Lithium
Lithium (from Greek:λίθος lithos, "stone") is a chemical element with the symbol Li and atomic number 3. It is a soft, silver-white metal belonging to the alkali metal group of chemical elements. Under standard conditions it is the lightest metal and the least dense solid element.
At a glance
- Atomic number
- 3
- Atomic mass
- 6.94 u
- Phase
- Solid
- Density
- 0.534 g/cm³
- Melting point
- 453.65 K
- Boiling point
- 1,603 K
- First ionization energy
- 520.2 kJ/mol
- Electronegativity
- 0.98
- Electron affinity
- 59.6326 kJ/mol
- Molar heat capacity
- 24.86 J/(mol·K)
- Period
- 2
- Appearance
- silvery-white
Conditions and isotopes affect measured properties. Some properties of short-lived elements are predicted. Electronegativity uses the Pauling scale.
Lithium’s orbitals use a hydrogen-like approximation. Every orbital of each visible subshell is shown: in Shapes as the surface holding half its probability, with light and dark shades for opposite signs of the wavefunction; in Cloud as dots where its electrons are likely to be. Sizes are stepped by shell, like the Shell model.
Preparing the orbital view…
3 protons4 neutrons
Lithium-7: its most common form in nature, or its longest-lived if it has none. The nucleus is drawn far too big: it’s about 100,000 times smaller than the atom.
Turn up the heat
A step of 1 K is the same size as 1 °C, so the two scales are always 273.15 apart. Fahrenheit is different: its degrees are smaller and it starts elsewhere, so water freezes at 273.15 K, 0 °C and 32 °F.25 °C · 77 °FSolid
At this temperature, lithium is a solid.
At normal atmospheric pressure (1 atm). The temperature scale is logarithmic. The particle box is schematic: real samples hold vastly more atoms, and spacing and speeds are not to scale.
Pull the electrons off
LiNeutral atom · no charge
A neutral lithium atom. Removing its first electron takes 520 kJ/mol.
Lithium’s outer shell holds 1 electron. Electron 2 is the first from an inner shell: it sits closer to the nucleus with less shielding, so removing it takes 14× as much energy as the one before. That’s why lithium forms Li⁺ ions.
What does this tell us?
- The jumps let you count electrons. Between the dashed lines there are 1, then 2 bars. Read backwards, that’s 2, 1: the same electrons per shell as the shell model above. Jumps like these are part of the evidence that shells exist.
- The single electron before the first big jump is lithium’s valence electron, the one it uses in chemical reactions. That’s why lithium sits in group 1: every element in the group has the same number of outer electrons, so they react in similar ways.
- The numbers explain the charge. Removing electron 2 as well, to make Li²⁺, would cost 7,298 kJ/mol. Forming a compound gives back far less energy than that, so Li²⁺ doesn’t form in ordinary chemistry.
- Within a shell the steps rise gently. Each electron removed leaves fewer electrons pushing the others away, while the nucleus pulls just as hard, so the next one is held a little more tightly.
Show the values as a table
| Electron | Shell | Energy (kJ/mol) | × previous | Value |
|---|---|---|---|---|
| 1 | 2 | 520 | – | Measured |
| 2 | 1 | 7,298 | 14 | Calculated |
| 3 | 1 | 11,815 | 1.6 | Calculated |
Successive ionization energies of gas-phase atoms and ions from the NIST Atomic Spectra Database. Solid bars are measured; hatched bars were estimated from nearby measurements or calculated from quantum theory, as is usual for highly charged ions. Electrons are taken from the outermost shell first, a simplification: electrons in different subshells of the same shell also differ in energy. On the log scale each gridline is 10 times the one below.
Drop it in water
Ready to drop a small piece of lithium.
Floats and fizzes steadily, drifting slowly across the water. It stays solid and doesn’t catch fire.
- In water it
- Floats0.534 g/cm³, water is 1
- From the heat it
- Stays solidmelts at 181 °C
- How violent
2Li + 2H₂O → 2LiOH + H₂
Hydrogen gas fizzes off, and the metal hydroxide dissolves, making the water alkaline: a few drops of phenolphthalein indicator turn it pink.
Why it gets more violent down the group
Every alkali metal has one electron in its outer shell, and reacting means giving it away. Further down the group that electron sits in a shell further from the nucleus, shielded by more electrons inside, so it takes less energy to remove and the reaction runs faster.
- Lithium520 kJ/mol
- Sodium496 kJ/mol
- Potassium419 kJ/mol
- Rubidium403 kJ/mol
- Caesium376 kJ/mol
Energy to remove the outer electron (first ionization energy, NIST). Speed isn’t the same as energy: per atom, lithium’s reaction releases slightly more energy than sodium’s, it just releases it slowly. Francium’s value (393 kJ/mol) is a little higher than caesium’s, because of relativistic effects, so it may not be the most violent after all.
Don’t try this at home. Demonstrations use rice-grain-sized pieces behind safety screens; the heavier metals are only shown on video.
How does it compare?
Density
0.534 g/cm³12th lowest of 99
Melting point
454 K23rd lowest of 96
Boiling point
1,603 K31st lowest of 97
Electronegativity
0.989th lowest of 96
First ionization energy
520 kJ/mol9th lowest of 99
Elements 1–99 from the reference data; heavier elements are left out because only a few atoms have ever been made, so their bulk properties are predictions. First ionization energies come from NIST. Density uses a logarithmic scale, because gases are around a thousand times less dense than solids; gas densities are at 0 °C and 1 atm. Melting and boiling points are at normal pressure. Everyday temperatures and light sources in the pictures are approximate. Hover over a dot to see the element, or click it to compare.
Keep exploring
Explore the stories, imagery, and reference data in more depth. Properties with no value in the reference are marked unavailable.
- LithiumRoyal Society of Chemistry
- LithiumWikipedia
- Quantum numbers and electron configurationsPurdue
- Hydrogenic wavefunctionsNIST
- Ionization energiesNIST Atomic Spectra Database