Physical Properties
How this element behaves in real-world conditions.
- State (25°C)
- Solid
- Density
- 1.873 g/cm³
- Melting Point
- 28.44 °C
- Boiling Point
- 671 °C
Atomic Structure
Core identity and periodic table positioning.
Electromagnetic Properties
How this element attracts and exchanges electrons.
- Electronegativity
- 0.79
- Ionization Energy
- 3.894 eV
- Electron Affinity
- 0.472 eV
- Metallic Character
- Metal
Hero / Identity Section
Core identity profile for Cesium with periodic placement and electron context.
- Element Name
- Cesium
- Symbol
- Cs
- Atomic Number
- 55
- Atomic Mass
- 132.91
- Group
- 1
- Period
- 6
- Block
- S
- Category
- Alkali
- Standard State
- Solid
- Electron Configuration (Full)
- 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s1
- Electron Configuration (Noble Gas)
- [Xe] 6s1
- Valence Electrons
- 1
Quick Facts Card (Table Layout)
Fast-reference values for physical and energetic properties.
Atomic Radius
298 pm
Ionic Radius
Not available in current dataset
Electronegativity (Pauling)
0.79
1st Ionization Energy
3.894 eV
Electron Affinity
0.472 eV
Density
1.873 g/cm³
Melting Point
28.44 °C
Boiling Point
671 °C
Heat Capacity
Not available in current dataset
Thermal Conductivity
Not available in current dataset
Visual Components
Visual learning views for table position, shells, orbitals, and phase behavior.
Highlighted Position in Periodic Table Grid
Cs
Row 6, Column 1
Bohr Model Diagram
Cs
Educational shell model for electron arrangement.
Electron Shell Diagram
- K shell2
- L shell8
- M shell18
- N shell18
- O shell8
- P shell1
Orbital Configuration Diagram
1s2/2
2s2/2
2p6/6
3s2/2
3p6/6
4s2/2
3d10/10
4p6/6
5s2/2
4d10/10
5p6/6
6s1/2
Phase Illustration
Solid
Solid lattice
Atomic Structure Section
Nuclear composition and electron shielding interpretation.
- Protons
- 55
- Neutrons (Most Abundant Isotope Estimate)
- 78
- Electrons
- 55
- Electron Configuration Breakdown
- 2 • 8 • 18 • 18 • 8 • 1
- Shielding Explanation
- Core electrons (~54) shield part of the nucleus, reducing attraction felt by outer electrons compared with the full nuclear charge.
- Effective Nuclear Charge (Estimate)
- 1
Chemical Properties Section
Category-guided chemistry behavior with periodic context for comparison.
- Common Oxidation States
- +1 (dominant)
- Reactivity Summary
- Highly reactive, especially with water and oxygen. Reactivity generally increases down the group.
- Acid/Base Behavior
- Often forms strongly basic oxides and hydroxides.
- Bonding Behavior
- Mostly ionic bonding with nonmetals; metallic bonding in pure form.
- Typical Compounds
- Oxides, Hydroxides, Halides
- Periodic Trend Comparison (Group Neighbors)
- Compared with Rb, this element is lower in the group and typically has a larger atomic size and lower ionization tendency. Compared with Fr, this element is higher in the group and often shows a smaller radius with stronger effective attraction to valence electrons.
Isotopes & Nuclear Data
Isotope stability and abundance notes for learning-oriented nuclear context.
- Stable Isotopes
- Stable isotopes are known. Most abundant isotope is commonly represented near Cs-133.
- Radioactive Isotopes
- Radioactive isotopes exist alongside stable isotopes.
- Natural Abundance (%)
- Naturally occurring with isotope-dependent abundance.
- Half-life (If Applicable)
- Stable isotopes have no half-life; radioactive isotopes have isotope-specific half-lives.
- Nuclear Spin (Optional Advanced)
- Advanced isotope-level data is not included in the current core dataset.
- Most Abundant Isotope (Estimate)
- Cs-133
Applications & Uses
How this element appears in industry, biology, medicine, and technology.
- Industrial Uses
- Used in alloys, batteries, heat transfer salts, and specialty reagents.
- Biological Role
- Selected alkali ions (such as sodium and potassium) are essential in living systems.
- Medical Use
- Alkali salts are common in fluid/electrolyte support and buffering formulations.
- Technological Relevance
- Important for batteries, glass chemistry, and electrochemical systems.
- Environmental Impact
- Can alter pH and salinity in water/soil if released in large quantities.
Safety & Handling
General hazard guidance for educational reference and lab awareness.
- Toxicity
- Elemental forms can be hazardous due to strong reactivity; many salts are manageable with proper handling.
- Flammability
- Elemental forms are often flammable/reactive, especially with moisture.
- Storage Considerations
- Store reactive metals under inert oil/atmosphere away from moisture and oxidizers.
- Regulatory Classification
- Frequently regulated as reactive metals and/or corrosive materials depending on form.