron).
Common mistakes
The first mistake is miscounting: after argon (18), 4s2 (20), 3d2 (22). Verify: 2+2+6+2+6+2+2 = 22. The second mistake is writing 3d before 4s in the filling order sequence. While 4s fills before 3d, some references order by principal quantum number (3d then 4s).
A third common error is forgetting that Ti has unpaired electrons. Each of the two 3d electrons occupies a separate orbital, making Ti paramagnetic.
Titanium reference table
| Item | Value |
|---|---|
| Atomic number | 22 |
| Full configuration | 1s2 2s2 2p6 3s2 3p6 3d2 4s2 |
| Noble-gas notation | [Ar] 3d2 4s2 |
| Valence clue | 3d2 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 22 for a neutral Titanium 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 Titanium?
The neutral Titanium atom is written as 1s2 2s2 2p6 3s2 3p6 3d2 4s2. The shorthand form is [Ar] 3d2 4s2.
How many valence electrons does Titanium have?
Start from the outer-shell clue 3d2 4s2. For transition metals, inspect both s and d electrons carefully. Titanium has 4 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 Titanium have two unpaired electrons?
According to Hund's rule, the two 3d electrons occupy different d orbitals with parallel spins before any pairing occurs. This gives Ti two unpaired electrons.
Practice nearby concepts
Study notes and practice checks
From answer to understanding
Titanium is one of the most important transition metals industrially, known for its high strength-to-weight ratio and corrosion resistance. Its electron configuration [Ar] 3d2 4s2 explains its common +4 oxidation state.
Practice comparison
Compare Titanium (Ti) with Scandium (Sc) and Vanadium (V). Sc: [Ar] 3d1 4s2, Ti: [Ar] 3d2 4s2, V: [Ar] 3d3 4s2. The pattern shows the 3d subshell filling steadily across the first transition series.
Teacher and self-study notes
Use this page alongside the transition-metal section to explain why d-electron count determines magnetic properties, color, and oxidation state versatility. Ti2+ (two 3d electrons) and Ti4+ (no d electrons) have very different magnetic and optical properties.
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