Asked by: Isora Molenaar
science chemistry

Why does propene have a higher boiling point than ethene?

Last Updated: 19th June, 2021

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Boiling Points
Ethene, propene and the various butenes are gases at room temperature. Boiling points of alkenes depends on more molecular mass (chain length). The more intermolecular mass is added, the higher the boiling point. Intermolecular forces of alkenes gets stronger with increase in the size of the molecules.

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Correspondingly, why does ethene have a higher boiling point than ethane?

Ethane has stronger intermolecular attractions (van der Waal's forces) than ethene and so has the higher boiling point.

Similarly, do double bonds have higher boiling points? I thought they were more stable so they would have a higher boiling point. Cis double bonds prevent the tight packing between the hydrocarbon chain, thus lowering intermolecular attractions. This decreases boiling point.

Moreover, why do alkanes have higher boiling points?

As the chain length (numbers of carbons) increases the melting and boiling points of the alkanes gradually increase for these compounds. The reason that longer chain molecules have higher boiling points is that longer chain molecules become wrapped around and enmeshed in each other much like the strands of spaghetti.

What has the highest boiling point?

Carbon has the highest melting point at 3823 K (3550 C) and Rhenium has the highest boiling point at 5870 K (5594 C). According to google, Tungsten boils at 5555 C, but rhenium is 39 C higher at 5594 C. Also according to google, Tungsten melts at 3422 C, but Carbon's melting point is 128 C hotter, at 3550 C.

Related Question Answers

Yiling Uemlyanin

Professional

Which alkene has the highest boiling point?

Ethene, propene and the various butenes are gases at room temperature. All the rest that you are likely to come across are liquids. Boiling points of alkenes depends on more molecular mass (chain length). The more intermolecular mass is added, the higher the boiling point.

Hossein Chairi

Professional

Which alkane has the highest boiling point?

In an alkane, each carbon atom is sp3-hybridized with 4 sigma bonds (either C–C or C–H), and each hydrogen atom is joined to one of the carbon atoms (in a C–H bond).

Table of alkanes.
Alkane Methane
Boiling point [°C] -162
Melting point [°C] −182
Density [kg/m3] (at 20 °C) 0.656 (gas)
Straight-chain isomers 1

Najlaa Illarreta

Professional

Why ethane has low boiling point?

Ethane is a small molecule, consisting of two carbon atoms and 6 hydrogens. Small and nonpolar molecules don't have any intermolecular forces other than the London dispersion forces. Thus, since these forces aren't strong at all, it's not hard to break them, which therefore results in a low boiling point.

Sghir Lord

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Which normal alkene has the highest boiling point at 1 atmosphere?

Which normal alkene has the highest boiling point at 1 atmosphere? (1) C2H4; (2) C3H6; (4) C5H10.

Larraine Pawels

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Do alkynes have higher boiling points?

Alkynes have higher boiling points than alkanes or alkenes, because the electric field of an alkyne, with its increased number of weakly held π electrons, is more easily distorted, producing stronger attractive forces between molecules.

Rana Musalnikov

Explainer

Why do alkanes have low boiling points?

Melting and Boiling Point
Alkanes have low melting or boiling points because of the very weak intermolecular forces between alkane molecules. As the carbon chain gets longer, there are more electrons in a molecule. This means that there are more (relatively) stronger intermolecular forces between the molecules.

Eumelia Benages

Pundit

What are the properties of alkanes?

Solid alkanes are normally soft, with low melting points. These characteristics are due to strong repulsive forces generated between electrons on neighboring atoms, which are in close proximity in crystalline solids. The strong repulsive forces counterbalance the weak van der Waals forces of attraction.

Yunying Fornaro

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Which isomer has a higher boiling point?

In each case, the higher melting or boiling point is shown in red. You will notice that: the trans isomer has the higher melting point; the cis isomer has the higher boiling point.

Benyahia Redrado

Pundit

Why do alkenes have lower boiling points?

Intermolecular forces of alkenes gets stronger with increase in the size of the molecules. In each case, the alkene has a boiling point which is a small number of degrees lower than the corresponding alkane. Each alkene has 2 fewer electrons than the alkane with the same number of carbons.

Lester Narbalatz

Pundit

Why does branching increase stability?

The branching, it seems, means that the electronic structure is simply more compact and this decreases molecular surface area per atom and so leads to a lowering of energy and a concomitant increase in stability.

Peligros Muhlbach

Pundit

How branching affects boiling point?

Branching decreases the boiling point
So the increase of surface area increases the ability of individual molecules to attract each other. Branching in molecules decreases the surface area thereby decreasing the attractive force between individual molecules. As a result, the boiling point decreases.

Virgil Faulbaum

Teacher

Which hydrocarbon has the highest boiling point?

Boiling Points
Molecular Name Formula Boiling Point (°C)
methane CH 4 –164
ethane C 2H 6 –89
propane C 3H 8 –42
butane C 4H 10 –1

Marline Lisiecki

Beginner

Sia Ming

Beginner

Which intermolecular force has the highest boiling point?

The intermolecular forces increase with increasing polarization of bonds. The strength of intermolecular forces (and therefore impact on boiling points) is ionic > hydrogen bonding > dipole dipole > dispersion. Boiling point increases with molecular weight, and with surface area.

Shazia Androsik

Beginner

How do you determine melting point?

The melting point of an organic solid can be determined by introducing a tiny amount into a small capillary tube, attaching this to the stem of a thermometer centred in a heating bath, heating the bath slowly, and observing the temperatures at which melting begins and is complete.