Give the boiling point.
(Values rounded to 4sf)
−252.9°C
−423.2°F ; 20.27 K
The boiling point is the temperature at which the surrounding pressure exerted on the liquid is equal to the opposing pressure exerted by the vapour pressure of the liquid.
Give the melting point.
(Values rounded to 4sf)
−259.2°C
−434.5°F ; 13.99 K
The melting point is the temperature at which the solid and liquid forms of a substance can exist in equilibrium.
Give the boiling point.
(Values rounded to 4sf)
−268.9°C
−452.1°F ; 4.220 K
The boiling point of elements vary according to the applied pressure – all the data here assumes one atmosphere of pressure (standard condition).
Give the melting point.
(Values rounded to 4sf)
Unknown
Under 1 atm, it is believed helium will remain a liquid down to absolute zero.
Give the boiling point.
(Values rounded to 4sf)
1342°C
2448°F ; 1615 K
Applying heat to a liquid will increase its temperature right up to its boiling point.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the liquid particles, allowing it to transition to the gas phase.
Give the melting point.
(Values rounded to 4sf)
180.5°C
356.9°F ; 453.7 K
Applying heat to a solid will increase its temperature right up to its melting point.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the solid particles, allowing it to transition to the liquid phase.
Give the boiling point.
(Values rounded to 4sf)
2468°C
4474°F ; 2741 K
Extra for Experts: phase diagrams are charts used to depict the conditions (pressure and temperature mostly) at which thermodynamically distinct phases (i.e. solid, liquid, gas) occur or exist at equilibrium with each other.
The boiling point would be represented by the boundary line between liquid and gas at a given temperature and pressure.
Give the melting point.
(Values rounded to 4sf)
1287°C
2349°F ; 1560 K
Extra for Experts: only solids and gases exist in space because the pressure is zero and any liquid exposed would immediately boil or freeze.
Remember that pressure affects boiling points, as the vapour pressure of the liquid is at equilibrium with the surrounding pressure – liquids cannot stably exist in a zero-pressure environment (i.e. a vacuum).
Give the boiling point.
(Values rounded to 4sf)
4000°C
7232°F ; 4273 K
Extra for Experts: the critical point on a phase diagram represents a temperature and pressure value at which the liquid and gaseous phases merge together to form a single phase.
This is found towards the top-right of a traditional phase diagram, and represents supercritical fluids.
Give the melting point.
(Values rounded to 4sf)
2077°C
3771°F ; 2350 K
The melting point is the temperature at which the solid and liquid forms of a substance can exist in equilibrium.
Give the sublimation point.
(Values rounded to 4sf)
3825°C
6917°F ; 4098 K
Note there are theoretical values for melting and boiling points of carbon, however, in real life contexts, carbon actually sublimes (goes from solid to gas, skipping the liquid phase).
Give the boiling point.
(Values rounded to 4sf)
−195.8°C
−320.4°F ; 77.36 K
Extra for Experts: on a phase diagram, the triple point represents where all lines of equilibrium between phases intersect.
This is the exact temperature and pressure at which a substance can stably exist as a solid, liquid, and gas in equilibrium.
Give the melting point.
(Values rounded to 4sf)
−209.9°C
−345.8°F ; 63.29 K
The melting point of a substance is less dependent on pressure than the boiling point, but this is still an important factor affecting it.
This relationship though is not always as straightforward, and with some instances increased pressure after a certain point translates to a decrease in melting point.
Give the boiling point.
(Values rounded to 4sf)
−183.0°C
−297.4°F ; 90.20 K
Adding solutes or other substances can change the boiling point, such as the case with alloys of varying elements and compositions.
Give the melting point.
(Values rounded to 4sf)
−218.8°C
−361.8°F ; 54.36 K
The melting point is the temperature at which the solid and liquid forms of a substance can exist in equilibrium.
Give the boiling point.
(Values rounded to 4sf)
−188.1°C
−306.6°F ; 84.04 K
The boiling point is the temperature at which the surrounding pressure exerted on the liquid is equal to the opposing pressure exerted by the vapour pressure of the liquid.
Give the melting point.
(Values rounded to 4sf)
−219.7°C
−363.4°F ; 53.48 K
The melting point is less dependent on pressure than the boiling point, but this is still an important factor affecting it.
This relationship though is not always as straightforward, and with some instances increased pressure after a certain point translates to a decrease in melting point.
Give the boiling point.
(Values rounded to 4sf)
−246.0°C
−410.9°F ; 27.10 K
Applying heat to a liquid will increase its temperature right up to its boiling point.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the liquid particles, allowing it to transition to the gas phase.
Give the melting point.
(Values rounded to 4sf)
−248.6°C
−415.5°F ; 24.56 K
Applying heat to a solid will increase its temperature right up to its melting point.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the solid particles, allowing it to transition to the liquid phase.
Give the boiling point.
(Values rounded to 4sf)
882.9°C
1621°F ; 1156 K
Extra for Experts: only solids and gases exist in space because the pressure is zero and any liquid exposed would immediately boil or freeze.
Remember that pressure affects boiling points, as the vapour pressure of the liquid is at equilibrium with the surrounding pressure – liquids cannot stably exist in a zero-pressure environment (i.e. a vacuum).
Give the melting point.
(Values rounded to 4sf)
97.79°C
208.0°F ; 370.94 K
Phase diagrams are charts used to depict the conditions (pressure and temperature mostly) at which thermodynamically distinct phases (i.e. solid, liquid, gas) occur or exist at equilibrium with each other.
The line representing the equilibrium between solid and liquid for sodium would intersect the coordinate (97.79°C , 1 atm).
Give the boiling point.
(Values rounded to 4sf)
1090°C
1994°F ; 1363 K
Extra for Experts: the critical point on a phase diagram represents a temperature and pressure value at which the liquid and gaseous phases merge together to form a single phase.
This is found towards the top-right of a traditional phase diagram, and represents supercritical fluids.
Give the melting point.
(Values rounded to 4sf)
650°C
1202°F ; 923.2 K
The stronger the bonding between particles in a substance, the more energy is required to overcome these forces of attraction, and therefore it will have a higher melting point.
Give the boiling point.
(Values rounded to 4sf)
2519°C
4566°F ; 2792 K
Extra for Experts: On a phase diagram, the triple point represents where all lines of equilibrium between phases intersect.
This is the exact temperature and pressure at which a substance can stably exist as a solid, liquid, and gas in equilibrium.
Give the melting point.
(Values rounded to 4sf)
660.3°C
1221°F ; 933.5 K
The heat of fusion (enthalpy of fusion) is the energy absorbed by a unit mass of a particular solid once it’s reached its melting point in order for it to convert fully from a solid to a liquid, without a change in its temperature.
This also goes in the opposite direction, with it representing the amount of energy needed to be released for the substance to solidify again.
Give the boiling point.
(Values rounded to 4sf)
3265°C
5909°F ; 3538 K
The heat of vaporisation (enthalpy of vaporisation) is the energy absorbed by a unit mass of a particular liquid once it’s reached its boiling point in order for it to convert fully into a gas, without a change in its temperature.
This also goes in the opposite direction, with it representing the amount of energy needed to be released for the substance to liquify again.
Give the melting point.
(Values rounded to 4sf)
1414°C
2577°F ; 1687 K
Melting is a physical change rather than a chemical one, as this process is easily reversible and does not form a new substance, nor involve the transfer of electrons.
Give the boiling point.
(Values rounded to 4sf)
280.5°C
536.9°F ; 553.7 K
The boiling point of elements vary according to the applied pressure – all the data here assumes one atmosphere of pressure (standard condition).
Give the melting point.
(Values rounded to 4sf)
44.15°C
111.5°F ; 317.3 K
The melting point is the temperature at which the solid and liquid forms of a substance can exist in equilibrium.
Give the boiling point.
(Values rounded to 4sf)
444.6°C
832.3°F ; 717.8 K
The boiling point is the temperature at which the surrounding pressure exerted on the liquid is equal to the opposing pressure exerted by the vapour pressure of the liquid.
Give the melting point.
(Values rounded to 4sf)
115.2°C
239.4°F ; 388.4 K
The melting point is less dependent on pressure than the boiling point, but this is still an important factor affecting it.
This relationship though is not always as straightforward, and with some instances increased pressure after a certain point translates to a decrease in melting point.
Give the boiling point.
(Values rounded to 4sf)
−34.04°C
−29.27°F ; 239.1 K
Because its boiling point is so low, chlorine is a gas under standard conditions.
Give the melting point.
(Values rounded to 4sf)
−101.5°C
−150.7°F ; 171.7 K
Applying heat to a solid will increase its temperature right up to its melting point.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the solid particles, allowing it to transition to the liquid phase.
Give the boiling point.
(Values rounded to 4sf)
−185.9°C
−302.5°F ; 87.30 K
Applying heat to a liquid will increase its temperature right up to its boiling point.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the liquid particles, allowing it to transition to the gas phase.
Give the melting point.
(Values rounded to 4sf)
−189.3°C
−308.8°F ; 83.81 K
The weaker the bonding between particles in a substance, the less energy is required to overcome these forces of attraction, and therefore it will have a lower melting point.
Give the boiling point.
(Values rounded to 4sf)
759.0°C
1398°F ; 1032 K
Extra for Experts: only solids and gases exist in space because the pressure is zero and any liquid exposed would immediately boil or freeze.
Remember that pressure affects boiling points, as the vapour pressure of the liquid is at equilibrium with the surrounding pressure – liquids cannot stably exist in a zero-pressure environment (i.e. a vacuum).
Give the melting point.
(Values rounded to 4sf)
63.50°C
146.30°F ; 336.7 K
Phase diagrams are charts used to depict the conditions (pressure and temperature mostly) at which thermodynamically distinct phases (i.e. solid, liquid, gas) occur or exist at equilibrium with each other.
The line representing the equilibrium between solid and liquid for potassium would intersect the coordinate (63.50°C , 1 atm).
Give the boiling point.
(Values rounded to 4sf)
1484°C
2703°F ; 1757 K
Extra for Experts: The critical point on a phase diagram represents a temperature and pressure value at which the liquid and gaseous phases merge together to form a single phase.
This is found towards the top-right of a traditional phase diagram, and represents supercritical fluids.
Give the melting point.
(Values rounded to 4sf)
842.0°C
1548°F ; 1115 K
Calcium has a relatively high melting point, making it a solid at room temperature.
Give the boiling point.
(Values rounded to 4sf)
2836°C
5137°F ; 3109 K
Scandium is a transition metal with a high boiling point, meaning a larger energy input is required to convert it from liquid to gas.
Give the melting point.
(Values rounded to 4sf)
1541°C
2806°F ; 1814 K
Scandium has a relatively high melting point, easily making it a solid at room temperature.
Give the boiling point.
(Values rounded to 4sf)
3287°C
5949°F ; 3560 K
Extra for Experts: On a phase diagram, the triple point represents where all lines of equilibrium between phases intersect.
This is the exact temperature and pressure at which a substance can stably exist as a solid, liquid, and gas in equilibrium.
Give the melting point.
(Values rounded to 4sf)
1670°C
3038°F ; 1943 K
The heat of fusion (enthalpy of fusion) is the energy absorbed by a unit mass of a particular solid once it’s reached its melting point in order for it to convert fully into a liquid, without a change in its temperature.
This also goes in the opposite direction, with it representing the amount of energy needed to be released for the substance to solidify again.
Give the boiling point.
(Values rounded to 4sf)
3407°C
6165°F ; 3680 K
Boiling is a physical change rather than a chemical one, as this process is readily reversible and does not form a new substance, nor involve the transfer of electrons.
Give the melting point.
(Values rounded to 4sf)
1910°C
3470°F ; 2183 K
Adding solutes or other substances can change the melting point, such as the case with alloys of varying elements and compositions.
Give the boiling point.
(Values rounded to 4sf)
2671°C
4840°F ; 2944 K
The boiling point of elements vary according to the applied pressure – all the data here assumes one atmosphere of pressure (standard condition).
Give the melting point.
(Values rounded to 4sf)
1907°C
3465°F ; 2180 K
Alloys tend to have lower melting points than pure metals as the differing sizes of the atoms and their less regular arrangements leads to weaker bonding between them.
For example, a chromium cobalt alloy has a theoretical melting point of around 1330°C - although this of course varies with compositions of each element.
Give the boiling point.
(Values rounded to 4sf)
2061°C
3742°F ; 2334 K
Boiling is a physical change rather than a chemical one, as this process is readily reversible and does not form a new substance, nor involve the transfer of electrons.
Give the melting point.
(Values rounded to 4sf)
1246°C
2275°F ; 1519 K
The melting point is the temperature at which the solid and liquid forms of a substance can exist in equilibrium.
Give the boiling point.
(Values rounded to 4sf)
2861°C
5182°F ; 3134 K
The boiling point of elements vary according to the applied pressure – all the data here assumes one atmosphere of pressure (standard condition).
Give the melting point.
(Values rounded to 4sf)
1538°C
2800°F ; 1811 K
The melting point is less dependent on pressure than the boiling point, but this is still an important factor affecting it.
This relationship though is not always as straightforward, and with some instances increased pressure after a certain point translates to a decrease in melting point.
Give the boiling point.
(Values rounded to 4sf)
2927°C
5301°F ; 3200 K
Adding solutes or other substances can change the boiling point, such as the case with alloys of varying elements and compositions.
Give the melting point.
(Values rounded to 4sf)
1495°C
2723°F ; 1768 K
Applying heat to a solid will increase its temperature right up to its melting point.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the solid particles, allowing it to transition to the liquid phase.
Give the boiling point.
(Values rounded to 4sf)
2913°C
5275°F ; 3186 K
Applying heat to a liquid will increase its temperature right up to its boiling point.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the liquid particles, allowing it to transition to the gas phase.
Give the melting point.
(Values rounded to 4sf)
1455°C
2651°F ; 1728 K
The stronger the bonding between particles in a substance, the more energy is required to overcome these forces of attraction, and therefore it will have a higher melting point.
Give the boiling point.
(Values rounded to 4sf)
2560°C
4640°F ; 2833 K
Extra for Experts: Phase diagrams are charts used to depict the conditions (pressure and temperature mostly) at which thermodynamically distinct phases (i.e. solid, liquid, gas) occur or exist at equilibrium with each other.
The line representing the equilibrium between liquid and gas for copper would intersect the coordinate (2560°C , 1 atm).
Give the melting point.
(Values rounded to 4sf)
1084°C
1984°F ; 1358 K
Extra for Experts: The critical point on a phase diagram represents a temperature and pressure value at which the liquid and gaseous phases merge together to form a single phase.
This is found towards the top-right of a traditional phase diagram, and represents supercritical fluids.
Give the boiling point.
(Values rounded to 4sf)
907.0°C
1665°F ; 1180 K
Zinc is a transition metal with a relatively low boiling point.
Give the melting point.
(Values rounded to 4sf)
419.5°C
787.1°F ; 692.7 K
Zinc has a relatively low melting point compared to other transition metals of the same period.
Give the boiling point.
(Values rounded to 4sf)
2229°C
4044°F ; 2502 K
The heat of vaporisation (enthalpy of vaporisation) is the energy absorbed by a unit mass of a particular liquid once it’s reached its boiling point in order for it to convert fully into a gas, without a change in its temperature.
This also goes in the opposite direction, with it representing the amount of energy needed to be released for the substance to liquify again.
Give the melting point.
(Values rounded to 4sf)
29.76°C
85.58°F ; 302.91 K
Gallium has a low melting point, just above room temperature, which allows it to melt in your hand.
Give the boiling point.
(Values rounded to 4sf)
2833°C
5131°F ; 3106 K
Boiling is a physical change rather than a chemical one, as this process is readily reversible and does not form a new substance, nor involve the transfer of electrons.
Give the melting point.
(Values rounded to 4sf)
938.3°C
1721°F ; 1211 K
The heat of fusion (enthalpy of fusion) is the energy absorbed by a unit mass of a particular solid once it’s reached its melting point in order for it to convert fully into a liquid, without a change in its temperature.
This also goes in the opposite direction, with it representing the amount of energy needed to be released for the substance to solidify again.
Give the sublimation point.
(Values rounded to 4sf)
616.0°C
1141°F ; 889.2 K
Arsenic, a metalloid, has a moderately low ‘boiling’ point.
Note the use of the term sublimation as arsenic will go straight from a solid to a gas under standard pressure conditions at this temperature.
Give the melting point.
(Values rounded to 4sf)
816.8°C
1502°F ; 1090 K
Note that arsenic will only melt under non-standard pressure conditions (28 atmospheres), and would otherwise sublime at a temperature lower than this.
Give the boiling point.
(Values rounded to 4sf)
685.0°C
1265°F ; 958.2 K
Selenium, a nonmetal, has a moderately low boiling point when taking into consideration other elements of the same period.
Give the melting point.
(Values rounded to 4sf)
220.8°C
429.4°F ; 494.0 K
Selenium has a relatively low melting point, but is still easily a solid under standard conditions.
It would however be turned to a liquid on the surface of Venus (~464°C)!
Give the boiling point.
(Values rounded to 4sf)
58.80°C
137.8°F ; 332.0 K
Bromine is a nonmetal with a low boiling point, meaning little energy is required to overcome the forces of attraction between liquid bromine molecules in order to become its gaseous form.
Give the melting point.
(Values rounded to 4sf)
−7.200°C
19.04°F ; 266.0 K
Bromine has a relatively low melting point, making it a liquid at room temperature.
Give the boiling point.
(Values rounded to 4sf)
−153.4°C
−244.1°F ; 120.0 K
Because noble gases are monatomic structures, only weak London dispersion forces attract molecules to each other, leading to their very low boiling points as seen here.
Give the melting point.
(Values rounded to 4sf)
−157.4°C
−251.3°F ; 115.8 K
Krypton’s melting point is only a few degrees less than its boiling point (−153.4°C).
Give the boiling point.
(Values rounded to 4sf)
688.0°C
1270°F ; 961.2 K
Rubidium, an alkali metal, has a moderately low boiling point compared to other metals.
Alkali metals have lower melting and boiling points because of the wider interatomic distances in their crystal structures, meaning their bond energy is lower than other metals and easier to overcome with less heat needing to be applied.
Give the melting point.
(Values rounded to 4sf)
39.30°C
102.7°F ; 312.5 K
Rubidium has a low melting point, just above room temperature.
Alkali metals have lower melting and boiling points because of the wider interatomic distances in their crystal structures, meaning their bond energy is lower than other metals and easier to overcome with less heat needing to be applied.
Give the boiling point.
(Values rounded to 4sf)
1377°C
2511°F ; 1650 K
The boiling point of elements vary according to the applied pressure – all the data here assumes one atmosphere of pressure (standard condition).
Give the melting point.
(Values rounded to 4sf)
777.0°C
1431°F ; 1050 K
The melting point is the temperature at which the solid and liquid forms of a substance can exist in equilibrium.
Give the boiling point.
(Values rounded to 4sf)
3345°C
6053°F ; 3618 K
Adding solutes or other substances can change the boiling point, such as the case with alloys of varying elements and compositions.
Give the melting point.
(Values rounded to 4sf)
1522°C
2772°F ; 1795 K
The melting point is less dependent on pressure than the boiling point, but this is still an important factor affecting it.
This relationship though is not always as straightforward, and with some instances increased pressure after a certain point translates to a decrease in melting point.
Give the boiling point.
(Values rounded to 4sf)
4409°C
7968°F ; 4682 K
Zirconium, a transition metal, has a high boiling point.
The boiling point is the temperature at which the surrounding pressure exerted on the liquid is equal to the opposing pressure exerted by the vapour pressure of the liquid.
Give the melting point.
(Values rounded to 4sf)
1854°C
3369°F ; 2127 K
The stronger the bonding between particles in a substance, the more energy is required to overcome these forces of attraction, and therefore it will have a higher melting point.
Give the boiling point.
(Values rounded to 4sf)
4741°C
8566°F ; 5014 K
Applying heat to a liquid will increase its temperature right up to its boiling point.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the liquid particles, allowing it to transition to the gas phase.
Give the melting point.
(Values rounded to 4sf)
2477°C
4491°F ; 2750 K
Extra for Experts: Phase diagrams are charts used to depict the conditions (pressure and temperature mostly) at which thermodynamically distinct phases (i.e. solid, liquid, gas) occur or exist at equilibrium with each other.
The line representing the equilibrium between solid and liquid for niobium would intersect the coordinate (2477°C , 1 atm).
Give the boiling point.
(Values rounded to 4sf)
4639°C
8382°F ; 4912 K
Extra for Experts: The critical point on a phase diagram represents a temperature and pressure value at which the liquid and gaseous phases merge together to form a single phase.
This is found towards the top-right of a traditional phase diagram, and represents supercritical fluids.
Give the melting point.
(Values rounded to 4sf)
2622°C
4752°F ; 2895 K
Extra for Experts: On a phase diagram, the triple point represents where all lines of equilibrium between phases intersect.
This is the exact temperature and pressure at which a substance can stably exist as a solid, liquid, and gas in equilibrium.
Give the boiling point.
(Values rounded to 4sf)
4262°C
7704°F ; 4535 K
The heat of vaporisation (enthalpy of vaporisation) is the energy absorbed by a unit mass of a particular liquid once it’s reached its boiling point in order for it to convert fully into a gas, without a change in its temperature.
This also goes in the opposite direction, with it representing the amount of energy needed to be released for the substance to liquify again.
Give the melting point.
(Values rounded to 4sf)
2157°C
3915°F ; 2430 K
The heat of fusion (enthalpy of fusion) is the energy absorbed by a unit mass of a particular solid once it’s reached its melting point in order for it to convert fully into a liquid, without a change in its temperature.
This also goes in the opposite direction, with it representing the amount of energy needed to be released for the substance to solidify again.
Give the boiling point.
(Values rounded to 4sf)
4147°C
7497°F ; 4420 K
Boiling is a physical change rather than a chemical one, as this process is readily reversible and does not form a new substance, nor involve the transfer of electrons.
Give the melting point.
(Values rounded to 4sf)
2333°C
4231°F ; 2606 K
Alloys tend to have lower melting points than pure metals as the differing sizes of the atoms and their less regular arrangements leads to weaker bonding between them.
Give the boiling point.
(Values rounded to 4sf)
3695°C
6683°F ; 3968 K
The boiling point of elements vary according to the applied pressure – all the data here assumes one atmosphere of pressure (standard condition).
Give the melting point.
(Values rounded to 4sf)
1963°C
3565°F ; 2236 K
The melting point is the temperature at which the solid and liquid forms of a substance can exist in equilibrium.
Give the boiling point.
(Values rounded to 4sf)
2963°C
5365°F ; 3236 K
The boiling point is the temperature at which the surrounding pressure exerted on the liquid is equal to the opposing pressure exerted by the vapour pressure of the liquid.
Give the melting point.
(Values rounded to 4sf)
1555°C
2,831°F ; 1828 K
The melting point is less dependent on pressure than the boiling point, but this is still an important factor affecting it.
This relationship though is not always as straightforward, and with some instances increased pressure after a certain point translates to a decrease in melting point.
Give the boiling point.
(Values rounded to 4sf)
2162°C
3924°F ; 2435 K
Applying heat to a liquid will increase its temperature right up to its boiling point.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the liquid particles, allowing it to transition to the gas phase.
Give the melting point.
(Values rounded to 4sf)
961.8°C
1763°F ; 1235 K
Applying heat to a solid will increase its temperature right up to its melting point - note that this value for silver is relatively low.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the solid particles, allowing it to transition to the liquid phase.
Give boiling point.
(Values rounded to 4sf)
767.0°C
1413°F ; 1040 K
Cadmium has a relatively low boiling point, much like the other elements of this group (zinc and mercury).
This is because they have filled d-subshells and consequently the metallic bonding is weaker.
Give the melting point.
(Values rounded to 4sf)
321.1°C
609.9°F ; 594.2 K
Cadmium has weaker metallic bonding and so a lower melting point temperature.
Metallic bonding strength is determined by factors such as the number of protons in the metal cation, the number of delocalised electrons donated per atom, and the size of the ion (smaller ions lead to stronger bonds).
Give the boiling point.
(Values rounded to 4sf)
2027°C
3681°F ; 2300 K
The stronger the bonding between particles in a substance, the more energy is required to overcome these forces of attraction, and therefore it will have a higher boiling point.
Give the melting point.
(Values rounded to 4sf)
156.6°C
313.9°F ; 429.8 K
Indium is useful in making low melting-point alloys.
Give the boiling point.
(Values rounded to 4sf)
2586°C
4687°F ; 2859 K
The line on a phase diagram representing the equilibrium between liquid and gas for tin would intersect the coordinate (2586°C , 1 atm).
Give the melting point.
(Values rounded to 4sf)
231.9°C
449.5°F ; 505.1 K
Tin is a highly malleable metal with a relatively low melting point, reflective of weaker metallic bonding.
Metallic bonding strength is determined by factors such as the number of protons in the metal cation, the number of delocalised electrons donated per atom, and the size of the ion (smaller ions lead to stronger bonds).
Give the boiling point.
(Values rounded to 4sf)
1587°C
2889°F ; 1860 K
The (latent) heat of vaporisation, or enthalpy of vaporisation, is the energy absorbed by a unit mass of a particular liquid once it’s reached its boiling point in order for it to convert fully into a gas, without a change in its temperature.
This also goes in the opposite direction, with it representing the amount of energy needed to be released for the substance to liquify again (heat of condensation).
Give the melting point.
(Values rounded to 4sf)
630.6°C
1167°F ; 903.8 K
Powdered antimony can ignite at temperatures above its melting point and produce a green-white flame or even an explosion.
Give boiling point.
(Values rounded to 4sf)
988.0°C
1810°F ; 1261 K
Extra for Experts: On a phase diagram, the triple point represents where all lines of equilibrium between phases intersect.
This is the exact temperature and pressure at which a substance can stably exist as a solid, liquid, and gas in equilibrium.
Give the melting point.
(Values rounded to 4sf)
449.5°C
841.1°F ; 722.7 K
The (latent) heat of fusion, or enthalpy of fusion, is the energy absorbed by a unit mass of a particular solid once it’s reached its melting point in order for it to convert fully into a liquid, without a change in its temperature.
This also goes in the opposite direction, with it representing the amount of energy needed to be released for the substance to solidify again (heat of solidification).
Give the boiling point.
(Values rounded to 4sf)
184.4°C
363.9°F ; 457.6 K
The boiling point temperature will be higher with increased pressure.
Give the melting point.
(Values rounded to 4sf)
113.7°C
236.7°F ; 386.9 K
Applying heat to a solid will increase its temperature right up to its melting point.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the solid particles, allowing it to transition to the liquid phase.
Give the boiling point.
(Values rounded to 4sf)
-108.1°C
−162.6°F ; 165.1 K
Because noble gases are monatomic structures, only weak London dispersion forces attract molecules to each other, leading to their very low boiling points as seen here.
Give the melting point.
(Values rounded to 4sf)
−111.8°C
−169.2°F ; 161.4 K
Because noble gases are monatomic structures, only weak London dispersion forces attract molecules to each other, leading to their very low melting points as seen here.
Give the boiling point.
(Values rounded to 4sf)
671.0°C
1240°F ; 944 K
Applying heat to a liquid will increase its temperature right up to its boiling point.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the liquid particles, allowing it to transition to the gas phase.
Give the melting point.
(Values rounded to 4sf)
28.50°C
83.30°F ; 301.65 K
Alkali metals have lower melting and boiling points because of the wider interatomic distances in their crystal structures, meaning their bond energy is lower than other metals and easier to overcome with less heat needing to be applied.
Give boiling point.
(Values rounded to 4sf)
1845°C
3353°F ; 2118 K
Adding solutes or other substances can change the boiling point, such as the case with alloys of varying elements and compositions.
Give the melting point.
(Values rounded to 4sf)
727.0°C
1341°F ; 1000 K
The melting point is the temperature at which the solid and liquid forms of a substance can exist in equilibrium.
Give the boiling point.
(Values rounded to 4sf)
3464°C
6267°F ; 3737 K
Lanthanum has a very high boiling point.
The stronger the bonding between particles in a substance, the more energy is required to overcome these forces of attraction, and therefore it will have a higher boiling point.
Give the melting point.
(Values rounded to 4sf)
920.0°C
1688°F ; 1193 K
The melting point is less dependent on pressure than the boiling point, but this is still an important factor affecting it.
This relationship though is not always as straightforward, and with some instances increased pressure after a certain point translates to a decrease in melting point.
Give the melting point.
(Values rounded to 4sf)
3443°C
6229°F ; 3716 K
Cerium has a high boiling point.
The stronger the attractions between particles of a substance, the more energy there is required to overcome this, which is translated into higher boiling points.
Give the melting point.
(Values rounded to 4sf)
799.0°C
1470°F ; 1072 K
The line representing the equilibrium between solid and liquid for cerium would intersect the coordinate (799°C , 1 atm).
Give the boiling point.
(Values rounded to 4sf)
3520°C
6368°F ; 3793 K
Extra for Experts: Not all pure chemical substances have a triple point (where all three states of matter exist in equilibrium).
Give the melting point.
(Values rounded to 4sf)
931.0°C
1708°F ; 1204 K
Metallic bonding strength is determined by factors such as the number of protons in the metal cation, the number of delocalised electrons donated per atom, and the size of the ion (smaller ions lead to stronger bonds).
Give the boiling point.
(Values rounded to 4sf)
3074°C
5565°F ; 3347 K
The boiling point of elements vary according to the applied pressure – all the data here assumes one atmosphere of pressure (standard condition).
Give the melting point.
(Values rounded to 4sf)
1016°C
1861°F ; 1289 K
The melting point is the temperature at which the solid and liquid forms of a substance can exist in equilibrium.
Give the boiling point.
(Values rounded to 4sf)
3000°C
5432°F ; 3273 K
The boiling point is the temperature at which the surrounding pressure exerted on the liquid is equal to the opposing pressure exerted by the vapour pressure of the liquid.
Give the melting point.
(Values rounded to 4sf)
1042°C
1908°F ; 1315 K
The melting point is less dependent on pressure than the boiling point, but this is still an important factor affecting it.
This relationship though is not always as straightforward, and with some instances increased pressure after a certain point translates to a decrease in melting point.
Give the boiling point.
(Values rounded to 4sf)
1794°C
3261°F ; 2067 K
Applying heat to a liquid will increase its temperature right up to its boiling point.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the liquid particles, allowing it to transition to the gas phase.
Give the melting point.
(Values rounded to 4sf)
1072°C
1963°F ; 1345 K
Applying heat to a solid will increase its temperature right up to its melting point.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the solid particles, allowing it to transition to the liquid phase.
Give the boiling point.
(Values rounded to 4sf)
1529°C
2784°F ; 1802 K
The (latent) heat of vaporisation, or enthalpy of vaporisation, is the energy absorbed by a unit mass of a particular liquid once it’s reached its boiling point in order for it to convert fully into a gas, without a change in its temperature.
This also goes in the opposite direction, with it representing the amount of energy needed to be released for the substance to liquify again (heat of condensation).
Give the melting point.
(Values rounded to 4sf)
822.0°C
1512°F ; 1095 K
The (latent) heat of fusion, or enthalpy of fusion, is the energy absorbed by a unit mass of a particular solid once it’s reached its melting point in order for it to convert fully into a liquid, without a change in its temperature.
This also goes in the opposite direction, with it representing the amount of energy needed to be released for the substance to solidify again (heat of solidification).
Give the boiling point.
(Values rounded to 4sf)
3273°C
5923°F ; 3546 K
The stronger the bonding between particles in a substance, the more energy is required to overcome these forces of attraction, and therefore it will have a higher boiling point.
Give the melting point.
(Values rounded to 4sf)
1313°C
2395°F ; 1586 K
Melting is a physical change rather than a chemical one, as this process is readily reversible and does not form a new substance, nor involve the transfer of electrons.
Give the boiling point.
(Values rounded to 4sf)
3230°C
5846°F ; 3503 K
Extra for Experts: Not all pure chemical substances have a triple point (where all three states of matter exist in equilibrium).
Give the melting point.
(Values rounded to 4sf)
1359°C
2478°F ; 1632 K
Metallic bonding strength is determined by factors such as the number of protons in the metal cation, the number of delocalised electrons donated per atom, and the size of the ion (smaller ions lead to stronger bonds).
Give the boiling point.
(Values rounded to 4sf)
2567°C
4653°F ; 2840 K
Extra for Experts: only solids and gases exist in space because the pressure is zero and any liquid exposed would immediately boil or freeze.
Remember that pressure affects boiling points, as the vapour pressure of the liquid is at equilibrium with the surrounding pressure – liquids cannot stably exist in a zero-pressure environment (i.e. a vacuum).
Give the melting point.
(Values rounded to 4sf)
1412°C
2574°F ; 1685 K
The stronger the bonding between particles in a substance, the more energy is required to overcome these forces of attraction, and therefore it will have a higher melting point.
Give the boiling point.
(Values rounded to 4sf)
2700°C
4892°F ; 2973 K
Holmium has a high boiling point of 2700°C, which makes it useful in certain applications such as nuclear reactors and magnets.
Give the melting point.
(Values rounded to 4sf)
1472°C
2682°F ; 1745 K
Holmium has a relatively high melting point of 1472°C, which allows it to maintain its structural integrity at higher temperatures.
Give the boiling point.
(Values rounded to 4sf)
2868°C
5194°F ; 3141 K
The line representing the equilibrium between solid and liquid for erbium would intersect the coordinate (2868°C , 1 atm).
Give the melting point.
(Values rounded to 4sf)
1529°C
2784°F ; 1802 K
Erbium has a relatively high melting point of 1529°C, allowing it to maintain stability in relatively high-temperature applications.
Give the boiling point.
(Values rounded to 4sf)
1950°C
3542°F ; 2223 K
The (latent) heat of vaporisation, or enthalpy of vaporisation, is the energy absorbed by a unit mass of a particular liquid once it’s reached its boiling point in order for it to convert fully into a gas, without a change in its temperature.
This also goes in the opposite direction, with it representing the amount of energy needed to be released for the substance to liquify again (heat of condensation).
Give the melting point.
(Values rounded to 4sf)
1545°C
2813°F ; 1818 K
Thulium has a relatively high melting point of 1545°C, enabling it to withstand high-temperature environments.
Give the boiling point.
(Values rounded to 4sf)
1196°C
2185°F ; 1469 K
Applying heat to a liquid will increase its temperature right up to its boiling point.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the liquid particles, allowing it to transition to the gas phase.
Give the melting point.
(Values rounded to 4sf)
824.0°C
1515°F ; 1097 K
Ytterbium has a relatively low melting point of 824°C, which enables it to be easily manipulated and utilized in various technologies.
Give the boiling point.
(Values rounded to 4sf)
3402°C
6156°F ; 3675 K
Lutetium has a high boiling point, which contributes to its stability in high-temperature applications such as being a catalyst in oil refineries for hydrocarbon cracking.
Give the melting point.
(Values rounded to 4sf)
1663°C
3025°F ; 1936 K
The (latent) heat of fusion, or enthalpy of fusion, is the energy absorbed by a unit mass of a particular solid once it’s reached its melting point in order for it to convert fully into a liquid, without a change in its temperature.
This also goes in the opposite direction, with it representing the amount of energy needed to be released for the substance to solidify again (heat of solidification).
Give the boiling point.
(Values rounded to 4sf)
4600°C
8312°F ; 4873 K
Hafnium has a very high boiling point, which contributes to its durability and heat resistance in various industrial applications.
Give the melting point.
(Values rounded to 4sf)
2233°C
4051°F ; 2506 K
Hafnium has a relatively high melting point of 2233°C, making it suitable for use in high-temperature environments such as nuclear reactors.
Give the boiling point.
(Values rounded to 4sf)
5455°C
9851°F ; 5728 K
Extra for Experts: On a phase diagram, the triple point represents where all lines of equilibrium between phases intersect.
This is the exact temperature and pressure at which a substance can stably exist as a solid, liquid, and gas in equilibrium.
Give the melting point.
(Values rounded to 4sf)
3017°C
5463°F ; 3290 K
Melting is a physical change rather than a chemical one, as this process is readily reversible and does not form a new substance, nor involve the transfer of electrons.
Give the boiling point.
(Values rounded to 4sf)
5555°C
10,031°F ; 5828 K
Tungsten has what may be considered an exceptionally high boiling point.
Give the melting point.
(Values rounded to 4sf)
3414°C
6177°F ; 3687 K
Tungsten has the highest known melting point of all elements.
Give the boiling point.
(Values rounded to 4sf)
5590°C
10,094.6°F ; 5863 K
Rhenium has the highest known boiling point of all elements.
Give the melting point.
(Values rounded to 4sf)
3185°C
5765°F ; 3458 K
Rhenium has a high melting point, allowing it to withstand extreme temperatures in applications such as superalloys and electrical contacts.
Give the boiling point.
(Values rounded to 4sf)
5008°C
9046°F ; 5281 K
The boiling point of elements vary according to the applied pressure – all the data here assumes one atmosphere of pressure (standard condition).
Give the melting point.
(Values rounded to 4sf)
3033°C
5491°F ; 3306 K
Metallic bonding strength is determined by factors such as the number of protons in the metal cation, the number of delocalised electrons donated per atom, and the size of the ion (smaller ions lead to stronger bonds).
Give the boiling point.
(Values rounded to 4sf)
4428°C
8002°F ; 4701 K
The boiling point is the temperature at which the surrounding pressure exerted on the liquid is equal to the opposing pressure exerted by the vapour pressure of the liquid.
Give the melting point.
(Values rounded to 4sf)
2466°C
4471°F ; 2719 K
The melting point is the temperature at which the solid and liquid forms of a substance can exist in equilibrium.
Give the boiling point.
(Values rounded to 4sf)
3825°C
6917°F ; 4098 K
Applying heat to a liquid will increase its temperature right up to its boiling point.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the liquid particles, allowing it to transition to the gas phase.
Give the melting point.
(Values rounded to 4sf)
1768°C
3215°F ; 2041 K
Platinum has a relatively high melting point, allowing it to maintain its shape and effectiveness in high-temperature applications such as laboratory equipment and electronics.
Give the boiling point.
(Values rounded to 4sf)
2836°C
5137°F ; 3109 K
Adding solutes or other substances can change the boiling point, such as the case with gold alloys of varying elements and compositions.
Give the melting point.
(Values rounded to 4sf)
1064°C
1948°F ; 1337 K
Applying heat to a solid will increase its temperature right up to its melting point.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the solid particles, allowing it to transition to the liquid phase.
Give the boiling point.
(Values rounded to 4sf)
356.6°C
673.9°F ; 629.8 K
Mercury can evaporate even at room temperature, making it dangerous to handle in its liquid form.
Give the melting point.
(Values rounded to 4sf)
−38.83°C
−37.89°F ; 234.3 K
Mercury has a relatively low melting point of −38.83°C, making it a liquid at room temperature.
Give the boiling point.
(Values rounded to 4sf)
1473°C
2683°F ; 1746 K
The stronger the bonding between particles in a substance, the more energy is required to overcome these forces of attraction, and therefore it will have a higher boiling point.
Give the melting point.
(Values rounded to 4sf)
304.0°C
579.2°F ; 577.2 K
Small amounts of thallium can be alloyed with mercury to lower the melting point temperature by 20°C and allow it to be used in low-temperature thermometers and switches.
Give the boiling point.
(Values rounded to 4sf)
1749°C
3180°F ; 2022 K
The line representing the equilibrium between liquid and gas for lead would intersect the coordinate (1749°C , 1 atm).
Give the melting point.
(Values rounded to 4sf)
327.5°C
621.4°F ; 600.6 K
Lead has a relatively low melting point, making it malleable and easily shaped.
Give the boiling point.
(Values rounded to 4sf)
1564°C
2847°F ; 1837 K
The (latent) heat of vaporisation, or enthalpy of vaporisation, is the energy absorbed by a unit mass of a particular liquid once it’s reached its boiling point in order for it to convert fully into a gas, without a change in its temperature.
This also goes in the opposite direction, with it representing the amount of energy needed to be released for the substance to liquify again (heat of condensation).
Give the melting point.
(Values rounded to 4sf)
271.4°C
520.5°F ; 544.6 K
Bismuth has a relatively low melting point, making it suitable for use in low-melting alloys and fire detector systems.
Give the boiling point.
(Values rounded to 4sf)
962.0°C
1764°F ; 1235 K
Applying heat to a liquid will increase its temperature right up to its boiling point.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the liquid particles, allowing it to transition to the gas phase.
Give the melting point.
(Values rounded to 4sf)
254.0°C
489.2°F ; 527.2 K
Due to its radioactivitiy, a gram of polonium would produce so much heat it melts itself!
Give the boiling point.
(Values rounded to 4sf)
350.0°C
662.0°F ; 623.2 K
Astatine’s boiling point is only 50°C above its melting point.
Give the melting point.
(Values rounded to 4sf)
300.0°C
572.0°F ; 573.2 K
Any visible quantities of astatine would immediately be vaporised by the heat released from its radioactivity.
Give the boiling point.
(Values rounded to 4sf)
−61.70°C
−79.10°F ; 211.4 K
Because noble gases are monatomic structures, only weak London dispersion forces attract molecules to each other, leading to their very low boiling points as seen here.
Give the melting point.
(Values rounded to 4sf)
−71.00°C
−96.00°F ; 202.2 K
Because noble gases are monatomic structures, only weak London dispersion forces attract molecules to each other, leading to their very low melting points as seen here.
Give the boiling point.
(Values rounded to 4sf)
650.0°C
1202°F ; 923.0 K
Alkali metals have lower melting and boiling points because of the wider interatomic distances in their crystal structures, meaning their bond energy is lower than other metals and easier to overcome with less heat needing to be applied.
Give the melting point.
(Values rounded to 4sf)
21.00°C
70.00°F ; 294.2 K
Alkali metals have lower melting and boiling points because of the wider interatomic distances in their crystal structures, meaning their bond energy is lower than other metals and easier to overcome with less heat needing to be applied.
Give the boiling point.
(Values rounded to 4sf)
1500°C
2732°F ; 1773 K
Extra for Experts: Not all pure chemical substances have a triple point (where all three states of matter exist in equilibrium).
Give the melting point.
(Values rounded to 4sf)
696.0°C
1285°F ; 969.0 K
Alloys tend to have lower melting points than pure metals as the differing sizes of the atoms and their less regular arrangements leads to weaker bonding between them.
Give the boiling point.
(Values rounded to 4sf)
3200°C
5792°F ; 3473 K
The (latent) heat of vaporisation, or enthalpy of vaporisation, is the energy absorbed by a unit mass of a particular liquid once it’s reached its boiling point in order for it to convert fully into a gas, without a change in its temperature.
This also goes in the opposite direction, with it representing the amount of energy needed to be released for the substance to liquify again (heat of condensation).
Give the melting point.
(Values rounded to 4sf)
1050°C
1922°F ; 1323 K
Melting is a physical change rather than a chemical one, as this process is readily reversible and does not form a new substance, nor involve the transfer of electrons.
Give the boiling point.
(Values rounded to 4sf)
4785°C
8645°F ; 5058 K
The boiling point is the temperature at which the surrounding pressure exerted on the liquid is equal to the opposing pressure exerted by the vapour pressure of the liquid.
Give the melting point.
(Values rounded to 4sf)
1750°C
3182°F ; 2023 K
Applying heat to a solid will increase its temperature right up to its melting point.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the solid particles, allowing it to transition to the liquid phase.
Give the boiling point.
(Values rounded to 4sf)
4000°C
7232°F ; 4273 K
Protactinium has a high boiling point, which contributes to its stability in high-temperature environments.
Give the melting point.
(Values rounded to 4sf)
1572°C
2862°F ; 1845 K
Applying heat to a liquid will increase its temperature right up to its boiling point.
Once this is reached, additional heat will not change the temperature but instead go into providing energy to overcome the forces of attraction between the liquid particles, allowing it to transition to the gas phase.
Give the boiling point.
(Values rounded to 4sf)
4131°C
7468°F ; 4404 K
Uranium has a high boiling point, contributing to its stability and reliability in high-temperature applications such as nuclear reactors and nuclear weapons.
Give the melting point.
(Values rounded to 4sf)
1135°C
2075°F ; 1408 K
The melting point is less dependent on pressure than the boiling point, but this is still an important factor affecting it.
This relationship though is not always as straightforward, and with some instances increased pressure after a certain point translates to a decrease in melting point.
Give the boiling point.
(Values rounded to 4sf)
3902°C
7056°F ; 4175 K
The boiling point of elements vary according to the applied pressure – all the data here assumes one atmosphere of pressure (standard condition).
Give the melting point.
(Values rounded to 4sf)
644.0°C
1191°F ; 917.2 K
Neptunium has a relatively low melting point, which allows it to be manipulated with applied heat.
Give the boiling point.
(Values rounded to 4sf)
3228°C
5842°F ; 3501 K
Plutonium has a high boiling point, which contributes to its stability in high-temperature environments.
Give the melting point.
(Values rounded to 4sf)
639.5°C
1183°F ; 912.7 K
Plutonium has a relatively low melting point, allowing it to be easily shaped and used in various scientific and nuclear applications.
Give the boiling point.
(Values rounded to 4sf)
2011°C
3652°F ; 2284 K
The stronger the bonding between particles in a substance, the more energy is required to overcome these forces of attraction, and therefore it will have a higher boiling point.
Give the melting point.
(Values rounded to 4sf)
1176°C
2149°F ; 1449 K
The stronger the bonding between particles in a substance, the more energy is required to overcome these forces of attraction, and therefore it will have a higher melting point.
Give the boiling point.
(Values rounded to 4sf)
~3110°C
~5630°F ; ~3383 K
This value is an estimate due to limited data.
Give the melting point.
(Values rounded to 4sf)
1345°C
2453°F ; 1618 K
Curium has a relatively high melting point, enabling it to maintain stability and integrity under high-temperature conditions.
Give the boiling point.
(Values rounded to 4sf)
Unknown
The boiling point of berkelium is not well-documented due to its rarity and limited availability for study.
Give the melting point.
(Values rounded to 4sf)
986.0°C
1807°F ; 1259 K
Metallic bonding strength is determined by factors such as the number of protons in the metal cation, the number of delocalised electrons donated per atom, and the size of the ion (smaller ions lead to stronger bonds).
Give the boiling point.
(Values rounded to 4sf)
Unknown
The boiling point of californium is not well-documented due to its rarity and limited availability for study.
Give the melting point.
(Values rounded to 4sf)
900.0°C
1652°F ; 1173 K
Extra for Experts: Not all pure chemical substances have a triple point (where all three states of matter exist in equilibrium).
Give the boiling point.
(Values rounded to 4sf)
Unknown
Unknown
The boiling point of einsteinium is not well-documented due to its rarity and limited availability for study.
Give the melting point.
(Values rounded to 4sf)
860.0°C
1580°F ; 1133 K
Melting is a physical change rather than a chemical one, as this process is readily reversible and does not form a new substance, nor involve the transfer of electrons.
Give the boiling point.
(Values rounded to 4sf)
Unknown
Unknown
The boiling point of fermium is not well-documented due to its rarity and limited availability for study.
Give the melting point.
(Values rounded to 4sf)
1527°C
2781°F ; 1800 K
Alloys tend to have lower melting points than pure metals as the differing sizes of the atoms and their less regular arrangements leads to weaker bonding between them.
Give the boiling point.
(Values rounded to 4sf)
Unknown
Mendelevium is a synthetic element, and its boiling point has not been accurately determined.
Give the melting point.
(Values rounded to 4sf)
~827.0°C
~1521°F ; ~1100 K
Mendelevium is a synthetic element, and its melting point has not been accurately determined.
The given value is an estimated approximation.
Give the boiling point.
(Values rounded to 4sf)
Unknown
Nobelium is a synthetic element, and its boiling point has not been accurately determined.
Give the melting point.
(Values rounded to 4sf)
~827.0°C
~1521°F ; ~1100 K
Nobelium is a synthetic element, and its melting point has not been accurately determined.
The given value is an estimated approximation.
Give the boiling point.
(Values rounded to 4sf)
Unknown
Lawrencium is a synthetic element, and its boiling point has not been accurately determined.
Give the melting point.
(Values rounded to 4sf)
~1627°C
~2961°F ; ~1900 K
Lawrencium is a synthetic element, and its melting point has not been accurately determined.
The given value is an estimated approximation.
Give the boiling point.
(Values rounded to 4sf)
Unknown
Rutherfordium is a synthetic element, and its boiling point has not been accurately determined.
Give the melting point.
(Values rounded to 4sf)
Unknown
The melting point of Rutherfordium has not been accurately determined.
Further research is needed to establish this value.
Give the boiling point.
(Values rounded to 4sf)
Unknown
The boiling point of Dubnium has not been accurately determined.
Further research is needed to establish this value.
Give the melting point.
(Values rounded to 4sf)
Unknown
The melting point of Dubnium has not been accurately determined.
Further research is needed to establish this value.
Give the boiling point.
(Values rounded to 4sf)
Unknown
The boiling point of Seaborgium has not been accurately determined.
Further research is needed to establish this value.
Give the melting point.
(Values rounded to 4sf)
Unknown
The melting point of Seaborgium has not been accurately determined.
Further research is needed to establish this value.
Give the boiling point.
(Values rounded to 4sf)
Unknown
The boiling point of Bohrium has not been accurately determined.
Further research is needed to establish this value.
Give the melting point.
(Values rounded to 4sf)
Unknown
The melting point of Bohrium has not been accurately determined.
Further research is needed to establish this value.
Give the boiling point.
(Values rounded to 4sf)
Unknown
The boiling point of Hassium has not been accurately determined.
Further research is needed to establish this value.
Give the melting point.
(Values rounded to 4sf)
Unknown
The melting point of Hassium has not been accurately determined.
Further research is needed to establish this value.
Give the boiling point.
(Values rounded to 4sf)
Unknown
The boiling point of Meitnerium has not been accurately determined.
Further research is needed to establish this value.
Give the melting point.
(Values rounded to 4sf)
Unknown
The melting point of Meitnerium has not been accurately determined.
Further research is needed to establish this value.
Give the boiling point.
(Values rounded to 4sf)
Unknown
The boiling point of Darmstadtium has not been accurately determined.
Further research is needed to establish this value.
Give the melting point.
(Values rounded to 4sf)
Unknown
The melting point of Darmstadtium has not been accurately determined.
Further research is needed to establish this value.
Give the boiling point.
(Values rounded to 4sf)
Unknown
The boiling point of Roentgenium has not been accurately determined.
Further research is needed to establish this value.
Give the melting point.
(Values rounded to 4sf)
Unknown
The melting point of Roentgenium has not been accurately determined.
Further research is needed to establish this value.
Give the boiling point.
(Values rounded to 4sf)
Unknown
Copernicium is a synthetic element, and its boiling point has not been accurately determined.
Give the melting point.
(Values rounded to 4sf)
Unknown
The melting point of Copernicium has not been accurately determined.
Further research is needed to establish this value.
Give the boiling point.
(Values rounded to 4sf)
Unknown
Nihonium is a synthetic element, and its boiling point has not been accurately determined.
Give the melting point.
(Values rounded to 4sf)
Unknown
The melting point of Nihonium has not been accurately determined.
Further research is needed to establish this value.
Give the boiling point.
(Values rounded to 4sf)
Unknown
Flerovium is a synthetic element, and its boiling point has not been accurately determined.
Give the melting point.
(Values rounded to 4sf)
Unknown
The melting point of Flerovium has not been accurately determined.
Further research is needed to establish this value.
Give the boiling point.
(Values rounded to 4sf)
Unknown
The boiling point of Moscovium has not been accurately determined.
Further research is needed to establish this value.
Give the melting point.
(Values rounded to 4sf)
Unknown
The melting point of Moscovium has not been accurately determined.
Further research is needed to establish this value.
Give the boiling point.
(Values rounded to 4sf)
Unknown
The boiling point of Livermorium has not been accurately determined.
Further research is needed to establish this value.
Give the melting point.
(Values rounded to 4sf)
Unknown
The melting point of Livermorium has not been accurately determined.
Further research is needed to establish this value.
Give the boiling point.
(Values rounded to 4sf)
Unknown
The boiling point of Tennessine has not been accurately determined.
Further research is needed to establish this value.
Give the melting point.
(Values rounded to 4sf)
Unknown
The melting point of Tennessine has not been accurately determined.
Further research is needed to establish this value.
Give the boiling point.
(Values rounded to 4sf)
Unknown
The boiling point of Oganesson has not been accurately determined.
Further research is needed to establish this value.
Give the melting point.
(Values rounded to 4sf)
Unknown
The melting point of Oganesson has not been accurately determined.
Further research is needed to establish this value.
