Compare Sodium vs Lithium: Periodic Table Element Comparison Table and Properties
Compare the elements Sodium and Lithium on the basis of their properties, attributes and periodic table facts. Compare elements - Sodium and Lithium comparison table side by side across over 90 properties. All the elements of similar categories show a lot of similarities and differences in their chemical, atomic, physical properties and uses. These similarities and dissimilarities should be known while we study periodic table elements. You can study the detailed comparison between Sodium vs Lithium with most reliable information about their properties, attributes, facts, uses etc. You can compare Na vs Li on more than 90 properties like electronegativity, oxidation state, atomic shells, orbital structure, Electronaffinity, physical states, electrical conductivity and many more. This in-depth comparison helps students, educators, researchers, and science enthusiasts understand the differences and similarities between Sodium and Lithium.
Sodium and Lithium Comparison
Here's a detailed comparison between Sodium (Na) and Lithium (Li), focusing on their position in the periodic table, physical and chemical properties, stability, and uses.
Facts - Basic Element Details
| Name | Sodium | Lithium |
|---|---|---|
| Atomic Number | 11 | 3 |
| Atomic Symbol | Na | Li |
| Atomic Weight | 22.98977 | 6.941 |
| Phase at STP | Solid | Solid |
| Color | Silver | Silver |
| Metallic Classification | Alkali Metal | Alkali Metal |
| Group in Periodic Table | group 1 | group 1 |
| Group Name | lithium family | lithium family |
| Period in Periodic Table | period 3 | period 2 |
| Block in Periodic Table | s -block | s -block |
| Electronic Configuration | [Ne] 3s1 | [He] 2s1 |
| Electronic Shell Structure (Electrons per shell) | 2, 8, 1 | 2, 1 |
| Melting Point | 370.87 K | 453.69 K |
| Boiling Point | 1156 K | 1615 K |
| CAS Number | CAS7440-23-5 | CAS7439-93-2 |
| Neighborhood Elements | Neighborhood Elements of Sodium | Neighborhood Elements of Lithium |
History
| Parameter | Sodium | Lithium |
|---|---|---|
| History | The element Sodium was discovered by H. Davy in year 1807 in United Kingdom. Sodium derived its name from the English word soda (natrium in Latin). | The element Lithium was discovered by A. Arfwedson in year 1817 in Sweden. Lithium derived its name the Greek word lithos, meaning 'stone'. |
| Discovery | H. Davy (1807) | A. Arfwedson (1817) |
| Isolated | H. Davy (1807) | W. T. Brande (1821) |
Presence: Abundance in Nature and Around Us
Parts per billion (ppb) by weight / by atoms (1ppb =10^-7 %)
| Property | Sodium | Lithium |
|---|---|---|
| Abundance in Universe | 20000 / 1000 | 6 / 1 |
| Abundance in Sun | 40000 / 2000 | 0.06 / 0.01 |
| Abundance in Meteorites | 5600000 / 4800000 | 1700 / 4600 |
| Abundance in Earth's Crust | 23000000 / 21000000 | 17000 / 50000 |
| Abundance in Oceans | 11050000 / 2970000 | 180 / 160 |
| Abundance in Humans | 1400000 / 380000 | 30 / 27 |
Crystal Structure and Atomic Structure
| Property | Sodium | Lithium |
|---|---|---|
| Atomic Volume | 23.75 cm3/mol | 13.02 cm3/mol |
| Atomic Radius | 190 pm | 167 pm |
| Covalent Radius | 154 pm | 134 pm |
| Van der Waals Radius | 227 pm | 182 pm |
Atomic Spectrum - Spectral Lines | ||
| Emission Spectrum |  |  |
| Absorption Spectrum |  |  |
| Lattice Constant | 429.06, 429.06, 429.06 pm | 351, 351, 351 pm |
| Lattice Angle | π/2, π/2, π/2 | π/2, π/2, π/2 |
| Space Group Name | Im_ 3m | Im_ 3m |
| Space Group Number | 229 | 229 |
| Crystal Structure | Body Centered Cubic  | Body Centered Cubic |
Atomic and Orbital Properties
| Property | Sodium | Lithium |
|---|---|---|
| Atomic Number | 11 | 3 |
| Number of Electrons (with no charge) | 11 | 3 |
| Number of Protons | 11 | 3 |
| Mass Number | 22.98977 | 6.941 |
| Number of Neutrons | 12 | 4 |
| Shell structure (Electrons per energy level) | 2, 8, 1 | 2, 1 |
| Electron Configuration | [Ne] 3s1 | [He] 2s1 |
| Valence Electrons | 3s1 | 2s1 |
| Oxidation State | 1 | 1 |
| Atomic Term Symbol (Quantum Numbers) | 2S1/2 | 2S1/2 |
| Shell structure |  |  |
Isotopes and Nuclear Properties
Sodium has 1 stable naturally occuring isotopes while Lithium has 2 stable naturally occuring isotopes.
| Parameter | Sodium | Lithium |
|---|---|---|
| Known Isotopes | 18Na, 19Na, 20Na, 21Na, 22Na, 23Na, 24Na, 25Na, 26Na, 27Na, 28Na, 29Na, 30Na, 31Na, 32Na, 33Na, 34Na, 35Na, 36Na, 37Na | 3Li, 4Li, 5Li, 6Li, 7Li, 8Li, 9Li, 10Li, 11Li, 12Li |
| Stable Isotopes | Naturally occurring stable isotopes: 23Na | Naturally occurring stable isotopes: 6Li, 7Li |
| Neutron Cross Section | 0.53 | 0.045 |
| Neutron Mass Absorption | 0.0007 | - |
Chemical Properties: Ionization Energies and electron affinity
| Property | Sodium | Lithium |
|---|---|---|
| Valence or Valency | 1 | 1 |
| Electronegativity | 0.93 Pauling Scale | 0.98 Pauling Scale |
| Oxidation State | 1 | 1 |
| Electron Affinity | 52.8 kJ/mol | 59.6 kJ/mol |
| Ionization Energies | 1st: 495.8 kJ/mol 2nd: 4562 kJ/mol 3rd: 6910.3 kJ/mol 4th: 9543 kJ/mol 5th: 13354 kJ/mol 6th: 16613 kJ/mol 7th: 20117 kJ/mol 8th: 25496 kJ/mol 9th: 28932 kJ/mol 10th: 141362 kJ/mol 11th: 159076 kJ/mol | 1st: 520.2 kJ/mol 2nd: 7298.1 kJ/mol 3rd: 11815 kJ/mol |
Physical Properties
Lithium (0.535 g/cm³) is less dense than Sodium (0.968 g/cm³). This means that a given volume of Sodium will be heavier than the same volume of Lithium. Sodium is about 80.9 denser than Lithium
| Property | Sodium | Lithium |
|---|---|---|
| Phase at STP | Solid | Solid |
| Color | Silver | Silver |
| Density | 0.968 g/cm3 | 0.535 g/cm3 |
| Density (when liquid (at melting point)) | 0.927 g/cm3 | 0.512 g/cm3 |
| Molar Volume | 23.75 cm3/mol | 13.02 cm3/mol |
Mechanical and Hardness Properties
| Property | Sodium | Lithium |
|---|---|---|
Elastic Properties | ||
| Young Modulus | 10 | 4.9 |
| Shear Modulus | 3.3 GPa | 4.2 GPa |
| Bulk Modulus | 6.3 GPa | 11 GPa |
| Poisson Ratio | - | - |
Hardness - Tests to Measure of Hardness of Element | ||
| Mohs Hardness | 0.5 MPa | 0.6 MPa |
| Vickers Hardness | - | - |
| Brinell Hardness | 0.69 MPa | - |
Thermal and Electrical Conductivity
| Property | Sodium | Lithium |
|---|---|---|
Heat and Conduction Properties | ||
| Thermal Conductivity | 140 W/(m K) | 85 W/(m K) |
| Thermal Expansion | 0.000071 /K | 0.000046 /K |
Electrical Properties | ||
| Electrical Conductivity | 21000000 S/m | 11000000 S/m |
| Resistivity | 4.7e-8 m Ω | 9.4e-8 m Ω |
| Superconducting Point | - | - |
Magnetic and Optical Properties
| Property | Sodium | Lithium |
|---|---|---|
Magnetic Properties | ||
| Magnetic Type | Paramagnetic | Paramagnetic |
| Curie Point | - | - |
| Mass Magnetic Susceptibility | 8.8e-9 m3/kg | 2.56e-8 m3/kg |
| Molar Magnetic Susceptibility | 2e-10 m3/mol | 1.78e-10 m3/mol |
| Volume Magnetic Susceptibility | 0.0000085 | 0.00000137 |
Optical Properties | ||
| Refractive Index | - | - |
Acoustic Properties | ||
| Speed of Sound | 3200 m/s | 6000 m/s |
Thermal Properties - Enthalpies and thermodynamics
| Property | Sodium | Lithium |
|---|---|---|
| Melting Point | 370.87 K | 453.69 K |
| Boiling Point | 1156 K | 1615 K |
| Critical Temperature | 2573 K | 3223 K |
| Superconducting Point | - | - |
Enthalpies | ||
| Heat of Fusion | 2.6 kJ/mol | 3 kJ/mol |
| Heat of Vaporization | 97.7 kJ/mol | 147 kJ/mol |
| Heat of Combustion | - | -298 J/(kg K) |
Regulatory and Health - Health and Safety Parameters and Guidelines
| Parameter | Sodium | Lithium |
|---|---|---|
| CAS Number | CAS7440-23-5 | CAS7439-93-2 |
| RTECS Number | RTECSVY0686000 | RTECSOJ5540000 |
| DOT Hazard Class | 4.3 | 4.3 |
| DOT Numbers | 1428 | 1415 |
| EU Number | - | - |
| NFPA Fire Rating | 3 | 2 |
| NFPA Health Rating | 3 | 3 |
| NFPA Reactivity Rating | 2 | 2 |
| NFPA Hazards | Water Reactive | Water Reactive |
| AutoIgnition Point | 115 °C | 179 °C |
| Flashpoint | 4 °C | - |
Compare Sodium and Lithium With Other Elements
Compare Sodium and Lithium with other elements of the periodic table. Explore howSodium and Lithium stack up against other elements of the periodic table. Use our interactive comparison tool to analyze 90+ properties across different metals, non-metals, metalloids, and noble gases. Understanding these differences is crucial for applications in engineering, chemistry, electronics, biology, and material science.
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