Chemical Elements: Boiling Points Flashcards
Recall each element's boiling points to two decimal places.
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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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)
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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 boiling point.
(Values rounded to 4sf)
~3110°C
~5630°F ; ~3383 K
This value is an estimate due to limited data.
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 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 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 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 boiling point.
(Values rounded to 4sf)
Unknown
Mendelevium is a synthetic element, and its boiling point has not been accurately determined.
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 boiling point.
(Values rounded to 4sf)
Unknown
Lawrencium is a synthetic element, and its boiling point has not been accurately determined.
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 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 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 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 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 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 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 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 boiling point.
(Values rounded to 4sf)
Unknown
Copernicium is a synthetic element, and its boiling point has not been accurately determined.
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 boiling point.
(Values rounded to 4sf)
Unknown
Flerovium is a synthetic element, and its boiling point has not been accurately determined.
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 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 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 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.
