Element guide
Electron configuration of Tin (Sn)
The electron configuration of Tin is 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p2. In shorthand form it is written as [Kr] 4d10 5s2 5p2.
Use this page to connect the notation with atomic number 50, the p-block, and the valence pattern 5s2 5p2.
How to write the configuration
Configuration at a glance
Tin has atomic number 50, so a neutral atom has 50 electrons. The configuration 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p2 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] 4d10 5s2 5p2 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.
Tin is a post-transition metal in the p-block
Tin sits in group 14, directly below carbon and silicon. It has a completely filled 4d subshell, and the valence electrons are in the 5s and 5p orbitals. The p-block position means tin often forms compounds using both p-electrons, but the inert-pair effect becomes relevant for heavy p-block elements.
Step-by-step filling walkthrough: 1. Start with atomic number 50. 2. Follow the Aufbau sequence through 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p. 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 50.
The inert-pair effect
For tin and heavier group 14 elements, the ns2 electrons become increasingly reluctant to participate in bonding. This inert-pair effect means tin commonly shows both +2 (Sn2+) and +4 (Sn4+) oxidation states, unlike carbon which almost exclusively shows +4. The 5s2 pair is relatively inert due to relativistic effects and poor orbital overlap with ligands.
Real-world applications
- Tin plating protects steel from corrosion (tin cans are actually steel with a thin tin coating).
- Solder alloys typically contain tin and lead or tin and silver for electronics assembly.
- Indium tin oxide (ITO) is a transparent conductor used in touch screens and LCD displays.
- Bronze is an alloy of copper and tin that changed human civilization during the Bronze Age.
Common ions: Sn2+ (loses 5p2 electrons) and Sn4+ (loses 5s2 5p2 electrons). Both are important in inorganic chemistry.
Tin reference table
| Item | Value |
|---|---|
| Atomic number | 50 |
| Full configuration | 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p2 |
| Noble-gas notation | [Kr] 4d10 5s2 5p2 |
| Valence clue | 5s2 5p2 |
| 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 50 for a neutral Tin 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 Tin?
The neutral Tin atom is written as 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p2. The shorthand form is [Kr] 4d10 5s2 5p2.
How many valence electrons does Tin have?
Tin is in group 14 and has four valence electrons (5s2 5p2). However, due to the inert-pair effect, it often behaves as if only the two p-electrons are available.
What is the inert-pair effect?
The inert-pair effect describes how the ns2 electrons of heavy p-block elements become less available for bonding. For tin, this explains why Sn2+ compounds exist alongside Sn4+ compounds.
Why is tin used as a coating for steel?
Tin resists corrosion and is non-toxic. Its electron configuration gives it chemical stability in air and water, making it an effective protective layer for food containers.
Practice nearby concepts
Study notes and practice checks
Element-specific practice problems
Problem 1: Write the full electron configuration for neutral Tin and verify the electron count against 50.
Problem 2: Convert the full configuration to noble-gas shorthand notation.
Problem 3: Compare the configuration of Tin (Z=50) with Indium (Z=49) and Antimony (Z=51). How does the p-electron count change across these neighbours?
Problem 4: Predict the electron configurations of Sn2+ and Sn4+. Why does tin show both oxidation states while carbon only shows +4?
Problem 5: The d10 configuration is fully filled. How might this filled d-subshell affect tin's chemical properties compared to transition metals with partially filled d-orbitals?
Siguiente lectura
Guias relacionadas para continuar
Si quieres seguir con el mismo tema, aqui tienes paginas cercanas que amplian la tecnica, comparan variantes o te llevan a la siguiente rutina.